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