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Chapter 49: Problem 2

In which of the following are the oxidation number and the partial charge the same number? \(\mathrm{MgO} ; \mathrm{CO}_{2} ; \mathrm{NaF} ; \mathrm{H}_{2} \mathrm{O} ; \mathrm{CCl}_{4} ; \mathrm{NiCl}_{2}\).

Short Answer

Expert verified
In MgO, NaF, and NiCl2 the oxidation number and the partial charge are the same.

Step by step solution

01

Analysis of MgO

In MgO, the oxidation number of Mg is +2 and O is -2. There are no polar bonds in MgO hence, there is no charge separation and no partial charges are found. Therefore, in MgO, the oxidation number and the partial charge are the same.
02

Analysis of CO2

In CO2, the oxidation number of C is +4 and O is -2. There are polar bonds in CO2, however, due to its linear molecular geometry, the partial charges cancel out resulting in no net partial charge. Therefore, in CO2, the oxidation number and the partial charge are not the same.
03

Analysis of NaF

In NaF, the oxidation number of Na is +1 and F is -1. There are no polar bonds in NaF, hence there is no charge separation and no partial charges are found. Therefore, in NaF, the oxidation number and the partial charge are the same.
04

Analysis of H2O

In H2O, the oxidation number of H is +1 and O is -2. In H2O, the atoms have partial charges due to the polar nature of the O-H bonds and the bent geometry of the molecule does not allow these partial charges to cancel out. Therefore, in H2O, the oxidation number and the partial charge are not the same.
05

Analysis of CCl4

In CCl4, the oxidation number of C is -4 and Cl is +1. In CCl4, the atoms have partial charges due to the polar nature of the C-Cl bonds, however, due to its tetrahedral molecular geometry, the partial charges cancel out resulting in no net partial charge. Therefore, in CCl4, the oxidation number and the partial charge are not the same.
06

Analysis of NiCl2

In NiCl2, the oxidation number of Ni is +2 and Cl is -1. There are no polar bonds in NiCl2, hence there is no charge separation and no partial charges are found. Therefore, in NiCl2, the oxidation number and the partial charge are the same.

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Most popular questions from this chapter

Describe, in grammatically correct English sentences, how one can determine whether or not a reaction is an oxidation-reduction reaction.

Which is the better representation of the actual charge on an atom in a moleculethe formal charge; the partial charge; the oxidation state? Why?

Is a species that has an atom for which there is an increase in oxidation number oxidized or reduced? Is that species the oxidizing agent or the reducing agent?
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