M2O (M group 1) Na2O, K2O...

R(OH)2 (R: group 2) Ca(OH)2; Mg(OH)2
RO (R: group 2) CaO, MgO

ammonium salts:
NH4Cl, (NH4)2SO4, NH4NO3, (NH4)2S, (NH4)2CO3
salts: metal + đuôi acid
MgCl2, CaCO3, CuSO4

OXIDES = one element + oxygen
acidic oxide = non-metal + oxygen
ex: NO2, SO2, CO2, SO3, N2O5, P2O5, SiO2...
react with base
basic oxide: metal + oxygen
ex: K2O, MgO, CuO, FeO, CaO,...
react with acid
amphoteric oxide: ZnO, Al2O3
react with both of acid and base
neutral oxide: CO, NO, H2O
neither ... nor

 
acid: start with H
base: end with OH (Cao, Na2O)
oxide: element + oxide
salts: Metals/ NH4 + group (SO4, NO3, CO3, Cl, S, HCO3,...)

M2O (M group 1) Na2O, K2O...

R(OH)2 (R: group 2) Ca(OH)2; Mg(OH)2
RO (R: group 2) CaO, MgO
alkali (soluble base)

base + acid => salt + water
base + ammonium salt => salt + ammonia + water

ammonium salts:
NH4Cl, (NH4)2SO4, NH4NO3, (NH4)2S, (NH4)2CO3
salts: metal + đuôi acid
MgCl2, CaCO3, CuSO4

OXIDES = one element + oxygen
acidic oxide = non-metal + oxygen
ex: NO2, SO2, CO2, SO3, N2O5, P2O5, SiO2...
react with base
basic oxide: metal + oxygen
ex: K2O, MgO, CuO, FeO, CaO,...
react with acid
amphoteric oxide: ZnO, Al2O3
react with both of acid and base
neutral oxide: CO, NO, H2O
neither ... nor

 
acid: start with H
base: end with OH (Cao, Na2O)
oxide: element + oxide
salts: Metals/ NH4 + group (SO4, NO3, CO3, Cl, S, HCO3,...)

CHEMICAL REACTIONS

1) REACT WITH WATER
+) Alkali metals: general equation
M + H20 => MOH + H2
ex: sodium + water => sodium hydroxide + hydrogen
+ ) other metals:
Magnesium: react very slowly with cold water, but react vigorously with steam (hot water)
Mg + H2O (heat) -> MgO + H2
Mg + 2H2O (cold) -> Mg(OH)2 + H2
alkaline earth metals (Ca, Ba)
Ca + H2O => Ca(OH)2 + H2
Zinc:  (react with hot water and no react with cold water)
Zn + H2O (heat) -> ZnO + H2

2) REACT WITH DILUTE ACID (HYDROCHLORIC ACID/SULFURIC ACID)
condition: above H in rectivity serie (excess: Cu, Ag, Au, Pt...)
metal + acid => salt + hyrogen
ex:  Fe + HCl => FeCl2 + H2
       aluminium+sulfuric acid=>aluminium sulfate + hydrogen


3) REACT WITH OXGEN
metal + oxygen -> metal oxide

sodium + oxygen -> solium oxide

4) DISPLACEMENT REACTION

THE MORE REACTIVE METAL CAN DISPLACE THE LESS REACTIVE METAL FROM ITS COMPOUNDS
 (COMPOUNDS: oxide or salt solutions)

K - Na - Li - Ca - Mg - Al - C - Zn - Fe - Sn - Pb - H - Cu - Hg - Ag - Pt - Au

Al + Fe2O3 => Al2O3 + Fe
Mg + CuSO4 => MgSO4 + Cu

the more reactive metals, more stable compounds

5) THERMAL DECOMPOSITION  (HEAT)

metal carbonate => metal oxide + carbon dioxide
CaCO3 => CaO + CO2 (heat)
CuCO3 =>  CuO + CO2
metal nitrate => metal oxide + nitrogen dioxide + oxygen
Mg(NO3) => MgO + NO2 + 02
metal hydroxide => metal oxide + water
Fe(OH)2 => FeO + H2O

STOICHIOMETRY

no of mole = mass/molar mass
concentration (of solution) = mole/volume
mole (of gas) = volume / 24 (r.t.p)

If you increase the concentration of one reactant you are increasing the number of particles of that reactant in the same volume. If there are more particles of that reactant present then there is an increased chance that these particles will collide with the other reactant particles. The more often the particles collide, the faster the reaction. So increasing the concentration of a reactant increases the rate of the reaction.

The bigger the piece of solid, the slower it will react. If yo break a solid into smaller pieces, or if you grind it into a powder, the surface area of the solid is increased. This means there is more chance that particles of the solid can collide with the other reactant particles, so the reaction is faster.

The effect of a catalyst.
Using a catalyst is another way of changing a rate of reaction. A catalyst is a substance which is added to a reaction to make it happen faster. The catalyst is not changed during the reaction, it just increases the rate of the reaction.