Chem 2 Flashcards
First ionisation energy
The energy required to remove one electron from each atom in one mole of gassiest atoms of an element to form one mole of gassiest 1+ ions
Metallic bonding
Strong electrostatic attraction between cat ions and delocalised electrons
Disproportionation
Redox reaction where the same element as both oxidised and reduced
Chlorine and sodium hydroxide
Sodium chlorate sodium chloride and water
Solubility of halogens
Iodine insoluble in concentrated ammonia bromide soluble and concentrate on ammonia chlorine soluble and die loot ammonia
Test for carbonate
React with acid to form carbon dioxide use nitric acid then bubble through limewater solution of calcium hydroxide carbon dioxide reacts to form calcium carbonate a white precipitate turning limewater milky
Test for sulphate
Barium sulphate is insoluble add a previous Barium nitrate to solution if sulfate present white precipitate will phone
Test the halogens
Add silver nitrate form precipitate then add ammonia to test solubility
Test from Ammonium ions
Add aqueous hydroxide ions such as sodium hydroxide to a solution of ammonium irons ammonia gas is produced soluble in water will turn litmus paper blue
Activation energy
The minimum energy required from reactions take place
Standard conditions
100 KP a
298K
One moledm^3
Standard state physical state of substances under standard conditions
Standard enthalpy change of reaction
The enthalpy change that accompanies a reaction in the more the quantities shown in a chemical equation in standard conditions with all reactants and products in standard states
Enthalpy change of formation
Enthalpy change that takes place when one mole of a compound is formed from its elements understand the conditions with all reactants and products in a standard states
Enthalpy change of combustion
The entropy change that takes place when one mole of a substance reacts completely with oxygen understand it conditions with all reactants and products in their standard states forms CO2 and H2O
Enthalpy change of neutralisation
The energy change that the company is a reaction of an acid with a base to form one mole of H2O understand the conditions
Specific heat capacity
The energy required to raise the temperature of 1 g substance by 1K
Average bond enthalpy
The energy required to break one mole of specify type of bond in a gaseous molecule
Lattice enthalpy
A measure of the strength of ionic bonding in a giant ionic lattice accompanies the formation of one mole of an ionic compound from its gases ions understand and conditions
Standard enthalpy change of atomisation
The energy change that takes place in the formation of one mole of gassiest atoms from the element in at standard state understand and conditions always endothermic
First ionisation energy
The energy change required to remove one electron from each atom in one mole of gassiest atoms to form one mole of gassiest 1+ ions endothermic
Electron affinity
The energy change that takes place when one electron is added to each atom in one mole of gassiest atoms to form one mole of gassiest one minus ions
Enthalpy change of solution
The enthalpy change that takes place when one mole of a solid solid dissolves in a solvent if the solvent is water the ions from the ionic lattice finish up surrounded by water molecules as aqueous ions
Enthalpy change of hydration
When separate gassiest ions interact with the polo water molecules to form hydrated aqueous ions
Which elements form giant covalent structures
Carbon silicon and boron
Giant covalent lattice
Billions of atoms held together by network a strong covalent bonds
Electron pair repulsing theory
A model used in chemistry to explain and predict the shape of molecules and polyatomic ion is
Intermolecular forces
Week interactions between dipole of different molecules
