ALL reactions Chemistry AS

Metal + Oxygen

Metal Oxide

Metal + Acid

Salt + Hydrogen Gas

Metal + Water

Metal Hydroxide + Hydrogen (only for reactive metals like Na, K, Ca)

Metal + salt solution

New salt + New metal (based on reactivity series it displaces)

Non-metal + Oxygen

Non-metal oxide (acidic oxide)

Nonmetal oxide + Water

Acid

Acid + Base

Salt + Water

Acid + Carbonate

Salt + Water + CO2

Acid + Ammonia

Ammonium salt

Metal Carbonate decomp

Metal Oxide + CO2 (except Na,K)

Metal Hydroxide decomp

Metal Oxide + H2O (except Na,K)

Metal Nitrate decomp

Metal Oxide + NO2 + O2 (except Na, K → Nitrite + O2)

Displacement rules

1. Metal displaces less reactive metal from salt

2. Halogen displaces less reactive halogen from halide solution

Double Displacement

Two Ionic solutions → Insoluble salt + Soluble salt (Ppt made)

Solubility rules

• All sodium, potassium, ammonium salts soluble

• All Nitrates soluble

• Silver and lead chloride insoluble

• Barium, Calcium, Lead sulfate insoluble

• Most carbonates insoluble except SOPOAM

• Most hydroxides insoluble except SOPOAM, calcium is partial

complete combustion of hydrocarbon

Hydrocarbon + O2 → CO2 + H2O

Incomplete combustion of hydrocarbon

Hydrocarbon + O2 → CO + H2O

Cl2 + cold dilute NaOH

NaCl + NaOCl + H2O (bleach)

Cl2 + Hot conc. NaOH

NaCl + NaClO3 + H2O

Chlorination of water

Cl2 + H2O → ← HCl + HClO

NH4+ salt + Alkali (heated)

NH3 + H2O + Salt

H2O2 (decomp)

H2O + O2 (MnO2 catalyst)

Cations

• Aluminum → white ppt soluble in NaOH, insoluble in NH3

• Ammonium → No ppt, ammonia produced when warmed

• Barium → Faint white ppt in NaOH, no ppt in NH3

• Calcium → White ppt in NaOH, no ppt in NH3

• Chromium → grey-green ppt soluble in NaOH, insoluble in NH3

• Copper → Pale blue ppt in NaOH insoluble, soluble in NH3

• Iron (II) → Green ppt turns brown with air in NaOH, insoluble in both

• Iron (III) → red-brown ppt insoluble in both

• Magnesium → White ppt insoluble in both

• Manganese → off-white ppt brown with air, insoluble in both

• Zinc → White ppt soluble in both

Anions

Carbonate → CO2 with dilute acid

Chloride → White ppt with Ag+, soluble in NH3

Bromide → Cream ppt. with Ag+ partially soluble in NH3
Iodide → Pale yellow ppt with Ag+ insoluble in NH3

Nitrate → NH3 when heating with OH- and Al foil

Nitrite → Decolorizes acidified KMnO4

Sulfate → white ppt with Ba2+ insoluble in excess aq acid, white ppt with high Ca2+

Sulfite → White ppt with Ba2+, decolourises acidified KMnO4
Thiosulfate → Off-white ppt slowly with H+

Gas tests

Ammonia turns red litmus blue

CO2 gives white ppt with limewater

Hydrogen pops with lighted splint

Oxygen relights glowing splint

Alkene reactions

• H2/Ni for Alkane

• HX for haloalkane (Electrophilic addition)

• H2O and H3PO4 for alcohol (electrophilic addition)

• Polymerise for polymer

Haloalkane reactions

aq NaOH for alcohol with heat (Substitution)

NH3 for Amine (Addition)

KCN in ethanol and heat for Nitrile (Addition)

Ethanol and aq Silver nitrate for Halide ppts (Addition)

NaOH in ethanol and heat for Alkene (Elimination)

Alcohol Reactions

Sodium metal for sodium salt (AB reaction)

Acid with conc H2SO4 for ester (Condensation reaction)

HX with H3PO4 for Haloalkane (Nucleo substitution)

Acidified KMnO4 heat and distill for Primary Aldehyde

Heat under reflux for secondary Ketone

Heated catalyst or Conc acid for Alkene (dehydration)

Aldehyde/ Ketone reactions

NaBH4 → Alcohol

2,4 DNPH for orange ppt

Acid reactions

Alcohol and Conc H2SO4 for Ester

Reduction for Alcohol

Ester to Alcohol

Dilute acid /Alkali and heat (Hydrolysis)

Alkene to Diol

Cold, Dilute, Acidified KMnO4 (Oxidation)

Aldehyde to Carboxylic Acid

Heat Acidified KMnO4 under reflux (Full oxidation of Primary alcohol)

Alkane to Haloalkane

Cl2 or Br2 with UV light (Free radical substitution)