Nitrates (NO 3 - ) Chlorates (ClO 3 - ) Perchlorates (ClO 4 - ) Acetates (C 2 H 3 O 2 - ) Alkali Metal Compounds (Li +,Na +,K +,Rb +,Cs + ) Ammonium Compounds (NH 4 + ) Chlorides (Cl - ) Bromides (Br - ) Iodides (I - ) Sulfates (SO 4 2- )
All soluble All soluble All soluble Exceptions: AgC 2 H 3 O 2 All soluble Exceptions: KClO 4 All soluble All soluble All soluble Exceptions: Those that contain Ag +,Hg 2 2+, Pb 2+,PbCl 2 All soluble Exceptions: Those that contain Ag +,Hg 2 2+, Pb 2+,PbCl 2 Most are soluble Exceptions: SrSO 4,BaSO 4, CaSO 4,PbSO 4, HgSO 4,Hg 2 SO 4,Ag 2 SO 4 All soluble Exceptions: Those that contain Ag +,Hg 2 2+, Pb 2+,PbCl 2
Strong acids Strong bases Weak acids Weak bases Soluble ionic compounds Insoluble ionic compounds Molecules Partially soluble ionic compounds NO 2 - C 2 O 4
Strong electrolytes All soluble metal hydroxides Strong electrolytes Perchloric, HClO 4 ;Chloric, HClO 3 ; Hydrobromic, HBr; Hydrochloric, HCl; Hydroiodic, HI; Nitric, HNO 3 ; Sulfuric, H 2 SO 4 Weak electrolytes All molecular bases Weak electrolytes All acids other than the seven strong acids All nonelectrolytes All strong electrolytes All nonelectrolytes Nonelectrolytes except acids and molecular bases CO 2 NO 3 -
HNO 3 (dilute) HNO 3 (concentrated) Sn 2+ MnO 4 - (in acid solution) MnO 2 (in acid solution) MnO 4 - (in neutral or basic solution) H 2 SO 4 (hot, concentrated) SO 3 2- or SO 2 (aq) Na 2 O 2 H 2 O 2
NO 2 NO Mn 2+ Sn 4+ MnO 2 Mn 2+ SO 4 2- SO 2 H 2 O + O 2 NaOH
HClO 4 Cl 2 (dilute basic solution) Cl 2 (concentrated basic solution) Cr 2 O 7 2- (in acidic solution) S 2 O 3 2- NH 3 AX (aq) + BY (aq) Acid + Base Definition Acid
ClO - Cl - Cr 3+ ClO 2 - NH 4 + SO 2 Precipitation Reaction - Metathesis AY (s) + BX (aq) Definition A substance that is able to donate a H + ion (a proton) and, hence, increases the concentration of H + (aq) when it dissolves in water. Acid/Base Neutralization - Metathesis Salt + Water
Definition Base Definition Salt Metallic Oxide + Acid Nonmetallic oxide + Base Definition Metallic Oxide Definition Nonmetallic oxide Acid + Non-hydroxide base Definition Non-hydroxide base Group IA metal + Nonmetal Group IIA metal + Nonmetal
Definition An ionic compound formed by replacing one or more hydrogens of an acid by other cations. Definition A substance that is an H + acceptor; a base produces an excess of OH - (aq) when it dissolves in water. Double Displacement - Metathesis Salt + H 2 O Double Displacement - Metathesis Salt + H 2 O Definition Oxygen and a nonmentallic element. Ex: CO 2 Oxygen and a metallic element. Ex: Fe 2 O 3 Definition A base that does not contain an OH - group. Ex: Na 2 S Double Displacement - Metathesis Salt + Molecular gas Synthesis - Redox Salt (Metal ion + Nonmetal ion) Synthesis - Redox Salt (Metal ion + Nonmetal ion
AB Metal + Metal ion 2M(s) + 2H 2 O (Pattern for Group I) M(s) + H 2 O (Pattern for Group II) Mg(s) +H 2 O Halogen + Halogen ion Acid + Metal Molecular: Pb + H 2 SO 4 Net Ionic: Pb + H + + SO 4 2- Concentrated: Cu + H + + NO 3 - Diluted: Cu + H + + NO 3 -
Decomposition - Redox A + B Single Displacement - (Metal Displacement) Redox Metal + Metal ion Single Displacement Metal Displacement Pattern for Group II Redox M 2+ (aq) + 2OH - (aq) + H 2 (g) Single Displacement Metal Displacement Pattern for Group I Redox 2M + (aq) + 2OH - (aq) + H 2 (g) Single Displacement Halogen Displacement Redox Halogen + Halogen ion Single Displacement Metal Displacement Exception Mg Redox MgO(s) + H 2 (g) Single Displacement Exception Molecular: PbSO 4 + SO 2 + H 2 O Net ionic: PbSO 4 + SO 2 + H 2 O Single Displacement Hydrogen Displacement Redox Salt + Hydrogen Single Displacement Exception Diluted: Cu 2+ + H 2 O + NO Single Displacement Exception Concentrated: Cu 2+ + H 2 O + NO 2
Carbonates (CO 3 2- ) Phosphates (PO 4 3- ) Chromates (CrO 4 2- ) Sulfites (SO 3 2- ) Hydroxides (OH - ) Sulfides (S 2- ) Oxides (O 2- ) Acetate Bromite Bromate
Group I, (NH 4 ) 3 PO 3 Group I, (NH 4 ) 2 CO 3 Group I, (NH 4 ) 2 SO 3 Group I, (NH 4 ) 2 Cr 3 Group I, (NH 4 ) 2 S Group I, Sr(OH) 2, Ba(OH) 2 Exceptions: Ca(OH) 2 C 2 H 3 O 2 - or CH 3 COO - CaO, SrO, BaO BrO 3 - BrO 2 -
Hypochlorite Chlorite Chlorate Perchlorate Cyanide Thiocynate Dihydrogen Phosphate Hydrogen carbonate or bicarbonate Hydrogen sulfide Hydrogen sulfite or bisulfite
ClO 2 - ClO - ClO 4 - ClO 3 - SCN - CN - HCO 3 - H 2 PO 4 - HSO 3 - HS -
Hydroxide Iodate Manganate Nitrite Nitrate Carbonate Chromate Dichromate Hydrogen phosphate Permanganate
IO 3 - OH - NO 2 - MnO 4 2- CO 3 2- NO 3 - Cr 2 O 7 2- CrO 4 2- MnO 4 1- HPO 4 2-
Oxalate Peroxide Disulfide Sulfite Sulfate Thiosulfate Phosphite Phosphate Ammonium Mercury (I)
O 2 2- C 2 O 4 2- SO 3 2- S 2 2- S 2 O 3 2- SO 4 2- PO 4 3- PO 3 3- Hg 2 2+ NH 4 +
Cadmium (Cd) Hafnium (Hf) Chromium (Cr) Iridium (Ir) Cobalt (Co) Iron (Fe) Copper (Cu) Lutetium (Lt) Gold (Au) Manganese (Mn)
IV II III, IV II, III, VI II, III, V II, III III I, II II, III, IV, V, VI, VII I, III
Mercury (Hg) Paladium (Pd) Molybdenum (Mo) Platinum (Pt) Nickel (Ni) Rhenium (Re) Niobium (Nb) Rhodium (Rh) Osmium (Os) Ruthenium (Ru)
II, IV Hg +, Hg 2+, Hg 2 2+ II, IV II, III, IV, V, VI II, III, IV, V, VII II, III II, III, IV II, III, IV, V II, III, IV, V, VIII II, IV, VIII
Scandium (Sc) Tungsten (W) Silver (Ag) Vanadium (V) Tantalum (Ta) Yttrium (Y) Technetium (Tc) Zinc (Zn) Titanium (Ti) Zirconium (Zr)
III, IV, V, VI III II, III, IV, V I III III, IV, V II IV, VI, VII III, IV II, III, IV
HClO 2 Ca(OH) 2 Pb(SO 4 ) 2 CO 2 NaOH H 2 SO 4 NH 3 CH 3 COOH Cu(NO 3 ) 2 Sr(OH) 2
Nonelectrolyte (partially soluble ionic compound) Weak acid/weak electrolyte Nonelectrolyte Nonelectrolyte (insoluble ionic compound) Strong acid/strong electrolyte Strong base/strong electrolyte Weak acid/weak electrolyte Weak (molecular) base/weak electrolyte Strong base/strong electrolyte Strong electrolyte (soluble ionic compound)