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Chapter 14: Problem 11

What is an oxidation number?

Short Answer

Expert verified
An oxidation number represents the degree of oxidation of an atom in a compound, and it's the hypothetical charge an atom would have if all bonds to atoms of different elements were 100% ionic. The method to calculate depends on the state of the atom and its bonding conditions.

Step by step solution

01

Understanding Oxidation Number

The oxidation number denotes the degree of oxidation of an atom in a chemical compound. It represents the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic.
02

Procedure to Calculate Oxidation Number

The oxidation number of an atom is lait calculates as follows: 1. The oxidation number of an atom in its elemental state is always zero. 2. The oxidation number of an ion equals the charge of the ion. 3. Hydrogen generally has an oxidation number of +1. Oxygen generally has an oxidation number of -2. 4. The sum of the oxidation numbers of all atoms in a neutral molecule equals zero, while in an ion it equals the ionic charge.
03

Providing Examples

Let's provide a couple of examples: 1. In H2O, the oxidation number of each H (Hydrogen) is +1 and that of O (Oxygen) is -2. 2. In NaCl, the oxidation number of Na (Sodium) is +1 and that of Cl (Chloride) is -1.

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Most popular questions from this chapter

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Algae in swimming pools is sometimes treated by adding \(\mathrm{CuSO}_{4}\) as a fungicide. Copper sulfate can be prepared by the addition of hot \(\mathrm{H}_{2} \mathrm{SO}_{4}\) to \(\mathrm{Cu}\) metal. $$ \mathrm{Cu}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{SO}_{2}(g) $$ Balance this equation, adding \(\mathrm{H}^{+}(a q)\) and \(\mathrm{H}_{2} \mathrm{O}(l)\) as necessary.

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In the following oxidation-reduction reactions, identify the oxidizing agent, the reducing agent, and the number of electrons transferred. (a) \(6 \mathrm{I}^{-}(a q)+\mathrm{BrO}_{3}^{-}(a q)+6 \mathrm{H}^{*}(a q) \longrightarrow\) \(3 \mathrm{I}_{2}(a q)+\mathrm{Br}^{-}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l)\) (b) \(5 \mathrm{Br}^{-}(a q)+\mathrm{BrO}_{3}^{-}(a q)+6 \mathrm{H}^{*}(a q) \underset{3 \mathrm{Br}_{2}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l)}{\longrightarrow}\) (c) \(\mathrm{XeF}_{4}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Xe}(g)+4 \mathrm{HF}(a q)+\mathrm{O}_{2}(g)\) (d) \(\mathrm{Pb}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Pb}^{2+}(a q)+\mathrm{H}_{2}(g)\)

Determine which of the following represent oxidationreduction reactions. For reactions that involve oxidationreduction, determine the oxidizing and reducing agents. (a) \(2 \mathrm{Na}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_{2}(g)\) (b) \(\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{HF}(g)\) (c) \(\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) (d) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{NaCl}(a q) \longrightarrow\) \(\mathrm{PbCl}_{2}(s)+2 \mathrm{NaNO}_{3}(a q)\) (e) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)\)
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