U2 CHEM bonding/ionisation energy/strucutre

what are ionisation energies

amount of energy required to remove one mole of electrons from one mole of gaseous atoms of an element to form one mole of gaseous ions

what are factors affecting ionisation energies

• nuclear charge

• shielding of the outer shell from the nucleus by inner shells

• subshells

• number of shells

define metallic bonding

electrostatic attraction between sea of delocalised electrons and positive metal ions

what is ionic bonding

when metals and non-metals bond

what is covalent bonding

2 atoms share pair of electrons and held between 2 nuclei atoms by electrostatic forces of attraction

what is the relationship between bond lengths and strength

• depends on size of atomic radius of atoms involved

• number of covalent bonds between atoms

• strength of electrostatic attraction between nuclei and shared pair of electrons

name the 4 different types of covalent bonds

• single covalent bond

• double covalent bond

• triple covalent bond

• triple covalent bond including dative covalent

what is molecular orbital model

when atomic orbital of 2 atoms overlap,holds 2 atoms being shared

what is sigma molecular orbital model

if atomic orbital overlap end to end

what is pi molecular orbital model

if atomic orbitals overlap sideways

giant metallic strucutre contains…

• high melting point

• good electrical conductivity

• insoluble often react

Giant ionic strucutre contains..

• high melting point

• poor electrical conductivity when solid good when molten or dissolved in water

• generally soluble

Giant covalent contains..

• very high melting point

• poor electrical conductivity

• insoluble

simple molecular strucutre contains..

• low melting point

• poor electrical conductivity (some molecules ionise in water then conduct)

• most insoluble depends on polarity

what is electron pair repulsion theory

• shape of molecule or ion that is governed by arrangement of electron pairs around central atom

• greater numberNAM of electron pairs greater the repulsion and smaller the bond angle

NAME TYPES OF BOND ANGLES

• linear

• trigonal pair

• octahedral

types of bonds with NON BONDING Electron PAIRS

• tetrahedral

• pyramidal

• non-linear

polar

atoms have unequal pull on the electrons

non -polar

atoms have equal pull on electrons in bond

what are intermolecular forces

forces that occur between molecules much weaker than covalent bonding

what is temporary dipole

build up of electrons and the side molecules cause another molecule to act the same

what is permanent dipole

electrons pulled more towards 1 side of molecule