Oxidation and Reduction Reactions (Redox Reactions) - AP Chemistry (copy)

Electrons

Redox reactions are centralized around the transfer of what?

Oxidation definition:

Oxidation is the loss of electrons, giving them away and subsequently offsetting the charge to be neutral or positive

Reduction definition:

Reduction is a gain of electrons, thus its charge is offset by becoming more negative

Atoms in elemental form have oxygen #s of 0

Oxidation Rules #1:

Monotomic ions have an oxidation # thats the charge or the ion

Oxidation Rules #2:

Non-metals have varying oxidation numbers

Oxidation Rules #3:

• Oxygen is usually 2- except when with the peroxide ion (O2^2-), which makes it 1-

• Hydrogen is 1+ when bonded to nonmetals, 1- when bonded to metals, and can only occur when bonded onto strong base metals (the alkali metals)

• Fluorine is 1-, with other halogens being 1- (except when combined with oxygen)

SUB Oxidation Rules #3:

The sum of oxidation #s in a neutral compound is 0, except if its a compounded ion in which it will equal the charge of that ion

Oxidation Rules #4:

Single replacement reactions have the form:

A+BX --> AX + B