Bonding
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Shape and bond angle of atom with 2 BP and 0 LP
Linear 180°
Shape and bond angle of atom with 3 BP and 0 LP
Trigonal planar 120°
Shape and bond angle of atom with 2 BP and 1 LP
Bent (V-shape) 118°
Shape and bond angle of atom with 4 BP and 0 LP
Tetrahedral 109.5°
Shape and bond angle of atom with 3 BP and 1 LP
Trigonal pyramidal 107°
Shape and bond angle of atom with 2 BP and 2 LP
Bent (V-shape) 104.5°
Shape and bond angle of atom with 5 BP and 0 LP
Trigonal bipyramidal 90° and 120°
Shape and bond angle of atom with 4 BP and 1 LP
Trigonal pyramidal or see-saw 89° and 119°
Shape and bond angle of atom with 3 BP and 2 LP
Trigonal planar or T-shape 120° or 89°
Shape and bond angle of atom with 6 BP and 0 LP
Octahedral 90°
Shape and bond angle of atom with 5 BP and 1 LP
Square pyramid 89°
Shape and bond angle of atom with 4 BP and 2 LP
Square planar 90°
Ionic bonding
electrostatic attraction between oppositely charged ions in a lattice
Formulas of the following compound ions sulfate, hydroxide, nitrate, carbonate and ammonium
SO4 2- OH - NO3 - CO3 2- NH4 +
Define dative covalent bond
covalent bond formed by one atom donating its lone pair of electrons to another atom
Metallic bonding
attraction between delocalised electrons and positive ions arranged in a lattice
4 types of crystal structure
ionic metallic macromolecular (giant covalent) molecular
Why do pairs of electrons in the outer shell of atoms arrange themselves as far apart as possible
To minimise repulsion
Lone pair–lone pair repulsion is _____ than lone pair–bond pair repulsion, which is _____ than bond pair–bond pair repulsion
Greater Greater
Define electronegativity
power of an atom to attract the pair of electrons in a covalent bond
Ionic crystal structure properties, using sodium chloride as an example
-strong electrostatic forces of attraction between oppositely charged ions in a giant lattice -high melting point -can conduct electricity when molten or aqueous, as not in lattice -brittle, as like charges repel when layers of alternating charges are distorted -breaks lattice into fragments
Metallic crystal structure properties, using aluminium as an example
-strong electrostatic forces of attraction between positive nucleus and sea of delocalised electrons in a giant lattice -hence high melting point -malleable as layers can slide over each other -good conductors as sea of delocalised electrons can carry a flow of charge
Simple molecular crystal structure properties, using iodine as an example
-covalently bonded -held together by weak Van der Waals between molecules -low melting and boiling points -poor conductors as no charged particles
Macromolecular crystal structure properties, using diamond and graphite as examples
-rigid due to strength of giant lattice -very high melting point as each atom has multiple covalent bonds -sometimes has flat sheets which has delocalised electrons, hence can conduct electricity