A2 Chemistry Keywords

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  • Created by: Ciara4
  • Created on: 23-11-18 20:40
Lattice Enthalpy
The enthalpy change when one mole of an ionic compound is converted to gaseous ions.
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Enthalpy of atomisation
The enthalpy change when one mole of gaseous atoms is formed from the element in its standard state.
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First electron affinity
The enthalpy change when one mole of gaseous atoms is converted into gaseous ions with a single negative charge.
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Enthalpy of solution
The enthalpy change when one mole of a solute dissolves in water.
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Enthalpy of hydration
The enthalpy change when one mole of gaseous ions is converted to one mole of aqueous ions.
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Feasible
A reaction for which ΔG < 0.
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Entropy
A measure of disorder (randomness)
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Free energy change
ΔG=ΔH-TΔS
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Rate of Reaction
The change of the concentration (amount) of a reactant or product with respect to time
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Order of reaction (with respect to a reactant)
The power to which the concentration of a reactant is raised in the rate equation.
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Order of reaction (overall)
The sum of the powers to which the concentration terms are raised in the rate equation.
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Rate constant
The proportionality constant which links the rate of the reaction to the concentrations in the rate equation.
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Rate determining step
The slowest step in the mechanism of a reaction.
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Brønsted acid
Proton donor
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Brønsted base
Proton acceptor
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Kw
Kw=[H+][OH−]
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Ka
Ka = [H+][ A-] / [HA]
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pH
pH=-log10[H+]
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pKw
pKw=-log10Kw
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Buffer solution
A solution which resists changes in pH on addition of small amounts of acid or alkali.
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Monobasic acid
Donates one proton per molecule.
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Asymmetric chiral centre
An atom which has four different atoms or groups attached.
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Optical isomers
Molecules which exist as non-superimposable mirror images.
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Optically active
A sample which rotates the plane of plane polarised light.
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Racemic mixture
A 50:50 mixture of two optical isomers.
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Monoester
An ester which contains only one ester group.
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Transesterification
A reaction where the alkyl group of an ester is exchanged with the alkyl group of an alcohol.
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Biodiesel
A fuel, similar to diesel, which is made from vegetable sources. e.g. from the reaction of **** seed oil with methanol.
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Delocalisation (arenes)
The π electrons are spread over several atoms.
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Base peak
Peak of greatest abundance in a mass spectrum.
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Molecular ion peak
A peak produced by an ion formed by the removal of one electron from a molecule.
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M+1 peak
A peak produced by a molecular ion with an increased mass due to the presence of one carbon-13 atom.
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Fragmentation ion
A positively charged ion produced when the molecular ion breaks apart.
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Low resolution nmr
A spectrum which does not show the spin-spin splitting pattern.
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High resolution nmr
A spectrum which does show the spin-spin splitting pattern.
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Doublet
A signal which appears as a pair of lines of equal intensity
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Triplet
A signal which appears as three lines in the approximate intensity ratio (1:2:1)
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Quartet
A signal which appears as four lines in the approximate intensity ratio (1:3:3:1)
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Back titration
Method where an excess of a reagent is reacted with a sample. The unreacted reagent is then determined by titration.
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Rf values
Retardation factor, this is calculated using the expression: Rf = Distance moved by spot/ Distance moved by solvent
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Retention times
The time taken from injection until a component reaches the detector.
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Transition metal
An element which forms at least one stable ion with a partially filled d-subshell.
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Complex
A central metal atom or ion with ligands bonded by co-ordinate bonds.
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Ligand
An ion or molecule with a lone pair of electrons which forms a co-ordinate bond with a central metal atom or ion in a complex.
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Coordination number
The number of co-ordinate bonds to a central metal atom or ion in a complex.
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Monodentate
A ligand which uses only one lone pair of electrons to form a co-ordinate bond with a central metal atom or ion in a complex.
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Bidentate
A ligand which uses two lone pairs of electrons to form two co-ordinate bonds with a central metal atom or ion in a complex.
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Polydentate
A ligand which uses many lone pairs of electrons to form more than two co-ordinate bonds with a central metal atom or ion in a complex
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Standard electrode potential
The potential difference measured when a half-cell is connected to the standard hydrogen electrode under standard conditions.
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e.m.f
The potential difference measured when two half-cells are connected.
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Primary amine
Only one carbon atom directly bonded to the nitrogen atom and therefore has the (-NH2) group.
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Secondary amine
Two carbon atoms directly bonded to the nitrogen atom
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Tertiary amine
Three carbon atoms directly bonded to the nitrogen atom
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Coupling
A reaction in which two benzene rings are linked together through an azo (-N=N-) group.
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Dehydration of amides
A reaction which involves the elimination of water from the amide.
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Zwitterions
Ions which have a permanent positive and negative charge but which are neutral overall.
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Primary structure (proteins)
Sequence of amino acids joined by peptide links in the chain.
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Secondary situation (proteins)
The twisting/coiling of the chain to form a β-pleated sheet/α- helix by intramolecular hydrogen bonding.
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Tertiary structure (protein)
The bending/folding of the secondary structure to give a precise 3D shape held together by hydrogen bonding/disulfide bridges/ionic interactions/van der Waals’ forces.
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Enzyme
A protein which is a biological catalyst.
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Active site
The site on the surface of the enzyme into which the substrate fits.
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Induced fit
The substrate induces a change of shape of the active site of the enzyme
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Condensation polymers
Polymers formed by the elimination of small molecules such as water or hydrogen chloride when monomers bond together.
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Biodegradable polymers
A polymer which can be hydrolysed by the action of microorganisms.
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DNA replication
The process by which a double stranded DNA molecule is copied to produce two identical DNA molecules.
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GLC-MS
A gas liquid chromatograph attached to a mass spectrometer.
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Sequestering
The formation of a complex so that an ion is no longer available for reactions.
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Other cards in this set

Card 2

Front

The enthalpy change when one mole of gaseous atoms is formed from the element in its standard state.

Back

Enthalpy of atomisation

Card 3

Front

The enthalpy change when one mole of gaseous atoms is converted into gaseous ions with a single negative charge.

Back

Preview of the back of card 3

Card 4

Front

The enthalpy change when one mole of a solute dissolves in water.

Back

Preview of the back of card 4

Card 5

Front

The enthalpy change when one mole of gaseous ions is converted to one mole of aqueous ions.

Back

Preview of the back of card 5
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