Topic 2 Bonding + Structure Flashcards
What is Ionic Bonding
Between oppositely charged ions. Strong electrostatic attraction
Smaller ionic radius and higher ionic charge have what effect
Increases strength of bond
3 Physical properties of ionic compounds
High melting point
Non conductor of electricity when solid but conductor when molten or liquid
Brittle
What is Covalent bonding
Electrostatic attraction between a shared pair of electrons and the nuclei
Long bond vs short bond strength why
short is stronger due to increased electrostatic attraction
London Forces
Instantaneous dipole, induced dipole
More electrons means more london forces
Pernament dipole caused by
polarity of atoms in molecule
What causes hydrogen bonding
slightly positive hydrogen and slightly negative other molecule
branched vs non branched boiling
Branched is lower due to worse packing together
Why alcohols have a high boiling point
Hydrogen bonding
Trend in boiling point of hydrogen halides
HF is very high then increasing from HCL to HI. Increase in London forces (van der waals) outweighs electronegativity difference or length of bond
Metallic Bonding is what
Strong electrostatic attraction between metal ions and sea of delocalised electrons
Where are giant lattices present
Ionic solids (giant ionic lattices)
Covalently bonded solids (giant covalent lattices)
Solid metals (giant metallic lattices)
Structure of covalently bonded substance
Simple molecular
Allotropes of carbon
Diamond - Everything has 4 covalent bonds
Graphite - Graphene layers with 3 covalent bonds, London forces between layers
Graphene - Thin sheet 3 covalent
