Chemistry: The Central Science Chapter 4

Solubility rules

Rules that state which compounds are soluble and which are insoluble.

Soluble ionic compounds

NO3⁻ (Exceptions: NONE)

CH3COO⁻ (Exceptions: NONE)

Br⁻ (Exceptions: Ag⁺, Hg₂²⁺, Pb²⁺)

I⁻ (Exceptions: Ag⁺, Hg₂²⁺, Pb²⁺)

Cl⁻ (Exceptions: Ag⁺, Hg₂²⁺, Pb²⁺)

SO₄²⁻ (Exceptions: Ba²⁺, Hg₂²⁺, Pb⁺, Sr²⁺

Insoluble ionic compounds

S²⁻ (Except: NH₄⁺, Alkali metal, Ca²⁺,Ba²⁺, Sr²⁺)

OH⁻ (Except: NH₄⁺, Alkali metal, Ca²⁺,Ba²⁺, Sr²⁺)

CO₃²⁻ (Except: NH₄⁺, Alkali metal)

PO₄³⁻ (Except: NH₄⁺, Alkali metal)

Neutralization

Acid+Base→Salt+Water

Exceptions: Sulfide and hydroxide ion react to produce H₂ gas.

Redox

Oxidation: Loss of electrons

Reduction: Gain of electrons

Redox rules

1). Elemental form is always zero. Ex: P₄ = 0, H₂ = 0

2). Nonmetals usually have negative oxidation numbers.

3). H + nonmetal = H⁺ and H+ metal = H⁻

4). Fluorine= 1⁻ in all compounds

5). Other halogens = 1⁻, but when it is an oxyanion = 1⁺

6). Sum of redox: H₃O⁺ = (3⁺) + (2⁻) = 1⁺

Molarity

mol/V

Aqueous Solution

Water is the dissolving component

Electrolyte

Any substance whose aqueous solution contains ions

Nonelectrolyte

No IONS.

Strong electrolyte

Ions that completely dissociate in water

Weak electrolyte

Ions that partially dissociate in water

Precipitation reactions

Reactions in which an insoluble product, called a precipitate, forms.

Metathesis reactions

When a metal and nonmetal exchange partners

Molecular equation

Complete chemical formula of reactants and products are used

Complete ionic equation

Shows all dissolved strong electrolytes as their component ions

Net ionic equation

When spectator ions are omitted

Acid

Proton donor. Strong acids are strong electrolytes. Weak acids are weak electrolytes.

Base

Proton acceptor. Strong bases are strong electrolytes. Weak bases are weak electrolytes.

Oxidation numbers

Keep track of electrons during a chemical reaction. Oxidation results in increased number, whereas reduction results in decreased number.

Displacement reactions

Metals+acids and metals+salts

Titration

Combination of known and unknown concentration to determine the unknown concentration. The equivalence point allows the quantities of the reactants to reach an end point. An indicator can then be used to show the end point which coincides with he equivalence point.