Chapter 22, Problem 22.43QP

Interpretation Introduction

Interpretation:

Oxidation number of  transition metal in each of the following compounds has to be determined.

(a) $\left[Co{\left(N{O}_2\right)}_3{\left(N{H}_3\right)}_3\right]$ (b) $\left[Ni{\left(N{H}_3\right)}_4{\left(H_{2}O\right)}_2\right]{\left(N{O}_3\right)}_2$

(c) ${\left[Pt{\left(en\right)}_2\right]}^{2+}$ (d) $N{a}_3\left[CoC{l}_6\right]$

Concept Introduction:

Oxidation number of an element refers to the charge it carries in its elemental state and in its compounds.

Some of the rules for assigning oxidation number to an element are stated below -

• Oxidation number of an element in its pure elemental form is zero. 
• Oxidation number of a mono atomic ion is equivalent to charge of the mono atomic ion.
• Oxidation number of Fluorine is always $1.$
• Sum of oxidation numbers of all atoms in a neutral compound becomes zero.