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Minimalist Aesthetic Slideshow by Slidesgo

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SO4: sulfate
NO3: nitrate
CO3: carbonate
F: Floride
Cl: chloride
Br: Bromide
I: iodide
S: sunfide
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NaNO3, CaCO3, (NH4)2SO4, CuCl2, PbI2, K2SO4, FeBr2, TiO2, MgS, Al2(SO4)3

NaCl: sodium chloride
...

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Acid: start with H (HCl, H2SO4, HNO3..)
turn red litmus paper; pH 1-6

Base: end with OH
MOH (M; group 1) NaOH, LiOH, Fe(OH)2

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,...)

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NOBLE GASES
Properties
x Density increases down group
x M.p. and b.p. increases down the group
x Don’t conduct electricity
x Don’t take part in chemical reactions

Uses
x Helium- filling balloons and aircrafts because it is lighter than air and will not catch fire.
x Argon – filling (tungsten) light bulbs to stop the filament reacting with oxygen.
x Neon – is used in advertising signs because it glows red

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Reactions Of Metals With Water | Reactions | Chemistry | FuseSchool

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IGCSE Chemistry Revision - Part 7 - Metals and Non-metals

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Alloy & their Properties | Properties of Matter | Chemistry | FuseSchool

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Testing for Hydrogen, Oxygen, Carbon Dioxide, Ammonia and Chlorine | Tests | Chemistry | FuseSchool

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GCSE Chemistry - Tests for Anions - Carbonate, Sulfate and Halide Ions (2026/27 exams)

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How to test for negative ions | The Chemistry Journey | The Fuse School

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Find out all the basics of testing for negative ions. Make sure to watch our video on testing for positive ions, too: http://youtu.be/4TgW0hGnqL0 At Fuse School, teachers and animators come together to make fun & easy-to-understand videos in Chemistry, Biology, Physics, Maths & ICT. Our OER are available free of charge to anyone.

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IGCSE Chemistry Revision - Part 1 - Tests for Cations

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Acid: start with H (HCl, H2SO4, HNO3..)
turn red litmus paper; pH 1-6
acid + base => salt + water
acid + metal => salt + hydrogen
acid + metal carbonate => salt + carbon dioxide + water

Base: turn blue litmus paper; pH 8-14
end with OH
MOH (M; group 1) NaOH, LiOH, Fe(OH)2

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)

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ACID
acid + metal -> salt + hydrogen
HCl + Mg -> MgCl2 + H2
acid + base / alkalis -> salt + water (neutralisation)
LiOH + H2SO4 -> Li2SO4 + H2O
acid + metal carbonate -> salt + carbon dioxide + water
HCl + MgCO3 -> MgCl2 + CO2 + H2O
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BASE
base + acid  (same)
base + ammonium salt -> salt + ammonia gas + water
NaOH + NH4Cl -> NaCl + NH3 + H2O
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METAL
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

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The effect of temperature
if you increase the temperature of the reactants, their particles move around faster. By moving around faster, the particles collide with each other more often. The more often the reactant particles collide, the faster the reaction. So increasing the temperature of a reaction increases the rate of the reaction.
The effect of concentration

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 effect of surface area

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.

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ACID: start with H (HCl; H2SO4; HNO3)
- pH: 0-6
- indicator turn into: red
BASE: end with OH (Mg(OH)2; NaOH;...)
alkalis: soluble base (group 1) NaOH, Li2O,...
-pH: 8-14
- indicator turn into: blue
OXIDE: element + oxygen
- basic oxide: metal + oxygen:  K2O; FeO
- acidic oxide: non-metal + oxygen: CO2; N2O; SO3....
- neutral oxide: NO; CO; H2O
- amphoteric oxide: Al2O3; ZnO
SALTS: metal/NH4 + đuôi of acid
MgSO4; NH4Cl, CaCO3

ACID + BASE => SALT + WATER
HCl + NaOH +> NaCl + H2O

ACID + METAL => SALT + HYDROGEN GAS
H2SO4 + Mg => MgSO4 + H2

ACID + METAL CARBONATE => SALT + CARBON DIOXIDE + H2O
2HCl + CaCO3 => CaCl2 + CO2 + H20

BASE + AMMONIUM => SALT + AMMONIA + WATER
LiOH + NH4Cl => LiCl + NH3 + H2O

METAL + WATER => METAL HYDROXIDE + HYDROGEN
2Na + 2H2O => 2NaOH + H2

METAL + OXYGEN => METAL OXIDE
Cu + O2 => CuO

Displacement reactions: metal more reactive can displace metal less reactive from its compound
- Mg + CuSO4 => MgSO4 + Cu
- Al + Fe2O3 => Al2O3 + Fe

Thermal decomposion: heat
Metal carbonate=> metal oxide + carbon dioxide
calcium carbonate => calcium oxide + carbon dioxide
Metal hydroxide => metal oxide + water
Fe(OH)3 => Fe2O3 + H2O
Metal nitrate => metal oxide + nitrogen dioxide + oxygen
Cu(NO3)2 => CuO + NO2 + O2