Keywords

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  • Created by: Jadziah16
  • Created on: 29-03-17 11:25
number of protons in the nucleus
Proton number
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number of protons and neutrons in the nucleus
Mass number
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atoms of an element with different numbers of neutrons and different masses
Isotopes
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average mass of an atom relative to 1/12 of the mass of a carbon-12 atom
Relative atomic mass
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mass of a particular isotope relative to 1/12 of the mass of a carbon-12 atom
Relative isotopic mass
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a region that can hold up to 2 electrons with opposite spins
Orbital
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energy change when one mole of electrons is removed from one mole of gaseous atoms to form one mole of 1+ ions
1 st ionisation energy
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energy change when one mole of electrons is removed from one mole of gaseous positively charged ions
Successive ionisation energy
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average mass of a molecule relative to 1/12 of the mass of a carbon-12 atom
Relative molecular mass
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average mass of an entity relative to 1/12 of the mass of a carbon-12 atom
Relative formula mass
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number of particles present in a mole (6.02 x 10 23 mol -1 )
Avogadro constant
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simplest whole number ratio of the atoms of each element in a compound
Empirical formula
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actual number of atoms of each element in a molecule
Molecular formula
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The ratio in which the reactants react and products are produced
Stoichiometry
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(mass of desired product/mass of all reactants) x 100
Atom economy
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electrostatic attraction between oppositely charged ions
Ionic bond
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a shared pair of electrons
Covalent bond
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attraction between positive ions and delocalised electrons
Metallic bond
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forces of attraction and repulsions between charged particles
Electrostatic forces
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ability of an atom to attract the electrons in a covalent bond
Electronegativity
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reaction in which heat energy is given out
Exothermic
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reaction in which heat energy is absorbed
Endothermic
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Temperature 298K, pressure 100 kPa
Standard conditions
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Enthalpy change when the reaction occurs in the of reaction, molar quantities shown in the chemical equation
Enthalpy change of reaction
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Enthalpy change when one mole of a compound is formed from its elements in their standard states
Enthalpy change of formation
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Enthalpy change when one mole of a substance is completely burnt in oxygen
Enthalpy change of combustion
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Total enthalpy change is independent of route
Hess’s Law
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Energy needed to break one mole of gaseous bonds
Average bond enthalpy
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the minimum energy a particle needs to react
Activation energy
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provides an alternative reaction pathway with a lower activation energy
Catalyst
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Forwards and backwards reaction proceed at same rate. Concentrations of reactants and products is constant
Features of dynamic equilibrium
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When the conditions on a system in equilibrium are changed, the equilibrium moves to oppose the change
Le Chatelier’s Principle
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loss of electrons or increase in oxidation number
Oxidation
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gain of electrons or decrease in oxidation number
Reduction
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a reaction in which an element is simultaneously oxidised and reduced
Disproportionation
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patterns repeated across different periods (rows of the Periodic Table)
Periodicity
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group of atoms responsible for characteristic reactions of the molecule
Functional Group
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a series of molecules with the same functional group but each successive member differing by CH2
Homologous series
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same molecular formula different structural formula
Structural isomers
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same structural formula different arrangement of the bonds in space
Stereoisomers
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a compound that contains hydrogen and carbon only
Hydrocarbon
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contains only single C-C bonds
Saturated
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contains one or more double C=C bonds
Unsaturated
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mixture of compounds of similar boiling point
Fraction
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contains an unpaired electron
Radical
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Electron pair donor
Nucleophile
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electron pair acceptor
Electrophile
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breaking a long chain alkane into a shorter chain alkane and an alkene
Cracking
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Other cards in this set

Card 2

Front

number of protons and neutrons in the nucleus

Back

Mass number

Card 3

Front

atoms of an element with different numbers of neutrons and different masses

Back

Preview of the front of card 3

Card 4

Front

average mass of an atom relative to 1/12 of the mass of a carbon-12 atom

Back

Preview of the front of card 4

Card 5

Front

mass of a particular isotope relative to 1/12 of the mass of a carbon-12 atom

Back

Preview of the front of card 5
View more cards

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