lewis structure

We’ll talk about  BeCl2 lewis structure, formal charges, geometry, hybridization and their respective uses in this article.

Becl2 or Beryllium Chloride is an inorganic compound which is hygroscopic in nature and soluble in only polar solvents. It can be either white color solid or colorless in nature. The properties of BeCl2 is quite similar to aluminum chloride due to diagonal relationship.

How to draw Becl2 lewis structure?

Before jumping directly to the lewis structure, one should aware of the following terms like valence electrons and the octet rule.

Becl2 valence electrons

The term valence electron count refers to the actual number of electrons that participate in the bond formation. Generally, electrons that are present far from the nucleus are considered as valence electrons as they are readily available in the outermost shells of their respective atoms.

Be stands for Beryllium, an element of the periodic table with atomic number 4 and  with electronic configuration  of [He] 2s² whereas Cl ( chlorine) is part of halogen family with electronic arrangement of [Ne] 3s²3p⁵.

Hence, Be has 2 valence electrons and Cl has 7

Becl2 lewis structure octet rule

 A lewis structure is valid only when the intended entity passes the octet rule. According to the octet rule after the bond formation every atom should have stable electronic configuration.

Let’s draw lewis dots for BeCl₂ by following the above mentioned rules:

• Count the number of electrons that are available for bond formation ( ie. Valence electron)
•  Select the position of central atom on the basis of electronegativity factor as per rule “ most electropositive atom will occupy the center and atom with electronegative character will occupy the outer positions”
• Now, assign the all available electrons pairs in such a way that each of participating atoms must left with a stable configuration.

By following the above rules, we get the pictorial representation of Becl2 lewis structure:

Becl2 lewis structure lone pairs

Lone pairs are those non-bonding electrons which  stay as spectators during the process  chemical reaction and do not contribute towards bond formation. Generally, in lewis dots, they represented by dots towards the outer side.

 As, it is clear from the Becl2 lewis structure, Be do not have any lone pairs associated with it whereas chlorine has 6 lone pairs

Becl2 lewis structure resonance

Generally, resonance refers to the exchange of electrons from one bond to another. Conversely, resonance structure only possible only if the involved atoms either unsaturated or have empty d orbitals.

Can resonating structure possible for Becl2?

No, this is because Be does not any d orbitals in its valence shells and hence, resonating structure can not be possible for Becl2.

Becl2 lewis structure formal charge

Formal charge refers to the overall charge carried by a compound.

Formal charge for any compound can be found by using the above formula.

Calculation of formal charge for Berlyium atom

Valence electrons = 2 ( as belong to second group)

Unbonded electron count = 0

Bonded electrons = 4

F.C =  2 – 0 –  4/2 =  0

Calculation of formal charge for chlorine atom

Total valence count = 7

Unbonded electron count = 6

Bonded electrons = 2

F.C = 7 -6 – 2/2 =  0

Hence total formal charge on BeCl2 = 0

Becl2 hybridization

Hybridisation is a process in which two or more atomic orbitals of comparable energies overlap with each other to form hybrid orbitals.

Let’s see how hybridization happens in BeCl2 step by step:

1. Ground state of Be ( Z=4) [He] 2s²
2. Ground state of Cl ( z= 17) [Ne] 3s²3p⁵

• Excited sate of Be and Cl

• Formation of compound BeCl2

As it is clear from the given figure that formation of BeCl2 involve S and P orbitals and hence hybridisation is SP.

Becl2 lewis structure shape

As per  VSEPR theory, the expected molecular geometry of BeCl2 is found to be linear in shape.

This is because the central atom ie Be has no lone pairs around it and hence left no space for lone pair- lone pair repulsions and also two chlorine atoms attached to the Be also present far from each other in the  two different directions.

 All the arrangement of the atoms in that BeCl2 makes it a linear molecule.

Read more about Gold Structure and Characteristics

Becl2 lewis structure angle

Since the BeCl2 attains Sp hybridization.  The bond angle is expected to 180ºwith  beryllium as central atom containing no  lone pair with it.

Hence, there is no chance for any no disorientation at the  central atom which makes it’s  a perfect linear  shape with a bond angle of 180º. The general structure for linear geometry is given below:

Frequently asked questions

Is Becl2 ionic?

A compound is called ionic only if ionic bonds are established during the formation of the intended compound. However, in the case of BeCl2, the ionic bond cannot be formed because Berliyum has ionization energy around 900 kJ/mol which is relatively higher than the chlorine.

Therefore, the compound BeCl2 is not ionic but covalent in nature.

 What is the solubility of Becl2?

Due to the ionic nature of BeCl2, it is soluble in all polar solvents las given below:

water

acetone

DMSO.

However, it is insoluble in a non-polar solvent like CCl4.

Is Becl2 polar or nonpolar?

The BeCl2 molecule has a linear shape and also both Chlorine atoms attached to the BeCl2 also are in chemically same environment ie has same electronegative. As a result,  the dipole  moment of the BeCl2  molecule becomes zero leaving behind no partial charge.

Is Becl2 acidic or basic?

In order to know the acidic and basic character of BeCl2, Let’s examine the reaction of BeCl2 with water molecule.

BeCl2 + H2O → Be(OH)2 + 2 HCl

As you can observe here, when BeCl2 dissolved in water it produces a strong acid and hence it shows BeCl2 is acidic in nature.

Give physical characteristics of the compound BeCl2.

It gives yellow appearance

Boiling point = 482 °C

Melting point = 399 °C

Density = 1.899 g/cm³

State of matter is solid at room temperature

What are the uses of BeCl2?

1.During synthesis of many beryllium compounds BeCl2 formed as reaction intermediates.

 2. For electrolytic extraction of beryllium BeCl2 is used as  a raw material.

Is BeCl2 toxic in nature?

Direct contact with human skin cause irritation and leads to some allergic reactions. Moreover, longer exposure to this compound can cause lung cancer.

How BeCl2 is prepared?

BeCl2 can be prepared by reacting Berliyum metal with chorine at high temperature as shown above:

Be + Cl₂ → BeCl₂

What kind of structure BeCl2 have in solid and liquid state?

 BeCl2 have a polymeric chain structure in the solid state in which Be atom has four chlorine atoms in its surrounding. Out of 4, two chlorine atoms attached to the central atom via covalent bond and rest two with the coordinate bond as shown in the above figures

 In the case of liquid state, polymeric structure of Becl2 is dissociates into monomers and exist as BeCl2 in linear shape.

Conclusion

To conclude, Becl2 has sp hybridization with a linear geometry , followed the octet rule and reported with zero formal charges.

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The colorless Germanium tetrachloride appears as a fuming liquid.

As a covalent compound, its boiling and melting point are low and is used as intermediate  for optical processes.

How to draw Gecl4 lewis structure?

With using the atomic symbols of Germanium and Chlorine, the GeCl4 lewis structure shows the covalent nature by distribution of the outer orbit electrons, spread around the particular atom in GeCl4 molecule.

In modern Periodic table the halogen atom Chlorine is in group 17 with electronic arrangement [Ne] 3s2 3p5 and Germanium atom contains its outer orbit electrons in 4s and 4p with filled 3d orbital, the arrangement is [Ar] 3d10 4s2 4p2 as a group 14 element.

Hence four Chlorine and Germanium jointly have 32 electrons means sixteen pairs of electrons for molecule formation as they are in the outer shell and can be energized easily for low attraction by the nucleus.

As penta-atomic molecule, have to choose the central atom, here Ge is for its electro-positivity which will be in center and the halogen atoms are written around it with dot sign of valence electrons.

Gecl4 lewis structure resonance

In GeCl4 lewis structure, Chlorine atoms have unshared electron, which can delocalize from the parent atom and form different resonating structure, among these, which have the ‘zero’ formal charge that would be the stable configuration.

Chlorine is more electronegative than the Germanium atom,creats a partial positive charge over the Germanium atom which also occupies vacant 4d orbital as a element of 4^th period, so Pi (π) back bonding occurs i.e.3pπ (Cl) – 4dπ (Ge) in the molecule.

In the molecule Germanium has no unshared electron over it but for vacant orbital it has, the unshared electron of Chlorine atom can delocalize to that orbital and spread over two atoms which results in the formation of the partial pi (π) bonding in the molecule.

As the nonbonding electrons of the ligand, Chlorine atom involves in the bonding which is opposite to the normal electronic transition, it is called back bonding, produce resonating GeCl4 lewis structure.

Gecl4 lewis structure shape

Molecular geometry and shape are two slightly different things which we can clearly understand by the orbital hybridization of central atom of a covalent molecule, where central atom possesses lone pair that disturbs the geometry.

If there is no unshared electrons (so no steric repulsion) the geometry and shape of molecule becomes same which is in case of GeCl4 lewis structure as the geometry is tetrahedral (for sp3 hybridized central atom), the shape also be tetrahedral.

Gecl4 lewis structure formal charge

Formal charge is calculated for atom of molecule, to find the stable canonical form where it is assumed that equal distribution of bonding electron cloud in a covalent molecule with help of total valence electron, bonding and unshared electrons.

In the stable canonical form of GeCl4 lewis structure Ge has no unshared electrons, so the formal will be, (4- 0- 8/2) = 0 and with three pairs of unshared electrons the formal charge of Cl will be, (7- 6- 8/2) = 0; which indicates the energetic stability.

Gecl4 lewis structure angle

In the covalent type of bonding which is formed by hybridized orbital overlapping, the angle between such bonding electron cloud is measured, depends on the hybridization of the outer orbital of central atom which participated in bonding.

In the GeCl4 lewis structure the more electro-positive atom is Germanium whose 4s and 4p orbital intermixes, form sp3 hybridized orbital, so the atom has no unshared electrons which disturb the geometry by repulsion, make the bond angle accurate 109.5̊ as for sp3.

Gecl4 lewis structure octet rule

Eight electrons have to be distributed in the last filled orbit, wave functions of specific energy for satisfy the stabilization energy, known as Octet rule which stability naturally inert gases have, causes their inactive nature.

From the Periodic table we can say Ge have to transfer or accept four electrons which is very difficult where Cl needs one more electron to stabilize its configuration as a result Ge shares four electrons with four Cl atoms in GeCl4 lewis structure to satisfy the rule.

Gecl4 lewis structure lone pairs

Valence electron pair only spread over the parent atom and does not take part in the bond formation, makes higher electron cloud concentration of lone pair which causes steric repulsion and disturbs the geometry of a molecule.

From the hybridization we see the Germanium has no unshared electron as four valence electrons are hybridized to form bonding and for each of Cl atom of GeCl4 lewis structure they have six unshared electrons as one of 3p electron overlap with Ge sp3 orbital electron.

Gecl4 valence electrons

Valence electrons are the last shell containing electrons which are far apart from nucleus so energetically available for excitation in the chemical reaction as they loosely bound by nuclear force and if there is ‘d’ (diffused) orbital make more easy.

Being a ‘p’ block element of group 14 in 4^th Period, Ge has two electrons in 4s and two in 4p whereas each Cl has seven electrons in 3s and 3p orbital, so total thirty two loosely bounded electrons of five atoms participated in molecule formation as valence electrons.

Gecl4 hybridization

Hybridization is the concept for central atom of covalent compounds where energetically not equivalent atomic orbitals intermix to form orbital with same energy so atomic hybrid orbital overlapping will become easier in molecule formation.

Being a ‘p’ group atom the central atom Germanium has four outer shell electron in 4s and 4p, while sharing these electrons for better overlapping the 4s and 4p orbitals mixes up, creating new hybrid orbital ‘sp3’ with new shape and energy than previous.

Gecl4 solubility

At a certain temperature GeCl4 solubility in any solvent is measured by the concentration which can be dissolved until the equilibrium occurs in the solution which is dependent on its nonpolar nature as well as having vacant d orbital.

Being a nonpolar molecule it easily dissolve in the solvents like benzene, ether, Chloroform, CCl4 as these are also nonpolar in nature, also slightly dissolve in dilute HCl or dilute H2SO4 for slightly electrolytic nature for metalloid Ge but not in concentrated one.

Is Gecl4 soluble in water?

GeCl4 is soluble in water as it readily hydrolyses in spite of being a covalent molecule, because of the two reasons; it is in period 4 with diffused ‘d’ orbital in group 14, makes it larger size and for ‘d’ orbital it can accept nucleophilic attack.

At the time of nuclephilic attack of water, it don’t have to face resist for large atomic size of Ge and ‘d’ orbital can extent coordination, so Ge-Cl bond breaks and Ge-hydroxyl bond forms with production of  GeCl3(OH) and Hydrochloride (HCl) acid as side product.

Inthe reaction further four HCl molecule releases from one GeCl4 molecule and GeO2 from as the product of the Hydrolysis reaction.

Is Gecl4 a strong electrolyte?

As Ge is metallloide in nature, show some semiconductor nature so GeCl4 lewis structure can be act as electrolyte sometime but not strong as metallic electrolytes.

Is Gecl4 acidic or basic?

Any molecule that release hydrogen ion (H+) in solution or accept electron is considered to be an acid. In the molecule GeCl4, germanium can bear electron from donor making it some acidic in nature.

For having vacant diffused 4d orbital it can bear nucleophilic attack by accepting electron pair and make coordination number higher.

Is Gecl4 polar or nonpolar?

In the Germanium chloride molecule, electro-negativity of Cl is 3.16 and that of Ge is 2.01 on the basis of Pauling scale, makes bond electron cloud pulling capability difference, results polar bond formation but for the highly symmetric nature the overall polarity of GeCl4 become zero.

If this electro-negativity difference is 0.4 or more than that a charge separation occurs in the bond, which results a polar bond (vector quantity) as Dipole moment (µ) can be calculated by multiplication of the separated charge (δ) and distance between charges (r) in the bond.

As Ge atom of GeCl4 lewis structure has no unshared electrons, so the geometry can’t be distorted by the steric effect of lone pair, makes it highly symmetric so that the dipole moment vector can cancel out each other and make GeCl4 non polar molecule.

Is Gecl4 a lewis acid or base?

GeCl4 is a lewis acid as it can accept electron cloud from donor and extent it coordination for having ‘d’ orbital as it belongs to period 4 of Periodic table, while it possess partial positive charge as Chlorine is highly electronegative atom.

Ge has four outer orbit electrons distributed in 4s and 4p, so transfer of these can be a highly energy required process. Hence by sharing the electrons it tends to form molecule and for vacant 4d orbital it also accept electrons as a lewis acid.

Is Gecl4 linear?

The geometry and shape of GeCl4 is tetrahedral, not linear.

Conclusion:

For having diffused vacant 4d orbital GeCl4 lewis structure shows some unexpected properties, different than its upper period element like Carbon.

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This article illustrates that Gef4 stands for germanium tetrafluoride and Informs us about atomic charges, angles, dipole moments, bond lengths, bond lengths, and total energy.

The lewis structure of Gef4 has four single bonds in Germanium and Fluorine atoms. In the lewis structure of Gef4, the Ge atoms are present in the center, and fluorine atoms are lying around the Ge atoms.

How to draw Gef4 lewis structure?

Valence electrons present in molecules are represented by a dot structure that is called the lewis dot structure. To find chemical bonding in a molecule the lewis structure is the simplest method that predicts molecular geometry.

To draw lewis structure following steps are used:

Step1:

Find the valence electrons in the given molecules of Gef4, Ge consists in its outermost shell 4 valence electrons and fluorine consists of 7 valence electrons in its outermost shell. 

Thus total valence electrons in the Gef4 molecule are 32.

Step2 :

After counting the valence electrons of the molecule find the element which is least electronegative and make it the central atom of that molecule.

For Example, In the Gef4 molecule Germanium is the least electronegative element and consists of the position of the center atom.

Step3:

Draw a skeleton of the Gef4 lewis structure and connects all the atoms through single bonds.

Step4:

After drawing the skeleton of the Gef4 lewis structure, place the lone pairs to each atom in the molecule. As Germanium is the center atom does not contain lone pairs because all valence electrons participate in single bond formation. 

The surrounding atom fluorine consists of one lone pair of at beach three fluorine atoms. This will give 3 lone pairs of electrons on the fluorine atom.

Step5:

Now consider the octet of each atom in Gef4 molecules, if the octet is not complete then draw the double or triple bond to satisfy the octet of each element.

In the case of the Gef4 molecule octet of each element is complete and satisfied. So the final gef4 lewis structure is as drawn below.

Gef4 lewis structure resonance

If we are talking about the Gef4 lewis structure Germanium forms single bonds with fluorine. When we can draw two or more valid Lewis structures for the same molecule, we have resonance. 

Resonance occurs only when a molecule contains at least one double bond. Single-bond molecules never exhibit resonance.

Gef4 lewis structure shape

For the structure of Gef4 lewis structure, Ge consists of 4 bonding orbitals bonded with a fluorine atom and exhibits tetrahedral shapes. It is a tetrahedron pyramids structure that consists of 4 corners and 4 triangular faces.

Gef4 lewis structure formal charge

Formal charges (q) represent atoms’ charges in molecules when covalent bonds are formed. An atom’s charge is determined by the difference between its valence electrons available in its free neutral state and its valence electrons assigned in a Lewis structure.

The equation to find the formal charge in Gef4 are as follows:

F = V- N – ½ B

Where,

F = Formal Charge on Gef4(0)

V = Valence Electron(4)

N = Number of non-bonding valence electrons in Gef4 (0)

B = Total number of bonding electrons in Gef4 (4)

So the formal charge on Gef4 is zero.

Gef4 lewis structure angle

Gef4 has tetrahedral geometry, because of that Gef4 only has bonded pairs of electrons, the bond angles are 109.5 degrees, however, if there were unbonded electron pairs, they would push the other atoms further away and reduce the bond angles.

Thus Gef4 has a 109.5° bond angle.

Gef4 lewis structure octet rule

In the Gef4 lewis structure, we will see that fluorine is present surrounding the germanium atom and become the outer element. So we have to complete the octet of the fluorine atom because it has 7 valence electrons in its outer shell and required one more electron to complete the octet. 

Thus in the lewis structure of Gef4, all atoms follow the octet rule.

Gef4 lewis structure lone pairs

In Gef4  lewis structure, Ge forms 4 single bonds with fluorine atoms and used all valence electrons in the bonding but on the fluorine, there are remaining 6 lone pairs of electrons.

Thus there is total lone pair of electrons is 6*4=24 in Gef4 molecules.

Gef4 valence electrons

The valence electrons are used to form bonds with the atom’s other electrons. In the germanium electronic configuration are  4s2,4p2 in its Lewis structure, the valence electron in Germanium is four and in fluorine (2s2,2p5) is seven (4*7=28). As a result, the Gef4 molecule has 32 total valence electrons.

Gef4 hybridization

Hybridization is the simplest form of the distribution of electrons in different energy level orbitals and collects information about the compound and all of its related properties. The number of valence electrons in Gef4 is 32, from 32 valence electrons, 4 participate in bond formation and 28 are non-bonding electrons.

Thus steric numbers are found and calculated by adding lone pairs of electrons on the central atom and these are present around the central atoms.

E.C of Ge in Ground State: 3d¹⁰,4s²,4p²

E.C of Ge in Excited state:4s¹,4px¹,4py¹,4pz¹

The hybridization of Gef4 is sp3.

Gef4 solubility

Germanium fluoride is a colorless gas with a characteristic odor that is garlic-like in smell. It is soluble in water and reacts with water and forms hydrofluoric acids.

Is Gef4 soluble in water?

Yes, The Gef4 lewis structure is slightly soluble in water, and in water, it dissociates in ions and becomes ionic.

Is Gef4 a strong electrolyte?

The electrolyte is that which dissociates into ions that are positive and negative ions when making a solution in water. Gef4 is ionic and slightly dissolved in water thus it behaves as an electrolyte.

Is Gef4 acidic or basic?

The Gef4 is behaving as acid, its acidic nature means that molecules accept the electrons in solution, and in water, it reacts and forms hydrofluoric acids. Thus the Gef4 lewis structure is acidic.

Is Gef4 polar or nonpolar?

Nonpolar molecules are those in which symmetrically distribution of charge over all the atoms that are present in the molecules and dipole moment is zero.

Yes, Gef4 has zero dipole moment and shows nonpolar properties.

Is Gef4 a lewis acid or base?

Gef4 act as lewis acids, because Ge has d-orbital which is ready to accept electrons, and lewis acid means accepting the electrons in their vacant orbitals.

Is Gef4 linear?

No, Gef4 is not linear because it shows tetrahedral geometry and shows sp3 hybridization and this will give tetrahedron pyramid-type of shapes with an angle of 109.5 degrees.

Is Gef4 paramagnetic or diamagnetic?

The magnetism displayed by diamagnetic materials is known as diamagnetism. Materials become freely magnetized when they are exposed to a magnetic field. However, compared to the magnetic field, the magnetization is moving in the opposite direction.

Gef4 is diamagnetic as its dipole moment is zero and if we see its hybridization, it is sp3 hybridized and all the electrons are paired. Thus pairing of electrons shows that the Gef4 lewis structure is diamagnetic.

Gef4 boiling point

The temperature at which the vaopur pressure of a liquid is equal to the pressure of a liquid that is present surrounding that liquid at which liquid changes into vapour is called the boiling point. 

Thus, the Gef4 has boiling point equal to −36.5 °C. 

Gef4 bond angle

The Germanium tetrafluoride has a 109.5-degree bond angle with sp3 hybridization and tetrahedral molecular shape.

Conclusion

Gef4 stands for germanium tetrafluoride. Lewis structure of Gef4 has four single bonds in Germanium and Fluorine atoms. Valence electrons present in molecules are represented by a dot structure that is called the lewis dot structure. If we are talking about the Gef4 lewis structure, Germanium forms sp3 hybridization with a 109.5-degree bond angle.

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Iron (III) Bromide (FeBr3) has quite stable polymeric structure, generally known as Ferric bromide.

The brown color solid inorganic compound can be used as oxidant, removes electron in redox reaction or used as catalyst in bromination where concentration of FeBr3 remains same after and before reaction but it affect the rate of reaction.

How to draw febr3 lewis structure?

With using the atomic symbols, the FeBr3 lewis structure shows the distribution of the outer orbit electrons in formation of the molecule, as an ionic compound for the electronic transition the charges are shown upper outside of bracket around atom.

Count the valence electrons of the molecule:

In modern Periodic table the halogen atom Bromine is in group 17 with outer shell electronic distribution in 4s, 4p orbital: [Ar] 3d10 4s2 4p5 where Iron is in group no 8 and being transition metal with incomplete electronic arrangement in 3d orbital; [Ar] 3d6 4s2.

Outer orbit electrons are mostly loosely bounded by nucleus force but in addition the d orbital being more diffused in nature it can easily exchange electron cloud. Orbital is energetically most stabilized in their full filled or half filled electronic configuration.

Cover the Octet rule:

To form energetically stable molecule (unreactive), all atoms must have full filled last orbit with eight electrons by transferring electrons, referred as Octet rule.

Iron transfers three electrons from 4s and 3d jointly results remaining of five electrons in 3d orbital, which is a stabilize configuration for the half filled 3d orbital and forms Iron (III). The electrons are accepted by the vacant 4p orbital to satisfy the stabilization rule.

 

Calculate the formal charge of the individual atom:

As FeBr3 is ionic molecule so the formal charge is not calculated where we consider the electro-negativity of individual atoms, opposite of the covalent molecule, where the electron pulling ability of atoms is consider equally.

Skeletal formation of the BrCl lewis structure:

FeBr3 is a tetra-atomic molecule, where Iron (Fe) is the central atom, more electro positive than halogen atom. The atomic symbols are written inside brackets, by electron transferring they possess charges which are shown outside of bracket.

Is febr3 ionic or covalent?

When metal and non-metal elements from molecule, there fully electronic transfer is occurred from metallic orbital to vacant non-metallic orbital in spite of electron cloud sharing, produces ionic compound.

Bromine is a non metal element where Iron is a transition metal element, are joined together by fully transferring electron cloud of Fe having diffused 3d orbital electron to vacant 4p orbital of halogen atom, hence FeBr3 lewis structure is ionic in nature.  

Being an ionic molecule we can see the melting point of the FeBr3 lewis structure is quite high, (200 ̊ C) as the opposite charges are bound by strong electrostatic force and are arranged in a proper design of repetition in crystalline structure, result in a high lattice energy.

Is febr3 an acid or base?

FeBr3 lewis structure contains Fe atom which is a transition metal having 3d orbital, and Fe combines with electro-negative halogen atom Br, makes the molecule a lewis acid, capable of accepting electron.

In metal halide FeBr3, because of difference in electron cloud pulling capability Fe contains partial positive charge and because of having vacant 3d orbital it adopted electron pair accepting ability, as a result used as a catalyst in aromatic bromination reaction.

In bromination of Benzene FeBr3 is used with Br2 for its strong lewis acid nature, it polarizes the Bromine molecule with partial charges and combine with it by accepting electron cloud which makes easy for benzene electron cloud to do nucleophilic attack.

Is febr3 soluble?

FeBr3 solubility in any solvent is measured by the amount of concentration that can be dissolved until the equilibrium occurs means the concentration of reactant compound and the product compound result balance in that condition (like temp.)

Solubility in water:

As a polar solvent, water (H2O) has partial charges over it for difference of electro-negativity between atoms and can dissolve polar molecules. Because of greater power of pulling electron cloud toward it, Oxygen carries partial negative charge.

FeBr3 has Iron atom which has (+3) charge over it as it transfer two 4s and one 3d electrons and three Bromine atoms which accepts electrons so that have negative charge (-1), so charge separation is there and as a result can easily dissolve in water like polar solvent.

Solubility in ether:

Ether has polar Carbon- Oxygen bond (Oxygen is highly electronegative than Carbon) as its molecular formula is R-O-R´ where R and R´ are two different alkyl groups, so it has some dipole moment  causes ether a polar solvent.

FeBr3 is an ionic compound, contains oppositely charged ions bounded with electrostatic force, so can dissolve in polar solvent. But the polarity differs with length of hydrocarbon chain of ether as with increasing it the interaction between ether and FeBr3 decrease.

Solubility in ethanol:

Methanol, ethanol or propanol have small hydrocarbon chain (hydrophobic part) with the hydroxyl group (-OH) which is polar for Oxygen atom with high electro-negativity (electron pulling ability) result in becoming polar solvent.

So ionic compound like FeBr3, having charge distribution can soluble in ethanol.

Is febr3 a salt?

A salt have two portion called cation with positive charge and anion with negative charge, the amount of the charge will be equal so that the salt molecule will be neutral without any charge. If they contain the ionic part forming with one atom, are called monatonic salt.

In neutralization reaction, FeBr3 is formed having oppositely charged metal ion iron (III) and non-metal bromide ion, and as one iron atom combines with three bromide ions, produces neutral salt. As the ionic parts are not combination of atoms, the salt is monatomic.

In the neutralization reaction of strong acid (HBr) and weak base (Fe(OH)3) where the strong acid is neutralized and forms the ionic compound as salt FeBr3 and water.

Being an ionic compound Salts have some crystalline structure where the ions are arranged in certain manner of repetition which also can be seen in case of FeBr3 lewis structure where it crystallizes in the trigonal R-3 space group.

Conclusion:

Having transition metal, iron with ‘d’ orbital effects properties of FeBr3.

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In this article, we discuss trichloride of group 13^th element. Let’s discuss GaCl3 lewis structure and different important facts.

GaCl3 or gallium trichloride is an example of trihalide of group 13^th element. Ga is very stable in its +3 oxidation state because at that state its electronic configuration will be d¹⁰. Ga is the main group metal so it has an affinity to bind with electronegative atoms like Cl. Due to electron deficiency, GaCl3 is exist as a dimer form in solid-state, Ga₂Cl₆ like Al₂Cl₆.  In the dimer form, it will form a 3c-4e bond.

GaCl3 has a high boiling point and very low melting point. GaCl3 is sp² hybridized. Ga has filled d electrons so 4s and 4p orbitals participate in the hybridization or any kind of bond formation. The low oxidation state of Ga can permit to involved in complex formation for the GaCl3.

1.    How to draw GaCl3 lewis structure?

For a p block element or any kind of element that can form a molecule, it is necessary to draw their lewis structure to observe the bond structure, bonding, method, etc. Let us consider drawing the GaCl3 lewis structure.

Step 1- The first step is counting the valence electrons of every atom in the molecule and added together. So first we calculate the valence electrons in the GaCl3 lewis structure. Ga is p block group 13^th element. The electronic configuration of Ga is [Ar]3d¹⁰4s²4p¹. So, it has a vacant d orbital and three valence electrons in the 4 s and 4 p orbitals. Again, Cl is also a p block element but it belongs to the halogen family group 17^th element. The configuration of Cl is [Ne]3s²3p⁵. So, it has seven electrons in its valence shell. So total valence electrons in the GaCl3 lewis structure is 3+(7*3)=24 electrons.

Step 2 – in the 2^nd step, we have to decide on the central atom of any molecule. In the GaCl3 lewis structure, Ga is a p block metal so it shows a positive charge, so its electronegativity is very low and for this reason, Ga will be chosen as the central atom in the GaCl3 lewis structure. Three Cl atoms are present on the three sides of the central Ga atoms.

Step 3 – In this step, we have to calculate how many numbers of bonds are required according to the Octet rule. According to the octet rule every p block elements try to complete its valence shell by eight electrons. So, for the  GaCl3 lewis structure electrons needed according to the octet rule will be, 8*4 =32 electrons. In the solid-state, GaCl3 exists as a dimer, so in the dimer, the electrons needed will double from the monomer. So, the electrons needed will be 32*2 = 64 electrons.

But the valence electrons for the GaCl3 monomer will be 24 and for the dimer, it will be 24*2 =48 electrons. In the dimer, there will be a metal-metal double bond and there are four electrons will be needed.  So, in the GaCl3 dimer required bonds apart from metal-metal bonds will be, 1/2(64-4-48) = 6 bonds, and in the GaCl3 monomer the required bonds will be 3 bonds.

Step-4 In the fourth step we added all the atoms by the required number of bonds. In the GaCl3 lewis structure, there will be a minimum of three bonds are there so, Ga and three Cl atoms are attached via three single bonds.

Step-5 In this step we try to fulfill the octet of every atom in the GaCl3 lewis structure. After adding the three bonds the octet of Ga is completed via the formation of a dimer. But for the Cl, six electrons exist in their valence shell and for completing the octet they exist as lone pairs over the Cl atoms.

2.    GaCl3 lewis structure shape?

The shape of the molecule depends on the hybridization, mode of bonding, and presence of surrounding atoms. There are three surrounding atoms for Ga in GaCl3 lewis structure, so the acceptable shape is planar trigonal.

Ga is a p block element and has only three electrons in its valence shell and they are forming a bond with three Cl atoms. There are no other electrons are present in the valence shell of Ga in the GaCl3 lewis structure. GaCl3 is an AX₃ type of molecule without lone pairs of central atoms, so according to the VSEPR theory, it should adopt planar trigonal geometry. Again, from hybridization, we can say that if the central atom is sp² hybridized so the shape of the molecule will be planar trigonal.

3.    GaCl3 lewis structure angle?

For a planar trigonal molecule, a bond angle is expected to be 120⁰. If there is no deviation factor present, like lone pairs -bond pair repulsion, the large size of surrounding atoms, etc. In the GaCl3 the Cl-Ga-Cl bond angle is 120⁰.

In the GaCl3 lewis structure, Cl-Ga-Cl is around 120⁰. So, it is evident from the structure of GaCl3 that it is planar trigonal and there is no lone pair-bond pair repulsion. Actually, in the GaCl3 lewis structure, there is no deviation factor is present, so the bond angle is ideally 120⁰.

4.    GaCl3 valence electrons

The number of valence electrons for GaCl3 lewis structure is calculated for Ga and three Cl atoms individually. Ga and Cl both are p block elements, so we only count the electrons in the p orbitals, because those electrons are the valence electrons for GaCl3.

In the GaC3 lewis structure, Ga and Cl have three and seven electrons in their valence shell respectively. The electronic configuration of Ga and Cl are[Ar]3d¹⁰4s²4p¹  and  [Ne]3s²3p⁵ respectively. So, the total valence electrons in the GaCl3 lewis structure are, 3+(7*3)=24

5.    GaCl3 lewis structure lone pairs

In the GaCl3lewis structure, only cl atoms have the lone pairs, not central Ga. All the valence electrons of Ga are involved in the bond formation.

From the electronic configuration, it is evident that there are only three electrons in the valence shell for Ga and all the electrons are involved in the bond formation and no electrons are there in the valence shell of Ga. So, Ga is lack of lone pair.

But Cl has seven electrons in its valence orbitals so, it has seven valence electrons and only one electron is involved in the bond formation and the rest of the six electrons exist as three pairs of lone pairs. So, there are only Cl atoms containing lone pairs in the GaCl3 lewis structure.

So, the total lone pairs in the gaCl3 lewis structure are 3*3 = 9 pairs of lone pairs.

6.      GaCl3 lewis structure formal charge

GaCl3 lewis structure is partially charged or neutral is predicted from its formal charge value. Accounting for the same electronegativity for Ga and Cl we should calculate the formal charge of the molecule.

It is a theoretical concept, so formal charge has a specific formula, and the formula is,

F.C. = N_v – N_l.p. -1/2 N_b.p.

The formal charge over Ga is, 3-0-(6/2) = 0

The formal charge over Cl is, 7-6-(2/2) = 0

So, the GaCl3 lewis structure is neutral from its formal charge value.

7.    GaCl3 lewis structure octet rule

In the GaCl3 lewis structure, only Cl has completed its octet by completing the valence shell with eight electrons, and Ga is not completed its octet.

Cl has seven electrons in its valence shell and it shares one bond via two electrons with Ga and completed its octet to make a single bond. But in the case of Ga, there are three electrons in the valence shell and Ga makes three bonds with shre three more electrons, so there are six electrons in the valence shell of Ga and it is not complete its octet. That’s why Ga can accept more electrons to fulfill its electron deficiency and makes dimer to complete the octet.

When it forms a dimer then both Ga atoms in dimer form complete their octet via bridging the cl atoms. This model can be explained via 3c-4e bonding.

8.    GaCl3 lewis structure resonance

There are no such electron clouds present over the Ga atoms for delocalization in different skeleton forms. That’s why the GaCl3 lewis structure does not show any resonating structure.

9.    GaCl3 hybridization

From the shape of the molecule and involvement of the orbital, we can say that GaCl3 lewis structure is sp2 hybridized.

We can calculate the GaCl3 hybridization by using the following formula,

H = 0.5(V+M-C+A)

In the GaCl3 lewis structure, the central Ga atom is, ½(3+3+0+0) =3 (sp² hybridized).

If the central atom of a molecule is involved in three orbitals in hybridization then it will be sp² hybridized.

Let us understand the hybridization of GaCl3 lewis structure,

From the box diagram of the GaCl3 lewis structure, it is evident that central Ga is sp² hybridized where only 4s and 4p orbitals are involved and there are vacant p orbitals in Ga, so the GaCl3 monomer does not complete its octet.

10.    GaCl3 solubility

GaCl3 is soluble in the following solvents,

• Water
• Benzene
• CCl₄
• CS₂

11.    Is GaCl3 soluble in water?

As discussed, the previous GaCl3 is very much soluble in water, as it vacant p orbital so there the lone pairs of oxygen atom can be attacked and for this reason, it can produce an adduct and result is soluble in water. GaCl3 is very moisture sensitive.

12.    Is GaCl3 a strong electrolyte?

Yes, GaCl3 is a very strong electrolyte, in an aqueous solute, the ion can readily be ionized to Ga³⁺ and 3Cl^–, both ions are good conductors of electricity and both are soluble in water, making the solution a good conductor of electricity.

13.    Is GaCl3 polar or nonpolar?

GaCl3 is dissolved in water, so it is a sign that GaCl3 is a polar molecule. The electronegativity difference between GA and Cl is huge which makes the molecule polar. Again, due to the asymmetric shape, the mackerel has some resultant dipole moment.

14.    Is GaCl3 acidic or basic?

GaCl3 is acidic, rather it is a very strong Lewis acid.

15. Is GaCl3 a lewis acid or base?

In the GaCl3 lewis structure, there is a vacant p orbital present for Ga, this p orbital is energetically accessible and it can take electrons or lone pairs from a suitable lewis base and acts as stronger lewis acid, But in the dimer from the vacant p orbital is filled upon bond formation so, the dimer is not a good lewis acid.

16. Is GaCl3 paramagnetic or diamagnetic?

After the bond formation all the valence electrons of GaCL3 and even for Ga(III_ all the d electrons are paired up. So, Gacl3 or Ga(III) is diamagnetic in nature.

17. Is GaCl3 linear?

No, GaCl3 is not linear, the GaCL3 lewis structure shape is trigonal planar and it is evident from the bond angle and its hybridization value too.

18. GaCl3 bond angle

The GaCl3 lewis structure shape is trigonal planar and the hybridization value is sp2, so the bond angle is 1200.

19. GaCl3 boiling point

The boiling point of GaCl3 is very high because in the solid state two Ga centers are linked strongly and the solid is liquified. In the liquid state since Ga-Ga bonds are extremely strong at the very high temperature required to break those bonds, Thus, it has a very high boiling point.

Conclusion

In the GaCl3 lewis structure, Ga is sp² hybridized but there is electron deficiency in the Ga center and to fulfill, the deficiency GaCl3 is exist as a dimer form via 3c-4e bonding.

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In this article, we should discuss the FeCl2 lewis structure. Let’s talk about the FeCl2 lewis structure and 9 different characteristics fact.

FeCl2 is often known as ferrous chloride. The ferrous term is coming for Fe in a +2 oxidation state. In the FeCl2 Fe is in a +2 oxidation state. The electronic configuration of Fe(II) is d⁶. Being a FeCl2 is a coordination compound, Cl is not only a counter ion here it also acts as a ligand. The geometry of the FeCl2 lewis structure is the bent shape, although in the crystal form it adopts an octahedral shape.

As Cl is a soft filed ligand, the electronic paired up is not formed in the d orbital. So, Fe(II) is a d⁶ high spin system here. Only one subset is paired due to six electrons present in five subsets. FeCl2 lewis structure can be ionized to ferrous and chloride ions.

Some important facts about FeCl2

FeCl2 is a white solid crystalline molecule. It is a paramagnetic solid due to the presence of four unpaired electrons in the d orbital. The color of its tetrahydrate form is greenish, due to its octahedral shape and the Laporte transition occurs. But in anhydrate form is white.

Anhydrates form can be prepared by the reaction of steel waste with hydrochloric acid.

Fe + 2 HCl → FeCl₂ + H₂

The melting point and boiling points of FeCl2 are950 k and 1296 K respectively.

1.    How to draw FeCl2 lewis structure?

Drawing the FeCl2 lewis structure is not an easy task. As FeCl2 is a coordination compound rather than a covalent molecule. So here d electrons will be involved in the bond formation and it is not easy to manage d electrons for drawing the lewis structure because d electrons follow the 18 electrons rule rather an octet rule. So, we try to draw the FeCl2 lewis structure easily in the following manners.

Step 1– At first, we should count the valence electrons for Fe as well as Cl. The valence electrons of Fe are d electrons and p electrons for Cl atoms and added together. In the FeCl32 lewis structure, the valence electrons for Fe are 6 as it is in a +2 oxidation state, and all the electrons belong from its d orbital only, for three Cl atoms is 7*2 = 14. So, the total valence electrons are 6+14 = 20.

Step 2 – Fecl2 will follow the 18 electron rule because it is a coordination compound.it is similar to the octet rule of a coordination molecule. The electrons that will be needed for the FeCl2 lewis structure will be 8 + (2*8) = 24 because the octet rule required 8 electrons in the valence shell for every atom. We get the available valence electrons are 20 from the previous calculation for FeCl2. Now the required electrons will be (24-20) = 4 electrons and the minimum number of bonds required that all the three atoms should be connected in this molecule is 4/2 = 2 bonds.

Step 3- Now time for deciding on the central atom in the FeCl2 lewis structure. Fe is here central atom as it is electropositive because it is a transition metal, whereas Cl is from the halogen family and it is a more electronegative atom.

Step 4 – Connect two Cl atoms with the central Fe via the minimum number of required single bonds i.e. two. So, Fe makes two single bonds with two Cl atoms from its d orbital electrons in the FeCl2 lewis structure.

Step -5 After the bond formation we have to check the number of lone pairs available over the molecule. So, we check which atoms in the FeCl2 lewis structure contain lone pairs. In the FeCl2 lewis structure, Fe is +2 oxidation state, so it is a d⁶ system and it has no lone pairs in its d orbital. So, we check the lone pairs over Cl atoms. Cl is group 17^th element and from the halogen family. So, after bond formation, it has three pairs of lone pairs. So, the lone pairs are assigned only over the Cl atoms.

All the octet is complete after the bond formation and lone pairs are assigned, so no need to add any kind of multiple bonds in the FeCl2 lewis structure.

2.    FeCl2 hybridization

The bonding method of coordination compound or metallic compound is different. They do not follow the rule of the Valence Bond Theory (VBT). They will follow CFT i.e. Crystal Filed Theory. Hybridization is a corollary of VBT. So, it is difficult to determine the hybridization of FeCl2 lewis structure.

So, we predict the hybridization of FeCl2 lewis structure from its shape. The shape is bent and two surrounding atoms are present and no involvement of lone pairs, so there will be two orbitals are involved in the hybridization and the hybridization will be sp.

In the hybridization, FeCl2 does not involve its d electrons, because they are not it’s outermost orbital and due to the presence of weak field ligand Cl, only the outer orbital will contribute, they are 3s and 4p orbital. So, it is another example of an outer orbital complex like FeCl3.

If we use the typical formula for the calculation of hybridization, H = 0.5(V+M-C+A),

H = ½(2+2+0+0) =2 (sp), Fe has two electrons apart from six electrons in its d orbital and two Cl atoms are present. From VSEPR theory if the number of orbitals mixed in hybridization is 2 then the central atom is sp² hybridized.

Let us draw and understand the hybridization of the FeCl2 lewis structure.

From the box diagram of Fe(II), we can say that only 4s and 4p orbitals are involved in the bond formation for the FeCl2 lews structure. So, the hybridization is sp. 4s and 4p orbitals are outer orbital for Fe, so it is an outer orbital complex. When it forms tetrahydrates, then four water molecules bind with four unpaired electrons in the d orbital and makes an octahedral complex.

1.    Is FeCl2 ionic or covalent?

The coordination compound is somewhat covalent. But in the FeCl2 lewis structure, Fe and Cl two ions can be separated due to large ionic differences and also show ionic character. In the aqueous solution, it can be ionized easily, and Fe(II) easily polarize chloride anions.  So FeCl2 is ionic besides covalent character.

2.    Is FeCl2 soluble in water?

Any polar molecule will be soluble in a polar solvent (like dissolve like). Water is a polar protic solvent and it can form an H bond also. FeCl2 is a polar molecule because the charge difference between Fe and Cl is so high and due to its bent shape, it makes polar. So, naturally, FeCl2 is soluble in water.

3.      Is FeCl2 aqueous?

After soluble in water any molecule, then that form is called an aqueous form of that particular molecule. As discussed previously that the FeCl2 lewis structure is soluble in water, so after soluble, the whole solution is called an aqueous solution of FeCl2. So FeCl2 can make an aqueous solution easily after being soluble in water.

In the aqueous solution, FeCl2 can easily be ionized to separate the two ionic forms.

FeCl2(aq) = Fe²⁺ (aq) + 2Cl^–(aq)

4.    Is FeCl2 a salt?

The reaction between acid and base always gives us salt and water. So, if a molecule is produced after the reaction between an acid and basic molecule then it is called salt. Salt is the combination of counter cation of a basic molecule and counter anion of acidic molecules.

If we reacted ferrous hydroxide with hydrochloric acid we should get FeCl2 as a salt along with water as a side product.

Fe(OH)₂ + 2HCl = FeCl₂ + 2H₂O

So basically, salt is the neutralization part of an acid and base after reaction and salt does not have any acidic as well as basic property in it. So FeCl2 is salt.

5.    Is FeCl2 a strong electrolyte?

A substance that dissolves in water or any other polar solvent to produce ions and a solution that conducts electricity is called electrolytes. In the aqueous solution of FeCl2, we already see that FeCl2 is fully ionized in that solution to form ferrous and chloride ions. Those ions are very good conductors of electricity. So, if we passed the current in the aqueous solution of FeCl2, then it can carry the current in a very good way. So FeCl2 is a strong electrolyte.

6.    Is FeCl2 a precipitate?

If a compound is insoluble in water then it can be precipitated down the reaction vessel. But FeCl2 is soluble in water so there is no chance for FeCl2 to exist as a precipitate. The precipitate can also form due to the reaction of two compounds and in an aqueous solution, the product will be insoluble in water.

7.    Does FeCl2 react with HCl?

When we reacted Fe with HCl the FeCl2 is formed instead of FeCl3. Because FeCl2 is a thermodynamically more stable product. It is a displacement reaction and metal can easily displace the H₂ from HCl, so FeCl2 is formed instead of FeCl3.

Conclusion

FeCl2 is also a coordination compound and it can form tetrahydrates adopting octahedral geometry. Cl is weak filed ligand so the system is sigh spin and Fe is +2 oxidation state. So, the electronic configuration will be d⁶ high spin. FeCl2 is soluble in water and a strong electrolyte.

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Cu[(nh3)4] 2+ Lewis structure and 7 facts on Cu[(NH3)4]2+ ion that is named as Tetraamine copper ion in chemistry would be described in this article. The facts would be revealed through the sketch of Lewis structure of this complex compound.

The facts that would be described illustrating internal characteristics of the compound are:

• Cu[(NH3)4]2+ Name
• Cu[(NH3)4]2+ Oxidation number
• Cu[(NH3)4]2+ Magnetic moment
• Cu[(NH3)4]2+ Shape
• Cu[(NH3)4]2+ Colour
• Cu[(NH3)4]2+ Coordination number
• Cu[(NH3)4]2+ Lewis structure
• Cu[(NH3)4]2+ Reaction with HCl

Cu[(NH3)4]2+ Name

A complex compound is always need to hold a specific name which is defined by applying the rules given by IUPAC (International Union of Pure and Applied Chemistry) with the help of its chemical formula.

The name given by IUPAC to Cu[(NH3)4]2+ is Tetraamine copper. Tetraammine is defined for highlighting four amino group that are attached with one copper ion. 

Cu[(NH3)4]2+ Oxidation number

Oxidation number is one of the importance characteristics, which defines the electronic excesses or deficiency in the compounds that is the gain, or loss of electron in the centre atom.

The oxidation number of Cu in Tetraamine copper is +2 as the overall complex ion has deficiency of two electrons and (NH3)4 (ammonia) compound possesses zero oxidation number.

Cu[(NH3)4]2+ Magnetic moment

Magnetic moment refers to the characteristic, which indicates the magnetic dipole moment, that is the tendency of objects or element to align with a specific amount of magnetic field.

This compound imposes paramagnetic effect. The magnetic moment of Cu[(NH3)4]2+ is 1.73 B.M. this property is reliable in imposing the fact regarding the number of n paired electron in this compound. There is a specific formula helps to calculate the number of unpaired electron.

The formula is number of unpaired electron = √n(n+2) where N refers to the amount of magnetic moment. Therefore , this reveals that one unpaired electron present in the compound [√n(n+2) = √1.73(1.73+2) = 1].

Cu[(NH3)4]2+ Shape

Shape of the compounds is revealed by calculating the number of electron present on the compounds. Electronic configuration of the compounds are reliable in reflecting the idea about the shape of the compound. The electronic configuration of Cupper in Cu[(NH3)4]2+ is  1s2 2s2 2p6 3s2 3p6 3d0 4s0. Cu shows dsp2 hybridisation with one paired electron. The compound shows square planner shape in chemistry instead of tetrahedral geometry.

Cu[(NH3)4]2+ Colour

Colour of compounds depends on the exchange of electron in the orbitals. The movement of electrons from one orbital to another can influence the oxidation number and reflects a definite to the elements of compounds.

Normally, Copper has no unpaired electron with filled D10 orbital therefore, it shows colourless appearance. In Cu[(NH3)4]2+, Copper gets an unpaired electron after the addition of ammonia and this gives a dark blue appearance to the overall ion.

Cu[(NH3)4]2+ Coordination number

Coordination n umber refers to the number of atoms coordinate or creates bonds with the other participated atom in the formation of the overall complex structure.

As four-ammonia compound, get attached with one Cu2+ ion which denotes the fact that the compound holds four coordination number. This complex ion has four strong ligands that is why it is considered as a stable coordination compound in the series.

Cu[(NH3)4]2+ Lewis structure

The number of valence electron present in Cu is 1 but in Cu2+ it becomes 9. Four NH3 compounds hold four Nitrogen atoms each of them has single lone pair after bonding with three Hydrogen molecules. Therefore, total number electrons present in four NH3 compounds are 8.

A partial sharing of electros between Cu2+ and NH3 compounds takes place to get stability. According to Lewis method of drawing, the structure of this compound Cu gets the centre position in the geometry.

The complete sketch of Lewis structure reveals that this compound creates covalent bonding as Cu is a metal and NH3 appears as a non-metal rather an Ionic compound. This structure is relevant one to represent the electronic arrangements and lack of electrons in the complex ion.

Cu[(NH3)4]2+ Reaction with HCl

Hydrochloric acid  (HCl) is a strong corrosive acid which reacts with the compounds easily. The reaction between this complex ion and HCl is kind of reaction which imposes a colour changing effect as a chemical property of the acid in reacting with ions.

HCl first gives out aqueous  solution of Tetraamine copper (II) in presence of oxygen. Then it gives excess Chlorince atom I th middle of the reaction. The balanced chemical equation is being shared below to describe its process and its cause of showing colour changing effect.

Cu[(NH3)4 (H2O)2]2+ + 4Cl = [CuCl]2- + 4NH3 + 2H2O

The Chlorine atom is added with the copper as strong presence of HCl breaks the ion. Another part of the complex ion that is NH3 (Ammonia) gets extracted from the compound. This is ligand displacement reaction as here the displacement of strong ligand Ammonia takes place in presence of strong acid.

The addition of Chloride ions with copper turns the dark blue colour of aqueous solution of Tetraamine copper (II) intro green colour. This happens due to the transition of electrons. However, after the displacement of  ammonia this change in the colour occurs Tetrachloro copper (II) complex and water molecule appear as the main product of this reaction.

Conclusion

This article has made a broad discussion on Tetraamine copper (II), one of the complex ion and coordination compound in Chemistry. The exceptional facts about this compound and its reaction with Hydrochloric acid have been explained in this article.

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XeO3 Lewis Structure

The XeO3 Lewis structure refers to the arrangement of atoms and electrons in the XeO3 molecule. Understanding the Lewis structure of XeO3 is crucial in comprehending its chemical properties and behavior. In this section, we will explore two important concepts related to the XeO3 Lewis structure: the Octet Rule and Resonance.

Octet Rule

The Octet Rule is a fundamental principle 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. Valence electrons are the electrons in the outermost energy level of an atom.

In the case of XeO3, Xenon (Xe) is the central atom, and it belongs to Group 18 of the periodic table, also known as the noble gases. Noble gases have a full octet of electrons in their outermost energy level, except for helium, which has only two electrons. Since Xenon has eight valence electrons, it can form bonds with other atoms to achieve a stable electron configuration.

Oxygen (O), on the other hand, belongs to Group 16 and has six valence electrons. To satisfy the Octet Rule, each oxygen atom needs two additional electrons to complete its octet.

Resonance

Resonance is a phenomenon that occurs when multiple Lewis structures can be drawn for a molecule, and the actual structure is a combination or hybrid of these resonance structures. Resonance structures are represented by double-headed arrows between them.

In the case of XeO3, resonance can be observed due to the presence of multiple oxygen atoms. Each oxygen atom can form a double bond with the central Xenon atom, resulting in a different arrangement of electrons. By drawing the resonance structures, we can visualize the different possibilities for electron distribution.

The resonance structures of XeO3 show that the double bonds can be delocalized, meaning that the electrons are not localized between specific atoms but are spread out over the molecule. This delocalization contributes to the stability of the molecule.

It is important to note that while resonance structures are used to represent the electron distribution in a molecule, the actual structure of XeO3 is a hybrid of these resonance structures.

In summary, the XeO3 Lewis structure follows the Octet Rule, with Xenon having eight valence electrons and each oxygen atom having a total of eight electrons. Additionally, resonance occurs in XeO3 due to the multiple oxygen atoms, resulting in a hybrid structure that contributes to the stability of the molecule. Understanding the XeO3 Lewis structure provides valuable insights into the chemical properties and behavior of this compound.

Structure of XeO3

XeO3, also known as xenon trioxide, is an inorganic compound composed of xenon and oxygen atoms. In this section, we will explore the structure of XeO3, including its Lewis structure, molecular geometry, VSEPR theory, and molecular shape.

Lewis Structure Formal Charge

The Lewis structure of a molecule provides a visual representation of the arrangement of atoms and electrons. It helps us understand the bonding and electron distribution within the molecule. In the case of XeO3, the Lewis structure can be determined by following a few steps.

1. Count the total number of valence electrons: Xenon (Xe) belongs to Group 18 of the periodic table, so it has 8 valence electrons. Oxygen (O) is in Group 16 and has 6 valence electrons each. Since there are three oxygen atoms in XeO3, the total number of valence electrons is 8 + (6 x 3) = 26.

2. Determine the central atom: In XeO3, xenon (Xe) is the central atom as it is less electronegative than oxygen.

3. Connect the atoms: Connect the central atom (Xe) to the surrounding oxygen atoms (O) using single bonds.

4. Distribute the remaining electrons: Distribute the remaining electrons around the atoms to satisfy the octet rule. In this case, xenon will have 8 electrons around it, while each oxygen atom will have 8 electrons as well.

The Lewis structure of XeO3 can be represented as:

O
|
Xe=O
|
O

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms in a molecule. In XeO3, the central xenon atom is surrounded by three oxygen atoms. The arrangement of these atoms gives rise to a specific molecular geometry.

The molecular geometry of XeO3 can be determined using the VSEPR (Valence Shell Electron Pair Repulsion) theory. According to this theory, electron pairs around the central atom repel each other and try to maximize their separation.

In XeO3, the central xenon atom has three bonding pairs and one lone pair of electrons. The repulsion between these electron pairs leads to a trigonal pyramidal molecular geometry. The three oxygen atoms are positioned around the central xenon atom, forming a pyramid-like shape.

Molecular Shape

The molecular shape of XeO3 is closely related to its molecular geometry. In this case, the molecular shape refers to the overall shape of the molecule, taking into account the positions of the atoms and the lone pairs of electrons.

Due to the trigonal pyramidal molecular geometry, XeO3 has a bent molecular shape. The three oxygen atoms are not symmetrically arranged around the central xenon atom, resulting in a bent shape.

To summarize, the Lewis structure of XeO3 shows the arrangement of atoms and electrons, while the molecular geometry and shape reveal the three-dimensional arrangement of atoms and lone pairs. Understanding the structure of XeO3 helps us comprehend its chemical properties and behavior in various reactions.

XeO4 2- Lewis Structure

The XeO4 2- ion is an interesting molecule with a unique Lewis structure. In this section, we will explore the Lewis structure of XeO4 2- and discuss its molecular geometry, shape, bond angles, hybridization, and valence electrons.

Lewis Structure

To understand the Lewis structure of XeO4 2-, we need to determine the total number of valence electrons in the molecule. Xenon (Xe) is a noble gas and has 8 valence electrons. Oxygen (O) has 6 valence electrons each. Since there are four oxygen atoms in XeO4 2-, the total number of valence electrons is:

8 (Xe) + 4 × 6 (O) + 2- (charge) = 32

To distribute these electrons, we start by placing the xenon atom in the center, surrounded by the four oxygen atoms. Each oxygen atom forms a single bond with the xenon atom, utilizing 2 valence electrons. This accounts for 8 electrons (4 × 2) out of the 32.

Next, we place the remaining 24 electrons as lone pairs on the oxygen atoms. Each oxygen atom can accommodate 3 lone pairs, which adds up to 12 electrons (4 × 3). This leaves us with 12 electrons to distribute.

To complete the Lewis structure, we place the remaining 12 electrons as lone pairs on the xenon atom. This gives us a total of 32 electrons, satisfying the octet rule for all atoms.

Molecular Geometry and Shape

The molecular geometry of XeO4 2- is tetrahedral. The xenon atom is at the center, with the four oxygen atoms arranged symmetrically around it. This arrangement results in a tetrahedral shape, where the bond angles between the xenon-oxygen bonds are approximately 109.5 degrees.

Hybridization

The hybridization of the xenon atom in XeO4 2- is sp3. In the formation of the bonds, the xenon atom hybridizes its 5p orbitals with one of its 5s orbitals. This results in four sp3 hybrid orbitals, which are used to form sigma bonds with the oxygen atoms.

Valence Electrons

XeO4 2- has a total of 32 valence electrons. These electrons are involved in the formation of chemical bonds and lone pairs, contributing to the stability and reactivity of the molecule.

Summary

In summary, the Lewis structure of XeO4 2- consists of a central xenon atom bonded to four oxygen atoms. The molecule has a tetrahedral shape, with bond angles of approximately 109.5 degrees. The xenon atom undergoes sp3 hybridization, forming sigma bonds with the oxygen atoms. XeO4 2- has a total of 32 valence electrons, which play a crucial role in its chemical behavior. Understanding the Lewis structure of XeO4 2- provides insights into its molecular properties and helps explain its reactivity in various chemical reactions.

XeO3 Polar

XeO3 is a chemical compound that consists of xenon (Xe) and oxygen (O) atoms. In order to understand whether XeO3 is polar or nonpolar, we need to examine its Lewis structure and molecular geometry.

Lewis Structure of XeO3

The Lewis structure of XeO3 helps us visualize the arrangement of atoms and electrons in the molecule. It is a diagram that shows the bonding and nonbonding electrons around the central atom, xenon.

To determine the Lewis structure of XeO3, we first need to know the total number of valence electrons in the molecule. Xenon is in Group 8 of the periodic table, so it has 8 valence electrons. Oxygen, on the other hand, is in Group 6, so each oxygen atom contributes 6 valence electrons. Since there are three oxygen atoms in XeO3, we have a total of 8 + 3(6) = 26 valence electrons.

Next, we arrange the atoms in the molecule, with xenon as the central atom and the oxygen atoms surrounding it. We then distribute the valence electrons around the atoms, making sure to satisfy the octet rule (where each atom wants to have 8 electrons in its outermost shell).

After distributing the electrons, we may find that there are still some electrons left. In the case of XeO3, we have 26 – 26 = 0 electrons remaining. This means that we have successfully distributed all the valence electrons.

XeO3 Molecular Geometry

The molecular geometry of XeO3 refers to the three-dimensional arrangement of atoms in the molecule. It is determined by the number of bonding and nonbonding electron pairs around the central atom.

In XeO3, xenon is surrounded by three oxygen atoms. Each oxygen atom forms a double bond with xenon, resulting in a total of six bonding electron pairs. Since there are no lone pairs of electrons on xenon, the electron pair geometry and molecular geometry are both trigonal planar.

XeO3 Bond Angles

The bond angles in XeO3 are the angles formed between the central atom (xenon) and the surrounding atoms (oxygen). In a trigonal planar molecular geometry, the bond angles are all equal. In the case of XeO3, the bond angles between xenon and oxygen are approximately 120 degrees.

XeO3 Polarity

To determine whether XeO3 is polar or nonpolar, we need to consider the molecular geometry and the polarity of the individual bonds.

In XeO3, the xenon-oxygen bonds are polar due to the difference in electronegativity between xenon and oxygen. Oxygen is more electronegative than xenon, which means it attracts the shared electrons in the bond more strongly. As a result, the oxygen atoms have a partial negative charge, while the xenon atom has a partial positive charge.

However, since XeO3 has a trigonal planar molecular geometry, the polarities of the individual bonds cancel out. This is because the bond dipoles are symmetrically arranged around the central atom, resulting in a nonpolar molecule overall.

In conclusion, XeO3 is a nonpolar molecule despite having polar bonds. This is due to the symmetric arrangement of the bond dipoles in the trigonal planar molecular geometry.

SeO3-2 Lewis Structure

The Lewis structure of SeO3-2, also known as selenite ion, can be determined by following a few simple steps. The Lewis structure helps us understand the arrangement of atoms and electrons in a molecule or ion. In the case of SeO3-2, we need to consider the valence electrons of selenium (Se) and oxygen (O) to draw the structure accurately.

To begin, let’s take a look at the valence electrons of each element involved. Selenium is in Group 6A of the periodic table, so it has six valence electrons. Oxygen, on the other hand, is in Group 6A as well and has six valence electrons. Since there are three oxygen atoms in SeO3-2, we have a total of 18 valence electrons to work with.

Now, let’s proceed with drawing the Lewis structure of SeO3-2:

1. Start by placing the selenium atom in the center. Since it is the least electronegative element, it tends to be the central atom in this molecule.

2. Next, arrange the oxygen atoms around the selenium atom. Remember that each oxygen atom should be bonded to the selenium atom.

3. Distribute the remaining valence electrons around the atoms to satisfy the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with eight valence electrons.

4. If there are any remaining valence electrons, place them on the central atom (in this case, selenium) to complete its octet.

By following these steps, we can draw the Lewis structure of SeO3-2. Here is the resulting structure:

Atom	Valence Electrons
Selenium (Se)	6
Oxygen (O)	6

In the Lewis structure of SeO3-2, selenium is surrounded by three oxygen atoms. Each oxygen atom is bonded to the selenium atom, and the remaining valence electrons are distributed around the atoms to satisfy the octet rule.

It is important to note that the Lewis structure only represents the arrangement of valence electrons and does not provide information about the actual shape or bond angles of the molecule. To determine the molecular geometry and bond angles of SeO3-2, we need to consider the concept of hybridization and the VSEPR theory, which stands for Valence Shell Electron Pair Repulsion theory.

XeO3 Lewis Structure Molecular Geometry

The XeO3 molecule is an interesting compound that exhibits a unique Lewis structure and molecular geometry. In this section, we will explore the Lewis structure of XeO3 and its corresponding molecular geometry.

Lewis Structure of XeO3

The Lewis structure of a molecule provides a visual representation of the arrangement of atoms and electrons within the molecule. It helps us understand the bonding and electron distribution in the compound. In the case of XeO3, we can determine its Lewis structure by following a few simple steps.

1. Count the total number of valence electrons: Xenon (Xe) belongs to Group 18 of the periodic table, so it has 8 valence electrons. Oxygen (O) has 6 valence electrons. Since there are three oxygen atoms in XeO3, we have a total of 8 + 6 * 3 = 26 valence electrons.

2. Determine the central atom: In XeO3, the xenon atom (Xe) is the central atom since it is less electronegative than oxygen.

3. Connect the atoms: Place the oxygen atoms (O) around the xenon atom (Xe) using single bonds.

4. Distribute the remaining electrons: Distribute the remaining valence electrons around the atoms to satisfy the octet rule. In the case of XeO3, we have 26 – 6 * 3 = 8 electrons left. Place these electrons as lone pairs on the oxygen atoms.

The final Lewis structure of XeO3 can be represented as follows:

O
|
O--Xe--O
|
O

Molecular Geometry of XeO3

The molecular geometry of a compound describes the three-dimensional arrangement of atoms in a molecule. It is determined by the arrangement of electron pairs around the central atom. In the case of XeO3, the central atom is xenon (Xe), and it is surrounded by three oxygen atoms (O).

To determine the molecular geometry of XeO3, we can use the valence shell electron pair repulsion (VSEPR) theory. According to this theory, electron pairs (both bonding and non-bonding) repel each other and try to stay as far apart as possible to minimize repulsion.

In XeO3, the xenon atom (Xe) has three bonding pairs and one lone pair of electrons. The presence of the lone pair affects the molecular geometry. The three oxygen atoms are arranged in a trigonal planar geometry around the xenon atom, with bond angles of approximately 120 degrees.

However, due to the presence of the lone pair, the molecular geometry of XeO3 is distorted from the ideal trigonal planar shape. The lone pair occupies more space than the bonding pairs, resulting in a bent or V-shaped molecular geometry. The bond angles between the oxygen atoms are slightly less than 120 degrees.

To summarize, the molecular geometry of XeO3 is bent or V-shaped, with bond angles slightly less than 120 degrees.

In conclusion, the Lewis structure of XeO3 reveals the arrangement of atoms and electrons in the molecule, while the molecular geometry describes the three-dimensional arrangement of atoms. Understanding the Lewis structure and molecular geometry of XeO3 helps us comprehend its chemical properties and behavior.

XeO3 VSEPR

The VSEPR (Valence Shell Electron Pair Repulsion) theory is a model used to predict the molecular geometry of a molecule based on the arrangement of its electron pairs. In the case of XeO3, which is the chemical formula for xenon trioxide, we can apply the VSEPR theory to determine its molecular geometry.

XeO3 consists of a central xenon atom bonded to three oxygen atoms. To understand the molecular geometry of XeO3, we need to consider the arrangement of the electron pairs around the central xenon atom.

According to the VSEPR theory, electron pairs repel each other and try to maximize their separation. This leads to different molecular geometries, such as linear, trigonal planar, tetrahedral, and so on.

In the case of XeO3, the xenon atom has three bonding pairs and one lone pair of electrons. The lone pair is not involved in bonding and occupies more space than the bonding pairs. As a result, the lone pair exerts a stronger repulsion on the bonding pairs, causing the molecule to adopt a specific molecular geometry.

To determine the molecular geometry of XeO3, we can use the AXE notation, where A represents the central atom (xenon), X represents the number of atoms bonded to the central atom (oxygen), and E represents the number of lone pairs on the central atom (xenon).

In the case of XeO3, the AXE notation is AX3E, indicating that there are three oxygen atoms bonded to the central xenon atom and one lone pair on the xenon atom.

Based on this AXE notation, we can determine that the molecular geometry of XeO3 is trigonal pyramidal. The three oxygen atoms are arranged in a triangular planar shape around the central xenon atom, and the lone pair occupies the fourth position, giving the molecule a pyramidal shape.

The molecular geometry of XeO3 can also be visualized using a Lewis structure. A Lewis structure is a diagram that represents the arrangement of atoms and electrons in a molecule. In the case of XeO3, the Lewis structure would show the xenon atom in the center, bonded to three oxygen atoms, and with one lone pair of electrons.

Overall, the VSEPR theory helps us understand the molecular geometry of XeO3, which is trigonal pyramidal. This knowledge is crucial in understanding the physical and chemical properties of XeO3 and its behavior in various reactions.

XeO3 Molecular Shape

The molecular shape of XeO3, or xenon trioxide, can be determined by examining its Lewis structure and electron geometry. The Lewis structure of XeO3 reveals the arrangement of atoms and lone pairs around the central xenon atom, while the electron geometry provides information about the overall shape of the molecule.

Lewis Structure of XeO3

To understand the molecular shape of XeO3, let’s first examine its Lewis structure. The Lewis structure of XeO3 can be determined by following a few simple steps:

1. Count the total number of valence electrons in the molecule. Xenon (Xe) is in Group 18 of the periodic table and has 8 valence electrons, while each oxygen (O) atom has 6 valence electrons. Therefore, the total number of valence electrons in XeO3 is 8 + 3(6) = 26.

2. Determine the central atom. In XeO3, xenon (Xe) is the central atom as it is less electronegative than oxygen (O).

3. Connect the central atom to the surrounding atoms using single bonds. In XeO3, xenon (Xe) forms single bonds with each oxygen (O) atom.

4. Distribute the remaining electrons as lone pairs around the atoms to satisfy the octet rule. In XeO3, xenon (Xe) has 2 lone pairs, while each oxygen (O) atom has 2 lone pairs.

The Lewis structure of XeO3 can be represented as follows:

O
|
O - Xe - O
|
O

Electron Geometry and Molecular Shape

The electron geometry of XeO3 is determined by considering both the bonded and lone pairs of electrons around the central xenon (Xe) atom. In XeO3, xenon (Xe) is surrounded by four electron domains – three single bonds and one lone pair.

Based on the electron domain geometry, XeO3 has a trigonal pyramidal shape. The three oxygen (O) atoms are positioned in a triangular arrangement around the central xenon (Xe) atom, while the lone pair occupies the fourth position, giving the molecule a pyramidal shape.

Bond Angles and Hybridization

The bond angles in XeO3 can be determined by examining the molecular shape. In a trigonal pyramidal molecule like XeO3, the bond angles between the central atom and the surrounding atoms are less than the ideal 109.5 degrees due to the presence of the lone pair.

In XeO3, the bond angles between the xenon (Xe) atom and the oxygen (O) atoms are approximately 103.5 degrees. This deviation from the ideal bond angle is a result of the repulsion between the lone pair and the bonding pairs.

The hybridization of the central xenon (Xe) atom in XeO3 can be determined by examining the electron domain geometry. Since XeO3 has four electron domains, the hybridization of xenon (Xe) is sp3. This means that the four orbitals of xenon (Xe) hybridize to form four sp3 orbitals, which are then used to form the sigma bonds with the oxygen (O) atoms.

In summary, the XeO3 molecule has a trigonal pyramidal shape, with bond angles of approximately 103.5 degrees and a hybridization of sp3 for the central xenon (Xe) atom. Understanding the molecular shape of XeO3 is crucial in predicting its chemical properties and reactivity.

How is the Lewis structure of XeO3 similar to SBr2?

The Lewis structure of XeO3, similar to sbr2 lewis structure and detailed facts, reveals some similarities between the two molecules. Both XeO3 and SBr2 are composed of a central atom (Xe and S, respectively) surrounded by three outer atoms (O and Br). In both structures, the central atom forms multiple bonds to the outer atoms, resulting in a trigonal planar molecular geometry. However, key differences lie in the electronegativity and valence electron counts of the atoms involved.

XeO3 Lewis and its Structure

XeO3, also known as xenon trioxide, is an interesting compound that exhibits a unique Lewis structure. In this section, we will explore the Lewis structure of XeO3 and delve into its molecular geometry, shape, bond angles, hybridization, and valence electrons.

Lewis Structure of XeO3

The Lewis structure of XeO3 represents the arrangement of atoms and valence electrons in the compound. It provides a visual representation of how the atoms are bonded and the distribution of electrons. To determine the Lewis structure of XeO3, we need to consider the valence electrons of each atom involved.

Xenon (Xe) is a noble gas and has a full octet of electrons in its outer shell. Oxygen (O), on the other hand, has six valence electrons. Since there are three oxygen atoms in XeO3, we have a total of 18 valence electrons from oxygen. Adding the 8 valence electrons from xenon, we have a total of 26 valence electrons.

To distribute these electrons, we start by placing a single bond between xenon and each oxygen atom. This accounts for 6 electrons (2 electrons for each bond). Next, we distribute the remaining 20 electrons as lone pairs around the oxygen atoms, ensuring that each oxygen atom has an octet of electrons. The Lewis structure of XeO3 can be represented as follows:

O
||
Xe--O
||
O

Molecular Geometry and Shape of XeO3

The molecular geometry of XeO3 is trigonal pyramidal. This means that the three oxygen atoms are arranged in a triangular shape around the central xenon atom, with one lone pair of electrons on each oxygen atom. The presence of the lone pairs causes a distortion in the shape, resulting in a pyramidal structure.

Bond Angles in XeO3

The bond angles in XeO3 refer to the angles formed between the central xenon atom and the surrounding oxygen atoms. In the case of XeO3, the bond angles are approximately 103.5 degrees. This angle is slightly less than the ideal tetrahedral angle of 109.5 degrees due to the repulsion between the lone pairs of electrons and the bonding pairs.

Hybridization in XeO3

The hybridization of XeO3 can be determined by examining the electron arrangement around the central xenon atom. In XeO3, the central xenon atom is surrounded by three oxygen atoms and one lone pair of electrons on each oxygen atom. This arrangement suggests that the xenon atom undergoes sp3 hybridization, forming four sp3 hybrid orbitals. Three of these orbitals are used for bonding with the oxygen atoms, while the fourth orbital contains the lone pair of electrons.

Valence Electrons in XeO3

The valence electrons in XeO3 are the electrons involved in bonding and determining the chemical properties of the compound. In XeO3, the xenon atom contributes 8 valence electrons, while each oxygen atom contributes 6 valence electrons. Adding these together, we have a total of 26 valence electrons in XeO3.

In conclusion, XeO3 exhibits a unique Lewis structure with a trigonal pyramidal molecular geometry. The bond angles are approximately 103.5 degrees, and the xenon atom undergoes sp3 hybridization. Understanding the Lewis structure and properties of XeO3 provides valuable insights into its chemical behavior and reactivity.

Frequently Asked Questions

Q: What is the Lewis structure of XeO3?

A: The Lewis structure of XeO3 shows that xenon (Xe) is the central atom bonded to three oxygen (O) atoms.

Q: How does the octet rule apply to the Lewis structure of XeO3?

A: The octet rule states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight valence electrons. In the Lewis structure of XeO3, xenon (Xe) has expanded its valence shell to accommodate more than eight electrons.

Q: Is there resonance in the Lewis structure of XeO3?

A: No, there is no resonance in the Lewis structure of XeO3. Resonance occurs when multiple valid Lewis structures can be drawn for a molecule, but in the case of XeO3, only one Lewis structure is possible.

Q: Can you explain the structure of XeO3?

A: The structure of XeO3 is trigonal pyramidal. It consists of a central xenon (Xe) atom bonded to three oxygen (O) atoms. The Xe-O bonds are arranged in a pyramid-like shape, with the xenon atom at the apex.

Q: What is the formal charge in the Lewis structure of XeO3?

A: In the Lewis structure of XeO3, the formal charge on xenon (Xe) is zero, while each oxygen (O) atom carries a formal charge of -1.

Q: What is the molecular geometry of XeO3?

A: The molecular geometry of XeO3 is trigonal pyramidal. It has a central xenon (Xe) atom bonded to three oxygen (O) atoms, with one lone pair of electrons on the xenon atom.

Q: How do you draw the Lewis structure of XeO4 2-?

A: The Lewis structure of XeO4 2- shows that xenon (Xe) is the central atom bonded to four oxygen (O) atoms. The overall charge of the molecule is -2.

Q: Is XeO3 a polar molecule?

A: Yes, XeO3 is a polar molecule. The presence of a lone pair on the central xenon (Xe) atom and the bent molecular geometry result in an uneven distribution of charge, making the molecule polar.

Q: How do you draw the Lewis structure of SeO3 2-?

A: The Lewis structure of SeO3 2- shows that selenium (Se) is the central atom bonded to three oxygen (O) atoms. The overall charge of the molecule is -2.

Q: What is the molecular geometry of XeO3 according to VSEPR theory?

A: According to VSEPR theory, the molecular geometry of XeO3 is trigonal pyramidal. The presence of one lone pair on the central xenon (Xe) atom leads to this molecular shape.

Q: How many valence electrons are there in XeO3?

A: XeO3 has a total of 26 valence electrons. Xenon (Xe) contributes 8 valence electrons, while each oxygen (O) atom contributes 6 valence electrons.

Also Read:

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Let us talk about FeCl3 lewis structure and 13 important characteristic features of FeCl3 in this article.

FeCl3 is the chemical formula of ferric chloride. The Central Fe is in a +3 oxidation state here. So, the Fe is named ferric. Cl is not here present as a counter ion also it acts as a ligand here, cause FeCl3 is a coordination compound rather than a covalent molecule. So, it has different coordination properties along with covalent properties. The molecular shape is trigonal planar but in coordination chemistry, it adopts octahedral geometry, the vacant site is filled with a water molecule causing ferric chloride to exist as a crystal form.

Cl here acts as a weak filed ligand, so no electrons in d orbital exist as paired form. It is a high spin complex. Fe(III) is a d⁵ system and all the electrons exist single spin only with no paired form. FeCl3 molecule can be fully ionized by charge separation of ferric and chloride.

1.    How to draw FeCl3 lewis structure?

Drawing of lewis structure of coordination compound is very difficult because it does not follow the general rule of the covalent molecule. Because this is a coordination molecule and it has some coordination property in it. Lewis dot structure can give us a proper picture of the molecular shape, valence electrons, etc. A few steps are there in the drawing of the lewis dot structure.

Step 1– At first, we count the valence d electrons for Fe and p electrons for Cl atoms and added together. In the FeCl3 lewis structure, the valence electrons for Fe are 5 as it is in a +3 oxidation state, and all the electrons from its d orbital only, for three Cl atoms is 7*3 = 21. So, the total valence electrons are 5+21 = 26.

Step 2 – Being a coordination compound FeCl3 will follow the 18 electron rule it is like the octet rule of a coordination molecule. The electrons that will be needed for the FeCl3 lewis dot structure will be 8 + (3*8) = 32 because the octet rule required 8 electrons in the valence shell for every atom. The available valence electrons are 26 from the previous calculation we get. Now the required electrons will be (32-26) = 6 electrons and the minimum number of bonds required that all the four atoms can be connected in this molecule is 6/2 = 3 bonds.

Step 3– Now time for choosing the central atom. Fe is here central atom as it is electropositive metal and its size is comparatively large. Because Fe is a transition metal and metal shows electro positivity where Cl is from the halogen group and it has more electronegativity.

Step 4 – Connect all the atoms with the central atom Fe via the minimum number of required single bonds i.e. three. So, Fe makes three single bonds with three Cl atoms from its d orbital electrons.

Step 5– Now calculate the number of lone pairs and their position of them. Fe is a group d element and it is +3 oxidation state in FeCl3 so it is a d⁵ system, and all the five electrons are present at the five subsets of the d orbital so it has no lone pairs. Cl belongs to the halogen family also it is group 17^th element and it has seven electrons in its valence shell and only one electron is involved in the bond formation so, the rest six electrons are assigned as three pairs of lone pairs. Three Cl atoms contain three pairs of lone pairs.

2.    FeCl3 lewis structure shape

The shape of any coordination molecule depends on the coordination number of the central metal atom. The structure may be varying cause some metal center can expand their coordination number. But in the covalent molecule, it depends on the VSEPR theory.

In FeCl3 lewis structure, Fe is +3 oxidation state, so it has 5 d electrons and this is the valence electrons for Fe(III). Now three Cl atoms, each contribute one electron, and all three contribute three electrons. Now total electrons count for the FeCl3 lewis structure will be 5+3 =8 electrons. According to the VSEPR (Valence Shell Electrons Pair Theory), the molecule AX₃ adopts tetrahedral geometry having lone pair over the central atom if the electrons count will be 8. Again, from coordination chemistry, the molecule will be tetrahedral if the coordination number will be 4.

But here the scenario is different. Neither the coordination number of Fe(III) is 4 nor does it contain any lone pairs. So, the shape is decided by the surrounding atoms and there are three surrounding atoms present and the best acceptable shape will be trigonal planar.

3.    FeCl3 valence electrons

Although FeCl3 is a coordination compound it has also valence electrons. Fe and Cl separately have a certain number of valence electrons. There will be some electrons present in the outermost orbital or valence orbital of Fe and Cl atoms.

Iron is a 4th-period element. It is also a d block element which means the outermost orbital of Fe is the d orbital. In the FeCl3 lewis structure, Fe is +3 oxidation state, so its electronic configuration becomes 3d⁵. So, it has five electrons in its d orbital. D has five subsets and Cl is a weak field ligand. So, every subset contains one unpaired electron. So, iron has five valence electrons.

Now for Cl, it belongs to the halogen family that is group 17^th element. So, naturally, it has seven electrons in the valence shell. Three Cl atoms have 3*7 =21 valence electrons.

So, the total number of valence electrons in the FeCl3 lewis structure is 5+21=26 electrons.

4.    FeCl3 lewis structure formal charge

Each molecule has a formal charge may be the value will be zero for a neutral covalent molecule but there is some value over a particular ion if that ion possesses ionic character. Even in coordination molecule also shows the formal charge.

The formula we can use to calculate the formal charge of any covalent or coordination molecule 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 or outermost orbital, 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.

Remind that we always consider the same electronegativity for atoms to calculate the formal charge of a molecule.

In the FeCl3 lewis structure, we have to calculate the formal charge separately for Fe and Cl.

The formal charge over Fe is, 6-0-(6/2) =+3

Iron has a 3d6 system in transition metal cause 4s electrons we cannot consider due to strong ionization energy.

The formal charge over Cl is, 7-6-(2/2) = 0

This result implies that Fe is in a +3 oxidation state which means it has a +3 charge over it and the formal charge also Fe is +3 here.

So, we can conclude that formal charge also predicts the ionic nature or amount of charge of every single atom in a particular molecule.

5.    FeCl3 lewis structure angle

In a covalent molecule bond angle depends on the VSEPR theory or hybridization value but in coordination com pound bond angle depends on the coordination number of a central metal atom or several ligands present in it.

In the FeCl3 lewis structure, there are three ligands present surrounding the Fe center. So, the geometry according to one metal center and three surrounding ligands will be trigonal planar is perfect. All the ligands have the same and equivalent so no need to adjust their position by changing the bond angle. We know that the bond angle of a trigonal planar geometry shape is 120⁰.

So here the Cl-Fe-Cl bond angle is expected to be 120⁰. The lone pairs over Cl are not a problematic situation here so no need for the deviation of bond angle. Again, Cl is weak filed ligand, so Fe is high spin here and the geometry and bond angle are solely decided from the ligand site only and the bond angle is 120⁰.

6.    FeCl3 lewis structure octet rule

Every atom will follow the octet rule and try to complete its valence shell after the bond formation in a covalent molecule. But in coordination compound will follow the 18 electrons rule. It is like the octet rule of the organometallic complex.

In the FeCl3 lewis structure, Cl is halogen so it has completed its octet by accepting one electron in its valence shell as it has already seven electrons in it. During the bond formation with Fe, one electron from Cl and one d electron from Fe site share to form a covalent or coordination bond. Thus, the Cl atom completes its octet.

But in the case of Fe, it is a d block transition element, so it should follow the 18 electron rule rather than an octet. In FeCl3 lewis structure, Fe is in a +3 oxidation state so it has 5 d electrons in its valence shell and accepts 3 more electrons from three Cl atoms via sharing to complete its octet. Fe has 26 electrons and deducted from 18 electrons rule it ahs 8 electrons and this is how it can complete its octet.

7.    FeCl3 lewis structure lone pairs

In the FeCl3 lewis structure, there are only present lone pairs over 3 Cl atoms only. Fe does not contain any lone pair. The valence electrons of Fe are 4s orbital and after bond formation, the electrons of d orbital did not participate in the valence shell.

Being halogen Cl belongs to group 17^th. So, it has seven electrons in the outermost 3s and 3p orbitals. But after the bond formation, there are six electrons present and they exist as three pairs of lone pairs (one in 3s orbital and the other two in 3p orbital).

But in the case of Fe, the outermost orbital is 4s, but in Fe(III) the valence shell is 3d, where five electrons are present in five different subsets. After the bond formation with three Cl atoms rests two electrons do not pair up because of the higher exchange energy of the 3d orbital, so Fe does not contain lone pairs.

8.      FeCl3 lewis structure resonance

For resonance, we need the electron-rich center or any atom which contains more electrons clouds that can be delocalized in different skeletons of that particular molecule. Both are absent in the case of FeCl3 lewis structure.

In the FeCl3 lewis structure, Fe is d block metal so it possesses a positive charge, so it is lack electron density. Again, Cl is more electronegative so it cannot release the electron density from it. So there is no resonance occurs in the FeCl3 lewis structure.

9.    FeCl3 hybridization

For any coordination molecule, it is very difficult to find out its state of hybridization. Because they are violated valence bond theory. So, we cannot find out the hybridization of such a compound.

But if we consider its shape so it can say that as it adopts trigonal planar structure then it should be sp² hybridized. But Fe is a 3d element so it does not has 3s orbital form bond formation. So, we consider the 4s and 4p orbital here.

If we use the typical formula for the calculation of hybridization, H = 0.5(V+M-C+A),

H = ½(3+3+0+0) =3 (sp²), Fe has three electrons apart from five electrons from the d orbital and three Cl atoms are present. From VSEPR theory if the number of orbitals mixed in hybridization is 3 then it is sp² hybridized.

As 4s and 4p orbitals are involved here so it is called the outer orbital complex.

Lets us draw and understand the hybridization of the FeCl3 lewis structure.

So, from the box diagram, we can say that the s and p orbitals which are involved in the hybridization are 4s and 4p, and outer electrons only contribute so the complex is the outer orbital complex.

10.    FeCl3 solubility

Fecle3 is soluble in the following solution,

• Water
• Ethanol
• Methanol
• Acetone
• diethyl ether

11.    Is FeCl3 ionic?

Yes, FeCl3 is an ionic molecule, as it is a coordination compound but it can be ionized as Fe³⁺ and Cl^–. So FeCl3 lewis structure is an ionic molecule.

12.    Is FeCl3 acidic or basic?

FeCl3 is a good Lewis acid. In the FeCl3 lewis structure, we can see that Fe is +3 oxidation state and it has five electrons in the d orbital and the highest number of electrons accumulated by the d orbital is 10. So, it can accept electrons in its d orbital so it acts as lewis acid.

13.    Is Fecl3 polar or nonpolar?

FeCl3 is a polar molecule. Most of the ionic molecules will be polar and FeCl3 is ionic so it has polarity. The electronegativity difference between Fe and Cl is very high so there is a dipole moment generated and it makes polar.

14.    Is FeCl3 tetrahedral?

No, FeCl3 is not tetrahedral, because there are no lone pairs on the  Fe center. It is a trigonal plannar shape.

15.      Is FeCl3 linear?

No, FeCl3 is not linear it is a trigonal planar shape. In the lattice crystal, it is octahedral.

Conclusion

FeCl3 is a coordination compound rather than a covalent molecule. It has coordination property and Cl is not a counter ion here it is a weak filed ligand thus it makes the bond with a higher oxidation state of Fe like Fe(III).

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• Asbr3 lewis structure
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• Pcl3 lewis structure
• Bi3 lewis structure

In this article, we look into the sbh3 lewis structure, shape, formal charge and its hybridization.

SbH3 has three single bonds between the Antimony atom and each Hydrogen atom in its Lewis structure. The Antimony (Sb) atom is in the centre, surrounded by three Hydrogen atoms (H). The antimony atom have a one electron pair.

SbH₃ is a colourless, flammable gas that smells like rotten eggs. It is a severely hazardous heavy antimony counterpart of ammonia. Because SbH₃ is extremely unstable, it is seldom found outside of labs.

1. How to draw Lewis structure for SbH₃?

Steps to Draw the Lewis Structure of SbH3 as follows:

Step 1: Determine how many valence electrons there are in total

To draw the Lewis structure of SbH3, you must first figure out how many valence electrons there are in the molecule.

Valence electron calculations in SbH₃:

Antimony is a periodic table group 15 element. As a result, antimony has 5 valence electrons.

On the periodic chart, hydrogen belongs to group 1.

As a result, the valence electron in hydrogen is 1.

In the SbH₃ molecule, the total amount of Valence electrons is 5 + 1(3) = 8.

Step 2: Select the centre atom and keep H always outside

Always place the least electronegative atom in the centre when choosing the centre atom.

The hydrogen in the SbH₃ molecule is less electronegative than antimony. We must, however, keep hydrogen outdoors due to legal requirements. As a result, antimony should be positioned in the centre, surrounded by the remaining three hydrogen atoms.

Step 3: Place the two electrons between the atoms to illustrate the chemical bond

Place two electrons between each antimony atom and hydrogen atom to show a chemical bond.

Step 4: Complete the octet on each atoms

Each hydrogen and antimony atom should have eight electrons around it. As a result, the construction must be stable.

Step 5: Check the stability of Lewis structure by calculating the formal charge on each atom

The formula for the calculation of the formal charge as follows:

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

Antimony contains five Valence electrons, two Nonbonding electrons and six Bonding electrons

Hydrogen contains one Valence electron, zero Nonbonding electrons and two Bonding electrons.

The formal charge on antimony is found to be zero.

The formal charge on hydrogen is zero.

2. SbH₃ Lewis structure shape:

In order to find out Shape, consider only bond pair of electrons but for Geometry, need to consider lone pair of electrons along with bond pairs. The shape of the SbH3 molecule is Trigonal pyramidal.

3. SbH₃ Lewis structure formal charges:

The formula for the calculation of the formal charge as follows:

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

Antimony contains five Valence electrons, two Nonbonding electrons and six Bonding electrons

Hydrogen contains one Valence electron, zero Nonbonding electrons and two Bonding electrons.

The formal charge on antimony is found to be zero.

The formal charge on hydrogen is zero.

4. SbH₃ Lewis structure lone pairs:

In SbH3 Lewis structure, antimony has 5 valence electrons and each hydrogen has one valence electron. The central atom antimony has one lone pair of electrons.

5. SbH₃ hybridization:

The hybridization of SbH₃ molecule is found to be sp³.

6. SbH₃ Lewis structure octet rule:

The octet rule asserts that atoms gain, lose, or share electrons to establish a stable electron configuration with eight valence electrons while producing compounds. In the Lewis structure of SbH3, all of the atoms have fulfilled their octet number of electrons.

Conclusion:

In the above article, we studied about Lewis structure of Stibine molecule and its shape, hybridization, lone pairs, octet rule, formal charge calculation.

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• Ibr3 lewis structure
• Xebr2 lewis structure
• Nah lewis structure
• Xef4 lewis structure
• Brf5 lewis structure
• Sno2 lewis structure
• Hco2 lewis structure
• Gef4 lewis structure
• N2o3 lewis structure
• Sp3 lewis structure