Definitions For AS OCR Chemistry 2016

Definitions from glossary in the book.

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A species that releases H+ ions in solution.
Acid
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The minimum energy required to start a reaction by the breaking of bonds.
Activation Energy
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The process that occurs when a gas, liquid or solute is held to the surface of a solid.
Adsorption
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Containing carbon atoms joined in a non-aromatic ring.
Alicyclic
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All carbon atom chains excluding aromatic rings.
Aliphatic
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A base that dissolves in water and releases hydroxide ions.
Alkali
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A carbon chain that contains one or more benzene rings.
Aromatic
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A region around the nucleus that can hold up to two electrons with opposite spins.
Orbital
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The average enthalpy change when breaking by homolytic fission one mole of a given type of bond in the molecules of a gaseous species.
Average Bond Enthalpy
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A compound that neutralises an acid to form a salt.
Base
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A compound that only contains two elements.
Binary Compound
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An ion that contains a positively charged carbon ion.
Carbocation
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A shared pair of electrons in which one of the bonding species has provided both bonding electrons. AKA Co-ordinate bond.
Dative Covalent Bond
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Release of an adsorbed substance from a surface.
Desorption
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A redox reaction in which the same element is both oxidised and reduced.
Disproportionation
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A measure of the attraction between a bonded atom and the electrons in the bond.
Electronegativity
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Electron pair acceptor.
Electrophile
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The heat content in a chemical system.
Enthalpy
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Enthalpy difference between reactants and products in a reaction.
Enthalpy Change
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An area on an infrared spectrum below 1500cm^-1 that gives a characteristic pattern for different compounds.
Fingerprint Region
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The energy required to remove one electron from each atom in 1 mole of gaseous atoms of an element to form 1 mole of gaseous 1+ ions.
The First Ionisation Energy
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A three dimensional lattice structure held together by covalent bonds.
Giant Covalent Lattice
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A three dimensional lattice structure of atoms, bonded together by strong ionic bonds.
Giant Ionic Lattice
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A three dimensional lattice structure of positive ions and delocalised electrons, bonded together by strong metallic bonds.
Giant Metallic Lattice
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A series of organic compounds with the same functional group but with each successive member differing by CH2.
Homologous Series
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The electrostatic attraction between positive metal ions and delocalised electrons.
Metallic Bonding
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An atom or group of atoms that is attracted to an electron defficient carbon atom, where it donates a pair of electrons to form a new covalent bond.
Nucleophile
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The bond formed by the sideways overlap of two P orbitals, containing two electrons and with the electron density concentrated above and below the centre of the two bonding atoms.
Pi Bond
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An ion containing more than one atom.
Polyatomic ion
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The continual boiling and condensing of a mixture back into the original container to ensure the reaction takes place fully, without the contents of the flask boiling dry.
Reflux
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A bond formed by the overlap of two S orbitals, one from each bonding atom, and consists of two electrons with the electron density directly in the middle of the two atoms.
Sigma Bond
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The product of a reaction in which the H+ ions from the acid are replaced by metal or ammonium ions.
Salt
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A group of atomic orbitals with the same principal quatum number. AKA a main energy level.
Shell
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The repulsion effect between different shells.
Shielding
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The energy required to raise the temperature of 1g of a substance by 1K.
Specific Heat Capacity
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The enthalpy change that occurs when one mole of a substance reacts completely with oxygen under standard conditions with all reactants in their standard states.
Standard Enthalpy Change of Combustion
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The enthalpy change that occurs when one mole of a compound is formed from its constituent elements under standard conditions with all reactants and products in their standard states.
Standard Enthalpy Change of Formation
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The enthalpy change that accompanies the reaction of an acid by a base to form one mole of water under standard conditions with all the reactants and products in their standard states.
Standard Enthalpy Change of Neutralisation
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100kPa and 298K
Standard Conditions
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An acid that fully dissociates in solution.
Strong Acid
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A group of orbitals of the same type within a shell.
Sub-Shell
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An acid that only partially dissociates in solution.
Weak Acid
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The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and the concentrations do not change.
Dynamic Equilibrium
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Other cards in this set

Card 2

Front

The minimum energy required to start a reaction by the breaking of bonds.

Back

Activation Energy

Card 3

Front

The process that occurs when a gas, liquid or solute is held to the surface of a solid.

Back

Preview of the front of card 3

Card 4

Front

Containing carbon atoms joined in a non-aromatic ring.

Back

Preview of the front of card 4

Card 5

Front

All carbon atom chains excluding aromatic rings.

Back

Preview of the front of card 5
View more cards

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