1. Metallic Bonding
1.1. Valence electrons delocalised to form a 'sea of electrons'
1.2. Conducts electricity, malleable
2. Intermolecular Forces
2.1. London Dispersion Forces
2.1.1. Happens within every molecule(covalently bonded stuff)
2.1.2. Between non-permanent positive side of one molecule and non-permanent negative side of other molecule(determined by instantaneous electron distribution, which I think we could predict?)
2.1.3. Weakest since most all molecules have it
2.1.4. The only force present in Diatomic molecules
2.2. Hydrogen Bonds
2.2.1. Only between Hydrogen and Oxygen, fluorine and nitrogen(because very high electronegativity value)
2.2.2. Strongest force(meaning molecules with hydrogen bonds tend to have higher boiling points relative to the ones without)
2.3. Permanent Dipole Dipole
2.3.1. Between Polar Molecules(Dipole Moment)
2.3.2. More positive side attract to more negative side
3. Covalent Bonding
3.1. Polar Covalent Bonds
3.1.1. 0<=electronegativity difference<=1.8
3.1.1.1. One atom more positive, vice versa
3.1.1.1.1. induces a dipole moment-from more positive side to more negative side
3.2. Non Polar Covalent Bonds
3.2.1. Electronegativity Difference=0
3.2.1.1. Diatomic Molecules
3.3. Sigma and Pi
3.3.1. Sigma
3.3.1.1. Side on overlap
3.3.1.1.1. s-s
3.3.1.1.2. s-p
3.3.1.1.3. p-p
3.3.2. Pi
3.3.2.1. Overlap
3.3.3. Hybridisation- mixing of s and p electrons creating a new sp orbital after raising s electrons
3.3.3.1. sp3
3.3.3.1.1. 4 electron domains
3.3.3.2. sp2
3.3.3.2.1. 3 electron domains
3.3.3.3. sp
3.3.3.3.1. 2 electron domains
3.4. Polar Molecule
3.4.1. When dipole moments don't balance out
3.4.1.1. one side of molecule partially positive, vice versa
3.5. Allotropes of Carbon
3.5.1. Diamond
3.5.1.1. Giant Covalent structure
3.5.1.1.1. Very hard
3.5.1.1.2. Very Strong
3.5.1.1.3. Doesn't conduct electricity because no free electrons
3.5.2. Graphite
3.5.2.1. Giant Covalent, layered structure
3.5.2.1.1. Soft, weaker than diamond because layers are not covalently bonded, London forces
3.5.2.1.2. Malleable because layers can slide over
3.5.2.1.3. Conducts electricity because free electrons delocalized
3.5.3. Graphene
3.5.3.1. One layer of graphite
3.5.3.1.1. Very strong because no intermolecular forces, but lower melting point than diamond. Strongest material known to man
3.5.3.1.2. Conducts electricity the most well
3.5.4. Fullerene, C60, Buckyballs, not giant covalent
3.5.4.1. Football shaped, molecule of 60 carbons singly and doubly bonded together(the bonds change from time to time because there are resonance structures)
3.5.4.1.1. Not hard because intermolecular forces weak
3.5.4.1.2. Conducts electricity because electrons are delocalized when switching resonance structure