Formulation and Nomenclature in Inorganic Chemistry
1. Oxidation Numbers
Definition:
An integer representing the ability of an element to combine with another element. Hydrogen, with
an oxidation number of +1, is used as the reference.
Electron Exchange:
The oxidation number represents the number of electrons an atom gains or loses (partially or fully)
when forming a compound.
- Negative oxidation number: The atom gains electrons.
- Positive oxidation number: The atom loses electrons.
- Metals generally have positive oxidation numbers, while non-metals have negative ones.
Examples:
1. Fluorine (F):
Fluorine has an oxidation number of -1 because it gains one electron to achieve a noble gas
configuration.
F (Z = 9): 1s^2 2s^2 2p^5
2. Magnesium (Mg):
Magnesium has an oxidation number of +2 because it loses two electrons to reach a noble gas
configuration.
Mg (Z = 12): 1s^2 2s^2 2p^6 3s^2
Page 1
1. Oxidation Numbers
Definition:
An integer representing the ability of an element to combine with another element. Hydrogen, with
an oxidation number of +1, is used as the reference.
Electron Exchange:
The oxidation number represents the number of electrons an atom gains or loses (partially or fully)
when forming a compound.
- Negative oxidation number: The atom gains electrons.
- Positive oxidation number: The atom loses electrons.
- Metals generally have positive oxidation numbers, while non-metals have negative ones.
Examples:
1. Fluorine (F):
Fluorine has an oxidation number of -1 because it gains one electron to achieve a noble gas
configuration.
F (Z = 9): 1s^2 2s^2 2p^5
2. Magnesium (Mg):
Magnesium has an oxidation number of +2 because it loses two electrons to reach a noble gas
configuration.
Mg (Z = 12): 1s^2 2s^2 2p^6 3s^2
Page 1
