Precipitaion and redox rules

These flashcards cover key concepts related to ionic compounds solubility rules and oxidation-reduction rules necessary for understanding precipitation reactions and REDOX reactions.

Solubility Rule

A guideline for determining whether an ionic compound will dissolve in water.

Always Soluble Compounds

All Group 1 salts, nitrates (NO3-), acetates (CH3COO-), and ammonium (NH4+) are always soluble.

Exceptions to Solubility

Chlorides, bromides, and iodides are soluble except for compounds with mercury (Hg), lead (Pb), and silver (Ag).

Not Soluble Compounds

Phosphates (PO4^3-), carbonates (CO3^2-), hydroxides (OH-), sulfides (S2-), and oxides (O2-) are not soluble unless paired with Group 1 or ammonium (NH4+).

Oxidation State Rule #1

Any element alone with a charge of 0 has an oxidation state of 0.

Monatomic Ion

A single atom with a charge that has an oxidation state equal to its charge.

Neutral Species Rule

The sum of the oxidation states in a neutral species must equal 0.

Polyatomic Ion Rule

The sum of oxidation states in a polyatomic ion must equal the charge of the ion.

Oxidation State of Fluorine (F)

The oxidation state of fluorine in compounds is always -1.

Oxidation State of Hydrogen (H)

The oxidation state of hydrogen is +1 in most compounds, -1 as a hydride.

Oxidation State of Oxygen (O)

The oxidation state of oxygen is usually -2, with exceptions such as peroxides.

Oxidation State of Chlorine (Cl)

Chlorine typically has an oxidation state of -1, except in compounds with oxygen or fluorine.

Oxidation States of Groups

Group 1 elements are +1, Group 2 elements are +2, Group 6 elements are typically -2, and Group 5 typically is -3.

N2O4 Example

To find oxidation states: 2(N) + 4(-2) = 0 implies oxidation state of N in N2O4 is +4.