Unit 5 - Principles and Applications of Science II
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Unit 5 applied science chemistry exam notes
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Unit 5 - Principles and Applications of Science II
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PEARSON (PEARSON)
Lecture notes for Unit 5 applied science chemistry exam.
I cover almost everything if not everything, that could possibly be brought up in the exam.
hope you find these nots useful
Unit 5 - Principles and Applications of Science II
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Recap
Formula for aluminium oxide: Al2O3
Aluminium oxide is also known as: Alumina
Aluminium oxide is amphoteric: this means it can react as either a base or acid
Electrolysis
The cell contains molten sodium chloride.
Molten means the sodium chlorides been liquified by heat.
The sodium chloride has to be molten so the ions can move around for electric current to
flow
An ion is a particle with a charge (positive or negative)
diaphragm cell
The diaphragm prevents the hydrogen from travelling from right to left to stop a reaction
occurring
This is one way chlorine is manufactured
And one way hydrogen is manufactured
Transition metals
Transition metals are block d elements that have an ion with an incomplete d sub-shell.
Properties of transition metals:
- variable oxidation states
- Coloured compound
- Catalyst : changes oxidation state temporary, and then returns to original state
Organic chemistry
, Propane: C3H6
Butene: C4H10
Formula for Alkane: CnH2n+2
Formula for Alkene: CnH2n
3D representation of Methane:
Alkanes boiling points increases as the chain length increases. This is because more energy
is required to break the intermolecular forces between the atoms.
Orbitals
An orbital is a region of space that can be occupied by up to two pairs of electrons
- S- orbitals are spherical
- P- orbitals are lobe shaped
Covalent bond: shared pair of electrons
When a covalent bond forms, hybrid orbitals arise:
Single covalent bonds are sigma bonds which arise from the head- on overlap of s or p
orbitals.
Free radical mechanism
stages:
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