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Reaction Types
Synthesis
Decomposition
Single Replacement
Double Replacement
Combustion
A+BC
CA+B
AB + C  CB + A ( A and C are cations)
AB + CD  AD + CB
Hydrocarbon + O2  CO2 + H2O
Hydrides (synthesis)
Ionic Hydrides
2Na + H2  2NaH
Metallic Hydrides
(with transition elements)
Molecular Hydrides H2 + F2  2HF (covalent --- molecular)
Oxides
Acidic Oxides
NM oxide + water  acidic oxide (oxy acids) (SYN)
The NM (nonmetal) oxide is the acidic anhydride (except N2O, NO, and CO)
SO3 + H2O  H2SO3 (synthesis) N2O5 + H2O  2HNO3 P2O5 + 3H2O  2H3PO4
Basic Oxides
M oxide + water  hydroxides (SYN)
The M (metal) oxide is the basic anhydride
Na2O + H2O  2NaOH (synthesis)
Amphoteric Oxides (Aluminum, Tin, and Zinc) (lead and mercury)
Exhibit acid or base character
IF a metal forms more than one oxide, the BASE character DECREASES as the
oxidation state of the metal INCREASES.
Peroxide
Each O has a -1 charge (oxidation #)
2Na(s) + O2(g)  Na2O2(s) (SYN), 2H2O2  2H2O + O2 (DECOMP)
Superoxides
Each O has a -1/2 charge
K(s) + O2(g)  KO2(s)
Unstable – Decomposes
H2CO3  H2O + CO2
H2SO3  H2O + SO2
NH4OH  NH3 + H2O
(H can be replaced by an alkali metal)
SYNTHESIS
A+BC
*1 )Metal oxide + water  Metal hydroxide (base) (SYN)
Na2O + H2O  2NaOH
*2) Non metal oxide + water  acid
CO2 + H2O  H2CO3
*3) Metal oxide + CO2  Metal Carbonate (SYN) (recall H2O + CO2  H2CO3)
CaO + CO2  CaCO3
*4) Metal oxide + SO2  Metal Sulfite (SYN) (recall H2O + SO2  H2SO3)
CaO + SO2  CaSO3
Nonmetal oxide (acid) + Metal oxide (base)  salt (neutralization)
SO2 + CaO  CaSO3, SiO2 + CaO  CaSiO3, P4O10 + 6Li2O4Li3PO4
CO2 + Na2O  Na2CO3
Nonmetal oxide (acid anhydride) + water  acid
SO3 + H2O  H2SO4
Metal oxide (basic anhydride) + water  base
CaO + H2O  Ca(OH)2
DECOMPOSITION
CA+B
*1) Metal Hydroxide(base)  Metal oxide + water (DECOMP)
2NaOH  Na2O + H2O
*2) Acid  Nonmetallic oxide + water
H2CO3  CO2 + H2O
*3) Metal Carbonate  Metal oxide + CO2
Na2CO3  Na2O + CO2
*4)Metal Sulfite  Metal oxide + SO2
Na2SO3  Na2O + SO2
Metal Bicarbonate  Metal oxide + H2O + CO2
NaHCO3  Na2O + H2O + CO2 (H2CO3)
Metal Chlorate  Metal chloride + O2
NaClO3  NaCl + O2
Metal Nonmetal  Metal cation + Nonmetal anion
NaCl  Na+ + Cl-
CaSO4 + H2O
SINGLE REPLACEMENT
AB + C  CB + A
Metal + Acid  Metal salt + H2(g) (SR)
Mg(s) + 2HCl(aq)  MgCl2 + H2(g)
Metal + water or base  metal hydroxide or oxide + H2(g) (SR)
Na(s) + 2H2O  2NaOH(aq) + H2(g)
2Al(s) + 2KOH(aq) + 6H2O(l)  2K[Al(OH)4](aq) + 3H2(g)
Metal hydride + H2O  Metal hydroxide + H2(g) (SR)
CaH2(s) + 2H2O(l)  Ca(OH)2(aq)+ 2H2(g)
DOUBLE REPLACEMENT
AB + CD  AD + CB
Metal Carbonate (or bicarbonate) + Acid  Metal salt + CO2(g) + H2O(l) (DR)
NaCO3(aq) + 2HCl(aq)  2NaCl(aq) + CO2(g) + H2O(l)
H2CO3  H2O + CO2
NiCO3(aq) + H2SO4(aq)  NiSO4(aq) + CO2(g) + H2O(l)
Metal Sulfide + Acid  Metal salt + H2S (DR)
NaS(aq) + 2HCl(aq)  2NaCl(aq) + H2S(g)
Metal Sulfite + Acid  Metal salt + SO2(g) + H2O(l) (DR)
Na2SO3(aq)+ 2HCl(aq)  2NaCl(aq) + SO2(g) + H2O(l)
H2SO3  H2O + SO2
Ammonium Salt + Strong Base  Metal salt + NH3(g) + H2O(l) (DR)
NH4Cl(aq) + NaOH  NaCl + NH3(g) + H2O(l)
NH4OH  NH3 + H2O
Metallic oxide (base) + Acid  Salt + H2O
Fe2O3 + HCl  FeCl3 + H2O
Non metallic oxide (acid) + Base  Salt + H2O
CO2 + NaOH  NaCO3 + H2O
Acid + Metal  Salt + H2
2HCl + Zn  ZnCl2 + H2
COMBUSTION
Substance + Oxygen gas  Oxides of the elements
2CuS + 3O2  2CuO + 2SO2
CS2 + 3O2  CO2 + 2SO2
C3H8 + 5O2  3CO2 + 4H2O
IONIC EQUATIONS
Strong acid + salt of weak acid salt of strong acid + weak acid
Complete eqn => HCl + KOAc  KCl + HOAc
ionic eqn => H+ + Cl- + K+ + OAc-  K+ + Cl- + HOAc
net ionic eqn => H+ + OAc-  HOAc
weak acid + weak base  conjugate base + conjugate acid
HF + NH3  F- + NH4+ , HOAc + NH3  OAc- + NH4+
Weak acid + Strong base  water + conjugate base
HF + NaOH  HOH + FStrong acid + weak base  conjugate acid (weak) + water
HCl + Fe(OH)2  FeCl2 + HOH