The Knowledge Organiser includes everything you need to ace GCSE Chemistry Paper 1 as well as ALL 4 REQUIRED PRACTICALS with mark schemes for 6 markers on certain practicals. NOTE: Any and all images on the notes belong to their respective owners.
, Chapter 1 – Separating Techniques
Filtration Crystallisation Chromatography Simple Distillation
- Used to separate - Used to obtain solid - Used to separate - Used to separate 2 mixtures
insoluble substances crystals from a pigments of soluble - The mixtures are heated first and gas
from a liquid. solution. dyes is produced
- The gas goes into a condenser and
- A circle of filter - The solution is - Stationary Phase: the then it will condense into a liquid.
paper is folded to heated to let some of phase that doesn’t
make a cone and the solvent evaporate. move e.g. the paper Fractional Distillation
placed into a filter - Used to separate mixtures with
funnel. - Heating should be - Mobile Phase: different boiling points
stopped when small solvent moves - Example: Crude Oil Separation
- Gravity pulls down crystals form. through the paper
the liquid and solid carrying different Crude oil is extracted from underground, it is a
particles which are - The rest is left to substances fossil fuel so non-renewable.
caught by the filter evaporate at room It is heated up and gas travels into a fractionating
paper. temp to get a good - Example: Drug Tests column which has a temp gradient from hot to
sample of crystals. cold.
- Example: mixture of Rf Value = distance
pigment / distance Different compounds from the mixture of crude oil
sand or salt, NaCl and - Example: salt from turn into their condensed state at their boiling
solvent travelled
water seawater points.
, Chapter 1 – Atomic Structure
Atoms History of the Atom
- Molecule: chemically 1) John Dalton – Atom is a plain sphere that makes up everything
bonded atoms 2) JJ Thomson – Created the plum pudding model, the whole sphere being positive and
- Compound: with randomly scattered – charge electrons
chemically bonded 2 or 3) Rutherford – Discovered the concentrated part of positive in the middle. This was
more different element from the gold foil experiment
atoms 4) Niels Bohr – Discovered shells and that electrons weren’t randomly scattered.
- Mixture: 2 or more 5) James Chadwick – Discovered neutrons and the model we have today
atoms
- Ions: atoms with a Gold Foil Experiment
charge - The experiment was carried out by Geiger & Marsden.
- Atoms don’t have an
overall charge as the + Experiment:
and – subatomic - They shot alpha ray particles at a piece of gold foil.
- They expected for the alpha rays to shoot straight
particles are equal
through the foil at a 180 degrees angle.
- Isotopes: atoms with
the same number of Observations:
protons but different - Some rays went straight through, showing that most of the atom was empty space.
number of neutrons. - Many rays deflected back at large and small angles thus showing that the atom had a
- Electrons: 2, 8, 8, 8… dense positive nucleus in the middle.
, Chapter 2 – The Periodic Table
Transition Metals Group 1 (Alkali Metals)
- Located between groups 2 and 3 on the periodic table Reactivity:
- Large central block in the periodic table - Vigorous reactions with water
- Creates compounds (salts) - Forms metal oxides
- Forms ionic compounds (with Group 7)
Physical Properties: - Reactivity increases going down
- Good Conductors of Heat & Electricity o Outer electron needs to be lost
- Hard and Strong o Going down, shells increase
- High Density and high melting points (expect Mercury) o Electron shielding decreases
o Electrons can be lost easily
Chemical Properties: Properties:
- Multiple Oxidation states - Soft
- Therefore, coloured compounds - Relatively low m/b points
- e.g. Iron III Chloride - Low Densities
Comparison
- Transition Metals are less reactive than Group 1 e.g. they don’t react readily with oxygen, water, and chlorine.
- Transition Metals have high density and high melting points, whereas Group 1 have low density and low mp.
- Transition Metals have to be heated strongly for a reaction to occur:
- 2Cu + O2 2CuO
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