Summary FULL COURSE IGCSE CHEMISTRY PEARSON EDEXCEL NOTES
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Course
Science
Institution
GCSE
Full in depth notes in line with IGCSE Chemistry Pearson edexcel specification got me a 9 in my IGCSE in Summer 2022. All triple award content covered.
Chemistry Notes
States of matter:
Solid:
- Fixed arrangement
- Vibrate in fixed positions
- Little kinetic energy
- Strong forces between them
Liquid:
- Intermediate forces of attraction between them
- Vibrate more than solids
- No fixed positions
- Random movement
Gas:
- Weak forces
- Far apart Condensation and
- Random and rapid movement evaporation in a
closed container
occur
Changes of state simultaneously
Solid —> Liquid (melting)
Liquid —> Solid (freezing)
Liquid —> Gas (boiling/evaporating)
Gas —> Liquid (condensation)
Evaporation of a water puddle:
- Particles have differing kinetic energy
- Particles with the most kinetic energy
evaporate first (leave surface of puddle)
- Remaining particles have lower average
Definitions kinetic energy
Diffusion: net movement of particles from an area of high
concentration to an area of low concentration (down a
concentration gradient).
Examining diffusion using ammonia and hydrochloric acid:
Big glass tube at each end, at one end add hydrochloric
acid, at the other end, add ammonia.
Both of the substances concentration will be high at
either end of the tube.
The particles will diffuse.
, Where particles meet a white ring will form (ammonium
chloride).
When the white ring forms shows the speed of diffusion.
The ring forms closer to the hydrochloric acid end as
ammonia has diffused further and faster due to its
having a lower relative atomic mass.
Solutions
- Solute: solid which dissolves in solvent
- Solvent: liquid in which the solid dissolves
- Solution: solvent-solute mixture
- Saturated Solution: a solution where no more solute can
dissolve in the solvent
- Solubility: mass of solute needed to dissolve in 100g of
solvent in order to form a saturated solution
Key Definitions
Atom: smallest particle of a substance that can exist
Element: contains only one type of atom (cannot be
split by chemical means)
Compounds: 2+ chemically combined elements (cannot
be separated)
Mixture: 2+ NOT chemically combined elements (can be
separated)
Molecule: 2+ atoms bonded together (same/different
elements)
Period: number of e- shells
Group: number of e- in outer shell
Pure substances: only one material in substance
therefore have a fixed boiling point (don’t boil at a
range of temperatures)
Relative atomic mass: ratio of the average mass of an
element when compared with one atom if carbon-12
“Bottom” number: atomic number (proton number and
therefore e- number)
“Top” number: mass number (total number of protons
and neutrons added together)
Isotope: atoms of same element with the same proton
number (different neutron number)
, Separation Techniques
Filtration: Separate insoluble solid from solvent (sand + water)
= filter funnel
= paper
Evaporation: Soluble solute needs separating from solvent
(copper sulfate + water)
= tripod
= gauze
= evaporating basin
Separating Funnel: Separating immiscible (un-mixable) liquids
(oil + water)
Simple Distillation: Different boiling point liquids
(ethanol + water)
1. boil the mixture
2. liquid with the lowest boiling point evaporates first
Fractional distillation: separate many liquids with many
different boiling points
Chromatography: separate dyes, inks, food colourings
= the ink which travels the furthest has the highest solubility
RF formula: distance travelled by component / distance
travelled by solvent
Abundance calculations
‘The abundance of Cl-35= 75% + abundance of Cl-37= 25%.
Calculate the relative atomic mass of Cl’
(Mass of isotope A x percentage) + (Mass of isotope B x percentage)
100
= (35 x 75)+(37 x 25) = 35.5g (3s.f)
100
Halogens (group 7)
- Low boiling and melting points
- Poor conductors of heat + electricity
Elements:
Fluorine (yellow gas) Iodine sublimes
Solid -> Gas
Grey/black solid -> Purple
vapour
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