Chemistry
Chemistry
13th Edition
ISBN: 9781259911156
Author: Raymond Chang Dr., Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 10, Problem 10.120QP

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of the carbon monoxide and its corresponding formal charges should be drawn.  The bond order of carbon monoxide with that of molecular orbital theory should be compared.  Also to found out which atom of carbon monoxide forms bond with Fe2+ of hemoglobin.

Concept Introduction:

  • Lewis structures which also known as Lewis dot structures represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.
  • A formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.
  • Formal charge of an atom can be determined by the given formula.

Formalcharge(FC)=(no.ofvalenceelectroninatom)12(no.ofbondingelectrons)(no.ofnon-bondingelectrons)

  • Dipole moment occurs when there is a difference in the electronegativity of atoms in a bond which results in charge separation.

(a)

Expert Solution
Check Mark

Answer to Problem 10.120QP

  1. (a) Lewis structure of the carbon monoxide and its corresponding formal charges is Chemistry, Chapter 10, Problem 10.120QP , additional homework tip  1
  2. (c) It was found out that carbon atom of carbon monoxide forms bond with Fe2+ of hemoglobin.

Explanation of Solution

Given molecule is CO.

Lewis structure of carbon monoxide is drawn below.

Chemistry, Chapter 10, Problem 10.120QP , additional homework tip  2

  • The total number of valence electrons is found to be 10, where carbon and oxygen atom contribute 4 and 6 electrons respectively.

The 8 electrons getting after reducing two electrons for each bond from the total valence electron are distributed on atom to complete the octet. After the distribution of electrons, atoms does not obey octet rule so triple bond is formed carbon and oxygen atoms.

The formal charge carbon monoxide

Chemistry, Chapter 10, Problem 10.120QP , additional homework tip  3

The formal charge carbon monoxide is calculated,

  • Carbon atom

Number of valenceelectron=4Number of bondingelectron=6Number of non-bondingelectron=2

Substituting these values to the equation,

FC=4-(12×6)-2=-1

  • Oxygen atom (a)

 Number of valenceelectron=6Number of bondingelectron=6Number of non-bondingelectron=2

Substituting these values to the equation,

FC=6-(12×6)-2=+1

Due to the difference in the electronegativity of carbon and oxygen atoms, the C-O bond is polar. So carbon atom gets a partial positive charge whereas oxygen atoms gets partial negative charge which means concentration of electron density is expected to have on oxygen atom. After calculating the formal charges, the negative charge is assigned on the carbon atom. Thus carbon monoxide is expected to have low dipole moment.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of the carbon monoxide and its corresponding formal charges should be drawn.  The bond order of carbon monoxide with that of molecular orbital theory should be compared.  Also to found out which atom of carbon monoxide forms bond with Fe2+ of hemoglobin.

Concept Introduction:

  • Lewis structures which also known as Lewis dot structures represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.
  • A formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.
  • Formal charge of an atom can be determined by the given formula.

Formalcharge(FC)=(no.ofvalenceelectroninatom)12(no.ofbondingelectrons)(no.ofnon-bondingelectrons)

  • Dipole moment occurs when there is a difference in the electronegativity of atoms in a bond which results in charge separation.

In molecular orbital theory, when the bonding takes place the atomic orbitals that take part combine to get a new orbital that has the properties of the whole molecule. The newly formed orbitals are known as molecular orbitals and only contain a maximum of two electrons. The number of newly formed molecular orbital is equal to the number of atomic orbitals involved in the bonding.

There are two types of molecular orbitals,

  1. a) Bonding molecular orbitals: sharing of electron density is between the nuclei and has comparatively lower energy and fills first.
  2. b) Antibonding molecular orbitals: Two nuclei are pulled by the electrons density in opposite direction and have higher energy comparing to bonding molecular orbital.

(b)

Expert Solution
Check Mark

Explanation of Solution

Total number of electrons in carbon monoxide is 14 where carbon and oxygen atom have 6 and 8 electrons respectively.

Electronic configuration of CO is (σ1s)2(σ1s*)2(σ2s)2(σ2s*)2(π2px)2(π2py)2(σpz)2.

The bond order of CO is determined.

The bond order gives an idea about the stability of a molecule. It can be calculated using the molecular orbital theory. The stability of a molecule increase as the bond order increases.

Bond order =(No.ofe-inbondingorbitals)-(No.ofe-inantibondingorbitals)2

No.ofe-inbondingorbitals=8No.ofe-inantibondingorbitals=2

Bondorder=12(8-2)=3

The bond order of CO is 3 which is similar to the triple bond that drawn in Lewis structure. CO and N2 is isoelectronic which means they  have same number of valence electrons and atoms.

Conclusion

The bond order of carbon monoxide with that of molecular orbital theory was compared.

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of the carbon monoxide and its corresponding formal charges should be drawn.  The bond order of carbon monoxide with that of molecular orbital theory should be compared.  Also to found out which atom of carbon monoxide forms bond with Fe2+ of hemoglobin.

Concept Introduction:

  • Lewis structures which also known as Lewis dot structures represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.
  • A formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.
  • Formal charge of an atom can be determined by the given formula.

Formalcharge(FC)=(no.ofvalenceelectroninatom)12(no.ofbondingelectrons)(no.ofnon-bondingelectrons)

  • Dipole moment occurs when there is a difference in the electronegativity of atoms in a bond which results in charge separation.

(c)

Expert Solution
Check Mark

Answer to Problem 10.120QP

  1. (d) It was found out that carbon atom of carbon monoxide forms bond with Fe2+ of hemoglobin.

Explanation of Solution

Fe2+ is the metal presence in hemoglobin. When carbon monoxide enters the blood stream Fe2+ cation forms bond with a negatively charged atom. Carbon monoxide is a neutral compound. While calculating the formal charge of CO, it is found that carbon has negative charge. So Fe2+ tend to make bond with carbon atom (OC-Fe2+) instead of oxygen atom (CO-Fe2+).

Conclusion

The Lewis structure of the carbon monoxide and its corresponding formal charges was drawn. Also it was found out that carbon atom of carbon monoxide forms bond with Fe2+ of hemoglobin.

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