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The enthalpy change in a reaction (performed under standard conditions) between the number of moles of reactants shown in the chemical equation.

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The enthalpy change when one mole of a substance is completely combusted in oxygen (under standard conditions).

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The proportion of products to reactants in an equilibrium

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At dynamic equilibrium, the forward and backward reactions are taking place at the same time.

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A reducing agent gains electrons, becoming oxidised in the process.

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An oxidising agent accepts electrons, becoming reduced in the process.

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An equation showing electrons being accepted or giving up.

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Splitting of molecules into smaller parts in a mass spectrometer

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Positive ion formed in the mass spectrometer(when an electron is removed)from the whole molecule.

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Metal hydrides are metals which have been bonded to hydrogen to form a new compound.

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Metal halides are compounds between metals and halogens

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Metal peroxides are metal-containing compound with ionic or covalently bonded peroxide (O₂ 2−).

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The co-ordinate number of an ion in a crystal lattice is the number of nearest neighbours of opposite charge.

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The relative atomic mass, Ar, is the average mass of one atom of an element relative to one twelfth of the mass of one atom of Carbon-12.

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The number of protons/electrons in the nucleus. (BOTTOM NUMBER)

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The number of protons and neutrons (nucleons) in the nucleus of an atom. (TOP NUMBER)

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Atoms having the same number of protons but different numbers if neutrons.

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A bond formed by the electrical attraction between positive and negative ions.

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A particle where the number of electrons does not equal the number of protons.

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The model describes metals as containing positive ions bonded together by their attraction to a 'sea' of electrons. This is metallic bonding.

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The number of electrons that need to be added to(or taken away from) an element to make it neutral.

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A cluster of 2 protons and 2 neutrons

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The free electrons can carry thermal energy around the lattice.

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The free electrons allow a current to pass through the metal.

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A covalent bond has a pair of electrons with opposed spin shared between 2 atoms with each atom giving electrons.

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The hydrogen bond is a relatively strong intermolecular bond having a hydrogen atom joined to a highly electronegative element in a molecule and bonding to another electronegative element in another molecule.

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The relative isotopic mass is the mass of an atom of an isotope relative to one twelfth of the mass of an atom of Carbon-12.

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The average mass of a molecule relative to one twelfth of the mass of an atom of Carbon-12

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The amount of material containing the same number of particles as there are atoms in 12g of the Carbon-12 isotope.

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The mass of one mole of a substance.

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The simplest formula showing the simplest whole number ratio of the amount of elements present.

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Shows the actual number of atoms of each element present in the molecule. It is a simple multiple of the empirical formula.

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The volume per mole of a gas.

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A species with a lone pair of electrons that can b donated to electron deficient species

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A coordinate bond is a type of covalent bond where both electrons come from one atom.

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Fast moving electrons, therefore negatively charged.

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The measure of the electron-attracting power of an atom in a covalent bond.

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High energy electromagnetic radiation, therefore no charge.

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The strong bonding between the atoms in a molecule and governs the internal structure of a molecule.

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The time taken for the radioactivity of a radioisotope to fall to half its initial value.

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A region in an atom that can hold up to two electrons with opposite spin.

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The weak bonding holding the molecules together and governs physical properties like boiling point.

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The amount of energy required to remove 1 mole of electrons from a mole of the gaseous atoms or ions.

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The repulsion between electrons in a different

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A measure of the energy needed to remove each electron in turn until all the electrons are removed from an atom.

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Include all types of intermolecular force whether dipole or induced dipole.

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Valence Shell Electron Pair Repulsion

Groups of electrons around an atom (i.e. a pair of electrons in the same orbital) will repel each other and take up the positions as far apart as possible

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A pair of electrons that do not make up a bond.

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A pair of shared electrons that make up a covalent bond.

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The position of equilibrium shifts to try to cancel out any changes that you introduce.

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1. Prevent waste
2. Increase atom economy
3. Use safer methods, chemicals and solvents
4. Increase energy efficiency
5. Use renewable raw amterilas
6. use catalysts
7. prevent pollution and accidents
8. biodegradable products

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one that fully dissociates in aqueous solution.

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One that is partially dissociated in an aqueous solution.

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The enthalpy change when one mole of substance is formed from its constituent elements in their standard states.

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The total enthalpy change for a reaction is independent of the route taken from reactants to product.

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The average bond enthalpy is the average value of the enthalpy required to break a covalent bond in a gaseous molecule.

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The energy needed to start off a reaction

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The change in concentration of a reactant or product per minute.

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A compound of hydrogens and carbon containing no C to C multiple bonds

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A compound of hydrogen and carbon containing no C to C multiple bonds

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Series of compounds with the same functional group.

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Isomerism that occurs in alkenes due to restricted rotation about the double bond

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Compounds with the same molecular formula but different structural formulae (ie. arrangement of atoms)

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Combustion that occurs with excess oxygen

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Combustion that occurs in insufficient oxygen.

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A electron deficient species that can accept a lone pair of electrons

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A covalent bond breaks and each atom retains 1 of the electrons that was in the bond.

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A covalent bond breaks and 1 atom takes both electrons in the pair.

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A species with an unpaired electron

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Initiation - reaction that starts the process
Propogation - reaction by which the process continues
Termination - reaction that ends the process

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A bond formed by the sideways overlap of p electrons

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A carbon-containing positively charged ion.

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The joining of a very large number of monomer molecules to make a large polymer molecule

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An alkane in which one or more hydrogen atom have been replaced by a halogen

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process of continuous evaporation and condensation.

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Reaction with water to produce a new product.

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The more collisions between particles in a certain time, the faster the reaction.

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One that involves the loss of a small molecule to produce a double bond

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A homologous series containing OH as the functional group.

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An enzyme-catalysed reaction that converts sugars to ethanol

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A homologous series containing COOH as the functional group

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Splitting of molecules in a mass spectrometer into smaller parts.

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The wave number range at which a particular bond absorbs radiation

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One that releases energy to the surroundings, there s a temperature rise and  ΔH is negative

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Takes energy in from surroundings and temperature drops. ΔH is positive.

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catalyst is in the same phase (state) of the reactants

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1. Accepts electrons, becoming reduced in the process(group 7)
2. Give electrons, becoming oxidised in the process(metals).

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Catalyst is in a different state from the reactants