FORMULAS hydroxideOH -

FORMULAS sulfateSO 4 2-

FORMULAS sulfiteSO 3 2-

FORMULAS chlorateClO 3 -

FORMULAS perchlorateClO 4 -

FORMULAS nitrateNO 3 -

FORMULAS carbonateCO 3 2-

FORMULAS phosphatePO 4 3-

FORMULAS cyanideCN -

FORMULAS bariumBa 2+

FORMULAS calciumCa 2+

FORMULAS nitrideN 3-

FORMULAS sulfideS 2-

FORMULAS ammoniumNH 4 +

FORMULAS carbonic acid H 2 CO 3

FORMULAS nitric acidHNO 3

FORMULAS sulfuric acid H 2 SO 4

FORMULAS hydrobromic acid HBr

FORMULAS acetic acidCH 3 COOH

FORMULAS ammoniaNH 3

FORMULAS nitrous acid HNO 2

FORMULAS phosphatePO 4 3-

Reactions metallic oxide + nonmetallic oxide simple combination

Reactions CaO + SO 3  CaSO 4

Reactions acid + metalsingle replacement gives: hydrogen gas and a salt

Reactions **Pb is dropped into hot sulfuric acid PbSO 4 + SO 2 + H 2 O

Reactions **Copper is added to concentrated nitric acid  Cu 2+ + H 2 O + NO 2

Reactions nonmetallic oxide and water  an acid

Reactions SO 3 + H 2 O  H + + SO 4 2-

Reactions “acidified” means it is a ________ reaction REDOX

Reactions Transition metal and NH 3 /CN - /SCN - /OH - forms a COMPLEX ION

Reactions hydrocarbon and oxygen  H 2 O + CO 2

Reactions metallic oxide + water  a base

Reactions Li 2 O + H 2 O  Li + + OH -

Reactions “solution” means WRITE AS IONS!!!!!!! (unless WA)

Reactions Group 2 + water  H 2 + M 2+ + OH -

Reactions **Mg + H 2 O  MgO + H 2 an exception

Reactions **Na + O 2  Na 2 O 2 an exception

Solubility Rules S 2- CO 3 2- PO 4 3- CrO 4 2- INSOLUBLE **except group 1 or NH 4 +

Solubility Rules all nitrates, group 1, NH 4 + SOLUBLE

Solubility Rules INSOLUBLE HALIDES (Cl - Br - I - ) Ag + Pb 2+ Hg 2 2+

Solubility Rules INSOLUBLE SULFATES Ba 2+ Ca 2+ Pb 2+ Hg 2 2+ Sr 2+

Solubility Rules Hydroxides are INSOLUBLE **except group 1 or NH 4 +

Solubility Rules sulfides chromates hydroxides carbonates phosphates INSOLUBLE **except group 1 or NH 4 +

Redox H2O2 H2O2  H 2 O + O 2

Redox HClO 4  Cl -

Redox Cr 2 O 7 2-  (in acid) Cr 3+

Redox Na 2 O 2  Na + + OH -

Redox MnO 4 -  (in acid) Mn 2+

Redox “acidified” H +  H 2 O

Redox MnO 2  (in acid) Mn 2+

Redox MnO 4 -  (in base or neutral) MnO 2

Redox H 2 SO 4  (hot/conc.) SO 2

Redox Cl 2  ( dilute base ) ClO -

Redox Cl 2  ( conc. base ) ClO 2 -

Redox Cl -  (halide) Cl 2 (halogen)

Redox Na  (metal) Na + (ion)

Redox HNO 3  (conc.) NO 2

Redox HNO 3  (dilute) NO

Net Ionic Reactions lead (II) nitrate solution and sodium chloride solution are mixed Pb 2+ + Cl -  PbCl 2

Net Ionic Reactions strontium chloride solution and sodium sulfate solution are mixed Sr 2+ + SO 4 2-  SrSO 4

Net Ionic Reactions solid calcium carbonate is heated CaCO 3  CaO + CO 2

Net Ionic Reactions solid aluminum hydroxide is heated Al(OH) 3  H 2 O + Al 2 O 3

Net Ionic Reactions strontium metal is dropped into 4M sulfuric acid Sr + SO H +  SrSO 4 + H 2

Net Ionic Reactions iron (III) nitrate solution and an ammonium thiocyanate solution are mixed Fe 3+ + SCN -  Fe(SCN) 6 3-

Net Ionic Reactions solutions of hydrochloric acid and potassium hydroxide are mixed H + + OH -  H 2 O

Net Ionic Reactions solutions of ammonia and hydrofluoric acid are mixed NH 3 + HF  NH F -

Net Ionic Reactions hydrochloric acid is added to a solution of potassium acetate H + + CH 3 COO -  CH 3 COOH

Net Ionic Reactions nitrous acid is added to a solution of sodium hydroxide HNO 2 + OH -  H 2 O + NO 2 -

Net Ionic Reactions POCl 3 + H 2 O  H 3 PO 4 + H + + Cl -

Net Ionic Reactions MgO + CO 2  MgCO 3

Net Ionic Reactions Mg + N 2  Mg 3 N 2

Net Ionic Reactions K + O 2  KO 2 **(a superoxide)