Chapter 4.5 Oxidation - Reduction (redox) Reactions

Question 1

oxidation

Answer 1

the loss of electrons

Question 2

reduction

Answer 2

the gain of electrons

Question 3

oxidizing agent

Answer 3

the species doing the oxidizing (causing the electron loss)

Question 4

reducing agent

Answer 4

the species doing the reducing (causing the electron gain)

Question 5

oxidation number (oxidation state)

Answer 5

the charge the atom would have if electrons were transferred completely, not shared

Question 6

General rules for assigning an oxidation number (O.N.) (3)

Answer 6

1. For an atom in its elemental form, O.N. = O
2. For a monoatomic ion, O.N. = ion charge (sign before numeral)
3. The sum of O.N. values for the atoms in a molecule or formula unit of a compound equals zero. The sum O.N. values for the atoms in a polyatomic ion = the ions charge

Question 7

Rules for Specific Atoms: Group 1A

Answer 7

O.N. = +1 in all compounds

Question 8

Rules for Specific Atoms: Group 2A

Answer 8

O.N. = +2 in all compounds

Question 9

Rules for Specific Atoms: Hydrogen

Answer 9

O.N. = +1 in combination w/ nonmetals
O.N. = -1 in combination w/ metals and boron

Question 10

Rules for Specific Atoms: Fluorine

Answer 10

O.N. = -1 in all compounds

Question 11

Rules for Specific Atoms: Oxygen

Answer 11

O.N. = -1 in peroxides (two oxygens covalently bonded together, ex. H2O2)
O.N. = -2 in all other compounds (except w/ Fluorine)

Question 12

Rules for Specific Atoms: Group 7A

Answer 12

O.N. = -1 in combinations w/ metals, nonmetals (except O), all other halogens lower in the group