Balancing Equations

Carbonic Acid

H₂CO₃(aq)→ H₂O(l)+ CO₂(g)

Sulfurous Acid

H₂SO₃(aq)→ H₂O(l)+ SO₂(g)

Ammonium Hydroxide

NH₄OH(aq)→ H₂O(l)+ NH₃(g)

Example of Precipitation

Pb(NO₃)₂(aq)+ 2KI(aq)→ PbI₂(s)+ 2KNO₃(aq)

Example of Gas Formation

Na₂S(aq)+ 2HCl(aq)→ 2NaCl(aq)+ H₂S(g)

Example of Neutralization

HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H₂O(l)

Dissociation vs Decomposition

Dissociation separates the ions

Single-Replacement- Halogens+ Halide Ions

Y₂+ BX(aq)→ X₂+ BY(aq)

Single-Replacement- Metal+ Metal Ions

A+ BX→ B+ AX

Single-Replacement- Metal+ Water

A+ H₂O→ AOH+ H₂(g)

Single-Replacement- Metal+ Acid

A+ HX→ AX(a salt)+ H₂(g)

Solids (s)

metal (except Hg), many nonmetals (I₂), and ionic Compunds

Liquids (l)

Hg, Br₂

Gases (g)

(H₂, O₂, N₂, F₂, Cl₂), nonmetal oxides (NO, NO₂, CO,CO₂, SO₂, NH₃₎

Aqueous (aq)

Acids (HCl), Solution of ionic compound (NaCl)

Synthesis- (Elements) metals+ nonmetals→

binary ionic compound

Synthesis- (Elements) nonmetal+ nonmetal→

molecular compound

Synthesis- (Oxides+Water) metal oxide+ water→

metal hydroxide

Synthesis- (Oxides+Water) nonmetal oxide+ water→

acid (H₂SO₃, H₂CO₃)

Decomposition-

AX→ A+ X

Decomposition of Binary Compounds

→ element+ element

Decomposition of Binary Compounds Example

HgO+ heat→ 2Hg(l)+ O₂(g)

Decomposition of Acids

→ nonmetal oxides+ H₂O (H₂CO₃, H₂SO₃)

Decomposition of Metal Hyrdoxides (bases)

→ metal oxide+ H₂O(g)

Decomposition Metal Carbonates

→ metal oxide+ CO₂

Decomposition Metal Chlorates

→ metal chloride+ O₂

Liquids (Alkanes and Alcohols)

Alkanes (C₅H₁₂-C₁₀H₂₂), alcohols

Gases (Alkanes and Alcohols)

Alkanes(Methane CH₄- Butane C₄H₁₀)

Combustion of HydroCarbons

Hydrocarbon+ O₂→ CO₂(g)+ H₂O(l)