lewis structure

In this article we are going to discuss the ba(oh)2 lewis structure and 13 important facts regarding its lewis structure and characteristics.

Barium hydroxide is produced when barium oxide is dissolved in water. It exists in white granular form. It is used as a dehydrating agent and used for the removal of sulphur from various compounds.

Ba(oh)2 Lewis Structure Drawing

Ba(oh)2 is formed by two elements i.e. one is barium atom and the other is hydroxide group. Ba is a congener of alkaline earth metal i.e. group (II) and oxygen is a congener of group 16 family. Barium has atomic number of 56. Its outermost shell electronic configuration is [Xe] 6s2. When it losses two electrons it gains the nearest noble gas configuration of Xe.

When Ba atom lost its 2 electrons Ba+2 ion is produced. In case of hydroxide radical, O atom is singly bonded with H atom i.e. it contains a total of 7 electrons. When 2 Oh radicals gains 1 electron each which are rejected by Ba it gets stable nearest noble gas configuration of Ne. Then Ba+2 and 2 Oh- ions are attached by columbic force of attraction and ba(oh)2 is formed.

Ba(oh)2 Lewis Structure Resonance

Resonance is an empirical method in which electrons moving from one atom to another by losing and gaining of electrons. Barium hydroxide is a neutral compound with zero formal charge (f.c) on it. As resonance takes place Ba(oh)2  breaks into Ba+2ion and 2 OH- ions.

Both barium and hydroxide ions are stabilized because both gains stable nearest noble gas configuration after resonance i.e. Ba2+ ion possess Xenon (Xe) noble electronic configuration and hydroxide ion acquires Neon (Ne) noble gas configuration, both the ions fulfilled their octet after resonance.

Ba(oh)2 Lewis structure shape

According to VSEPR theory ba(oh)2 has octahedral co-ordination geometry. In the crystal structure of ba(oh)2 6 Ba2+ ions are surrounding by 6 Oh- ions and 6 Oh- ions are surround by 6 Ba2+ ions.

For this reason both Ba2+ and Oh- ions have co-ordination number equals to 6. Because of this fact that ba(oh)2 has octahedral shape and acquires d2sp3 hybridization.

Ba(oh)2 Lewis Structure Formal Charges

In barium hydroxide overall formal charge on the compound is Zero. Ba(oh)2 ionizes to form Ba2+ and 2 Oh- ions. Barium has +2 formal charges which are cancelled out by 2 hydroxide -1 formal charge.

In the cubic crystal lattice structure of barium hydroxide 6 Ba2+ ions are surround by 6 Oh- ions and 6 Oh- ions are surrounded by 6 Ba2+ ions making the whole compound is electrically neutral.

Ba(oh)2 Lewis structure angle

As we seen from ba(oh)2 lewis structure, ba(oh)2 has octahedral geometry with d2sp3 hybridization and according to octahedral geometry the angle must be 900. Ba(oh)2 also possess the same bond angle which is equal to 900.

Ba(oh)2 Lewis Structure Octet Rule

In the lewis structure of barium hydroxide both barium and hydroxide ions fulfilled their octet. When ba(oh)2 is produced ba lost its two electrons from valance shell to acquire the nearest noble gas configuration of Xe which have 8 electrons in its valance shell (5s²5p⁶) i.e. octet is fulfilled.

Hydroxide radical gains two electrons which is rejected by ba atom to acquires the nearest noble gas configuration of neon which also possessed 8 valance electrons (2s2 2p6). Hence both barium and oh radical fulfilled their octet.

Ba(oh)2 Lewis Structure Lone Pairs

When we see the ba(oh)2 lewis structure zero lone pair present on Ba atom and 1 lone pair of electrons present on hydroxide ion.

This is due to the fact that barium losses its two electron to form Ba2+ion which does not contain any lone pair of electron in it. But 2 Oh radical gains 1 electron each which is rejected by Ba atom and is converted into 2 Oh- ions in which 1 lone pair of electrons present on each Oh- ion.

Ba(oh)2 Valance Electrons

Firstly to find out the total no of valance electron in Ba(oh)2, it is important to find out the electronic configuration of Ba atom. The electronic configuration of Ba atom is [Xe] 6s2 and we see from electronic configuration of ba that there are 2 electrons in the valance shell of Ba atom.

There is 7 electrons in the Oh radical. The total valance electrons that exist on ba(oh)2 will be equal to the (sum of the valance electron of Ba atom and oh radical) i.e. equals to (1*2)+(7*2)=16. There are 16 valance electrons in ba(oh)2.

Ba(oh)2 Hybridization

When ba(oh)2 breaks down Ba+2 and 2 Oh-ions are formed. Barium hydroxide exists in a cubic crystal lattice structure. Both barium atom and hydroxide radical possess d2sp3 hybridization i.e. ba(oh)2 has octahedral co-ordination geometry.

In the crystal lattice structure of barium hydroxide each Ba+2 ion is surrounded by six Oh- ions and each Oh-ion is surrounded by 6 Ba+2ions. Hence both barium ion and htdroxide ion have same co-ordination number which is equal to 6.

Ba(oh)2 Solubility

In ba(oh)2 due to greater electronegativity of oh group and lesse electronegativity of barium atom it exists in Ba2+ and 2 oh- ions i.e. opposite dipoles are produced. As different dipoles created on Ba2+ and oh- ions it is a polar compound.

It is soluble in polar solvents e.g. ethanol (C2H5OH), dilute mineral acids like HCl, HBr, HF etc and also soluble in water. But it is not soluble in nonpolar solvents like acetone, ether etc. When barium hydroxide reacts with water it produces Ba2+ ions and hydroxide ions. This medium is basic in nature.

Is Ba(oh)2 Ionic?

Ba(oh)2 is an ionic compound. This is due to the fact that ba(oh)2 disintrigates to give Ba2+ and Oh- ions when it dissolves in aqueous solution or in molten state. This is an essential characteristic of ionic compound.

It conducts electricity in aqueous or in molten state. This is because of the presence of Ba2+ and Oh- ions in both the states and we also know that ions carry current. Like ionic compounds ba(oh)2 is soluble in polar solvents for example water, methanol etc.

Is Ba(oh)2 Polar Or Nonpolar?

Barium hydroxide is a polar compound. This is because of the fact that in barium hydroxide both barium atom and hydroxide radical have difference in electronegativity and hence opposite dipole creates on barium and hydroxide radical.

Due to lower electronegativity of barium it acquires positive dipole on it and due to higher electronegativity of O atom Oh radical possesses negative dipole. As because opposite dipoles creates on barium hydroxide, it is an ionic compound with high dipole moment. Hence ba(oh)2 is a polar compound.

Is Ba(oh)2 acidic or basic?

Ba has greater tendency to loss electrons i.e. it has metallic characteristics. Ba(oh)2 is basic in nature. This is due to the fact that it is a hydroxide of a metal which usually basic in nature.

When we dissolve barium hydroxide in water, it dissociates in water to form Ba2+ and Oh- ions. We know from Arrhenius theory that the compound which gives Oh- ions in solution are alkaline or basic in nature.

By considering the above mentioned facts we can conclude that ba(oh)2 is a stable ionic compound. As it is an ionic compound it is polar in nature as well as soluble in polar hydrophilic solvents and ba(oh)2 is an alkaline hydroxide because it gives Oh- ions in aqueous solution.

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Bromo difluoride (BrF₂) can be considered as a interhalogen compound. Here we will discuss about the BrF₂ Lewis structure and how it helped us to study about its geometry, hybridisation, lone pairs etc.

There are a total of 21 valence electrons in Brf2 Lewis structure in which the central atom bromine (Br) has 9 electrons in its outer shell ie 4 electrons from the bonds formed with 2 fluorine atoms and 5 non bonded (2 lone pairs and one unpaired) electrons. It violates the octet rule.

Brf2 valence electrons

BrF₂ compound has 21 odd number valence electrons in its outer most shell.

Bromine and fluorine both belongs to the p block elements and also comes under the 17^th group. We know that the valence electron number of an atom will be 10 minus its group number so,

Valence electron of Br = 17-10 = 7

Valence electron of F = 17-10 = 7

Therefore, the total valence electron of BrF₂ = 7 + 7(2) =21

How to draw Brf2 Lewis structure?

BrF2 Lewis structure is drawn depending on the valence electrons of Br and F atoms.

1)Know the total number of valence electrons present

Total number of valence electrons present in BrF₂ is 21 (7 electrons from bromine and 14 electrons from 2 fluorine atoms).

2)Select the less electronegative atom as the central atom and place the remaining atoms around surrounding the central atom.

Br is less electronegative compared to F atom and hence is selected as the central atom and the 2 fluorine atoms are placed around Br

  F     Br     F

3)Bond the central atom and outer atoms by pairing its valence electrons.

  F  :  Br  :   F

Among the 21 valence electrons of BrF₂ 4 valence electrons are used for bond formation between bromine and 2 fluorine atoms so there are remaining 17 non bonded electrons present.

4)The remaining non-bonded electrons are distributed among the atoms to complete its octet.

There are 17 non bonded electrons present and hence each fluorine atoms take 6 electrons each from non-bonded electrons to complete its octet (6 from non-bonded electrons and 2 from single bond formed with bromine). Thus 2 fluorine atoms take 12 nonbonded electrons.

The remaining 5 non bonded electrons are placed on Br atom thus it acquires a total of 9 electrons (5 from nonbonded electrons and 4 from bond formed) as it can have an expanded octet.

Brf2 Lewis structure lone pairs

If we look into central atom Br in the BrF2 Lewis structure it has 5 non bonded electrons in it. It means it has Br has 2 lone pair of electrons and a single unpaired electron

 There are 6 non bonded electrons present in each fluorine atom i.e. there are 3 lone pair of electrons present in each fluorine atom.

Brf2 Lewis structure octet rule

BrF₂ violate the octet rule of having 8 electrons configuration because the central domain atom Br has 9 electrons in its outermost shell and can have an expanded octet.

The reason is Br atom belongs to the 4^th period on the periodic table having n=4 so it has an empty 4d orbital which can accommodate more electrons and can take part in hybridisation.

Brf2 Lewis structure formal charge

Formal charge of Brf2 Lewis structure is zero.

Formal charge on an atom in a Lewis structure = total number of valence electrons in the free atom -the total number of non-bonding (lone pair) electrons -half the total number of bonding electrons.

Formal charge on Bromine atom

Total number of valence electrons in bromine atom = 7

Total number of non-bonding electrons in bromine = 5

Total number of bonding electrons in bromine atom =4

 Formal charge = 7-5-4/2 = 7-5-2 =7-7 = 0

Therefore, the formal charge of bromine atom is = 0

Formal charge on fluorine atom

Total number of valence electrons in fluorine atom = 7

Total number of non-bonding electrons in fluorine = 6

Total number of bonding electrons in fluorine atom =2

 Formal charge = 7-6-2/2 =7-6-1 =0

Therefore, the formal charge of fluorine atom is = 0

Thus, the total formal charge of the atoms in BrF₂ will be = 0

Brf2 hybridization

The hybridization state of BrF₂ will be determined on the basis of the valence electrons of Br atom and number of fluorine atoms present.

Electronic configuration of F is [He] 2s² 2p⁵

Electronic configuration of Br is [Ar] 3d¹⁰ 4s² 4p⁵

It has a sp³ d hybridization with 2 lone pairs and one unpaired electron The hybridization state of BrF₂ compound is highly unstable because there are 3 unpaired electrons present in the excited as we can see from the above diagram and requires 3 electrons to pair with them.

But there are only 2 fluorine atoms in BrF₂ which can pair with only 2 electrons leaving one unpaired electron making it highly unstable and logically impossible to exist.

Here the only possible way is it can lose one electron and attain sp³ hybridization with 2 lone pair electrons which will be more stable than BrF₂.

It can also either bond with another one fluorine atom and become BrF₃ and attain sp³d hybridization with 2 lone pair electrons or gain one electron and become BrF₂^– with sp³d hybridization having 3 lone pair of electrons.

Brf2 Lewis structure shape

Due to the presence of odd number electrons in the central atom bromine and high repulsion between these 5 nonbonded electrons the shape of BrF₂ will be hard to determine.

According to the VSEPR theory steric number is one important factor used to determine the shape of a compound. Let’s say if a compound has steric number 4 then they have tetrahedral or square planar shape and if they have 5 steric number then they have trigonal bipyramidal shape.

But the steric number of BrF₂ is found to be 4.5 which is a decimal digit and hence hard to determine its shape.

Brf2 Lewis structure angle

As mentioned above that it was hard to determine the shape of BrF₂ due to the presence of odd number of electrons in its central atom having one single unpaired electron making it highly unstable and hence its hard to determine its bond angle as well.

Brf2 Lewis structure resonance

BrF2 Lewis structure does not have a resonance structure the reason is because it has an expanded octet with 9 electrons in its valence shell.

in BrF₂ the 2 fluorine atoms have a complete octet and cannot accommodate extra electrons and also for bromine atom it has 9 electrons in its outermost shell due to the presence of empty 4d orbitals and exceed the octet rule to have eight electron configurations.

Having one extra electron than needed so it does not need extra electrons to complete the octet and will not form bond using its lone pair electrons which will increase electron number and hence does not have resonance structure.

Is Brf2 ionic?

BrF2 will be a covalent compound because from its Lewis structure the bond between the Br atom and the 2 fluorine atoms are formed by the sharing of electrons and not by transferring of electrons.

If we also consider the electronegativity of BrF₂ the electronegative difference between Br and F is about 1.02 which comes under the covalent character range making it covalent.

Is Brf2 polar or nonpolar?

If we consider the electronegativity of the compound then its value ranges between 2.0 and 0.5 which is a range value for polar covalent compounds making it polar. But it will be hard to determine its polarity without its shape.

But BrF₂^– is non-polar because of its linear shape. BrF₂⁺ is polar and have bent shape.

Brf2 solubility

Solubility of BrF₂ will greatly depend on its polarity and for that shape of the compound is very important as polarity depends on the shape of a compound (substance with same polarities tends to be soluble in one another).

Is Brf2 acidic or basic?

The acidic and basic nature of BrF₂ is hard to determine due to the presence of 2 lone pair of electrons and one unpaired electron in its valence shell.

if it loses the lone pair of electrons then will act as Lewis base and if it accepts a pair of electron then will act as Lewis acid.

Conclusion –

From the above BrF₂ Lewis structure we can say that BrF₂ is highly unstable due to the presence of odd number of electrons in the central atom and making it hard to determine its shape also that it violates the octet rule.

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Bromine trifluoride (BrF3) has a central bromine (Br) atom with 7 valence electrons, forming bonds with three fluorine (F) atoms, each contributing 7 valence electrons. The Lewis structure shows two single Br-F bonds and one Br-F bond with a pair of dots (representing a lone pair) on the bromine atom in the bond, indicating a T-shaped molecular geometry. Two lone pairs on the bromine atom result in a total of 28 valence electrons. The bond angles are less than 90° for axial fluorines and 120° for equatorial fluorines. The electronegativity difference (Br: 2.96, F: 3.98) and the lone pairs on Br significantly influence BrF3’s reactivity and its use as a fluorinating agent.

Understanding the Basics

In chemistry, understanding the basics of valence electrons, molecular geometry, and chemical bonding is essential. These concepts help us determine the structure and properties of molecules. In this article, we will explore the valence electrons and Lewis structure of BrF3, discuss whether it is ionic or covalent, and determine if it is polar or nonpolar.

BrF3 Valence Electrons

To understand the valence electrons of BrF3, we need to look at the electron configuration of bromine (Br) and fluorine (F). Bromine has an atomic number of 35, meaning it has 35 electrons. The electron configuration of bromine is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^5. Fluorine, on the other hand, has an atomic number of 9 and an electron configuration of 1s^2 2s^2 2p^5.

To determine the total number of valence electrons in BrF3, we need to consider that bromine contributes 7 valence electrons (since it is in Group 7 of the periodic table) and each fluorine contributes 7 valence electrons. Since there are three fluorine atoms in BrF3, the total number of valence electrons is 7 + 3(7) = 28.

BrF3 Lewis Structure Name

The Lewis structure of BrF3 helps us visualize the arrangement of atoms and lone pairs in a molecule. In BrF3, bromine is the central atom, and the three fluorine atoms are bonded to it. The Lewis structure of BrF3 can be represented as follows:

F
|
F--Br--F
|
F

The name of the Lewis structure for BrF3 is bromine trifluoride.

Is BrF3 Ionic?

To determine if BrF3 is ionic or covalent, we need to consider the electronegativity difference between bromine and fluorine. Electronegativity is a measure of an atom‘s ability to attract electrons in a chemical bond. Bromine has an electronegativity of 2.96, while fluorine has an electronegativity of 3.98.

The electronegativity difference between bromine and fluorine is 3.98 – 2.96 = 1.02. Since the electronegativity difference is relatively small, BrF3 is considered a covalent compound rather than an ionic compound.

Is BrF3 Polar or Nonpolar?

To determine if BrF3 is polar or nonpolar, we need to consider the molecular shape and the presence of any lone pairs of electrons. In BrF3, the central bromine atom is surrounded by three fluorine atoms. The molecular shape of BrF3 is trigonal bipyramidal, with the three fluorine atoms forming a triangular base and the two remaining positions occupied by lone pairs of electrons.

The presence of lone pairs of electrons creates an uneven distribution of charge in the molecule, making BrF3 a polar molecule. The electronegativity difference between bromine and fluorine also contributes to the polarity of BrF3.

Drawing the Brf3 Lewis Structure

How to Draw Brf3 Lewis Structure?

Drawing the Lewis structure of Brf3 involves understanding the concept of valence electrons, molecular geometry, chemical bonding, and the octet rule. The Lewis structure is a visual representation of the arrangement of atoms and electrons in a molecule. It helps us understand the bonding and shape of the molecule.

To draw the Lewis structure of Brf3, we need to follow a step-by-step process:

1. Determine the total number of valence electrons:
2. Bromine (Br) is in Group 7A, so it has 7 valence electrons.
3. Fluorine (F) is in Group 7A, so it also has 7 valence electrons.
4. Since there are three fluorine atoms in Brf3, we multiply the number of valence electrons by 3.
5. Total valence electrons = 7 (Br) + 7 (F) x 3 = 28.
6. Identify the central atom:
7. In Brf3, bromine (Br) is the central atom because it is less electronegative than fluorine (F).
8. The central atom is usually the least electronegative element in the molecule.
9. Connect the central atom with the surrounding atoms:
10. Bromine (Br) forms covalent bonds with three fluorine (F) atoms.
11. Each bond consists of two electrons, one from bromine and one from fluorine.
12. Distribute the remaining electrons:
13. After connecting the atoms, distribute the remaining electrons around the atoms to satisfy the octet rule.
14. Octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable configuration with 8 electrons in their outermost shell.
15. Place any remaining electrons on the central atom:
16. If there are any remaining electrons after distributing them around the surrounding atoms, place them on the central atom as lone pairs.

Lewis Dot Structure of Brf3

The Lewis dot structure of Brf3 can be represented as follows:

Atom	Valence Electrons
Br	7
F	7

In Brf3, the bromine (Br) atom is surrounded by three fluorine (F) atoms. Each fluorine atom shares one electron with bromine, resulting in three covalent bonds. The remaining electrons are placed as lone pairs on the bromine atom.

Brf3 3D Lewis Structure

The 3D Lewis structure of Brf3 can be visualized as a trigonal bipyramidal shape. The bromine atom is located at the center, with the three fluorine atoms arranged in a triangular shape around it. The two lone pairs on the bromine atom are positioned in the axial positions, perpendicular to the triangular plane formed by the fluorine atoms.

It is important to note that the Lewis structure provides a simplified representation of the molecule’s electron arrangement. It helps us understand the bonding and shape of the molecule, but it does not account for the actual three-dimensional structure and the electron pair repulsion.

Detailed Analysis of Brf3 Lewis Structure

Bromine trifluoride (BrF3) is a chemical compound that consists of one bromine atom and three fluorine atoms. In order to understand its structure, we can analyze its Lewis structure, which provides valuable information about the arrangement of valence electrons and the molecular geometry.

Brf3 Lewis Structure Lone Pairs

In the Lewis structure of BrF3, we start by determining the total number of valence electrons. Bromine is in Group 7A, so it has seven valence electrons, and each fluorine atom contributes one valence electron. Therefore, the total number of valence electrons in BrF3 is 26.

To distribute the electrons, we place the bromine atom in the center and surround it with the three fluorine atoms. Each fluorine atom forms a single bond with the bromine atom, resulting in three covalent bonds. After forming these bonds, we are left with 23 electrons.

Next, we distribute the remaining electrons as lone pairs. Since each fluorine atom already has a full octet, the remaining electrons are placed on the bromine atom. In the case of BrF3, there are three lone pairs of electrons on the bromine atom. These lone pairs are important for determining the molecular shape and polarity of the molecule.

Brf3 Lewis Structure Octet Rule

The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with a full outer shell of eight electrons. In the case of BrF3, the bromine atom has a total of seven valence electrons and forms three covalent bonds with the fluorine atoms. By sharing these electrons, the bromine atom achieves a full octet, satisfying the octet rule.

Brf3 Lewis Structure Formal Charge

Formal charge is a concept used to determine the distribution of electrons in a molecule. It helps us understand the stability and reactivity of different structures. To calculate the formal charge of an atom, we compare the number of valence electrons it should have with the number of electrons it actually has in the Lewis structure.

In the Lewis structure of BrF3, the bromine atom has seven valence electrons and is surrounded by three bonding pairs and three lone pairs. By applying the formula for formal charge (valence electrons – lone pairs – 1/2 * bonding pairs), we find that the formal charge on the bromine atom is zero. This indicates that the Lewis structure of BrF3 is stable.

Brf3 Lewis Structure Resonance

Resonance structures are different representations of a molecule that can be drawn by moving electrons within the Lewis structure. In the case of BrF3, there are no resonance structures because the arrangement of electrons is fixed due to the presence of lone pairs on the bromine atom.

Understanding the Geometry and Hybridization

Valence electrons play a crucial role in determining the molecular geometry and chemical bonding of a molecule. The arrangement of these electrons around the central atom follows certain rules and theories, such as the octet rule and the electron pair repulsion theory. One such molecule that showcases these principles is bromine trifluoride (BrF3).

Brf3 Lewis Structure Molecular Geometry

To understand the molecular geometry of BrF3, we first need to determine its Lewis structure. The Lewis structure is a diagram that represents the arrangement of atoms and valence electrons in a molecule. In the case of BrF3, bromine (Br) is the central atom surrounded by three fluorine (F) atoms.

To draw the Lewis structure of BrF3, we start by counting the total number of valence electrons. Bromine has 7 valence electrons, and each fluorine atom contributes 7 valence electrons, giving us a total of 26 valence electrons.

Next, we arrange the atoms in a way that satisfies the octet rule, where each atom (except hydrogen) aims to have 8 electrons in its outermost shell. In the case of BrF3, bromine will be the central atom since it is less electronegative than fluorine.

We then distribute the remaining valence electrons around the atoms, ensuring that each atom has an octet. In the case of BrF3, we place three lone pairs of electrons on the bromine atom and one bonding pair between bromine and each fluorine atom. This arrangement gives us a total of 26 valence electrons, satisfying the octet rule for each atom.

Brf3 Lewis Structure Electron Geometry

The electron geometry of a molecule refers to the spatial arrangement of all the electron pairs around the central atom, including both bonding and lone pairs. In the case of BrF3, the electron geometry is trigonal bipyramidal.

To determine the electron geometry, we use the VSEPR (Valence Shell Electron Pair Repulsion) theory. According to this theory, electron pairs repel each other, causing them to arrange themselves as far apart as possible. In BrF3, the three bonding pairs and two lone pairs of electrons around the bromine atom adopt a trigonal bipyramidal arrangement.

Brf3 Hybridization

Hybridization is the process in which atomic orbitals mix to form new hybrid orbitals, which then participate in bonding. In the case of BrF3, the central bromine atom undergoes sp3d hybridization.

The sp3d hybridization involves the mixing of one s orbital, three p orbitals, and one d orbital to form five sp3d hybrid orbitals. These hybrid orbitals then arrange themselves in a trigonal bipyramidal geometry around the bromine atom, accommodating the bonding and lone pairs of electrons.

Physical and Chemical Properties of Brf3

Brf3 Solubility

When it comes to the solubility of Brf3, it is important to consider its molecular properties. Brf3 is a covalent compound composed of bromine (Br) and fluorine (F) atoms. It is known as bromine trifluoride and has a molecular formula of BrF3.

In terms of solubility, Brf3 is soluble in polar solvents such as water. This is due to the presence of polar covalent bonds between the bromine and fluorine atoms. These bonds result in a partial positive charge on the bromine atom and partial negative charges on the fluorine atoms. These partial charges allow Brf3 to interact with the polar molecules of water, leading to its solubility.

Is Brf3 Acidic or Basic?

To determine whether Brf3 is acidic or basic, we need to consider its chemical properties. Brf3 is a molecule that follows the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.

In the case of Brf3, the bromine atom has seven valence electrons, and each fluorine atom contributes one valence electron. This gives a total of 10 valence electrons for Brf3. According to the VSEPR theory (Valence Shell Electron Pair Repulsion theory), the molecule adopts a trigonal bipyramidal molecular geometry.

Due to the presence of lone pairs on the central bromine atom, Brf3 can act as a Lewis acid. A Lewis acid is a substance that can accept a pair of electrons during a chemical reaction. Therefore, Brf3 can exhibit acidic properties.

Does Brf3 Have a Dipole Moment?

To determine if Brf3 has a dipole moment, we need to consider the polarity of its bonds and the molecular shape. In Brf3, the bromine atom is more electronegative than the fluorine atoms. This results in polar covalent bonds between the bromine and fluorine atoms.

The molecular shape of Brf3 is trigonal bipyramidal, with the bromine atom at the center and the three fluorine atoms arranged around it. The polar bonds in Brf3 do not cancel each other out due to the asymmetrical arrangement of the atoms.

As a result, Brf3 has a net dipole moment, making it a polar molecule. The presence of a dipole moment indicates an uneven distribution of electron density within the molecule.

Comparisons and Contrasts

When it comes to understanding the polarity and chemical properties of molecules, it is important to consider factors such as valence electrons, molecular geometry, and chemical bonding. In this discussion, we will explore the comparisons and contrasts between two molecules: BrF3 and BF3. Specifically, we will delve into why BrF3 is polar, why BF3 is nonpolar, and why BF3 is considered a Lewis acid.

Why is BrF3 Polar?

To understand why BrF3 is polar, we need to examine its molecular structure and the distribution of its valence electrons. BrF3 consists of one bromine atom (Br) and three fluorine atoms (F). The central bromine atom is surrounded by three fluorine atoms, with two of them forming a T-shaped arrangement and the third fluorine atom occupying an axial position.

According to the VSEPR theory (Valence Shell Electron Pair Repulsion theory), the presence of three lone pairs of electrons on the central bromine atom creates an electron cloud that is not symmetrical. This uneven distribution of electrons results in a molecular shape that is trigonal bipyramidal. Due to the presence of lone pairs, the electron density is higher on one side of the molecule, making it polar.

Why BF3 is Nonpolar

In contrast to BrF3, BF3 is a nonpolar molecule. BF3 consists of one boron atom (B) and three fluorine atoms (F). The central boron atom is surrounded by three fluorine atoms, forming a trigonal planar molecular geometry. Unlike BrF3, BF3 does not have any lone pairs of electrons on the central boron atom.

The absence of lone pairs in BF3 results in a symmetrical distribution of electron density around the molecule. The three fluorine atoms are positioned at equal distances from the central boron atom, creating a molecule that is nonpolar. This means that the molecule has no net dipole moment and does not exhibit any significant charge separation.

Why is BF3 a Lewis Acid

Moving on to the Lewis acid properties of BF3, we need to consider its electron deficiency and its ability to accept electron pairs. BF3 is classified as a Lewis acid because it has an incomplete octet in its valence shell. Boron, the central atom in BF3, only has six valence electrons, which is two electrons short of a stable octet.

Due to this electron deficiency, BF3 readily accepts a pair of electrons from a Lewis base, forming a coordinate covalent bond. This ability to accept electron pairs makes BF3 a Lewis acid, as it can act as an electron pair acceptor in chemical reactions.

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References

In chemistry, understanding the concept of valence electrons is crucial for determining molecular geometry and chemical bonding. The octet rule, electron pair repulsion, and VSEPR theory play significant roles in predicting the molecular shape of a compound. One such compound is bromine trifluoride (BrF3), which consists of a central bromine atom bonded to three fluorine atoms.

To analyze the molecular shape of BrF3, we need to consider the valence electrons present in the molecule. Bromine (Br) has seven valence electrons, while each fluorine (F) atom has seven valence electrons. In total, we have 26 valence electrons in the BrF3 molecule.

Using the electron dot diagram, we can distribute the valence electrons around the central bromine atom. Since bromine has three bonds with fluorine atoms, we place three pairs of electrons between the bromine and fluorine atoms. This leaves two lone pairs of electrons on the bromine atom.

According to the VSEPR theory, the electron pairs around the central atom repel each other, resulting in a molecular shape that minimizes this repulsion. In the case of BrF3, the three bonding pairs and two lone pairs of electrons arrange themselves in a trigonal bipyramidal shape. The three fluorine atoms occupy the equatorial positions, while the two lone pairs occupy the axial positions.

Considering the concept of hybridization, the central bromine atom in BrF3 undergoes sp3d hybridization. This means that the bromine atom’s three 3p orbitals and one 3d orbital combine to form five sp3d hybrid orbitals. These hybrid orbitals then overlap with the fluorine atoms‘ 2p orbitals, resulting in five sigma bonds.

The molecular shape and hybridization of BrF3 can also be understood by examining its resonance structures. Resonance occurs when multiple Lewis structures can be drawn for a molecule, with only the arrangement of electrons changing. However, in the case of BrF3, resonance structures are not applicable as there is no delocalization of electrons.

For more information on valence electrons, molecular geometry, chemical bonding, the octet rule, electron pair repulsion, VSEPR theory, and other related topics in chemistry, you can visit the following resources:

• Chemistry LibreTexts
• Chemistry Explained
• Chemistry World

These resources will provide you with a comprehensive understanding of the concepts mentioned above and help you delve deeper into the fascinating world of chemistry.

Frequently Asked Questions

What is the Lewis structure of BrF3?

The Lewis structure of BrF3, or bromine trifluoride, consists of a central bromine atom surrounded by three fluorine atoms and two lone pairs of electrons. The bromine atom, as the central atom, forms five covalent bonds in total.

Does BrF3 follow the octet rule?

No, BrF3 does not follow the octet rule. The central bromine atom in BrF3 has ten electrons in its valence shell, exceeding the octet rule which states that an atom in a molecule will be stable with eight electrons in its outer shell.

What is the electron and molecular geometry of BrF3?

The electron geometry of BrF3 is trigonal bipyramidal, due to five regions of electron density – three bonds and two lone pairs. However, the molecular geometry, considering only the bonded atoms, is T-shaped.

Why is BrF3 polar?

BrF3 is polar because it has a non-symmetrical molecular geometry. The presence of lone pairs of electrons on the central atom (bromine) leads to an uneven distribution of electron density, resulting in a net dipole moment.

What is the hybridization of the central atom in BrF3?

The hybridization of the central atom in BrF3, which is bromine, is sp3d. This is due to the five regions of electron density around the bromine atom – three from the bonds with fluorine atoms and two from the lone pairs of electrons.

Does BrF3 have a dipole moment?

Yes, BrF3 does have a dipole moment. This is due to the molecule’s polar nature, which arises from its asymmetrical shape and the presence of lone pairs of electrons on the bromine atom.

Does BrF3 have resonance structures?

No, BrF3 does not have resonance structures. This is because all the fluorine atoms are equivalent and there is no possibility of forming equivalent structures by rearranging the electrons.

What is the bond angle in the BrF3 Lewis structure?

The bond angles in the BrF3 Lewis structure are less than 90 degrees between the fluorine atoms and less than 120 degrees between the fluorine atoms and the lone pairs.

What is the molecular shape of BrF3 according to the VSEPR theory?

According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, the molecular shape of BrF3 is T-shaped. This is due to the presence of three bonding pairs and two lone pairs of electrons around the central bromine atom.

Why is BF3 a Lewis acid?

BF3, or boron trifluoride, is a Lewis acid because it can accept a pair of electrons. The boron atom in BF3 only has six electrons in its valence shell, making it electron deficient and able to accept electron pairs from a Lewis base.

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Ba₃N₂, its lewis structure, shape, bond angle, hybridisation, stability were briefly discussed in this article.

Barium nitride is a compound with chemical formula Ba₃N₂ having three barium and two nitrogen atoms combined through ionic bond. Its molecular weight is 440 and has various applications.

How to draw Ba₃N₂ lewis structures ?

Lewis structure of a molecule is mainly drawn to understand how the bond formation takes place when two atoms or more got united. The lewis structure of a compound is drawn by considering only the valence electrons present in the outermost shell and it is represented as dots. So the structures drawn by this concept are called lewis dot structures.

Lewis dot structures can be drawn for both covalently bonded and ionic bonded compounds. Barium nitride is a compound having three barium and two nitrogen atoms. Barium is a second group alkaline earth metal and nitrogen is fifteen group element. There are certain rules or steps are there to reach up to the lewis structure of any compound.

• Calculate the total number of valence electrons. Here barium has 2 electrons in its outermost shell and nitrogen has five valence electrons. So the total number of valence electrons in barium nitride, Ba₃N₂ is 2×3+5×2 = 16 electrons.
• Three barium atoms with two valence electrons and two nitrogen atoms with five valence electrons are present in barium nitride, Ba₃N₂.

• Each barium atom donates its two electrons to nitrogen atom to form a barium cation, Ba²⁺. When nitrogen accepts this electrons it get converted to a anion called nitride,N^3-.

• So a positive barium cation and a negative nitride anion formed will undergo electrostatic force of attraction to form a stable compound called barium nitride.

Ba₃N₂  resonance

Resonance can be defined as the movement or the delocalistion of electrons present in an atom of any compound. Resonance can only seen in compounds with double bonds and the electrons involved with these bonds are easy to move across the bonds. While drawing the resonance structure the actual properties like the number of electrons present around the atom shouldn’t change.

Even though there is double bond in barium nitride it is not allowed to move across, because if they do so the molecular structure not exist. So there is no resonance structure for barium nitride.

Ba₃N₂  Shape

Barium nitride is a bent shaped molecule with Ba- N bonds. In which two barium – nitrogen bonds are double bonded while one of the barium is attached to two nitrogen atoms through single bonds.

Ba₃N₂  Formal charge

Formal charge is a charge assigned to an atom when it is get combined with other atoms to form a stable compound. The formal charge assigned to an atom can be easily found out by the below equation

Formal charge of an atom = ( Valence electrons – No. of lone pairs – No. of bonds formed)

Formal charge of  Barium in Ba₃N₂ = 2 – 0- 2

                                                        = 0

Formal charge of  Nitrogen  in Ba₃N₂ = 5 – 2- 3

                                                            = 0

So the formal charge of both the barium and nitrogen in Ba₃N₂ is 0.

Ba₃N₂ Bond angle

Bond angle is the angle made between three atoms when they combine together to form a stable compound. Since barium nitride is a molecule with bent shape its bond angle may be 109.4⁰. Since there is two lone pair of electrons are present in the nitrogen atoms there is a probability for a change.

Ba₃N₂ Octet rule

According to octet rule, when atoms combine together to form compounds they are found to be more stable when their outermost shell are filled with eight electrons. Atoms lose or gain electrons to obey the octet rule. In the case of barium nitride barium loses its two electrons to nitrogen.

Nitrogen atom accepts these two electrons from barium and got satisfied with eight electrons in its valence shell. So nitrogen atom satisfy octet rule.

Ba₃N₂ Lone pair of electrons

Lone pair of electron or non bonding electrons are the electrons present in the valence shell of an atom which doesn’t took participation in bond formation. Since they doesn’t form bonds they can be called as non bonding electrons.

The lone pair of electrons in barium is 0.

The lone pair of electrons in nitrogen is 2.

Ba₃N₂ valence electrons

The electrons present in the valence shell or the outermost shell of an atom is called as its valence electrons.

Number of valence electrons present in barium is 2 and nitrogen is 5.

So the total number of valence electrons in Ba₃N₂ is 16.

Ba₃N₂ Hybridisation

When the atomic orbitals of atoms with slightly different energies intermixes together to form atomic orbitals with same energy and shape that process  is called hybridisation. The new orbitals formed are called hybrid orbitals and their number is equal to that of the orbitals undergo hybridisation.

Hybridisation is a concept that we applied in the case of covalent compounds. Covalent bonds are formed by mutual sharing of electrons between the bonding  atoms. Barium nitride is not formed by this way. Here barium losses its electron while nitrogen accepts that to form bond. A mutual sharing can’t be seen here. So hybridisation can’t be applied for this compound.

Ba₃N₂ Solubility

Solubility can be defined as the ability of a substance or solute to get dissolved in a solvent to form a solution. The most commonly used solvents in field of chemistry is water, ethanol, acetone, ether, benzene etc. Barium nitride is soluble in water and are insoluble in organic solvents.

Barium nitride is a polar molecule and water is also a polar solvent. Therefore barium nitride easily soluble in water. Barium nitride reacts with water to form a solution of barium hydroxide and evolution of ammonia gas takes place.

  Ba₃N₂ + 6H₂O  → 3Ba(OH)₂ + 2NH₃

 Is Ba₃N₂  Ionic or not ?

An ionic bond is formed by the electrostatic force of  attraction between a positive and negative ion. The positive ion is called cation and negative ion is called anion. Barium nitride, Ba₃N₂ is an ionic compound.

Barium donates its two electrons to nitrogen to form Barium cation, Ba²⁺ and nitrogen accepts these electrons to form nitride ion, N^3-. Then these positive and negatively charged atoms attracts to form their ionic bond.

The electronegativity of barium and nitrogen is 0.89 and 3.04 respectively. Their electronegativity difference is 2.15. When compounds have electronegativity value greater than 1.7 then that compound will be ionic in nature. Here 2.15 is greater than 1.7 so barium nitride can be considered as an ionic compound.

Is Ba₃N₂ Polar or not ?

A compound is said to be polar in nature when the electronegativity difference of atoms present is more than 0.4. The electronegativity value of barium is 0.89 and nitrogen is 3.04. Their electronegativity difference is 2.15, which is greater than 0.4. So barium nitride, Ba₃N₂ is polar in its nature.

Is Ba₃N₂ Acidic or Basic ?

Barium nitride is an ionic compound which shows polar behaviour. An ionic compound is said to be acidic when it has hydrogen ion and basic when it has basic ions like hydroxide(OH^–) and oxide(O^2-) present in it.

Ionic compounds without the presence of these ions are called salts and they are formed by acid base reactions. Since there is no hydrogen and hydroxide ions present in barium  nitride it is neither acid nor base. So barium nitride can be considered as a salt.

Summary

Barium nitride, Ba₃N₂ is an ionic compound which is polar in nature. This article briefly explains about its lewis structures, lone pairs, valence electrons and hybridisation. Barium nitride is used as flux in GaN growth medium, precursor of metal nitrides and dopants in optical materials.

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This article explains the Lewis structure of barium fluoride, resonance, shape, formal charge, angle, octet rule, lone pairs of BaF₂ Lewis structure. Hybridization, solubility, ionic, polar nature, acidic and valence electron of barium fluoride is also explained.

BaF₂ is also called Barium fluoride. Barium has two electron in its outermost shell. It donates one electron with each fluorine atom and this electron is accepted by fluorine. BaF₂ Lewis structure shows that two Fluorine atoms and one Barium bonded by this method.

How to draw BaF₂ Lewis structure?

Below steps are followed to draw Lewis structure of BaF2:

Step 1: Count the available valence electron

Fluorine and Barium are part of halogen present in the 17^th group in periodic table, and second group consists of alkaline earth metals.

Two electrons are available in the outermost shell of barium hence, electron dot structure of barium is represented by Ba which is having two dots and fluorine has got seven electrons in its outermost shell, therefore electron dot structure of fluorine is written as F with seven dots.

Outermost valence shell electron of barium atom in BaF₂ = 2

Outermost valence shell electron of fluorine atom in BaF₂ = 7

Barium fluoride consists of two fluorine atoms therefore total available valence electrons= 2+7(2) = 16.

Step 2: Choose least electronegative atom and insert in the center of the molecule.

In the periodic table electronegativity value increases across a row that is left to right. Therefore, alkaline earth metal have lowest electronegativity while halogens have the highest.

Fluorine is the smallest halogen element with more electronegative than barium. The electronegative value of the barium is lower than that of the fluorine atom in the BaF₂ molecule. Hence Barium atom is kept in the center of the molecule due to its electronegative nature.

Step 3: The metal atom donates electron while the nonmetal atom accept them in ionic compound.

In BaF₂, barium is the metal which donate one electron with each fluorine atom and forms barium (ΙΙ) cation, whereas fluorine is the non-metal, each fluorine atom accept one electron from barium and forms fluoride anion.

Step 4: Combining two opposite charges, to get BaF2 Lewis structure.

Barium atom donates one electron to each fluorine atom and each fluorine atom receives one electron from barium to bring the stability and as a result of this both ions will have full valence shell due to which it exhibits noble gas electron configuration.

BaF2 Lewis structure can be represented as Ba2+ and F- with eight dots.

BaF₂ Lewis structure resonance:

A multiple Lewis structure represents the different ways of placing electron on the atom in a molecule. Resonance structure is possible for a molecule if there are multiple bonds and also it has formal charge with the presence of lone pair on the atoms of molecule.

BaF2 Lewis structure does not show any resonance structure as there is not bonding between the barium fluoride molecule. In addition to this, barium fluoride is a molecule containing barium as metal and fluorine as non-metal. Therefore resonance structure of BaF2 is not possible.

BaF₂ Lewis structure shape:

BaF2 is an ionic compound and there is no bonding between barium and fluorine ion, there is complete transfer of electrons within the molecule. Therefore BaF2 Lewis structure do not have any shape.

BaF₂ Lewis structure formal charge:

Formal charge nothing but the charge which is assigned to an atom so that equally shared electrons exists between the atoms in a molecule.

Formal charge= [Total number of valence electron in free state]-{[total number of lone pair

electron] + 1/2[total number of bonding electron]}

In the case of Barium:

Number of valence electron in potassium =2

Total number of lone pair electron = 0

Total number of bonding electron = 0

Formal charge of barium= 2-{0+1/2(0)}

                                         = +2

Formula charge on barium atom in barium fluoride Lewis structure is +2

For fluorine:

Number of valence electron in fluorine =7

Total number of lone pair electron in fluorine= 8

Total number of bonding electron = 0

Formal Charge of fluorine=7-{8+1/2(0)}

                                     =-1

The fluorine atom in BaF₂ Lewis structure has a formal charge of -1.

BaF₂ Lewis structure angle:

Lewis structure of BaF2 molecule does not have any bond angle as there is no bond present between the molecule as it is originally an ionic compound with the presence of metal and non-metal.

BaF₂ Lewis structure octet rule:

In BaF2 Lewis structure, barium metal belongs to the alkaline earth metal and it has 2 valence electron.

As there is no eight electron present in the barium atom so it has incomplete octet whereas each fluorine atom accepts one electron from barium so fluorine has eight electron with complete octet as a result negative charge for fluorine.

BaF₂ Lewis structure lone pair:

Pair of electrons that are not involved in bonding are termed as lone pair electrons.

Lone pair electron of Barium in Barium fluoride Lewis structure = 0

Lone pair electron of fluorine in barium fluoride Lewis structure = 4

BaF₂ valence electron:

Electronic configuration of barium is 1s²2s²2p⁶3s²3p⁶ 3d¹⁰4s²4p⁶4d¹⁰5s²5p⁶6s²

Outermost electron present in the barium is 2

Electronic configuration of fluorine is 1s²2s²2p⁵

Outermost electron present in the fluorine is 7

Two fluorine atom present in the barium fluoride therefore, the total number of valence electron of BaF₂ is 2+7(2) =16.

BaF₂ hybridization:

BaF2 Lewis structure does not show any hybridization as there is no mixing and recasting of atomic orbitals within the molecule, there is complete transfer of electrons between Ba metal and fluorine non-metal ion creating +2 charge on Ba and -1 charge on fluorine.

BaF₂ solubility:

Barium fluoride is slightly soluble in

• water
• calcium hydroxide
• lead dichloride

Barium fluoride is soluble in

• Hydrochloric acid
• Nitric acid
• Hydrogen cyanate
• Hydrofluoric acid
• Ammonium chloride

Barium fluoride is insoluble in

• Silver chloride
• Silver carbonate
• Calcium carbonate
• Lead dichloride

How BaF₂ is soluble in hydrochloric acid than water?

In aqueous solution barium fluoride is dissociate into Ba²⁺ and 2F^– ions.

BaF₂(s) ⇌ Ba²⁺ (aq) + 2F⁻ (aq)

F^– is a basic anion thus it can react with the acid, such that production of ions are formed is more than the formation of insoluble salt. Hence Barium fluoride is found to be less soluble in water compare to dilute hydrochloric acid.

F⁻+HCl → HF + Cl⁻

Why BaF₂ is soluble in hydrochloric acid than water?

Fluorine is highly electronegative in nature in BaF₂. Hence Barium gets partial positive charge and Fluorine gets a partial negative charge.

More is the ionic character present in a compound more readily it will dissociate into ions. Hydrochloric acid contains hydrogen ions.  When BaF₂ dissolvesin HCl more ions are formed Hence barium fluoride is more soluble in acidic solution.

Is BaF₂ ionic?

Yes barium fluoride is an ionic compound and is made up of barium (ΙΙ) cation and fluoride anion. As there is no presence of covalent or pi bonds within the molecule. There is only presence of charges on Ba metal and fluorine ion which makes the BaF₂ an ionic compound.

Why BaF₂ ionic? 

In BaF_2, the interaction between barium and fluorine is ionic in nature because complete transfer of ions is observed and there is no shared bonding. Therefore barium fluoride is ionic in nature.

How BaF₂ ionic? 

Barium has two electrons in its outermost shell and it donates one electron with each fluorine atom and forms barium (ΙΙ) cation, whereas fluorine is the non-metal, and each fluorine atom accepts one electron from barium and forms fluoride anion. Hence ionic bond is formed by complete transfer of electron as stated above.

Is BaF₂ polar or nonpolar?

Barium fluoride is polar in nature. Due to the presence of polar bonds with barium and fluorine it is polar in nature.

Why BaF₂ polar?

Barium fluoride is ionic in nature which contains the positively charged cation that is Ba²⁺and negatively charged anion that is F^–on it, which creates a dipole within the BaF₂ molecule which makes it polar.

How BaF₂ polar? 

Due to the presence of polar bond within positively charged Ba cation and negatively charged fluorine anion in BaF₂ molecule, there is the formation of polar bond within Ba and F^– ion, makes it a polar molecule.

Is BaF₂ acidic or basic?

BaF₂ is weakly acidic in nature.

Why BaF₂ weakly acidic?

Barium fluoride is a weak acid because it is a salt of barium hydroxide which is a weak base and hydrofluoric acid which is a strong acid. This reaction is called acid-base reaction.

Ba (OH)₂ + 2HF → 2H₂O + BaF₂

How BaF₂ weakly acidic?

Weak acid is the one which partially dissociates in water. In the case of Barium Fluoride when reacts with water, it does not fully dissociate its ion hence BaF₂ is termed as weak acidic in nature.

Summary:

BaF₂ consists of two ions i.e. Ba²⁺ cation and F^– anion. Ionic bond is formed between these two ions and it has got polarity and weak acidic nature. BaF₂ is found to be soluble acids such as in nitric acid, hydrochloric  and  is slightly soluble in water.

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The Lewis structure of AlH3, also known as aluminum hydride, is a diagram that represents the arrangement of atoms and electrons in the molecule. It helps us understand the bonding and geometry of the compound. In the Lewis structure of AlH3, aluminum (Al) is the central atom surrounded by three hydrogen (H) atoms. Each hydrogen atom forms a single bond with the aluminum atom, resulting in a trigonal planar geometry. The Lewis structure of AlH3 is crucial in predicting the chemical behavior and reactivity of the compound.

Key Takeaways

Atom	Number of Valence Electrons
Aluminum (Al)	3
Hydrogen (H)	1

Understanding Lewis Structures

What is a Lewis Structure?

A Lewis structure is a diagram that represents the arrangement of atoms and valence electrons in a chemical compound. It was introduced by Gilbert N. Lewis in 1916 and is also known as a Lewis dot diagram. Lewis structures are widely used in chemistry to understand the chemical bonding and molecular geometry of different compounds.

In a Lewis structure, the valence electrons of an atom are represented by dots or lines around the atomic symbol. These dots or lines indicate the number of valence electrons an atom possesses. For example, the Lewis structure of aluminum hydride (AlH3) shows that aluminum has three valence electrons, while each hydrogen atom has one valence electron.

Lewis structures are essential in understanding chemical bonding. They help us determine how atoms form covalent bonds by sharing electrons. By following the rules of Lewis structures, we can predict the electron pair arrangement and molecular geometry of a compound. This information is crucial in understanding the chemical properties and behavior of different substances.

Importance of Lewis Structures in Chemistry

Lewis structures play a vital role in the study of chemistry. They provide a visual representation of how atoms are connected and bonded in a molecule. By drawing Lewis structures, we can determine the electron configuration and predict the chemical properties of a compound.

One of the fundamental concepts in Lewis structures is the octet rule. According to this rule, atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight valence electrons. By applying the octet rule, we can determine the number of bonds an atom can form and the overall stability of a molecule.

Drawing Lewis structures also helps us understand the concept of resonance. Resonance structures occur when there are multiple ways to arrange the electrons in a molecule without violating the octet rule. These resonance structures contribute to the stability and reactivity of the compound.

Lewis structures are also used in molecular structure analysis and predicting bond angles. The VSEPR (Valence Shell Electron Pair Repulsion) theory, combined with Lewis structures, allows us to determine the three-dimensional shape of a molecule and the bond angles between atoms.

How to Draw Lewis Dot Structure for AlH3

Aluminum hydride (AlH3) is a chemical compound that can be represented using a Lewis dot structure. This structure helps us understand the arrangement of atoms and electrons in the molecule. By following a series of steps, we can draw the Lewis dot structure for AlH3 and gain insights into its chemical bonding and molecular geometry.

Step 1: Count Total Valence Electrons Present in AlH3 Molecule

To begin, we need to determine the total number of valence electrons present in the AlH3 molecule. Valence electrons are the outermost electrons of an atom that participate in chemical bonding. In AlH3, aluminum (Al) belongs to Group 3A of the periodic table and has three valence electrons, while hydrogen (H) has one valence electron. By multiplying the number of valence electrons for each atom by the number of atoms present, we can calculate the total number of valence electrons in AlH3.

Step 2: Identify the Central Atom in AlH3

In AlH3, aluminum (Al) is the central atom as it is less electronegative than hydrogen (H). The central atom is usually the least electronegative element in a molecule and forms bonds with other atoms. By placing the central atom in the center, we can proceed to the next step.

Step 3: Establish a Bond between Al and H Atom

Next, we need to establish a bond between aluminum (Al) and hydrogen (H) atoms. Aluminum can form three covalent bonds, while hydrogen can form only one. Covalent bonds involve the sharing of electrons between atoms. By connecting the central atom (Al) with the outer atoms (H) using single lines, we represent the covalent bonds in the Lewis dot structure.

Step 4: Complete Octet of the Outer Atoms (or Duplet) for Hydrogen Atom

Hydrogen (H) atoms in AlH3 only require two electrons to complete their outermost energy level, also known as a duplet. Since hydrogen has only one valence electron, it needs to share one electron with aluminum (Al) to achieve a duplet. By placing two dots around each hydrogen atom, we complete their octet (or duplet) in the Lewis dot structure.

Step 5: Check Formal Charge Value

Lastly, we need to check the formal charge values of each atom in the Lewis dot structure. Formal charge is a way to determine the distribution of electrons in a molecule. It helps us identify the most stable arrangement of electrons. The formal charge of an atom can be calculated by subtracting the number of lone pair electrons and half the number of shared electrons from the number of valence electrons. By ensuring that the formal charge values are minimized or equal to zero, we can verify the accuracy of our Lewis dot structure.

By following these steps, we can draw the Lewis dot structure for AlH3 and gain a better understanding of its molecular structure and chemical properties. Remember, Lewis structures are a useful tool in chemistry for analyzing and predicting the behavior of chemical compounds.

Understanding Formal Charge in AlH3

What is the Formal Charge in AlH3 and How is it Calculated?

Formal charge is a concept used in chemistry to determine the distribution of electrons in a molecule or ion. In the case of Aluminum Hydride (AlH3), understanding the formal charge can provide valuable insights into its chemical properties and behavior.

To calculate the formal charge of an atom in a molecule, we need to consider the number of valence electrons it possesses and its bonding arrangement. The formal charge is calculated by subtracting the number of lone pair electrons and half the number of shared electrons from the total number of valence electrons.

In AlH3, aluminum (Al) has three hydrogen (H) atoms bonded to it. Aluminum is a group 3 element and has three valence electrons, while hydrogen has one valence electron. By applying the formal charge calculation, we can determine the formal charge of each atom in AlH3.

Let’s break it down:

1. Aluminum (Al):
2. Valence electrons: 3
3. Lone pair electrons: 0
4. Shared electrons: 6 (each hydrogen contributes one electron)

5. Formal charge = 3 – 0 – 6/2 = 0

6. Hydrogen (H):

7. Valence electrons: 1
8. Lone pair electrons: 0
9. Shared electrons: 2 (shared with aluminum)
10. Formal charge = 1 – 0 – 2/2 = 0

From the calculations, we can see that both aluminum and hydrogen in AlH3 have a formal charge of 0. This indicates that the distribution of electrons in the molecule is balanced, with no atoms carrying an excess or deficit of electrons.

How to Find Formal Charge from Lewis Structure

A Lewis structure, also known as a Lewis dot diagram, is a visual representation of the arrangement of atoms and valence electrons in a molecule. It can be used to determine the formal charge of each atom in a compound like AlH3.

To find the formal charge from a Lewis structure, follow these steps:

1. Draw the Lewis structure of AlH3, representing the bonds between aluminum and hydrogen atoms.
2. Count the number of valence electrons for each atom.
3. Assign lone pair electrons and shared electrons based on the Lewis structure.
4. Apply the formal charge calculation for each atom using the formula mentioned earlier.

By following these steps, you can determine the formal charge of each atom in AlH3 and gain a better understanding of its electronic distribution.

It’s important to note that formal charge is a theoretical concept and does not represent the actual charge of the atoms in a molecule. It is a tool used to analyze the electron distribution and predict the reactivity of a compound.

The Octet Rule and AlH3

Does AlH3 Molecule Follow the Octet Rule?

The Octet Rule is a fundamental concept in chemistry that states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight valence electrons. This rule helps us understand the formation of chemical bonds and the stability of molecules.

Aluminum hydride (AlH3) is a chemical compound that consists of one aluminum atom bonded to three hydrogen atoms. To determine if AlH3 follows the Octet Rule, let’s analyze its Lewis dot diagram and examine its chemical bonding and molecular structure.

In the Lewis dot diagram of AlH3, we represent the valence electrons of each atom as dots or lines around the atomic symbol. Aluminum (Al) has three valence electrons, while hydrogen (H) has one valence electron. Therefore, the total number of valence electrons in AlH3 is [(3 * 1) + 3] = 6.

According to the Octet Rule, atoms tend to gain or lose electrons to achieve a stable electron configuration with eight valence electrons. In the case of AlH3, aluminum has three valence electrons and can form three covalent bonds with hydrogen atoms. Each hydrogen atom contributes one electron, resulting in a total of six valence electrons shared between aluminum and hydrogen.

Although AlH3 does not strictly follow the Octet Rule, it is still a stable molecule due to the presence of covalent bonds. The molecular geometry of AlH3 is trigonal planar, with the aluminum atom at the center and the three hydrogen atoms arranged symmetrically around it.

The electron pair around the aluminum atom in AlH3 is involved in covalent bonding, and the molecule adopts a trigonal planar shape to minimize electron repulsion. This arrangement allows for the most stable molecular structure.

The hybridization of AlH3 involves the mixing of atomic orbitals to form new hybrid orbitals. In this case, aluminum undergoes sp2 hybridization, resulting in three sp2 hybrid orbitals that overlap with the hydrogen 1s orbitals to form the covalent bonds.

The VSEPR theory (Valence Shell Electron Pair Repulsion theory) helps us predict the molecular geometry of AlH3 based on the arrangement of electron pairs. In AlH3, there are three bonding pairs and no lone pairs around the aluminum atom, resulting in a trigonal planar molecular geometry.

While AlH3 does not strictly adhere to the Octet Rule, it is a stable molecule due to the presence of covalent bonds and the adoption of a trigonal planar molecular structure. The chemical properties of AlH3 make it useful in various chemical reactions and as a reducing agent in organic synthesis.

Molecular and Electron Geometry of AlH3

What is the Molecular Geometry and Electron Geometry of AlH3 Molecule?

The molecular geometry and electron geometry of the AlH3 molecule refer to the arrangement of atoms and electron pairs around the aluminum and hydrogen atoms in the compound. To understand the molecular and electron geometry of AlH3, we can utilize the VSEPR (Valence Shell Electron Pair Repulsion) theory.

According to the VSEPR theory, the molecular geometry is determined by the repulsion between electron pairs around the central atom. In the case of AlH3, aluminum (Al) is the central atom, and it is surrounded by three hydrogen (H) atoms. Since AlH3 has no lone pairs of electrons on the central atom, the molecular geometry is trigonal planar. This means that the three hydrogen atoms are arranged in a flat, triangular shape around the aluminum atom.

The electron geometry, on the other hand, takes into account both the bonded electron pairs and the lone pairs of electrons around the central atom. In the case of AlH3, the electron geometry is also trigonal planar, as there are no lone pairs of electrons on the aluminum atom.

Use of VSEPR Theory to Determine Molecular/Electron Geometry of AlH3

The VSEPR theory is a useful tool in determining the molecular and electron geometry of chemical compounds. It is based on the idea that electron pairs, whether they are bonding or non-bonding, repel each other and tend to position themselves as far apart as possible. This repulsion determines the overall shape of the molecule.

To apply the VSEPR theory to AlH3, we consider the Lewis dot diagram of the compound. Aluminum has three valence electrons, while hydrogen has one valence electron each. By following the Lewis structure rules and drawing the Lewis structure of AlH3, we can determine the arrangement of atoms and electron pairs.

In AlH3, the aluminum atom forms covalent bonds with three hydrogen atoms, resulting in a total of three bonding electron pairs. Since there are no lone pairs of electrons on the aluminum atom, the molecular and electron geometry is trigonal planar.

What is the Bond Angle of AlH3 Molecule?

The bond angle of the AlH3 molecule refers to the angle between two hydrogen atoms bonded to the central aluminum atom. In a trigonal planar geometry, the bond angle is 120 degrees. This means that the hydrogen atoms in AlH3 are arranged in a triangular shape around the aluminum atom, with each hydrogen-aluminum-hydrogen bond angle measuring 120 degrees.

Understanding the molecular and electron geometry, as well as the bond angle, of AlH3 is essential in analyzing its chemical properties and reactions. By studying the molecular structure and properties of AlH3, scientists can gain insights into its atomic structure, chemical bonding, and overall behavior in chemical reactions.

Hybridization in AlH3

Find the Hybridization Number of AlH3 Molecule

To determine the hybridization number of the AlH3 molecule, we need to understand the concept of hybridization and its application in chemical bonding. Hybridization is a process in which atomic orbitals mix to form new hybrid orbitals, resulting in the rearrangement of electrons and the formation of covalent bonds.

In the case of AlH3, aluminum hydride, we have one aluminum atom (Al) and three hydrogen atoms (H). Aluminum belongs to Group 13 of the periodic table and has three valence electrons. Hydrogen, on the other hand, has one valence electron.

According to the octet rule, atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons. In the case of AlH3, aluminum can achieve this stability by sharing its three valence electrons with three hydrogen atoms.

To determine the hybridization number, we need to consider the number of electron pairs around the central atom, which is aluminum in this case. Each covalent bond consists of one electron pair. Therefore, the total number of electron pairs around aluminum is three.

Based on the VSEPR (Valence Shell Electron Pair Repulsion) theory, the electron pairs around the central atom repel each other and try to maximize their distance. This leads to a trigonal planar molecular geometry for AlH3.

Now, let’s determine the hybridization of aluminum in AlH3. The number of electron pairs (three) corresponds to sp2 hybridization. In sp2 hybridization, one s orbital and two p orbitals combine to form three sp2 hybrid orbitals. These hybrid orbitals are arranged in a trigonal planar geometry around the aluminum atom.

What is the Hybridization for AlH3 Molecule?

The hybridization of the AlH3 molecule is sp2. This means that the aluminum atom in AlH3 undergoes sp2 hybridization, resulting in the formation of three sp2 hybrid orbitals. These hybrid orbitals are involved in bonding with the three hydrogen atoms, forming three sigma bonds.

In the Lewis dot diagram of AlH3, the aluminum atom is represented by the symbol Al, surrounded by three dots representing its valence electrons. The hydrogen atoms are represented by the symbol H, each with a single dot representing its valence electron.

The chemical bonding in AlH3 involves the sharing of electrons between aluminum and hydrogen atoms, resulting in the formation of covalent bonds. The molecular structure analysis of AlH3 reveals a trigonal planar geometry, with the aluminum atom at the center and the three hydrogen atoms arranged symmetrically around it.

Resonance and Solubility of AlH3

Does AlH3 Molecule Show Resonance?

When it comes to the aluminum hydride molecule (AlH3), the question of whether it exhibits resonance arises. Resonance refers to the phenomenon where multiple Lewis structures can be drawn for a molecule, indicating the delocalization of electrons. However, in the case of AlH3, resonance structures are not typically observed.

To understand why AlH3 does not exhibit resonance, let’s take a closer look at its chemical bonding and molecular structure. Aluminum hydride has a Lewis dot diagram where aluminum (Al) is surrounded by three hydrogen (H) atoms. The valence electrons of aluminum and hydrogen participate in covalent bonds, resulting in the formation of the AlH3 molecule.

The molecular geometry of AlH3 is trigonal planar, with the aluminum atom at the center and the three hydrogen atoms arranged symmetrically around it. This arrangement satisfies the octet rule, where each atom in the molecule has a full outer electron shell. The absence of additional resonance structures can be attributed to the stable molecular structure of AlH3, which does not require electron delocalization.

Solubility of Aluminium Hydride

Moving on to the solubility of aluminum hydride (AlH3), it is important to note that AlH3 is not soluble in water. This lack of solubility can be attributed to the nature of the chemical compounds involved.

AlH3 is a covalent compound, and covalent compounds tend to have low solubility in water. This is because water is a polar solvent, meaning it has a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. In order for a compound to dissolve in water, it must have a similar polarity.

However, AlH3 is a nonpolar molecule, as the electronegativity difference between aluminum and hydrogen is relatively small. As a result, the attractive forces between AlH3 molecules are stronger than the interactions between AlH3 and water molecules, leading to insolubility.

Frequently Asked Questions

1. What is the Lewis Structure of AlH3?

The Lewis structure of AlH3 (Aluminum hydride) consists of an Aluminum atom surrounded by three Hydrogen atoms. Each Hydrogen atom shares one electron with Aluminum to form a covalent bond, satisfying the octet rule for Aluminum.

2. How can I identify a Lewis Structure?

A Lewis structure can be identified by its representation of atoms of a molecule, showing how the valence electrons are arranged among the atoms in the molecule. It includes lines to represent covalent bonds and dots to represent non-bonding electrons.

3. What is the Lewis Dot Structure of AlH3?

The Lewis dot structure of AlH3 is similar to its Lewis structure. It shows an Aluminum (Al) atom in the center with three Hydrogen (H) atoms surrounding it. Each Hydrogen atom shares one electron with Aluminum, forming a covalent bond.

4. How can I find the formal charge from a Lewis Structure?

The formal charge of an atom in a Lewis structure can be calculated using the formula: Formal Charge = Valence Electrons – (Non-bonding electrons + 1/2 Bonding electrons).

5. What is the molecular geometry of AlH3 according to its Lewis Structure?

The molecular geometry of AlH3, according to its Lewis structure, is trigonal planar. This is due to the three Hydrogen atoms being evenly distributed around the Aluminum atom, creating a flat, three-sided shape.

6. What is Al3+ in Chemistry?

In chemistry, Al3+ refers to the ion of Aluminum that has lost three electrons, resulting in a positive charge. It is often involved in ionic bonds with negatively charged ions.

7. What are Lewis Structures?

Lewis structures are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. They are used to predict the shape of a molecule and its polarity.

8. Is NH3 a Lewis Structure?

Yes, NH3 (Ammonia) has a Lewis structure. It consists of a Nitrogen atom bonded with three Hydrogen atoms and one lone pair of electrons on the Nitrogen atom.

9. What is the best Lewis Structure for CH2S?

The best Lewis structure for CH2S (Methanethiol) is one where the Carbon atom is in the center, bonded to two Hydrogen atoms and one Sulfur atom. The Sulfur atom also has two lone pairs of electrons.

10. What is the role of the VSEPR theory in determining the molecular geometry of AlH3?

The Valence Shell Electron Pair Repulsion (VSEPR) theory is used to predict the geometry of molecules based on the number of valence electron pairs. In the case of AlH3, the VSEPR theory predicts a trigonal planar geometry due to the three bonding pairs of electrons around the Aluminum atom.

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BH3 is the chemical formula of Boron tri- hydride. It is also known as Boranes.BH3 (borane) is comes under natural products which is originated from Erysimum inconspicuum. IUPAC name for BH3 is borane which is also known as trihydrido borane. BH3 consists of one boron atom and three hydrogen atoms. Molecular weight of Boron tri- hydride is 13.84. Here, in this editorial we are learning about BH3 lewis structure.

The Lewis structure of BH3 features Boron (B) as the central atom with three single bonds to three Hydrogen (H) atoms, resulting in an incomplete octet for Boron. Each bond represents a pair of shared electrons. Boron contributes three valence electrons, while each Hydrogen contributes one, totaling six valence electrons. This electron deficiency makes BH3 highly reactive and an electron pair acceptor, classifying it as a Lewis acid. BH3 often forms adducts with Lewis bases, exemplified in its dimerization to form B2H6 (diborane).

How to draw BH3 lewis structure?

To draw the lewis structure there are some rules to be followed like count total valence electrons, select the central metal atom which have lowest electronegativity, octet rule, formal charge, etc. In BH3 lewis structure, the boron atom belongs to 3rd group of periodic table and hydrogen atom belongs to 1st group of periodic table having 3 and 2 valence electrons respectively.

The Boron atom has electronegativity 2.04 and the hydrogen atom has electronegativity 2.2. So, boron atom has lowest electronegativity than hydrogen atom. Thus boron atom should be situated in the central position of the BH3 lewis structure. Then we have to make bonds between H and three H atoms to connect them with each other.

The BH3 lewis structure has three boron hydrogen (B-H) bonds. So, it has three bond pairs and zero lone electron pairs in BH3 leis structure. As the Born atom gains the central position due to lowest electronegativity, thus all the three hydrogen atom gets linked to boron atom.

BH3 valence electrons

To determine valence shell of BH3 lewis structure, check the group positions of B and H atoms in periodic table. The boron atom belongs to 3^rd group of periodic table and having three valence electrons in its outer shell orbital. Similarly hydrogen atom belongs to 1^st group of periodic table and thus having one valence electron in its outer shell orbital.

Boron total valence electrons = 03

Hydrogen total valence electrons = 01

BH3 lewis structure valence electrons = 03 (B) + 1 x 3 (H) = 3 + 3 = 6

Hence, BH3 lewis structure has total six valence electrons.

If we are doing bonding between boron and hydrogen atom we need the valence electrons for bonding. Thus, three valence electrons of boron atom and one valence electron of three hydrogen atoms, total six electrons get consumed in B-H bondings. So, we don’t have any more valence electrons for further sharing in BH3 lewis structure.

BH3 lewis structure octet rule

Octet rule tells us about the presence of complete eight electrons in its valence shell last orbital. Boron atom contains three valence electron as it is comes under 2^nd group of periodic table and hydrogen atom contains one valence electrons as it comes under the 1^st group of periodic table.

Both boron and hydrogen atoms share their valence electrons with each other to form three boron hydrogen (B-H) bonds. So, all the valence electrons of BH3 lewis structure get engaged in bonding remaining no electrons for further sharing.

Thus, boron atom contains six electrons after bonding, two electrons present in each B-H bonds. So, boron atom has incomplete octet. Similarly all three hydrogen atoms contain two electrons (bond pair electrons). Thus three hydrogen atoms also has incomplete octet. As both H and B atoms do not contain eight electrons, so they both have incomplete octet.

BH3 lewis structure formal charge

Formal charge calculation of any lewis structure is done by the following formula:

Formal charge = (valence electrons – non-bonding electrons – ½ bonding electrons)

Let us calculate the formal charge for BH3 lewis structure.

Boron atom: Boron atoms Valence electrons = 03

Boron atoms Lone pair electrons = 00

Boron atoms Bonding electrons = 06 (three single bond)

Formal charge on boron atom = (3 – 0 – 6/2) = 0

So, the boron atom has zero formal charge in BH3 lewis structure.

Hydrogen atom: Hydrogen atom have Valence electrons = 01

Hydrogen atom have Lone pair electrons = 00

Hydrogen atom have Bonding electrons = 2 (one single bond)

Formal charge on iodine = (1 – 0 – 2/2) = 0

So, all the three hydrogen atoms in BH3 molecule have zero formal charges.

BH3 lewis structure lone pairs

The BH3 lewis structure has total six valence electrons in its BH3 molecule. As boron atom has three valence electrons and hydrogen atom has one valence electron, which they get shared with each other for bonding between them i.e. forming three B-H bonds. Hence all the six valence electrons get used for bonding and no more valence electrons are remain for further sharing.

As one single B-H bond contains two electrons, thus 3 (bonds) x 2 (electrons) = 6. OR 6 (valence electrons) / 2 (electrons) = 3 bonds (B-H). Therefore, 6 (valence electrons) – 6 (bonding electrons) = 0. Hence, there are no lone pair electrons are present in B and H atoms in BH3 lewis structure.

BH3 lewis structure shape

BH3 lewis structure contains total three (B-H) covalent bonds forming within central boron atom and outer three hydrogen atoms. No lone electron pairs are present on central B atom and outer three H atoms of BH3 lewis structure. As the three H atoms joined with central boron atom, the BH3 lewis structure has trigonal planar geometry.

Even the shape and molecular geometry of BH3 lewis structure can be determine by VSEPR theory. According to VSEPR theory the AX3 generic formula is applicable on BH3 molecule. ‘A’ is denoted central atom i.e. Boron atom. ‘X’ is denoted number of bonding atoms attached to central atom i.e. three H atoms. Thus as per the VSEPR theory, any molecule follows a generic formula AX3, then it has a electron geometry and molecular geometry trigonal planar.

BH3 hybridization

Hybridization of any lewis structure or molecule is depends upon the calculation of its steric number. The formula for steric number is as follows:

Steric number = sum of number of central atoms connected bonded atoms and lone electron pair present on central atom

Steric number for BH3 = 3 (H atoms) + 0 (lone pair electrons) = 3

As the BH3 lewis structure has 3 calculated steric number means it has sp2 hybridization. Thus the BH3 lewis structure shows sp2 hybridization.

BH3 lewis structure angle

Bond angle is the angle which is formed within the central atom and any two bonding atoms. To form a bond angle there is a need of at least three elements or atoms in a molecule. As the BH3 lewis structure has trigonal planar geometry or shape, so it has 120 degree bond angle. Hence, in BH3 lewis structure the hydrogen boron hydrogen (H-B-H) bond angle formed of 120 degree.

BH3 lewis structure resonance

The resonance structure of any molecule is only possible when it contains multiple bonds (double or triple bonds) and also there should present some formal charges (+ve or –ve) with lone pair electrons present on that molecule.

In BH3 lewis structure, there are only three boron hydrogen (B-H) covalent bonds are present. All the three hydrogen atoms joined with central born atom with three single covalent bonds. Means multiple bonds are absent in BH3 lewis structure. Also no formal charges i.e. zero formal charge on B and H atoms. Even no lone electron pairs are present. So, BH3 molecule cannot show resonance structure.

BH3 solubility

BH3 (boron tri- hydride) is soluble in:

• Water ( decomposed completely at 100 degree temperature heating)
• Water (slightly soluble at 20 degree temperature heating)
• Concentrated sulphuric acid (H2SO4)
• Ethanol
• Benzene
• Ammonium hydroxide (NH4OH)

Is Bh3 ionic?

No, BH3 is not ionic in nature, it is a covalent molecule. As there are three boron hydrogen (B-H) covalent bonds are present in BH3 lewis structure, so it cannot form any charge or dipole to being ionic in nature. Thus BH3 lewis structure or molecule is covalent in nature.

Why BH3 is not ionic?

There is no formal charge is present on central boron atom and outer three hydrogen atoms and also there is no lone electron pair density on B and H atom. Thus it cannot form any positively charged cation or negative charge anion to make the molecule ionic in nature.

How BH3 is not ionic?

As all the three hydrogen atoms gets connected with central boron atom with single strong B-H covalent bonds i.e. three B-H covalent bonds are present in BH3 molecule. So, there is no chance for the formation of positive or negative ion within the molecule. Hence the BH3 molecule is not ionic rather it is covalent in nature.

Is BH3 acidic or basic?

BH3 lewis structure or molecule is considered as a lewsi acid. So, BH3 shows acidic nature and not basic nature.

Why BH3 is acidic?

The electron pair acceptor compound or molecule is known to be a lewis acid. BH3 is a lewis acid as it has only 6 valence electrons which gets used in bonding with three hydrogen atoms. Thus, BH3 molecule is being electron deficient and also it has empty ‘p’ orbitals to easily accept electrons from other molecules. Thus it is lewis acid.

How BH3 is acidic?

As the BH3 molecule do not have lone electron pairs because all six valence electrons get used in B-H bonding and also it has an incomplete octet. Because of this reasons BH3 molecule can readily accept electrons from any lewis bases which makes BH3 a lewis acid molecule.

Is BH3 polar or nonpolar?

BH3 lewis structure or molecule is non- polar in nature. As there is no polar bonds present in BH3 molecule. To determine the polar or non- polar nature of any molecule we should check two things i.e. presence of at least one covalent  polar bond and symmetry of molecule.

Why BH3 is non- polar?

Boron and hydrogen atoms have almost similar electronegativity i.e. 2.04 and 2.20. So there is not much difference between electronegativities of B and H atom, which makes the BH3 molecule non- polar in nature.

How BH3 is non- polar?

The BH3 molecule has symmetrical structure as all the three boron hydrogen (B-H) bonds have equal bond length, due to which the dipole moment creates in molecule gets cancel each other i.e. net zero dipole moment is present in BH3 molecule. Thus, it is non- polar molecule.

Conclusion:

BH3 consists of one B and three H atoms. BH3 has 6 valence electrons and three B-H covalent bonds. It is a lewis acid and non- polar molecule. Also it has no lone electron pairs and trigonal planar in shape with sp2 hybridization and 120 degree bond angle.

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Boron tribromide (BBr3) has a central boron (B) atom with 3 valence electrons, each forming a single bond with three bromine (Br) atoms, which contribute 7 valence electrons each. The Lewis structure depicts three single B-Br bonds and no lone pairs on boron, using 24 bonding electrons. BBr3 exhibits a trigonal planar geometry with bond angles of 120°, indicative of sp² hybridization. The molecule is nonpolar due to its symmetrical shape, despite the polar nature of B-Br bonds due to the electronegativity difference (B: 2.04, Br: 2.96). This structure affects its reactivity, especially in electrophilic aromatic substitution reactions.

BBr3 (Boron Tri- bromide) is a incensed liquid with no colour or amber in colour. It is quite toxic to inhale. It has a sharp (irritating / pungent) smell. Boron tri- bromide has molecular weight 250.53. The IUPAC name of Boron tri- bromide is Tri- bromo borone. In this editorial we are learning about the BBr3 lewis structure and its various facts.

How to draw BBr3 lewis structure?

While drawing any lewis structure main points to be noted are valence electrons of molecule, bonding with central atom, octet rule follow, formal charge count. In BBr3 there is one boron and three bromine atoms are present.

In BBr3 lewis structure, the boron atom is situated centrally surrounded by three bromine atom. The atom should be at central position which has low electronegativity. Boron has electronegativity 2.04 and bromine has electronegativity 2.96. That’s why boron atom with lowest electronegativity should be at central position.

The BBr3 lewis structure has three B-Br bonds, thus it has three bond electron pairs and nine lone electron pairs. As we selected the boron as central atom, the three bromine atoms get linked to the boron atom.

BBr3 valence electrons

To calculate the valence electrons in BBr3 lewis structure, first we have to check the positions of boron and bromine atom in the periodic table. As the boron atom belongs to 13^th group of periodic table, the B atom contains three valence electrons in its outer orbital. Similarly Bromine atom belongs to the 17^th group of periodic table, so it contains seven valence electrons in its outer orbital.

Total valence electrons in B atom = 3

Total valence electrons in Br atom = 7

Total valence electrons in BBr3 lewis structure = 3 (B) + 7 x 3 (Br) = 24

Thus, the BBr3 lewis structure has 24 total valence electrons.

If we are using six electrons in bonding between boron and bromine atom, so we are left with total eighteen valence electrons for distribution on three bromine atoms. Therefore, three bonds containing two electrons each ( 3 x 2 = 6 ), so we have 24 – 6 = 18 electrons for sharing.

BBr3 lewis structure octet rule

The octet rule says there should be eight electrons present to complete the octet of any element or atom. Now, we have remaining eighteen valence electrons for sharing in BBr3 lewis structure. So, put the remaining 18 electrons first on outer three bromine atoms to complete its octet.

As we have put all the remaining 18 valence electrons on three bromine atoms, so the single bromine atom now contains 8 electrons i.e. two bond pair electron in each single B-Br bonds and six valence electrons on each single bromine atom. So, the outer three bromine atoms of BBr3 lewis structure has complete octet.

Now we have used all the eighteen electrons by sharing on three bromine atoms. So, we don’t have more valence electrons remain for sharing. Thus, the central boron atom has only six electrons i.e. only three bond pair electrons containing two valence electrons each. So, the Boron atom has incomplete octet. Hence, in BBr3 lewis structure, B atom has incomplete octet and three Br atoms has complete octet.

BBr3 lewis structure formal charge

There is a formula to count formal charge on any lewis structure as follows:

Formal charge = (valence electrons – non-bonding electrons – ½ bonding electrons)

The calculation for formal charge on BBr3 molecule as follows:

Boron atom: Valence electrons on boron = 03

Lone pair electrons on boron = 00

Bonding electrons with boron = 06 (three single bond)

Formal charge on boron = (3 – 0 – 6/2) = 0

So, the boron atom has zero formal charge.

Bromine atom: Bromine atom have Valence electrons = 07

Bromine atom have Lone pair electrons = 06

Bromine atom have Bonding electrons = 2 (one single bond)

Formal charge on iodine = (7 – 6 – 2/2) = 0

So, all the three bromine atoms in BBr3 molecule have zero formal charges.

BBr3 lewis structure lone pairs

The BBr3 lewis structure contains total twenty four valence electrons, out of which six valence electrons are being bond pairs as they involved in bonding between three bromine atoms with the central boron atom. Thus, we are remained with eighteen valence electrons for further sharing on outer bromine atoms.

As we have put all the 18 electrons on three Br atoms, so each Br atom has complete octet with 8 electrons. Hence, each Br atom has one bond pair electron and three lone electron pairs. Therefore, in BBr3 lewis structure, B atom has no lone electron but Br atom has 9 lone electron pairs.

BBr3 lewis structure shape

As per the VSEPR theory, the generic formula the molecular geometry of BBr3 molecule is AX3. As the central boron atom is linked with three bromine atoms which has more electron density on it, so the BBr3 lewis structure has trigonal planar shape or geometry.

BBr3 hybridization

Hybridization of any molecule or lewis structure is determined by its steric number. To calculate the steric number of any molecule there is a formula:

Steric number = sum of number of bonded atoms joined to central atom and presence of lone electron pair on central atom

Steric number for BBr3 = 3 + 0 = 3

As the BBr3 lewis structure has 3 steric numbers, it is sp2 hybridized. So, the BBr3 lewis structure has sp2 hybridization.

BBr3 lewis structure angle

The BBr3 lewis structure has trigonal planar geometry and also it is sp2 hybridized. As the central boron atom is joined with three bromine atom surrounded to it thus having three B-Br bonds. So each bromine boron bromine bond ( Br-B-Br ) has 120 degree bond angle within it. Hence the BBr3 lewis structure has 120 degree bond angle in its structure.

BBr3 lewis structure resonance

Any molecule can show the resonance structure only if in the molecule there are multiple (double / triple) bonds present and also it has some formal ( positive or negative ) charge with the presence of lone electron pairs on atoms of molecule.

In BBr3 lewis structure, there is no multiple bonds are present. All the three bromine atoms get attached with the central boron atom with single covalent bonds i.e. three covalent (B-Br) bonds in BBr3 lewis structure. Also the formal charge on B atom and Br atom is zero. So, the resonance structure of BBr3 lewis structure is not possible.

BBr3 solubility

BBr3 (boron tri- bromide) is soluble in:

• Carbon tetrachloride (CCl4)
• Liquid sulphur dioxide (SO2)
• Sulphur dichloride (SCl2)
• Methyl cyclohexane (moderately soluble)
• Water (reacts violently)
• Di- chloro methane (CH2Cl2)

Is BBr3 ionic?

No, BBr3 molecule is not ionic compound. BBr3 molecule consists of two elements i.e. boron and three bromine atoms with are connected to each other with the covalent bonds. Also there is no negative or positive formal charge is present on B and Br atoms. Even the B and Br atoms are not showing the characteristics of being cation or anion.

Why BBr3 is not ionic?

Both B and Br atoms contains zero formal charge with covalent bonds, which makes BBr3 molecule a covalent compound. So, the BBr3 molecule is not ionic but it is a covalent inorganic compound. Hence, BBr3 is not ionic but covalent compound.

How BBr3 is not ionic?

The one B and all three Br atoms are attached with each other with single B-Br covalent bonds which is a strong bond. So, there is no formation of ions with positive or negative charge. So, it is not ionic but covalent in nature.

Is BBr3 polar or nonpolar?

BBr3 molecule is non- polar in nature, because the BBr3 molecule has a symmetrical arrangement of atoms in its structure. So the dipole which creates on B-Br molecule gets cancel each other makes it a non- polar molecule.

Why BBr3 is non- polar?

The B atom has 3 valence electrons and Br atom has 7 valence electrons, So Br needs only 1 electron for octet completion. As they forming three bonds with each other B atom shares its three valence electrons to three Br atoms and form covalent bonds. So, BBr3 molecule has symmetrical structure as each bromine atom making 120 degree bond angle with other Br atoms. Hence, all three Br atoms lie in a similar plane forming trigonal planar geometry.

How BBr3 is non- polar?

BBr3 is non- polar as each B- Br bonds having 120 degree bond angle within the molecule in same plane, so they are cancelling the dipole moment produced within the bonds. Hence, there is zero dipole moment creates in BBr3 molecule making it non- polar in nature. As the dipole get cancel in BBr3 molecule it is non- polar in nature.

Is Bbr3 acidic or basic?

BBr3 molecule shows the characteristic of lewis acid. So, it is acidic in nature and not basic in nature.

Why BBr3 acidic?

The acceptor of electron pair is known to be an acid compound. In boron halides like BBr3, they are good acceptor of electron cloud to form BBr3 molecule. BBr3 is a strong lewis acid as the bromine atom has much electron cloud to donate to other atoms, hence it is a strong lewis acid in nature.

How BBr3 is acidic?

In BBr3 lewis structure, there is no lone pair electron on central B atom but the outer three Br atoms has much electron cloud i.e. three lone pair electron on each Br atom. So, the BBr3 molecule can accept more electron and being an electron pair acceptor, the BBr3 molecule is a lewis acid.

Conclusion:

BBr3 lewis structure has 1 B and 3 Br atoms with zero formal charge. BBr3 is a covalent compound, acidic in nature and a non- polar molecule.

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In this article we are going to discuss the bao lewis structure and 13 important facts regarding its structure and characteristics.

Barium oxide is formed when barium is burned in presence of Oxygen. It is white crystal cubic structure solid which is non-flammable as well as hygroscopic in nature. The cathode ray tube is composed of bao. It is also used in making crown glasses and as a catalyst.

Bao Lewis Structure Drawing

Bao is formed by two elements i.e. one is barium (Ba) and other is oxygen (O). Ba is a member of alkaline earth metal i.e. group (II) and oxygen is a member of group 16. Barium has atomic number 56. Its electronic configuration is [Xe] 6s². When it losses two electron from 6s orbital it acquires the nearest noble gas configuration i.e. Xe (Z=54).

When Ba atom losses 2 electrons Ba+2 ion is formed. In case of oxygen, it has atomic number 8. Its electronic configuration is [He]2s²2p⁴. When it gains 2 electrons it gets nearest noble gas configuration of Ne in which octet is fulfilled. Then Ba+2 and O2- ions are attached by electrostatic force of attraction which is a strong force and bao is formed.

BaO Lewis Structure Resonance

Resonance is an empirical process in which electrons moves from one atom to another by losing and gaining of electrons. Barium Oxide is a neutral molecule having zero formal charge (f.c) on it. When resonance takes place BaO breaks into Ba⁺² ion and O^2- ion.

Both barium and oxide ion are stabilized because both possess stable nearest noble gas configuration after resonance i.e. barium ion acquires Xenon (Xe) noble electronic configuration and Oxide ion acquires Neon (Ne) noble gas configuration, both the ions fulfill their octet after resonance.

Bao Lewis structure shape

According to VSEPR theory bao has octahedral co-ordination geometry. In the crystal structure of bao 6 Ba2+ ions are surrounding by 6 O2- ions and 6 O2- ions are surround by 6 Ba2+ ions.

For this reason both Ba2+ and O2- ions have co-ordination number equals to 6. As because bao has octahedral shape it possess d2sp3 hybridization.

Bao Lewis Structure Formal Charges

In barium oxide overall formal charge on the compound is Zero. Bao ionizes to form Ba2+ and O2- ions. Barium has +2 formal charges which are neutralized by Oxygen 2- formal charge.

In the cubic crystal lattice structure of barium oxide 6 Ba2+ ions are surround by 6 O2- ions and 6 O2- ions are surrounded by 6 Ba2+ ions making the whole compound is neutral.

Bao Lewis structure angle

As we seen form bao lewis structure, bao has octahedral shape with d2sp3 hybridization and according to octahedral geometry the angle should be 900. Bao also possess the same bond angle which is equal to 900.

Bao Lewis Structure Octet Rule

In the bao lewis structure both barium and Oxygen atom fulfilled their octet. When bao is formed barium lost its two electrons to acquire the nearest noble gas configuration of Xe which have 8 electrons in its valance shell (5s25p6).i.e. octet is fulfilled.

Oxygen atom gains two electrons which is rejected by barium atom to possess the nearest noble gas configuration of neon which also possessed 8 valance electrons (2s²2p⁶). Hence both barium and oxygen atom fulfilled their octet.

Bao Lewis Structure Lone Pairs

When we see the bao lewis structure zero lone pair present on Ba and 2 lone pair of electrons present on oxide ion.

This is because of the fact that barium losses its two electron to form Ba2+ion which does not have any lone pair of electron on it. But Oxygen atom gains two electrons which is rejected by Ba atom and is converted into O2- ion in which two lone pair of electrons present.

Bao Valance Electrons

Firstly to find out the total valance electron in Bao, it is essential to know the electronic configuration of Ba and O atom. The electronic configuration of Ba is [Xe] 6s2 and we see from electronic configuration that there are 2 electrons in valance shell of Ba atom.

The electronic configuration of O atom is [He]2s2 2p4. There is 6 electrons in the valance shell of O atom. The total valance electrons that exist on bao will be equal to the (sum of the valance electron of Ba and O atom) i.e. equals to (1*2)+(6*1)=8. There are 8 valance electrons in bao.

Bao Hybridization

When bao breaks down Ba+2 and O2-ion is formed. Barium oxide exists in a cubic crystal like lattice structure. Both barium and oxygen possess d2sp3 hybridization i.e. bao has octahedral co-ordination geometry.

In the crystal lattice structure of barium oxide each Ba+2 ion is surrounded by six O2- ions and each O2-ion is surrounded by six Ba+2ions. Hence both barium ion and oxide ion have same co-ordination number which is equal to 6.

Bao Solubility

In bao due to higher electronegativity of O and lower electronegativity of Ba atom it exists in Ba2+ and O2- ions i.e. opposite dipoles are produced. As different dipoles created on Ba2+ and O2- ions it is polar in nature and it is soluble in polar solvents.

It is soluble in ethanol (C2H5OH), dilute mineral acids like HCl, HBr, HI etc and also soluble in alkalies like NaOH, KOH etc. But it is insoluble in nonpolar solvents like acetone, ether, liquid ammonia. When barium oxide reacts with water it forms barium hydroxide [Ba(OH)2] which is alkaline in nature.

Is BaO Ionic?

Bao is an ionic compound. This is due to the fact that bao dissociates to give Ba2+ and O2- ions when it dissolves in aqueous solution or in molten state. This is an important characteristic of ionic compound.

It also conducts electricity in aqueous or in molten state. This is due to the presence of Ba2+ and O2- ions in both the states and we know that ions carry current. Like ionic compounds bao is soluble in polar solvents e.g. water, ethanol etc.

Is Bao Polar Or Nonpolar?

Barium Oxide is a polar compound. This is because in barium oxide both barium and oxygen have different electronegativity and hence opposite dipole creates on barium and oxygen.

Due to less electronegativity of barium it accommodates positive dipole on it and due to higher electronegativity of O atom it possesses negative dipole. As because opposite dipole formed in barium Oxide, it is an ionic compound with high dipole moment. Hence bao is a polar compound.

Is BaO acidic or basic?

Ba has a tendency to loss electrons i.e. it is metallic in nature. This is because of the fact that Ba has lower electronegativity and also it acquires stable noble gas electronic configuration of Xe by losing 2 electrons.

We know that the oxide of a metal is basic in nature i.e. when basic oxide reacts with water it forms alkalies. In the similar way when bao reacts with water, it forms basic hydroxide i.e. barium hydroxide which is alkaline in nature. This is because it gives OH- ions in solution.

Conclusion

By considering the above mentioned facts we can conclude that bao is a stable ionic compound. As it is an ionic compound it is polar in nature as well as soluble in polar solvents and bao is a basic oxide because it is an oxide of a metal i.e. Ba.

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This topic is all about Bacl2 and how to draw bacl2 lewis structure, resonance, shape, formal charge, angle, the octet rule, lone pairs, valence electrons, hybridization, and their related properties.

The inorganic salt barium chloride is composed of cations and anions. Barium chloride is water soluble white solid salt. It is a yellow-green color when undergoes flames. The formula of barium chloride is BaCl₂. Barium chloride is toxic.

How to draw bacl2 lewis structure?

The periodic table group 2 element contains Ba elements having 2 valence electrons such that Ba has two dot lewis structures.

A chlorine atom has 7 valence electrons in its outermost shell, to complete its octet it will gain one electron and acquire one negative charge, and when they combine formation of ionic compounds occurs.

In ionic compounds, there is no sharing of electrons only the transfer of electrons takes place. 

Bacl2 lewis structure resonance

Barium which is metal and chlorine which is non-metal, when metal and nonmetals combine gives an ionic compound.

Ba⁺² combines With Cl^-1 to form BaCl₂ which is an ionic compound that is white. 

Bacl2 lewis structure shape

Bacl2 in natural conditions exists in the form of white crystals. This crystalline solid exists in an orthogonal structure.

Bacl2 lewis structure formal charge

Charges, or formal charges, are assigned to atoms in molecules. Barium with an electronic configuration= [Xe]6s², contains two valence electrons in the last shell.

Thus barium is a metal that belongs to the 2nd group of elements that always shows a +2 oxidation state. Thus in Bacl2, Ba possessed a +2 charge that loses the electrons, and two Chlorine gain 1electron having a -1 charge. Thus formal Charge on Bacl2 = Ba =+2, and 2Cl= -1.

Read more about Strong Electrolyte Examples

Bacl2 lewis structure angle

Bacl2 molecules have a linear shape with a 180 ° Bond angle.

It is an ionic compound with Ba⁺² Charge and Cl^-1.

Bacl2 lewis structure octet rule

Barium chloride is an ionic compound. This barium is the exception because it follows the octet rule and still does not have 8 electrons in its outer shell.

As Ba loses 2 electrons and becomes a stable noble gas electronic configuration as Ba= [Xe]6s²  it changes into Ba=[Kr] 5s²,4d¹⁰,5p⁶ . Thus no. of valence electron around the surrounding metal is less than 8.

Bacl2 lewis structure lone pairs

According to the lewis dot structure of bacl2, Ba has 2 valence electron and Cl have 7 valence electrons. Bacl2 is formed by the transfer of electrons from Ba to cl and after this, there are remaining lone pairs on the chlorine only.

Thus chlorine contains 6 lone pair and overall all compound is ionic.

Bacl2 valence electrons

Valence electrons are those which are present in the outermost shell of an atom.

How many Valence electrons are in Bacl2?

Barium belongs to group 2 in the periodic table that’s why consists of 2 valence electrons in its outermost shell of it.

Thus barium has +2 valency and in the case of chlorine, it has 7 valence electrons in its outermost shell.

Ba= 2 valence electrons

Cl= 7 valence electrons

Bacl2 hybridization

A pictorial and mathematical method to determine the bonding in a molecule is called hybridization.

What is the Hybridization of Bacl2?

Hybridization is the mixing of atomic orbitals that is of the same energy and form a new hybrid orbital.

In Bacl2 Molecules, there are Sp Hybrid orbitals are formed with linear structure and 180° Angle. So, the Hybridization of Bacl2 is Sp.

Bacl2 solubility

1. In water, barium behaves differently and it forms electrolytes in the water in the ratio of 1:2.
2. It dissolved in water and separated into cation(Ba⁺²) and anion (Cl^-1).
3. Solubility of Barium chloride in water = 358gm/lt at 20℃. 
4. Barium chloride is thus soluble in water at different temperatures, as Bacl2 gives cation and anion in water and water has H⁺ and OH^– ions so, it dissolves in water easily. Chloride of barium dissolves in methanol as well, but not in ethanol.

Is Bacl2 ionic?

Yes, Bacl2 ionic inorganic salt.

Barium chloride is formed by the combination of metals and non-metals, in general when metals combine with non-metals there is the formation of an ionic bond takes place.

Here transfer of electrons from Ba⁺² to Cl^-1 and due to this transfer formation of an ionic bond occurs. The oxidation state of Ba is +2 and the Oxidation state of Chlorine is -2.

How is Bacl2 ionic?

In general, when metals combine with nonmetals, an ionic bond is formed. There is another reason Bacl2 is ionic is the differences in their electronegativity.

As we can see in the periodic table Ba⁺² have electronegativity is 0.89 which is less than Cl^-1 that have 3.16. So this difference in electronegativity is greater than 2.0 which means the compound is ionic.

Is Bacl2 polar or nonpolar?

Bacl2 is polar due to solubility in water and the polarity of barium chloride is due to the difference in electronegativity between Barium and chlorine atoms.

The geometry of molecules is different like its Hybridization is sp and possess crystalline structure therefore their dipole moment do not cancel each other generate dipole and this become polar.

Is Bacl2 an acid?

The compound barium chloride is not acidic.

Reason:

By losing two electrons, barium becomes cation and chlorine becomes anion, creating an ionic compound. So when we made an aqueous solution it dissolved in water in the form of water-soluble salts. So Bacl2 is not acidic.

Why is Bacl2 neutral?

Barium chloride is neutral due to its aqueous solution and in aqueous solution formation of cations and anions which make the solution electrically neutral and the pH of the solution become neutral.

So we can say that when bacl2 is dissolved in water it forms an aqueous solution. It is formed of Ba(OH)₂ in water, Thus Ba(OH)₂ is a strong base, and HCl which are strong acids, this will leads to the form of a neutral salt called Bacl2.

Is Bacl2 a precipitate and why?

Yes, Bacl2 forms precipitate due to displacement reaction with K₂SO₄, this will leads to an insoluble sulfate product in water such as Barium sulfates.

Barium sulfate is in form of a precipitate. An insoluble precipitate is formed when two solutions are combined this is called a precipitate reaction and on the other hand displacement reaction is the displacement of one atom with another.

  BaCl₂ +K₂SO₄ —-> BaSO₄ + 2KCl

                              (Insoluble white ppt.)

Conclusion:

Solution of barium chloride(BaCl₂) is an inorganic salt and a water-soluble salt. The pH of the solution is neutral. Barium and chlorine ions are formed in water when it reacts with H⁺ and OH^– ions. Hence, it can be dissolved easily in water. Bacl2 is highly toxic.

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