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34 Cards in this Set
- Front
- Back
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Relative Atomic Mass |
(Average mass of one atom of an element) / (one twelfth the mass of an atom of carbon-12) |
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Relative molecular mass |
(Average mass of an entity) / (one twelfth the mass of an atom of carbon-12) |
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1 Mole |
Avogadro's number of particles |
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Empirical Formula |
Simplest ratio of atoms of each element in a compound |
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Molecular Formula |
Actual number of atoms of each element in a compound |
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Electronegativity |
The power of an atom to attract a pair of electrons in a covalent bond |
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Covalent bond |
Shared pair of electrons |
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Co-ordinate Bond |
A covalent bond in which both electrons are donated from one atom |
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Ionic bond |
Strong electrostatic forces of Attraction between oppositely charged ions |
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Metallic Bond |
Strong electrostatic forces between positive ions and delocalized electrons |
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Enthalpy change |
Heat change under standard conditions |
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Enthalpy of combustion |
Enthalpy change when 1 mole of a compound is burnt completely in oxygen and a standard conditions all substances in standard States |
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Enthalpy of formation |
The enthalpy change when 1 mole of a compound is formed from its elements under standard conditions with all substances in standard states |
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Hess's law |
The enthalpy change in a reaction is independent of the route taken and depends only on the initial and final States |
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Bond enthalpy |
Enthalpy required break one mole of covalent bonds |
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Mean Bond enthalpy |
Enthalpy required to break one mole of covalent bonds average over a range of compounds |
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Rate of reaction |
Change in concentration divided by time |
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Dynamic equilibrium |
Forward rate of reaction equals backwards rate of reaction Concentrations of reactants and products are constant |
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Activation energy |
The minimum energy for a reaction to occur |
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Catalyst |
A substance that speeds up the rate of reaction but is not used up It provides an alternative route that lowers activation energy |
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Oxidation |
Loss of electrons |
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Reduction |
Gain of electrons |
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Oxidising agent |
Gains electrons |
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Reducing agent |
Loses electrons |
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Test for chloride ions |
Add acidified (nitric acid) silver nitrate white precipitate will form Add dilute ammonia solution it will dissolve
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Test for bromide ions |
Add silver nitrate acidified with nitric acid a cream precipitate will form then add dilute ammonia the precipitate is partially soluble then add concentrated ammonia the precipitate will dissolve |
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Test for iodide ions |
Silver nitrate acidified with nitric acid yellow precipitate will form add concentrated ammonia precipitate will not dissolve |
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Carbonate ion test |
Add dilute hydrochloric acid the solution will fizz this is called effervescence |
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Sulphate ion test |
Add barium chloride solution acidified with nitric acid a white precipitate of barium sulphate is formed |
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Hydroxide ion test |
Add magnesium chloride a white precipitate is formed. Or add universal indicator and it will turn blue as hydroxide ions are alkaline |
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Magnesium ion test |
Add sodium hydroxide and a white precipitate will form |
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Barium ion test |
Add sulphuric acid a white precipitate formed |
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Ammonium ion test |
Warm carefully in a test tube with damp litmus paper over the top it should turn blue |
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Fluoride ion test |
Add silver nitrate acidified with nitric acid no visible change |
