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VCE Chemistry Key Facts

Key facts for organic chemistry, analysis, equilibrium, electrochemistry and mole calculations in VCE Chemistry. Written for study, not the official exam.

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Functional group of an alcohol
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1
Functional group of an alcohol
The hydroxyl group, -OH. Names end in -ol, such as ethanol.
2
Functional group of a carboxylic acid
The carboxyl group, -COOH. Names end in -oic acid, such as ethanoic acid.
3
Esterification
A carboxylic acid and an alcohol react (with an acid catalyst) to form an ester and water.
4
Naming an ester
Alkyl alkanoate: the alkyl part from the alcohol, the alkanoate part from the acid, for example methyl propanoate.
5
Oxidation of a primary alcohol
Alcohol to aldehyde and then to carboxylic acid. Acidified dichromate changes from orange to green.
6
Test for an alkene
Bromine water is decolourised as bromine adds across the C=C double bond.
7
Saponification
Hydrolysis of a triglyceride with NaOH gives glycerol and sodium salts of fatty acids (soap).
8
Condensation reaction of amino acids
The amine group of one joins the carboxyl group of another, forming a peptide bond and losing water.
9
Mass spectrometry
The molecular ion peak (highest m/z of the intact molecule) gives the relative molecular mass.
10
Infrared spectroscopy
Bonds absorb characteristic wavenumbers. C=O absorbs strongly at about 1680 to 1750 cm-1.
11
1H NMR n+1 rule
A signal is split into n + 1 peaks by n hydrogen neighbours, so a CH2 next to a CH3 shows a quartet.
12
HPLC
Retention time helps identify a compound. Peak area relates to its concentration.
13
Le Chatelier's principle
A system at equilibrium shifts to oppose a change in concentration, pressure or temperature.
14
Equilibrium constant, K
Products over reactants, each raised to its coefficient. K changes only with temperature.
15
Reaction quotient, Q
Q has the form of K but uses current concentrations. If Q < K, the reaction goes forward.
16
Effect of a catalyst on equilibrium
Both rates increase equally, so equilibrium is reached faster, but the position and K do not change.
17
Anode and cathode
Oxidation occurs at the anode and reduction at the cathode (AN OX, RED CAT).
18
Galvanic cell polarity
The anode is negative and the cathode is positive. Electrons flow in the external circuit from anode to cathode.
19
Standard cell potential
E cell = E (cathode) - E (anode), using standard reduction potentials.
20
Salt bridge
Allows ions to move between half-cells so that charge stays balanced.
21
Faraday's laws calculation
Q = It, n(e-) = Q / 96 500 C/mol, then use the half-equation to find moles of product.
22
pH of a strong acid
pH = -log10[H+]. For 0.010 M HCl, pH = 2.0.
23
Moles from mass
n = m / M, with m in grams and M in g/mol.
24
Gas volume at SLC
V = n x 24.8 L/mol at standard laboratory conditions (25 degrees Celsius, 100 kPa).
25
Secondary cell
A cell whose reaction can be reversed by an applied voltage, so it can be recharged, such as lithium-ion.

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