1. Unit 10: Reversible reactions
1.1. Define
1.1.1. Features of equilibrium
1.1.1.1. Dynamic
1.1.1.2. Occur in close system
1.1.1.3. Rate of forward reaction = backward reaction
1.1.1.4. The concentration of products and reactants are remain constant
1.1.2. Closed system
1.1.2.1. Where none of the reactants or products can escape the reaction mixture or container when the reaction is taking place
1.2. Effect
1.2.1. Temperature
1.2.1.1. Temperature increase => move to endothermic side
1.2.1.2. Temperature decrease => move to exothermic side
1.2.2. Pressure
1.2.2.1. Pressure increase => Shift to the side which having less molecule of gas
1.2.2.2. Pressure decrease => Shift to the side which having more molecule of gas
1.2.3. Surface area + catalyst
1.2.4. Concentration
1.2.4.1. Concentration increase => Equilibrium shift to the side that produce less substance
1.3. Reversible hydration of salt
1.4. Haber process
1.4.1. N2(g) + 3H2(g) <=> 2NH3(g)
1.4.2. 450°C and 200atm (iron is catalyst)
1.5. Contact process
1.5.1. Sulfur + are (V2O5 is catalyst)
1.5.2. 2SO2 + O2 -> 2SO3
1.5.3. SO3 + H2O -> H2S2O7
2. Unit 15: Air Pollution
2.1. Composition of air
2.1.1. Nitrogen - 78%
2.1.2. Oxygen - 21%
2.1.3. Argon - 0.9%
2.1.4. CO2 - 0.04%
2.1.5. other gas - 0.06%
2.2. Sulfur oxide (Breaking difficulties, from acid rain) (get from oil and coal) S(s) +O2(g) -> SO2(g)
2.3. Oxides of nitrogen (Form acid rain, photochemical smog, asthma) N2(g) +O2(g) -> NO(g)
2.4. Carbon dioxide (Prevent haemoglobin to carry oxygen around the body) 2CO(g) + 2NO(g) -> 2CO2(g) +N2(g)
2.5. Carbon dioxide (Increase global warming) CH4 + 2O2 -> CO2 + 2H2O
2.6. Particulates (respiration disease, cause cancer) 2C8H18 + 9O2 -> 16C + 18H2O
3. Periodic table
3.1. Group 1
3.1.1. Softer than most metal
3.1.2. Low melting point, density
3.1.3. Trend: Go down => Increase density and reactivity/ decrease melting point
3.1.4. React vigorously with water
3.1.5. Same chemical characteristic
3.1.6. Its salt will dissolve and give colourless solution
3.2. Group 7
3.2.1. Colour: F- yellow-green, Cl - pale green, Br - red-brown, I - gray-black, At - black
3.2.2. Trend: Go down => Increase boiling point/ darker colour, decrease reactivity
3.2.3. Diatomic
3.2.4. Poisonous
3.2.5. Most reactive than other non-metal
3.3. Transition element
3.3.1. Hard, strong, tough
3.3.2. High density/ boiling point
3.3.3. Make coloured compund
3.3.4. Variable oxidation state
3.3.5. Can act as catalyst
4. Unit 18: Seperating techniques
4.1. Solutions and solibility
4.1.1. A solvent is a substance that dissolves a solute
4.1.2. A solute is a substance that is dissolved in a solvent
4.2. Separating techniques
4.2.1. 1) Filtration:
4.2.1.1. Residue: The wasted substance is left after filter
4.2.1.2. Filtrate: Liquid have been purified
4.2.1.3. Dụng cụ: Beaker, filter paper
4.2.2. 2) Crystallisation
4.2.2.1. Steps
4.2.2.1.1. Heat the solution until the mixture is saturated (no more solute can be dissolved at a specific temperature) + form little crystal on the glass rod
4.2.2.1.2. Leave the solution to cool down
4.2.2.1.3. Remove the crystals form the solution by filtering
4.2.2.1.4. Wash it with distilled water
4.2.3. 3) Simple distillation (separate solvent from solute)
4.2.3.1. Steps
4.2.3.1.1. Heat the solution in the flask. As it boils, water vapour rises into the condenser, leaving the salt behind
4.2.3.1.2. The condenser is cold, so the water vapour condenses to water in it
4.2.3.1.3. The water drips into the beaker: It is called distilled water. A residue will remain in the flask
4.2.4. 4) Fractional distillation (separate liquids, gases from each other) (Ethanol)
4.2.4.1. Steps
4.2.4.1.1. Heat up the mixture until it reached the boiling point
4.2.4.1.2. Liquid of the mixture evaporate and passing through the fractionating column the get into the condenser, where cold water is supplied
4.2.4.1.3. After passing through the condenser, it becomes liquid again
4.2.4.1.4. Put a beaker at the end of the condenser to collect pure liquid
4.2.5. Chromatography (separate mixture of soluble substance)
4.2.5.1. They separate because of their different solubility and attraction
4.2.5.1.1. More soluble: Travel further
4.2.5.1.2. More attraction: Travel closer
4.2.5.2. Steps
4.2.5.2.1. Draw a base line by pencil (Make sure the solvent is under the baseline
4.2.5.2.2. Use locating agent to react with the sample to produce colour
4.2.5.3. Rf = Distance moved bt the substance / Distance moved by the solvent front
4.2.5.4. Checking purity
4.2.5.4.1. Only have one melting point and boiling point
4.2.5.4.2. Impurity sample
5. Unit 11: Acids and Bases
5.1. Define the term of acids and bases
5.1.1. Acid: Proton donors ( pH < 7 )
5.1.2. Base: Proton acceptor ( pH > 7 )
5.2. Indicator
5.2.1. Litmus
5.2.1.1. Acid: Blue litmus turn red
5.2.1.2. Base: Red litmus turn blue
5.2.2. Methyl orange
5.2.2.1. Acid: Red
5.2.2.2. Base: Yellow
5.2.3. Thymolphthalein
5.2.3.1. Acid: Colourless
5.2.3.2. Base: Blue
5.3. Strong acids and weak acids
5.3.1. Strong acids are completely dissociation
5.3.2. Weak acids are partially dissociation
5.4. Oxides
5.4.1. 1) Basic oxides: Formed when a metal element combines with oxygen. Example: Na2O, CuO, MgO, Fe2O3
5.4.2. 2) Acidic oxides: Formed when a non-metal element combines with oxygen. Example: Co2, So2, No2, P4O10
5.4.3. 3) Amphoteric oxides: Are both acidic and basic. Example: ZnO, Al2O3
5.4.4. 4) Neutral oxides: Neither acidic nor basic. Example: H2O, CO, NO
5.4.5. 3) Amphoteric oxides: Are both acidic and basic. Example: ZnO, Al2O3
5.4.6. 4) Neutral oxides: Neither acidic nor basic. Example: H2O, CO, NO
5.5. Preparation of salt
5.5.1. Crystallisation
5.5.2. Precipitation (Create insoluble salt)
5.5.2.1. Steps
5.5.2.1.1. Mix 2 soluble solution
5.5.2.1.2. Solid formed
5.5.2.1.3. Filter
5.5.2.1.4. Wash with distilled water and dry in oven
5.5.3. Titration (Create soluble salt)
5.5.3.1. Steps
5.5.3.1.1. Pour alkali/ acid into the burette
5.5.3.1.2. Pour alkali/ acid into the beaker which put under the burette
5.5.3.1.3. Use methyl orange as indicator
5.5.3.1.4. Drop the substance into the beaker by the burette “drop to drop” until the colour change
5.5.3.1.5. Read the volume on the burette
5.5.3.1.6. Redo the experiment without methyl orange
5.6. Preparation of salt
5.6.1. Crystallisation
5.6.2. Precipitation (Create insoluble salt)
5.6.2.1. Steps
5.6.2.1.1. Mix 2 soluble solution
5.6.2.1.2. Solid formed
5.6.2.1.3. Filter
5.6.2.1.4. Wash with distilled water and dry in oven
5.6.3. Titration (Create soluble salt)
5.6.3.1. Steps
5.6.3.1.1. Pour alkali/ acid into the burette
5.6.3.1.2. Pour alkali/ acid into the beaker which put under the burette
5.6.3.1.3. Use methyl orange as indicator
5.6.3.1.4. Drop the substance into the beaker by the burette “drop to drop” until the colour change
5.6.3.1.5. Read the volume on the burette
5.6.3.1.6. Redo the experiment without methyl orange
5.6.4. Solid + acid (Create soluble salt)