Chemistry
Chemistry
4th Edition
ISBN: 9780393919370
Author: Thomas R. Gilbert
Publisher: NORTON
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Chapter 9, Problem 9.65QP
Interpretation Introduction

Interpretation: The Lewis structure and shape of the given compound, the hybridization of the central atom and the resonating structure that has formal charge close to zero is to be identified.

Concept introduction: The Lewis structure represents all bonding and non-bonding electrons surrounding the atoms involved in a molecule. A molecule exhibits a particular geometry in space considering the steric hindrances of the bond pairs and the lone pairs of electron.

Resonance structures are different forms of a molecule in which the chemical connectivity of the atoms in a molecule is same but there distribution of electrons is different.

The formal charge is calculated by the formula,

Formalcharge=[(Numberofvalenceelectrons)(Numberofnonbondingelectronsaroundtheatom)12(Numberofbondingelectronsaroundtheatom)]

To determine: The Lewis structure and shape of the given compound, the hybridization of the central atom and the resonating structure that has formal charge close to zero.

Expert Solution & Answer
Check Mark

Answer to Problem 9.65QP

Solution

The Lewis structure of ClO4 is figure 1.

The resonating structure I has formal charge close to zero.

The shape of the molecule is tetrahedral and the hybridization of the chlorine is sp3d3

Explanation of Solution

Explanation

The atomic number of Cl is 17 .

The electronic configuration of Cl is,

[Ne]3s23p5

The number of valence electrons of Cl is 7 .

The atomic number of O is 8 .

The electronic configuration of O is,

1s22p22p4

The number of valence electrons of O is 6 .

The total number of valence electrons of ClO4 is,

7+4×6+1=32

The Lewis structure of ClO4 is,

Chemistry, Chapter 9, Problem 9.65QP , additional homework tip  1

Figure 1

Resonance structures are different forms of a molecule in which the chemical connectivity of the atoms in a molecule is same but there distribution of electrons is different.

The resonance structure of ClO2 is,

Chemistry, Chapter 9, Problem 9.65QP , additional homework tip  2

Figure 2

The formal charge is calculated by the formula,

Formalcharge=[(Numberofvalenceelectrons)(Numberofnonbondingelectronsaroundtheatom)12(Numberofbondingelectronsaroundtheatom)]

According to the I resonating structure of the given compound from figure 2,

  • Chlorine has fourteen bonding and zero nonbonding electrons.
  • Oxygen (a) has four bonding electrons and four nonbonding electrons.
  • Oxygen (b) has two bonding and six nonbonding electrons.
  • Oxygen (c) has four bonding electrons and four nonbonding electrons.
  • Oxygen (d) has four bonding and four nonbonding electrons.

The formal charge of chlorine in resonating structure 1 is calculated as,

Formalcharge=[(7)(0)12(14)]=0

The formal charge of oxygen (a) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(4)]=0

The formal charge of oxygen (b) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(2)]=1

The formal charge of oxygen (c) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(4)]=0

The formal charge of oxygen (d) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(4)]=0

According to the II resonating structure of the given compound from figure 2,

  • Chlorine has twelve bonding and zero nonbonding electrons.
  • Oxygen (a) has two bonding electrons and six nonbonding electrons.
  • Oxygen (b) has two bonding and six nonbonding electrons.
  • Oxygen (c) has four bonding electrons and four nonbonding electrons.
  • Oxygen (d) has four bonding and four nonbonding electrons.

The formal charge of chlorine in resonating structure 1 is calculated as,

Formalcharge=[(7)(0)12(12)]=+1

The formal charge of oxygen (a) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(2)]=1

The formal charge of oxygen (b) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(2)]=1

The formal charge of oxygen (c) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(4)]=0

The formal charge of oxygen (d) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(4)]=0

According to the II resonating structure of the given compound from figure 2,

  • Chlorine has fourteen bonding and zero nonbonding electrons.
  • Oxygen (a) has four bonding electrons and six nonbonding electrons.
  • Oxygen (b) has two bonding and six nonbonding electrons.
  • Oxygen (c) has four bonding electrons and six nonbonding electrons.
  • Oxygen (d) has four bonding and four nonbonding electrons.

The formal charge of chlorine in resonating structure 1 is calculated as,

Formalcharge=[(7)(0)12(14)]=0

The formal charge of oxygen (a) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(6)]=1

The formal charge of oxygen (b) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(2)]=1

The formal charge of oxygen (c) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(4)]=2

The formal charge of oxygen (d) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(4)]=0

According to the IV resonating structure of the given compound from figure 2,

  • Chlorine has ten bonding and zero nonbonding electrons.
  • Oxygen (a) has two bonding electrons and six nonbonding electrons.
  • Oxygen (b) has two bonding and six nonbonding electrons.
  • Oxygen (c) has two bonding electrons and six nonbonding electrons.
  • Oxygen (d) has four bonding and four nonbonding electrons.

The formal charge of chlorine in resonating structure 1 is calculated as,

Formalcharge=[(7)(0)12(10)]=+2

The formal charge of oxygen (a) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(2)]=1

The formal charge of oxygen (b) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(2)]=1

The formal charge of oxygen (c) in resonating structure 1 is calculated as,

Formalcharge=[(6)(6)12(2)]=1

The formal charge of oxygen (d) in resonating structure 1 is calculated as,

Formalcharge=[(6)(4)12(4)]=0

Resonating structure 1 has formal charge close to zero

The molecular shape of ClO2 is tetrahedral

From the resonating structure I it is concluded that the chlorine atom forms three pi bonds this means it uses three p orbitals, and the four sigma bonds are formed with three d orbitals and one s orbitals. Therefore, the hybridization of central atom chlorine in resonating structure I is sp3d3 .

Conclusion

The Lewis structure of ClO4 is figure 1.

The resonating structure I has formal charge close to zero.

The shape of the molecule is tetrahedral and the hybridization of the chlorine is sp3d3

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Chapter 9 Solutions

Chemistry

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