lewis structure

In this article we will discuss about Dibromine,Br₂ its lewis structure, properties and other facts.

Dibromine, Br₂ consists of two bromine atoms joined through a single bond. Bromine is one of the lightest element in halogen family. Dibromine is a reddish brown liquid with a pungent smell which is very toxic for inhalation.

  How to draw Br₂ 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. It uses dots and lines to depict electrons and bonds respectively.

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. Dibromine,Br₂ is chemical compound with two bromine atoms combined together. Let’s see how to draw the lewis structure of Br2.

• Calculate the total number of valence electrons. Bromine is a group 7 element having seven electrons in its valence shell. Since dibromine has two bromine atoms the total number of valence electrons present in Br₂ is 7×2 = 14 electrons.
• In this step we draw the symbols for two bromine atoms surrounding with their seven valence electrons.

• In the next step the two bromine atoms shares their one electron each other to form a single bond. Now both the bromine atoms are combined together and they attained stability by satisfying octet rule.

Br₂ 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 dibromine it is not allowed to move across, because if they do so the molecular structure  not exist. So there is no resonance structure for dibromine.

Br₂  Shape

Dibromine is a linear shaped molecule with one bromine – bromine sigma bonds. Br₂  is symmetrical in its structure.

Br₂ 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)

Valence electrons present in bromine is 7. In which 6 were lone pairs and one electron is shared to make bond with another bromine atom

Formal charge of  bromine is = 7-6-1

                                                = 0

So the formal charge of bromine in Dibromine, Br₂ is 0.

Br₂ Bond angle

Bond angle is the angle made between three atoms when they combine together to form a stable compound. Dibromine is a linear or symmetrical molecule with one Br- Br sigma bonds. The bond angle made by a linear molecule is 180⁰. So the bond angle of Br₂ is 180⁰.

 Br₂ 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 dibromine there is two bromine atoms.

Each bromine has seven electrons in its valence shell. It need one more electron to attain stability. When these two atoms combines together both of them shares their electrons to each other. Hence their valence shell is filled with eight electrons and they are stable now. Since both of the bromine atom has eight electrons in its valence shell Dibromine obeys octet rule.

Br₂ 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 one bromine is 3. So the total number of lone pair of electrons present in two bromine atoms of dibromine 6.

Br₂ valence electrons

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

Total number of valence electrons present in dibromine is 14.

Br₂ Hybridisation

According to the concept of hybridisation, the atomic orbitals with slightly different energies unites together to form atomic orbitals with same energy and shape. The new orbitals formed are stable and named as hybrid orbitals. The  number of hybrid orbitals is equal to that of the orbitals got united.

There is different types of hybridisation called

1. sp³
2. sp²
3. sp
4. sp³d
5. sp³d²
6. sp³d³

Hybridisation of a molecule can be found through a formula, which is

Hybridisation of a molecule = No. of sigma bonds + No. of lone pairs

 If the count is 4 then sp³ hybridisation ,3 then sp² and if 2 then sp.

In dibromine there is one sigma bond and three lone pair of electrons.

Hybridisation of Br₂ = 1+3  = 4

 So the hybridisation in dibromine is sp³. Its structure is linear.

Br₂ 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, chloroform  etc.

 Dibromine is slightly soluble in water because it is not a polar molecule like water. But dibromine is found to be soluble in most of the organic solvents like benzene, gasoline, chloroform, ether, methanol, ethanol, carbon disulphide, carbon tetra chloride,CCl₄.

 Is Br₂  Ionic or not ?

A covalent bond is formed by the sharing of electrons between the combining atoms but ionic bond formation takes place through the electrostatic force of attraction between a positive and negative ion. The positive and negative ions are cation and anion respectively.

Dibromine is formed by the mutual sharing electrons between two bromine atoms. So Br₂ is a covalent compound not an ionic compound.

Is Br₂ Polar or not ?

There are only two bromine atoms are attached together through a single bond in dibromine. So it is non polar in nature.

Is Br₂ Acidic or Basic ?

Dibromine is a lewis acid.  A lewis acid is a substance which can accepts electrons.

Summary

Dibromine is a chemical compound which exists as liquid and gas in room temperature. This article summarise the following key points

1. Dibromine is a covalent compound with non polar character.
2. Dibromine shows acidic behaviour.
3. Br₂ follows sp³ hybridisation.
4. It is soluble in organic solvents and sparingly soluble in water.
5. Its lewis structure drawing pattern.

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This article is regarding Brf5 lewis Structure, characteristics, and properties of Brf5.

Bromine pentafluoride, commonly known as Brf5, is a chemical used in the uranium processing industry and as a propellant for rockets. There is a liquid associated with this that is corrosive.

It becomes highly toxic and combustible when it reacts with organic matter. Brf5 lewis structure is an interhalogen compound with properties of Fluorinating.

How to draw Brf5 lewis structure?

In its outermost shell, bromine has seven valence electrons, which makes it a member of the halogen family. The halogen family also includes fluorine, which has 7 electrons in its outermost shell. So Bromine shares 5 electrons with fluorine and forms covalent bonds. 

Bromine valence electrons = 7

Fluorine valence electrons =7*5 =35

Total valence electrons = 42

Thus total electron pairs for bonding = 21, and participate in bond formation.

and remaining 1 pair as a lone pair. 

Bromine act as a central atom due to less electronegativity than fluorine. A Lewis dot structure consists of five Br-F bonds in Brf5.

Brf5 lewis structure resonance

In Lewis structure of Brf5 is composed of 42 valence electrons. We can distribute the valence shell around the nucleus to fill the outermost layers of each atom once we know how many there are in Brf5. There is no resonance observed in Brf5 and no isomers exist in Brf5.

The bromine (Br) atom makes up one of the five fluorine atoms in Brf5. While the bromine (Br) atom is in the center, the fluorine (F) atoms are scattered around it. 

Brf5 lewis structure shape

Brf5 has a pyramidal square shape. It indicates that the basic atom has a single pair of electrons.

The square pyramidal effect of BrF5 molecular structures is due to the individual electron pairs on the core bromine atom.

Brf5 lewis structure formal charge

The formal charge is found as (valence electrons- nonbonding electrons-½ bonding electrons).

Formal charge on Br = 7-5-2 =0

Formal charge on F = 7-6-1 =0

The Brf5 Lewis structure has a zero formal charge.

Brf5 lewis structure angle

Brf5 has an octahedral shape with a 90-degree angle. 

There is repulsion between each atom which should be explained by VSEPR Theory.

Brf5 lewis structure octet rule

A molecule needs eight electrons to complete its octet, which means they need 8 electrons in the outermost shell. This is known as the octet rule and is used to work out how close an atom is to a specific other atom or molecule.

In the Brf5 lewis structure, bromine (Br) belongs to period four, which means it has a valence electron capacity greater than eight. Once knowing that, how many electrons are present in Brf5, the distribution of electrons around the central atom is done. Thus Center atom Bromine in Brf5 lewis structure has expanded its octet.

Brf5 lewis structure lone pairs

Valence electron of Br = 7 and there are five sigma bonds present between bromine and fluorine atoms.

Hence, there is only one lone pair present in Bromine(Br) hybrid orbitals. These lone pairs of electrons are also called non-bonding electrons

Brf5 valence electrons

There are seven valence electrons present on the bromine(Br) atoms and seven valence electrons on fluorine(F) atoms. They both belong to the halogen family.

In total Brf5 consist of 42 valence electrons and is calculated as,

Bromine valence electrons = 7

Fluorine valence electrons =7*5 =35

Total valence electrons = 42

Brf5 hybridization

Bromine atom Electronic configuration: 1s² 2s²2p⁶ 3s²3p⁶3d¹⁰4s²4p⁵.

Or

Br = [Ar]4s² 3d¹⁰4p⁵

Some electrons are shifted to 4d-orbitals to obtain a pentavalency. There are two p-orbital that are unpaired. Bromine atoms at this point are excited and their will occurrence of hybridization takes place.

Four of the orbitals are 4s, three 4p, and two 4d, while the six steric nodes are involved in hybridization. So the Hybridization of Brf5 molecules is sp³d². There is a five sigma bond formation that occurs between five fluorine atoms and five valence electrons of bromine.

Brf5 solubility

Brf5 is soluble in water, it reacts with water violently and produces explosive and some toxic that is hazardous to human.

It is the fluorinating agent.

                                        BrF₅ + H₂O —-> HBrO₃ + HF

                                   Bromine                 Boric 

                               Pentafluoride              acid

Is Brf5 ionic?

For a molecule should be ionic its electronegativity difference should be more and one atom consist of a partial positive and another atom should possess a partial negative charge. So in the case of Bef5 Bromine(Br) and Fluorine (F) have an electronegativity difference of less than 1.02, so they are not ionic.

Since all halogens are non-metals, this electronegativity difference can only exist between metals and non-metals, Brf5 is not ionic.

Is Brf5 acidic or basic?

Brf5 lewis structure is highly reacting with water and forms boric acids.

As a result of highly electronegative halogens in this molecular structure, the molecule reacts with a variety of organic substances, including water (H₂O) also. Thus Brf5 lewis structure is having some basic properties because it acts as a metal fluoride and converts into [Brf4]⁺ and [Brf6]^–.

Is Brf5 polar or nonpolar?

The molecules are polar when the electrons are not evenly shared between the atoms in their covalent bonds.

It is a polar molecule with a square pyramidal molecular geometry and an asymmetric charge density centered on the nucleus. 

The molecule is composed of five fluorides surrounded by a central bromine atom and a lone pair of electrons.

It is therefore polar. Thus Brf5 lewis structure gives information about the polarity of molecules and its reactivity is also explained through it.

In terms of structure, Brf5, or bromine pentafluoride, is similar to PCl5, which has a bipyramidal trigonal structure. As the Brf5 Lewis structure is completely symmetric around the central phosphorus atom, there is no net dipole moment.

Conclusion

It has been established above via various illustrations and facts that Brf5 is a polar molecule. However, it is mostly used in aeronautical rocket propulsion. It consists of 42 valence electrons in total, due to the asymmetrical distribution of electrons it shows square pyramidal geometry. BF5 is a powerful fluorinating agent.

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In this article we are discussing about bro4- lewis structure, characteristics and 13 important facts regarding this.

Perbromate (bro4-) is an oxoanion of bromine. Like clo4-, io4- it is difficult to prepare. The molar mass of bro4- ion is 143.901 g/mol. When bro3- ion reacts with fluorine in alkaline medium, bro4- ion is produced. When perbromic acid losses one proton bro4- ion is produced.

Bro4- Lewis Structure Drawing

In the bro4- lewis structure we see that as bromine becomes bigger in size and less electronegative than O, br act as the central atom in the lewis structure of bro4- ion. Bromine has 7 valance electrons out of which 4 electrons take part in sigma bonding with 4 O atoms and forms 3 pi bonds with 3 O atoms.

There is no remaining electrons on br atom which act as lone pair of electron. O atom has 6 electrons in the valance shell out of which 1 is used in making sigma bond and another is used in making pi bond with br atom and remaining 4 electrons present as nonbonding electron pair on O atom.

Bro4- Lewis Structure Resonance

Resonance is an empirical process in which movement of electron pair takes place from one atom to another atom and the structure obtained by this process is called resonating or canonical structure.

Bro4- has 4 resonating structure in which each Br-O bond acquires partial double bond character through the process in which negative charge on O atom is delocalized with the empty ∏* antibonding orbital of Br=O bond.

Bro4- Lewis Structure Shape

According to VSEPR theory the shape of Bro4- is tetrahedral in which central Br atom is tetrahedrally surround by 3 O atoms and 1 O- ion. As lone pair absent in the central Br atom, Bro4- ion possesses true tetrahedral structure. As the shape is tetrahedral, the bond angle occurs in this compound is exactly 109.280.

Bro4- Lewis Structure Formal Charge

The formal charge on any atom or ion can be obtained by the formula which is given below:

Formal Charge (f.c) =V.E- B.E/2- N.E

 Where,

V.E= Total No of valance electrons, B= Total bonding electrons, N= Total No of nonbonding electrons.

Hence formal charge on br atom in bro4- ion = 7-14/2-0=0.

Formal charge on each double bonded O atom in bro4- ion =6-4/2-4=0.

Formal charge on single bonded O atom in bro4- ion =6-2/2-6=-1.

Hence formal charge on central br atom is 0.Each double bonded O atom has 0 and single bonded O atom has -1 formal charge making the overall compound is negatively charged.

Bro4- Lewis Structure Angle

In bro4- br uses sp3 hybrid orbitals to form bro4- ion. The structure of bro4- is tetrahedral. As lone pair of electron is not present in bro4- ion the angle is exactly same as that of in real tetrahedral structure. The angle in bro4- ion is 109.28⁰ i.e. the o-br-o bond angle is 109.28⁰.

Bro4- Lewis structure Octet Rule

In the bro4- lewis structure we see that each O atom has 8 valance electrons and fulfill their octet. In bro4- ion br forms 3 br=O bonds and 1 br-O bond making a total of 14 electrons around central br atom.

As br is a congener of 4^th period element br atom can increase their octet more than 8 electrons due to presence of vacant d orbital. Hence according to octet rule bro4- is a stable compound.

Bro4- Lewis Structure Lone Pair

The valance electron which does not take part in bonding is defined as lone pair of electrons or nonbonding electrons.

The formula which is used to calculate the lone pair of electron on the given atom is given below:

No of lone pair of electrons = no of valance electrons present on the atom-no of covalent bonds formed by that atom.

In bro4- ion lone pair present on br atom= 7-7=0 i.e. zero lone pair of electrons.

Lone pair of electrons present on each double bonded O atom=6-2=4 i.e. 2 lone pair of electrons.

Lone pair of electrons present on single bonded O- ion= 8-2=6 i.e.3 nonbonding electron pairs.

These lone pairs are shown in the lewis structure of bro4- ion on the given atoms as electron dots.

Bro4- Valance Electrons

At first, to calculate the total valance electron in bro4-, it is important to know the electronic configuration of br atom and O atom. The electronic configuration of br atom is [Ar₁₈] 4s2 3d10 4p5 and from electronic configuration we see that there are 7 electrons in the valance shell of br atom.

The electronic configuration of O atom is [He₂] 2s2 2p4 i.e. 6 valance electrons present in O atom.1 negative charge is also present. The total valance electrons in bro4- ion will be equal to the sum of the valance electron of br atom and O atom+1 negative charge i.e. (7*1)+(6*4)+1=32. There are 32 valance electrons in bro4- ion.

Bro4- Hybridization

Hybridization is the process of mixing of similar energy atomic orbitals to produce an equal number of hybrid orbitals.

The ground state valance shell electronic configuration of br atom is 4s2 4p5. In the ground state of br atom only 1 unpaired electron is present and to make bro4-, 4 unpaired electron is required. In the excited state br send its 1 4s electrons and 2 4p electrons into vacant d orbital making a total of 7 unpaired electrons.

In the next step 4 o atoms give their 1 unpaired electron to form 4 br-o sigma bonds and 4 O atoms give their remaining unpaired electron to form 3 br=O (pi) bonds. In this compound br uses sp3 hybrid orbital to make br-O bonds. According to sp3 hybridization, the geometry of bro4- ion will be tetrahedral.

Bro4- solubility

Bro4- ion is soluble in polar solvents like water, ethanol, methanol etc. When Hbro4 losses 1 proton bro4- ion is formed i.e. bro4- ion is a conjugate base of Hbro4.

Hence, bro4- ion behaves as a base and has a strong tendency to accept proton. When it reacts with water, bro4- ion accepts 1 proton from water to form Hbro4 and Oh- ions making the aqueous medium alkaline.

Is BrO4- Ionic?

Bro4- is an ionic compound. This is because of the fact that it is formed when Hbro4 losses 1 proton. It is an anionic species.

Like ionic species, it has a strong tendency to react with water and also aq. solution of bro4- ion conducts electricity like other ionic compounds does. Like other ionic compounds it has high melting point. These facts suggest that bro4- ion is an ionic compound.

Is Bro4- acidic or basic?

Bro4- ion is a basic compound. It is the conjugate base of Hbro4 acid. Like other bases, it has a strong tendency to accept protons to form acid.

It also has high electron density on it like other bases and donates its electron density towards a proton or a lewis acid. Hence it act as a lewis base and forms adduct with lewis acid.

Is Bro4- polar or nonpolar?

Bro4- is nonpolar in nature. A compound is said to be nonpolar if its dipole moment is equal to zero. In this compound 4 br-O bonds are polar this is due to electronegativity difference between br and O atom.

As O is more electronegative than br atom, br-o bond moment lies towards o atom. As bro4- has real tetrahedral shape 4 br-o bond moments cancel each other and hence dipole moment becomes equals to 0.

By considering the above mentioned facts, bro4- ion is an ionic, covalent compound which has tetrahedral geometry. It is basic in nature and has a tendency to accept proton from any protonic solvent. Bro4- ion is not much stable due large size difference between Br and O atom.

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We are going discuss about beryllium fluoride,BeF₂ lewis structure, hybridisation, valence electrons and other detailed information in this article.

Beryllium fluoride,BeF₂ is an inorganic compound which looks like a white solid substance. Its structure is similiar to quartz and has some special optical properties.

How to draw BeF₂ Lewis structures ?

 The bond formation between two or more atoms can be easily understand by illustrating its Lewis structure. While sketching the Lewis structure of an atom only its valence electrons are considered. The valence electrons and bonds between the atoms are indicated by some dots and lines respectively. Structures depicted  by this way are called Lewis dot structure.

We can draw Lewis dot structures for both covalently bonded and ionic bonded compounds. Beryllium fluoride is an inorganic compound having one  beryllium and two fluorine atom. Beryllium is a second group alkaline earth metal and fluorine is from halogen family. We have to keep certain rules for drawing the Lewis structure of any compound. They are

• For drawing the Lewis structure first we need to calculate the entire number of valence electrons present in the given compound. It is done by adding the electrons present in the outer shell of each atom. In BeF₂, Be has 2 and fluorine has 7 outer electrons. So in total, there is 2+7×2 = 16 electrons.
• In BeF₂, there is one beryllium atom having two valence electrons and two fluorine atoms with seven valence electrons.

•  Beryllium atom shares two of its valence electrons to the two fluorine atom and hence they form two Be – F single bonds.

• So the Lewis structure of  beryllium fluoride, BeF2 is 

BeF₂ Resonance

The delocalisation of electrons linked with an atom is the cause of resonance. Due to this process a molecule or compound can have more than one structures. Such structures are called its resonating structure or resonance structure. This process can be seen in double bonded compounds and compounds with lone pair of electrons.

When we draw this structure the molecular formula of the compound shouldn’t change. Since there is no double bond present in between beryllium and fluorine there is no resonance structure for beryllium fluoride.

BeF₂  Shape

Beryllium fluoride is made by sharing of electrons between one beryllium atom and two fluorine atoms. Its shape is linear. A linear molecule is a molecule where the atoms are arranged along a straight line. Here the two fluorine atoms are arranged on both the sides of beryllium through a straight line pattern.

BeF₂ Formal charge

The charge allotted to an atom as a result of its bond formation with another atom is called formal charge. The equation for finding the formal charge of an atom is 

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

Formal charge of Beryllium in BeF₂ = 2 – 0- 2

                                                        = 0

Formal charge of fluorine in BeF₂ = 7 – 6- 1

                                                            = 0

So the formal charge of both the beryllium and fluorine in BeF₂ is 0.

BeF₂ Bond angle

When atoms combines to form stable compound, an angle is formed in between the bonds. The angle formed as result of bond formation between two or more atoms is called bond angle.

Beryllium fluoride is a linear shaped molecule. In a linear shaped molecule the atoms will be arranged in straight line. So the bond angle between the beryllium and fluorine atoms is 180⁰.

BeF₂ Octet rule

Octet rule states that, whenever atoms undergo combination to form stable compounds their outermost shell should be filled with eight electrons. In the case of covalent compound they share their electrons to obey octet rule. In ionic compound they will either lose or gain electrons to make their octet filled.

In the case of beryllium fluoride, beryllium has two electrons and fluorine has seven a electrons in its valence shell. When beryllium shares its two electrons with two fluorine atoms then fluorine got satisfied with octet rule. After bond formation between Be and F the fluorine atom has eight electrons in its outer shell. But beryllium contains only four electrons. Molecules like hydrogen, helium, lithium, beryllium don’t need eight electrons in their valence shell to get stabilised. So beryllium in BeF₂ is an exception to octet rule.

BeF₂ Lone pair of electrons

Some of the electrons present in the valence shell doesn’t participate in bond formation and they will stay with the atom. Those electrons are termed as lone pair of electrons or non bonding electrons.

In beryllium there is no lone pair of electron.

The lone pair of electrons present  in Fluorine atom is 3.

BeF₂ Valence electrons

The electrons connected with an atom which can only participates in bond construction is known as valence electrons.

In Be there is two valence electrons and Fluorine there is seven valence electrons. So in total there is 2+7×2 = 16 valence electrons in BeF₂.

BeF₂ Hybridisation

 Sometimes atomic orbitals with various energies combines to form new orbitals with same energy and shape. This is called hybridisation. Hybrid orbitals are the new orbitals formed by this way. The number of orbitals formed will be equal to the number of orbitals undergo hybridisation.

The electronic configuration of  Be in its ground state is 1s² 2s². In the next step one electron in 2s orbital will be excited to the 2p_x orbital. Then its electronic arrangement changes to 1s² 2s¹ 2p¹. After this the 2s and 2p_x orbital overlap together to form two sp orbitals with same energy. The angle between these two orbitals is 180⁰ and they are oriented in opposite direction.

Then two fluorine atom shares one electron from its 2p_z  orbital to beryllium. This results the formation of  BeF₂ bond. This results the formation two sigma or single bond  between beryllium and fluorine. So the hybridisation in beryllium fluoride is sp hybridisation.

The orbitals formed as result of Hybridisation has 50% s character and 50% p character. This can be also termed as diagonal hybridisation.

BeF₂ Solubility

The capability of the substance to get dissolved in a solvent is called solubility. The frequently used solvents are water, ethanol, acetone, chloroform, ether, CCl₄, benzene. Beryllium fluoride is found to be miscible in water and are sparingly soluble in ethanol.

 Is BeF₂  Ionic or not ?

 A positive charged and negative charged ion attracts together to form ionic bond. These positive and negative ions are cation and anion respectively. A covalent bond is formed by the common distribution of electrons between the atoms with same or different electronegativity value.

Beryllium fluoride is formed by the sharing of atoms between beryllium and fluorine. So BeF₂ is a covalent compound with linear shape.

Is BeF₂ Polar or not ?

BeF₂ is a molecule which exhibits Non polar character. Because the two Be – F bonds are symmetrical to each other their dipole moment got cancelled each other. So the net dipole moment is 0. Therefore Beryllium fluoride is Non polar molecule.

Is BeF₂ Acidic or Basic ?

BeF₂ is acidic in nature. Lewis acid is an acid which can accepts electrons from other atoms. Beryllium fluoride can be a good lewis acid because beryllium can accepts more electrons.

Summary

Beryllium fluoride is an inorganic compound with formula BeF2.It is a white solid which is used as precursor for the synthesis of beryllium. This article explains the lewis structure of  beryllium fluoride and its other properties like its hybridisation, solubility, acidic behaviour and its polar nature.

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Carbon tetrabromide (CBr4) has a central carbon (C) atom with 4 valence electrons, bonded to four bromine (Br) atoms, each contributing 7 valence electrons. The Lewis structure shows four single C-Br bonds, with 8 bonding electrons and no lone pairs on carbon. The molecule adopts a tetrahedral geometry with bond angles of about 109.5°. Despite the polar C-Br bonds due to electronegativity differences (C: 2.55, Br: 2.96), CBr4 is nonpolar overall due to its symmetrical structure. This symmetry influences its physical properties and chemical behavior.

Facts on CBr4                      

Molecular Name	Tetrabromomethane Carbon Tetrabromide Chemical FormulaCBr4Central atom of the lewis structureCarbonlone pairs present on the central atom 0Molecular Geometry of CBr4TetrahedralElectron Geometry of CBr4TetrahedralBond Angle Br – C – Br109.5 degreeNo. of valence electron for CBr4	32
The formal charge of CBr4 molecule	0
Solubility	Insoluble in water Soluble in ether,chloroform,C2H5OH
Acidic or basic nature	CBr4 is neither acidic nor basic

How to draw Lewis dot structure for CBr4?

Following are the steps to follow to draw the Lewis structure of CBr4 molecule

 Step 1: Count total valence electrons present in CBr4 molecule

First step is to find the no. of valence electrons present in CBr4 molecule.

Carbon belongs to group 14th and Bromine belongs to group 17th of the periodic table.

Valence electron of Carbon = 4

Valence electron of Bromine = 7

	Valence electrons	Atom In CBr4	Total Electrons
C	4	1	4*1= 4
Br	7	4	7*4=28
			32

Step 2: Find least electronegative element in CBr4

Electronegativity increases in a period from left to right so Carbon is least electronegative than Bromine. Keep the least electronegative atom in the centre.

Now draw the skeletal structure of CBr4 molecule

Step 3: Put two electrons or a bond between C and Br atom

Step 4: Complete octet of the Outer atoms

Main group elements have tendency to attain octet configuration of their nearest noble gas element present in the 18 group. This is known as Octet Rule. Except hydrogen which completes duplet configuration like He

Complete the octet on outside atoms then move on to central atom

Step 5: Complete octet of central atom or make covalent bonds if necessary

There is no need of this step for CBr4 as the octet of central atom is already complete.

                         

                                                 

Step 6: Check formal charge value

Before we confirm that this is a perfect Lewis structure, we need to check the formal charge values

Formal charge = Valence electrons – (1/2) * bonding electrons – non-          bonding electrons

Valence electrons of Carbon = 4

Non-bonding electrons of carbon = 0

Bonding electrons of carbon = 8 (4 pairs)

Formal charge for carbon atom = 4 – 1/2*8 – 0 = 0

Valence electrons of Bromine = 7

Non-bonding electrons of Bromine = 6 (3 lone pairs)

Bonding electrons of Bromine = 2

Formal charge for Bromine atom = 7 – 1/2*2 – 6 = 0

As the C and Br elements have least possible formal charges, we have obtained suitable Lewis structure

                           

What is the formal charge in CBr4 and how it is calculated?

We can calculate formal charge by using the formula –

Formal charge = Valence electrons – (1/2) * bonding electrons – non-          bonding electrons

Valence electrons of Carbon = 4

Non-bonding electrons of Carbon = 0

Bonding electrons of carbon = 8 (4 pairs)

Formal charge for Carbon atom = 4 – 1/2*8 – 0 = 0

Valence electrons of Bromine = 7

Non-bonding electrons of Bromine = 6 (3 lone pairs)

Bonding electrons of fluorine = 2

Formal charge for Bromine atom =7 – 1/2*2 – 6 = 0

Formal charge on carbon and bromine atom in CBr4 Lewis dot structure is zero.

Does CBr4 molecule follow the octet rule?

CBr4 contains 32 valence electrons and all the atoms in CBr4 complete their octet as can be seen from the Lewis structure of CBr4 molecule. This proves that octet rule is followed by the CBr4 molecule.

How to find the molecular shape and electron geometry of CBr4 molecule?

In order to find the geometry (molecular/electron) of OF2 molecule, the three steps have to be followed. They are –

1)Count the lone pairs present on the central atom in the CBr4 Lewis structure

Or

Number of lone pairs can also be found by using the formula

Lone Pair =1/2*(V.E. –N.A.)

V.E.= valence electron on the central atom

N.A.= Number of atoms which are attached to the central atom

In CBr4 molecule, the valence electrons of central Carbon atom are 4 and four outer atoms are attached to it.

Lone Pairs = 1/2* (4 – 4) = 0

2) Find the hybridization number of CBr4 molecule

Hybridization of central atom can be found out by using the formula.

Hybridization number = N.A. + L.P

Where-

N.A.- is the number of atoms attached to the central atom

L.P. – is the number of lone pairs on the central atom

There are 4 atoms attached to the Carbon with no lone pairs present on it.

Hybridization number = 4 + 0 = 4

Hybridization number of CBr4 molecule is 4

So, hybridization of CBr4 molecule is Sp3

3) Use VSEPR Theory to determine CBr4 molecular/electron geometry

We have determined hybridization of CBr4 as SP3 and no lone pairs present on the central atom.

Now according to AXnEx notation of VSEPR theory we are going to find VSEPR notation for CBr4 molecule

AXnEx notation

Where-

A – is the central atom

X – is the number of atoms attached to the central atom

E – is the number of lone pairs of electrons on the central atom

According to the Lewis dot structure of Carbon Tetrabromide, central atom is Carbon which has 4 fluorine atoms are connected to it and no lone pairs present on it.

So CBr4 formula becomes AX4

According to VSEPR chart, the molecule with AX4 formula has molecular shape as tetrahedral and electron geometry tetrahedral.

Total Domains	General Formula	Bonded atoms	Lone Pairs	Molecular Shape	Electron Geometry
1	AX	1	0	Linear	Linear
2	AX2	2	0	Linear	Linear
	AXE	1	1	Linear	Linear
3	AX3	3	0	Trigonal Planar	Trigonal Planar
	AX2E	2	1	Bent	Trigonal Planar
	AXE2	1	2	Linear	Trigonal Planar
4	AX4	4	0	Tetrahedral	Tetrahedral
	AX3E	3	1	Trigonal Pyramid	Tetrahedral
	AX2E2	2	2	Bent	Tetrahedral
	AXE3	1	3	Linear	Tetrahedral

VSEPR CHART

                       

Is CBr4 molecule polar or non-polar?

CBr4 is a non-polar molecule is confirmed by three factors –

1)Electronegativity:

Bromine (electronegativity 2.96) is more electronegative than Carbon (electronegativity 2.55) Being more electronegative than Carbon, Bromine attracts electrons towards it more strongly.

The molecule is polar when the difference in electronegativity between the atoms in the molecule is greater than 0.4

The electronegativity difference between Carbon and Bromine is 0.41

2)Geometrical/Molecular Shape: 

Geometrical Structure of CBr4 molecule is tetrahedral.

The four dipoles of four C-Br bond are in opposite direction. Now, due to the tetrahedral geometry (which is symmetrical) all the dipoles get cancelled by each other.

3)Dipole Moment:

Due to the symmetric geometry of the CBr4 (tetrahedral) all the 4 dipoles get cancelled by each other resulting in overall 0 dipole moment for CBr4.

All these factors show that CBr4 is a non-polar molecule.

What is the Hybridisation for CBr4 molecule?

The central atom carbon atom shares four electrons with four Bromine atoms. Hence in the Lewis structure there is a presence of four bonding pairs of electrons on the carbon atom in Lewis structure of CBr4 molecule

To share the electrons with the Bromine atoms, the orbitals of Carbon atom undergo hybridization to accommodate the electrons.

The electronic configuration of Carbon and Bromine in ground state is –

Carbon in ground state 1s2 2s2 2p2

Bromine in ground state 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

Electronic configuration of Carbon after gaining four electrons to fulfil the octet by forming bonds with Bromine-

Carbon 1S2 2S2 2Px2 2Py2 2Pz2

Steric Number = Number of atoms bonded to central atom + Number of lone pairs of electrons attached to central atom

Steric Number = 4 + 0 = 4

So, hybridization for the central atom oxygen in CBr4 is Sp3

Does CBr4 molecule shows resonance?                                      

A molecule shows resonance when –

• The molecule has alternate double and single bonds.
• The molecule has presence of lone pair in conjugation with the double bond.

Carbon Tetrafluoride does not have a double bond so CBr4 does not show resonance.

Is CBr4 ionic or a covalent compound?

CBr4 is a covalent compound as the bond between Carbon and Bromine is formed by sharing of electrons.

Conclusion:

To summarize what we have discussed in this article –

The hybridisation of CBr4 molecule is Sp3. Both the molecular geometry and electron geometry of CBr4 is tetrahedral. The bond angle Br-C- Br is 109.5 degrees. The total valence electrons present in CBr4 molecule is 32.

.

                    

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CCl₂H₂ Lewis structure, and other important facts are going to be discussed in this article.

Dichloromethane, CCl₂H₂ is an organo chlorine compound. It is a colorless liquid which is volatile in nature and has chloroform like sweet smell. It can be used as a good solvent.

How to draw Lewis structure of  Dichloromethane, CCl₂H₂ ?

Atoms join together to form a stable bond by sharing their electrons. This process can be easily understand by drawing certain simple structures. These structures are called Lewis structure. Generally dots and lines are used to denote electrons and bonds in the Lewis structure.

So the structures designed on the basis of this is called Lewis dot structures.
Before drawing the Lewis structure of dichloromethane we need to understand which of the atoms are present here and their valence electrons.

• In dichloromethane there is one carbon atom attached with two hydrogen and chlorine.  Now let’s see the valence electrons in dichloromethane. Carbon contains four electrons, hydrogen has one and chlorine has seven electrons in their outer shell. So the total number is 4+1×2+7×2= 20 electrons.
• In the second step we draw the symbol of carbon atom surrounded with chlorine and hydrogen atoms. Their valence electrons are also indicated here.

• In the third step we show how they share their electrons each other to form the stable bond.

Dichloromethane, CCl₂H₂  Resonance

When atoms are linked with double bonds and lone pair of electrons, the electrons has a tendency to move across the bonds. This movement cause different structures for one molecule. This process is called resonance and structures are resonating structures.

It is important to maintain the structure of molecule as it is during the movement of electrons. In case of dichloromethane there is no double bond. The lone pair of electrons linked with chlorine atom doesn’t play a role for the making of resonance structure. So there is no resonating structure for dichloromethane.

Dichloromethane, CCl₂H₂  Shape

When two hydrogen atoms of methane got substituted by chlorine, then forms a compound called dichloromethane. The structure of dichloromethane is found to be tetrahedral. It is due to sp³ hybridization.

Dichloromethane, CCl₂H₂   Formal charge

The charge assigned to an atom due its  bond making with other atoms termed as formal charge. There is one equation for finding formal charge. It is

Formal charge =( valence electrons – No. of dots – No. of bonds)
The formal charge of four atoms in dichloromethane is

For carbon = (4-0-4) = 0
For chlorine = (7-6-1) = 0
For hydrogen = (1-0-1) = 0

Hence we understood that the formal charge assigned to dichloromethane is zero.

Dichloromethane, CCl₂H₂   Angle

The bond angle of dichloromethane is 109.5. There is two carbon – chlorine joined and carbon – hydrogen joined bonds are present in dichloromethane. The atoms attached to the central carbon are located on the corners of a tetrahedron.

Dichloromethane, CCl₂H₂   Octet Rule

When there is eight electrons are present in the outermost shell of an atom after bond formation then it is said to be stable. This rule can be called as octet rule. Here carbon and chlorine has eight electrons in the valence shell after bond making. So they fulfill octet rule.

But hydrogen has only two electrons. Certain atoms need not be filled with eight to exist as stable compound. Hydrogen needs only two electrons to remain stable and it is obtained after bond making. So it is stable but don’t obey octet rule due to the absence of eight electrons in its outer shell.

Dichloromethane, CCl₂H₂  Lone pair of electrons

Sometimes the whole valence electrons doesn’t involve in bond making. So those electrons that has no role in bond making process are called lone pair electron.

There is zero lone pair seen in hydrogen and carbon atom of dichlormethane  but we can see 3 lone pair in the chlorine atom. So in total there is six lone pairs are found in dichloromethane.

Dichloromethane, CCl₂H₂   Hybridisation

Atomic orbitals with different energy combines to form new set of orbitals with indifferent energy it is termed as hybridization. The new set formed will be equal to the orbitals got united. The speciality of the new orbitals are its identical shape and energy.

Let’s start with the electronic configuration of carbon first because it is the central atom.
Carbon_{( ground state)}  1s² 2s² 2p²

In the next step what happens is the excitation of one electron from 2s to 2p level. Then

Carbon _{( excited state)} 1s² 2s¹ 2p³

So these three orbitals that is one 2s and three 2p undergo hybridization to make four sp3 hybrid orbitals. At last the two hydrogen and chlorine atoms distributes their electrons to the central located carbon atom to form dichloromethane. The shape of dichloromethane thus made is tetrahedral with angle 109.5⁰. All the bonds are single bonds and are stable.

Dichloromethane, CCl₂H₂   Solubility

The capacity of a substance to be dissolved in a given solvent is its solubility. The solubility ability of compounds will be different. Some will be easily soluble in all solvents but some will not. Usually we use water, ethanol, acetone, ether as solvents.
Dichloromethane is not much soluble in water. It can be made water soluble by decreasing temperature of the system. When temperature is 60 then 5.2 g/L get dissolved, at 60 15.8g/L dissolves. But we found out that dichloromethane is soluble in organic solvents like ethyl acetate, ethanol, hexane, benzene,CCl4, ether, chloroform, phenol, aldehydes and ketones.

 Is Dichloromethane, CCl₂H₂   Ionic or Covalent ?

There are two types of bond, ionic and covalent. First one forms due to attraction between two oppositely charged ions. Latter is because of the mutual distribution of electrons between the atoms.

In dichloromethane there is zero charged ions. All atoms existing here shares their electrons each other to form the compound they want. So they made a covalent bond. So dichloromethane is not at all ionic.

Is Dichloromethane, CCl₂H₂   Acidic or not ?

Dichloromethane is found to be acidic. It acts a good Lewis acid. A Lewis acid has vaccant orbitals to accept electrons. This compound accepts electrons from other bases. So it is a Lewis acid like substance.

Is Dichloromethane, CCl₂H₂   polar or not ?

We all know that dichloromethane has one central carbon joined with two chlorine and hydrogen atoms. Here two carbon- chlorine and carbon- hydrogen bonds can be seen. Chlorine atom present here is electronegative in nature. It’s electronegativity is much more than that of carbon and hydrogen.

So there arises a dipole moment difference between the bonds made here. This is almost equal to 1.6 D. So it’s dipole moment value is not zero. This indicates that dichloromethane is found to be a polar molecule.

Summary

Dichloromethane is a organo chlorine compound. Its molecular weight is 84.93g/mol with refractive index 1.42. It is found in wetlands and emitted into atmosphere due to automobile emissions. It is used as a good solvent.

This article describes that dichlormethane is a covalently bonded molecule with polar behaviour which undergo sp³ hybridisation. It acts like a lewis acid and its valence electrons are also mentioned here.

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BeH₂ or berilium hydride is a linear compound with a bond angle 180⁰. The appearance of this compound is a white orthorhombic crystalline solid. The shape of the crystal is hexagonal with a very much high density 0.78 g.cm^-3. In this compound, beryllium is attached with the two hydrogen atoms with two covalent bonds.

BeH₂ (Beryllium hydride) features a linear Lewis structure: a central beryllium (Be) atom with 2 valence electrons forms single bonds with two hydrogen (H) atoms, each contributing 1 valence electron. The molecule uses 4 valence electrons total. BeH₂ has no lone pairs on the Be atom, resulting in a 180° bond angle. Electronegativity values: Be (1.57), H (2.20), suggesting polar covalent bonds. However, the molecule’s linear geometry leads to an overall nonpolar structure.

Let’s focus on the following topics described below.

How to draw BeH₂ lewis structure?

Lewis structure is nothing but a structural representation of any molecule with the nonbonding electrons around the respective atoms. The steps of drawing this structure are explained below-

1. Finding out the valance electrons: In BeH₂, Be is a s-block element and it has two valance electrons in its 2s orbital. Hydrogen has only one electron in its 1s orbital and this is the only outer most shell electron of hydrogen.
2. Determination of bonds and bonding electrons: Total two covalent bonds are present between Be and two hydrogen atoms in BeH₂ molecule. Thus, the number of bonding electrons are 2×2=4.
3. Finding out the nonbonding electrons: In BeH₂, all the valance electrons of Be are used up in bonding with hydrogen. So, no electrons are left as nonbonding electron pairs.

BeH₂ Lewis Structure Shape

The hybridization of the central atom plays the most important role to predict the structure or shape of any molecule. Besides that, the repulsive factor involving lone pairs and bond pairs. These repulsions are known as-

1. Lone pair- lone pair repulsion
2. bond pair-bond pair repulsion
3. lone pair-bond pair repulsion

The increasing order of the above repulsive factor is-

bond pair -bond pair repulsion < Lone pair – bond pair repulsion < Lone pair- lone pair repulsion.

BeH₂ is one of the most simplest molecule in which no lone pairs are present on central atom, Be. Be has two electrons in its outer most shell which are totally used up to form the two covalent bonds with two hydrogen atoms. Thus, the above repulsive factors become insignificant to determine the structure. Due to absence of any repulsions BeH₂ shows its actual geometrical structure and actual bond angle.

In this molecule, beryllium is sp hybridized with two bond pairs. The geometry of this molecule is linear with a bond angle 180⁰.

BeH₂ Lewis Structure Formal Charge

Formal charge is the theoretical charge on each of the atom of any molecule and it is assumed that electrons are shared between all the atoms irrespective pf electronegativity.

• Formal charge = Total number of valance electrons – number of electrons remain as nonbonded – (number of electrons involved in bond formation/2)
• Formal charge on beryllium, Be = 2 – 0 – (4/2) = 0
• Formal charge on each of the hydrogen atom, H = 1 – 0 – (2/2) = 0

Formal charge of each of the atom in BeH₂ molecule is zero. Thus, it is a neutral molecule with no charge.

BeH₂ Lewis Structure Angle

Structure angle is basically the angle between two bonds. Hybridization of central atom also determines the bond angle of any molecule. In some times lone pairs – lone pair repulsion and lone pair-bond pair repulsion also have impact on determining the molecular structure.

In this BeH₂ molecule, beryllium is sp hybridized and does not have any remaining electrons as nonbonded. Thus, the molecule shows its actual bond angle. Sp hybridization of central atom directs the bond angle to be 180⁰ and structure to be linear shaped.

Two Be-H bonds are aligned with the angle 180⁰ with each other keeping maximum distance between them.

BeH₂ Lewis Structure Octet Rule

Octet rule is one of the most significant rule in chemistry. It states that any molecule should contain eight valance electrons in their respective valance shell to achieve the nearest noble gas like electron configuration.

Octet rule is violated in BeH₂. Since beryllium has only two electrons in its valance shell, 2s orbital. After bonding two hydrogen atoms it gains two more electrons. But eight electrons of octet rule can’t be achieved by beryllium. Thus, it can’t have the electron configuration like its nearest noble gas of periodic table neon, Ne (2s2 2p6).

BeH₂ Lewis structure Lone Pairs

Valance electrons of any atom are basically two types-

1. Electrons involved in bonding (bonding electrons)
2. Nonbonding electrons or lone pair.

Those valance electrons do not participate in bond formation are defined as nonbonding electrons or lone pairs.

• Nonbonded electron = Total number of valance electron – number of bonded electrons.
• Nonbonding electrons on Be = 2 – 2 = 0
• Nonbonding electrons on each of the H atom = 1 – 1 = 0

Thus, BeH₂ has no lone pairs or nonbonding electrons in its structure.

BeH₂ Valence Electrons

Valance electrons are defined as the outer most shell electrons. These electrons are most loosely bound to the nucleus. So, nuclear attraction force on these electrons is minimum with respect to the inner shell electrons.

In most of the cases valance electrons are most reactive and they participate in different chemical reactions due to the least attraction force of nucleus on them.

Be has total 4 electrons in this manner, 1s² 2s². So, the number of valance electrons of Be are 2 (2s is the valance shell) and 1 for hydrogen (1s¹). These two electrons of Be and one electron of hydrogen are involved in two covalent bond formation. Thus, total number of valance electrons in BeH₂ are = {2+(2×1)} = 4

BeH₂ Hybridization

Hybridization is nothing but the mixing of two atomic orbitals to generate a new orbital. It is the most important parameter of determining the molecular shape. How can we detect the molecular shape from hybridization is shown in the following table.

Hybridization of central atom	Structure
sp	Linear
sp2	Trigonal planar
sp3	Tetrahedral
sp3d	Trigonal bipyramidal
sp3d2	Octahedral

From the above picture it is clear that Be is sp hybridized in this molecule. Two valance electrons of Be and one valance electron of each of the hydrogen are responsible for this sp hybridization. On s and one p orbital participate to form the mixing sp orbital in BeH₂ molecule.

The % contribution of both the s and p orbital is 50 in sp hybridization.

BeH₂ Solubility

BeH2 or beryllium hydride is an alkaline earth hydride which is insoluble in solvents that do not decompose this compound.

It decomposes in water and that is why it is soluble in water but it has no solubility in diethyl ether and toluene.

Is BeH₂ ionic?

No, BeH₂ is a covalent compound due to having two covalent Be-H bonds. It is not an ionic compound because-

• Both the participating atom, Be and H are nonmetal.
• The bonding electrons are shared between two beryllium and hydrogen, not entirely transferred from one atom to another atom.
• Melting point is also not so high, 250⁰ C or 523K.

Is BeH₂ polar or nonpolar?

Polarity of any molecule depends upon the two following parameters-

1. Bond moment of each bond present in the molecule
2. Orientation of the bond connecting central atom and substituent atoms.

In BeH₂, both the Be-H bonds are polar due to having electronegativity difference between Be and H. But these two bonds are aligned with an angle 180⁰.

Due to having this anti-parallel structure one bond moment is cancelled out by the another and the dipole moment becomes zero. Thus, BeH₂ is a nonpolar molecule.

Is BeH₂ acidic or basic?

BeH₂ is basically a lewis acid. Lewis acids are those molecule which can accept the electron pairs in their vacant orbital.

Be is an electron deficient atom because it has vacant 2p orbital which can easily accommodate electron pairs from any electron rich compounds or base. Thus, it acts like a lewis acid and show acidic properties.

Conclusion

Different facts of structure and bond angle with some explanations are explained through this article. We have come to know that BeH₂ is a linear crystalline water soluble compound with zero dipole moment.

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This article illustrates bebr2 complete information like bebr2 Lewis structure, characteristics, and other vital properties.

Beryllium bromide has the chemical formula Bebr2 are hygroscopic compound. The chemical Bebr2 is soluble in water and is used in nuclear reactors, x-ray lithography, computer parts, and as a catalyst.

The earth’s crust naturally contains beryllium, a rare element. On the other hand, bromine does not form by itself but can sometimes be found as crystallized mineral halide salts.

How to draw Bebr2 lewis structure?

Lewis Structure is the dot representation of electrons and shows how the bond formation takes place. In this different atoms with their valence electrons participate in chemical reaction or bond formation to create new molecules.

The atomic number of Beryllium is 4.

Electronic configuration of Be = 1s²,2s²

Valence electron in Be = 2

The atomic number of Bromine is 35.

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

Valence electron in Br =7

Bebr2 lewis structure resonance

When metal and nonmetal combine to form an ionic compound, the result is beryllium, which is a metal, and Bromine, which is a nonmetal.

The BeBr2 molecule has a different electronegativity from beryllium and bromine, meaning it has no dipole moment. Because of the equal charge distribution of negative and positive charges, its structure is similar to that of a carbon monoxide molecule.

Bebr2 lewis structure shape

The Lewis structure of beryllium clearly shows that it is a triatomic molecule. The participating atom in that molecule has a linear geometry and a 180° angle.

Beryllium is a less electronegative element than bromine. It is a tetrahedral polymer. Thus Be halides are not ionic they are covalent due to the high polarising power of Be+2, therefore its structure is shown above.

Bebr2 lewis structure formal charge

The formal charge is defined as the charge occupied by an atom that shares the electrons mutually and equally.

Formal Charge = Valence electron – Non bonding Valence electron – Bonding electron/2

Formal Charge = 2 – 0 – 4/2

                    Be = 0

Formal Charge = 7- 6 – 2/2

                     Br = 0

Thus the formal charge on the Bebr2 lewis structure is zero.

Bebr2 lewis structure angle 

Bebr2 has linear geometry and an angle of 180°. In the Bebr2 lewis, the structure beryllium is in the center and surrounded by two bromine atoms.

Bebr2 lewis structure octet rule

An atom’s outermost shell has eight electrons according to the octet rule. Beryllium only needs four electrons to complete its octet and become exceptional, whereas Bromine has seven valence electrons that can follow the octet rule but gain electrons from Be to form a stable electronic configuration.

Be Group 2 has two valence electrons. It is found in the periodic table of elements. Be is an exception because it does not adhere to the octet rule and instead expands its shell to accommodate more electrons.

Bebr2 lewis structure lone pairs

There are no lone pair electrons in the BeBr2 molecule’s center beryllium. Bebr2 lewis’s structure consists of two single bonds with beryllium atoms attached with two bromine atoms.

The center atom Be does have not lone pairs, it consists of two valence electrons.

Bebr2 valence electrons

An atom’s outermost electrons are known as valence electrons. Beryllium does not obey the octet rule, which states that all elements in the periodic table should have the same number of electrons.

This is because it only has two valence electrons, and this makes it less prone to breaking up as it undergoes chemical reactions.

Be= 2 valence electrons

2 Br = 7*2 valence electrons

Bebr2 hybridization

When one S orbital and one p orbital combine, a molecular orbital is formed which is called Sp Hybridization. During excitation, one valence electron shifts to the 2p shell from the 2s shell of beryllium. Sp hybridization produces equal parts s and p.

A sigma bond is formed when the fifth electrons of the second bromine atom bond to the left electron of the beryllium atom. The single covalent bond contains only a sigma bond and no pi bond.

Bebr2 solubility

Bebr2 are highly water-soluble molecules. Bebr2 is a molecule with a low pH value that is hygroscopic.

A cation should have the smallest size and an anion should have the largest size according to Fajan’s rule.

Is Bebr2 ionic?

No, Bebr2 is not ionic it is covalent molecules.

Ionic compounds are those which are made by the attraction of positive and negative charges and by only the transfer of electrons from one atom to the other.

Reason:

Be has two valence electrons and Br has seven. If we look at the periodic table, we can see that Be belongs to group 2 (Metal) and Br belongs to group 17 (Non-metal). Because metal and non-metal have different electronegativity, they may form an ionic bond. However, the electronegativity difference between these two is 1.39, indicating a polar covalent bond rather than an ionic bond.

It adheres to Fajan’s rule, which states that a molecule should be covalent when there is a large difference in the size of its cations or anions.

Because Be+2 has a smaller cation size and Br-1 has a larger anion size, Bebr2 is covalent.

Is Bebr2 polar or nonpolar?

The behavior of an atom that attracts a shared pair of valence electrons is known as polarity.

This is a nonpolar molecule because there is no dipole cloud on the beryllium bromide molecule. Separation of charge occurs in polar molecules, resulting in two distinct positive and negative ends.

When unequal charge separation occurs among the participating atoms, the dipole moment is formed. The bond formation will occur at the end that is experiencing the greatest effect of the dipole cloud. According to this description, beryllium bromide is nonpolar because the involved atoms have symmetrical charge distribution.

Is Bebr2 acidic or basic?

Bebr2 is hygroscopic and slightly acidic.

Beryllium bromide exhibits an anomaly in that it does not follow the octet rule. It cannot accommodate eight valence electrons due to its small structure and a limited number of shells. The molecular geometry is linear because all of the molecules involved are arranged in a straight line.

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This article should learn about BeI2 lewis structure, shape, bond angle, hybridization, and many more detailed fact.

In the BeI2 lewis structure, the shape of the molecule is linear having sp hybridization. The molecule is linearly shaped and two iodine each contain three pairs of lone pairs. As it is a linear molecule so the bond angle of I-Be-I is 180⁰.

BeI2 is a halogenated salt of alkaline earth metal. Be is alkaline earth metal and can form a strong base with respective anions. The charge over Be is +2 and it is fully satisfied by two iodide anions.

Some important facts about BeI2

BeI2 is solid in its physical state and the color is white. The molecule is hygroscopic which means it can hold the water molecule by absorbing it.

The molecule’s melting point and boiling points are 753 K and 863 K, respectively. In the lattice crystal structure, the BeI2 is orthorhombic.

In presence of elemental Iodine, BeI2 is formed and reacted with Be metal at 500-700⁰C temperature.

Be + I₂ =BeI₂

1.    How to draw BeI2 lewis structure?

Before proceeding with the lewis structure drawing we should know lewis structure or lewis dot structure can briefly describe the electrons involved in a molecule for bond formation.

First, we taking consideration of valence electron of Be as well as I. Here Be is a lack of two electrons where two I contain one more electron in their valence shell. Identify the central atom by the electropositivity so here Be is the central atom as Iodine is more electronegative.

The molecule is neutral so the charge over Be and I are fully satisfied by the bond formation so no need to add or remove electrons then three atoms are attached by a single bond only. After that, the lone pairs are assigned to the respective atoms that in over Iodines only.

2.    BeI2 lewis structure shape

In the BeI2 lewis structure, the whole electron density of the molecule lies on the central Be atom.

The structure is linear and Be atom is present at the central position where two iodines are at the terminal site. Lone pairs are present on the Iodines atoms only

3.    BeI2 valence electrons

From the BeI2 lewis structure, it is shown that the linear molecule is attached by a single bond only.

The ground state electronic configuration of Be is 1s²2s² and in the excited state i.e. for Be²⁺ the electronic configuration will be 1s², so valence electrons will be two. Again, for I the ground state electronic configuration is [Kr]4d¹⁰5s²5p⁵ so the valence electrons will be 7 as 5s and 5p are the valence shell for each I.

So, the total number of valence electrons in BeI2 is (7*2)+2 =16

4.    BeI2 lewis structure formal charge

The formal charge is a hypothetical concept accounting for the same electronegativity for all atoms.

The common formula for calculation of formal charge is, F.C. = N_v – N_l.p. -1/2 N_b.p.

Where N_v is the number of electrons in the valence shell, N_l.p is the number of electrons in the lone pair, and N_b.p  is the total number of electrons that are involved in the bond formation only.

Here in the BeI2 lewis structure, we calculate formal charge separately for Be as well as I.

Formal charge over Be is =2-0-4/2 = 0

Formal charge over I =7-6-2/2 =0

So, the overall molecule is neutral and it is also reflected in the formal charge.

5.      BeI2 lewis structure lone pairs

The lone pairs are those electrons that are not involved in the bond formation.

From the above BeI2 lewis structure we can see that the lone pairs are only over the I only. So, we add the total number of lone pairs in two I atoms, each I contains 3 pairs of lone pair because the valence electrons for I is 7 and one electron from that participate in bond formation. So, the remaining 6 electrons exist as 3 pairs of lone pairs and Be is lack of lone pair.

So total number of lone pairs in BeI2 is 6+6=12

6.    BeI2 lewis structure octet rule

The octet rule is for every atom is complete its valence shell by accepting or donating a respective number of electrons and trying to gain the nearest noble gas configuration.

In the BeI2 lewis structure, central Be is from the s block and I is from the P block element. Be is an II element whereas Iodine is a VIIA element which means Be has two electrons in its outermost shell and I have & electrons. Be already gain stability due to s orbital filled (s orbital contains maximum electrons) but for I short of one electron to complete its octet, so it shares one electron from Be and completes its octet.

7.    BeI2 lewis structure bond angle

A bond angle is a specific angle between atoms in a particular molecule.

From VSEPR(Valence Shell Electrons Pair Repulsion) theory we can say that in the BeI2 lewis structure the bond angle I-Be-I is 180⁰ that its shape is linear. There is no violation of that bond angle in this molecule due to the large size of I the lone pair lone pairs repulsion is minimized here. So BeI2 shows an ideal linear shape angle that is 180⁰.

8.    BeI2 lewis structure resonance

Resonance is a hypothetical concept that can describe the transfer of electron cloud in the same molecule but a different skeleton.

From the BeI2 lewis structure different skeleton forms, the stable is III as it contains more covalent bonds. After that, we consider the charge distribution of the atom, that if an electronegative atom gets a negative charge or an electropositive atom gets a positive charge is more stable than the reverse.

9.      BeI2 hybridization

Hybridization is also a hypothetical concept to determine the mode of bonding of a covalent molecule by mixing orbitals of two or more atoms to get hybrid orbitals.

The hybridization of any molecule is calculated by the formula

H = 0.5(V+M-C+A), where H= hybridization value, V is the number of valence electrons in the central atom, M = monovalent atoms surrounded, C=no. of cation, A=no. of the anion.

So here in the BeI2 lewis structure, the central Be atom has two valence electrons in its s orbital and two I atoms are present at the terminal position.

So, the hybridization of BeI2 is = ½ (2+2+0+0) =2 (sp)

Structure	Hybridization value	state of hybridization of central atom	Bond angle
Linear	2	sp /sd / pd	1800
Planner trigonal	3	sp2	1200
Tetrahedral	4	sd3/ sp3	109.50
Trigonal bipyramidal	5	sp3d/dsp3	900 (axial), 1200(equatorial)
Octahedral	6	sp3d2/ d2sp3	900
Pentagonal bipyramidal	7	sp3d3/d3sp3	900,720

From the above table, it is shown that if the hybridization value is 2 then the mode of hybridization is sp. So BeI2 is sp hybridized. Where S orbital of central Be and P orbital of two Iodine are mixing together to give a new sp hybrid orbital.

10.    BeI2 solubility

Solubility is the phenomenon to which extent a molecule will be soluble in a given solution.

BeI2 reacts with a water molecule to give a new compound. As it is a covalent molecule so its solubility in water is very poor. But it has a greater solubility in methanol and even carbon disulfide also.

11.    Is BeI2 ionic?

According to Fajan’s rule and ionic potential, we can say that no molecule is 100% ionic or covalent.

The size of Be2+ is small so it can easily polarize the larger anion like Iodide. Iodide is larger so it can be easily polarizable by Be2+ ion. So, the molecule possesses an ionic character along with its covalent nature. Be2+ has higher ionic potential as its size is small and charge density is also high so BeI2 shows ionic character.

13.    Is BeI2 polar or nonpolar?

If a molecule has some resultant dipole-moment then it is polar otherwise nonpolar.

From the above BeI2 lewis structure, we can see that there are two dipole-moment acts opposite to each other. So, the dipole moment of this molecule is zero. So BeI2 is nonpolar. The direction of the dipole-moment always acts from a more electropositive atom toward electronegative an atom.

Here Iodine is more electronegative and Be is electropositive so the dipole-moment acts from Be to I site. As the structure is linear so the direction of the two dipole-moment is opposite and cancels out each other to make the molecule nonpolar.

13.    Is BeI2 acidic or basic?

BeI2 itself is a neutral complex but it when reacts with water the solution turns acidic.

In BeI2 lewis structure, central Be is sp hybridized with vacant 2p orbital and the lone pairs of oxygen in water molecule can be attacked there and it can accept the electron and a strong acid hydrogen Iodide is formed.

BeI2 + 2H2O = Be(OH)2 + 2HI

So, it behaves as acidic in water solution, but in molecular form, there are two electronegative atoms I present, and the electronegativity of two halogens the accessibility of vacant p orbital will be increased.

Conclusion

From the above discussion of the BeI2 lewis structure we can conclude that the molecule has 16 valence electrons, sp hybridized, linear structure along with bond angle 180 degree, and six pairs of lone pair.

Be is not a complete octet but it is still stable due to zero formal charge and has a filled s orbital. Although it is neutral in an aqueous solution it can produce acid and has zero dipole moment making the molecule non-polar.

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In the BF3 Lewis structure, the shape of the molecule is planar trigonal having a bond angle of 120⁰. The central B atom is sp² hybridized. Three F atoms are present at the three corners of the trigonal moiety. Due to having a vacant site in B it can accept electrons or lone pairs and behaves as lewis acid.

Three F atoms and B are present in the same plane. The molecule is nonpolar due to zero dipole moment. The B-F bond length is near around 130 pm. It is isoelectronic with carbonate anion.

How to draw the BF3 Lewis structure

To accurately depict the Lewis structure for BF3 (Boron Trifluoride) follow the below steps:

Valence Electrons Calculation: For BF3, the total count of valence electrons is 24. This is calculated from Boron’s 3 valence electrons plus 21 from the three Fluorine atoms (each contributing 7 electrons).

Creating the Skeleton Structure: Boron, having the lower electronegativity compared to Fluorine, is placed in the center. Single bonds are drawn from Boron to each of the three Fluorine atoms. This step utilizes 6 out of the 24 valence electrons (2 electrons for each of the 3 bonds).

Completing the Octets for Fluorine: The next step involves distributing the remaining 18 electrons (24 total – 6 already used) to fill the octets of the Fluorine atoms. Each Fluorine atom receives 6 additional electrons to complete its octet, fully allocating the 24 valence electrons.

Examining Boron’s Electron Configuration: In this final structure, Boron is surrounded by 6 electrons, which come from its bonds with the Fluorine atoms. Boron does not achieve an octet, which is notable and acceptable for BF3. This configuration is stable for Boron and is an exception to the octet rule.

The Lewis structure for BF3 thus features a central Boron atom bonded to three Fluorine atoms, with each Fluorine atom satisfying the octet rule. Boron, however, does not fulfill the octet rule, having only six electrons in its valence shell. This is a characteristic trait of BF3 and reflects Boron’s ability to be stable in compounds even without completing an octet. This structure highlights the unique electronic configuration of BF3, demonstrating its stability despite Boron’s incomplete octet.

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