Bonding Notes
Electrostatic forces → oppositely charged ions → positive ions and delocalised electrons
Lattice structure
Electricity → free charged particles (electrons or ions) carry current or charge
- Ionic compounds = brittle
1. Small displacement causes contact of ions of same charge
2. Which repel and structure shatters
Can dissolve in water (polar solvents) as delta+ H attracted to polar non-metal and delta- oxygen
attracted to polar metal
- Covalent → within molecules (intramolecular), held together by electrostatic forces of
attraction between nuclei and shared electrons
- Dative covalent → lone pair →electron deficient (empty orbital)
Common is ammonia, H3O+ , F3BNH3
Coordinate bonds are of same strength and length as ordinary
covalent bonds
Simple molecular substances
Most covalent molecules stay as
molecules when dissolved in water
and will not conduct electricity. - Metallic bonding outer main levels of atoms merge so outer
Hydrogen chloride (HCl) reacts with electrons no longer associated with any one particular atom.
water to form ions → will conduct Giant structures as metallic bonding spreads throughout metal
electricity Electricity – an electron from -ve terminal join electron sea at
𝐻𝐶𝑙(𝑔) + 𝑎𝑞 → 𝐻 + (𝑎𝑞) + 𝐶𝑙 − (𝑎𝑞) one end of the wire as a different electron leaves wire at
positive terminal.
Also ethanoic acid in water
Strength of metals depends on charge and size
Electronegativity – F is 4.0 on Pauling scale F—O—N/Cl—Br
Generally, bond is non-polar if electronegativity difference is less than 0.4
Depends on 1. Nuclear charge 2. Atomic radius 3. shielding
Electron density – electron charge clouds in non-polar bonds, there is uniform distribution due to
same or very similar electronegativities.
Electrostatic forces → oppositely charged ions → positive ions and delocalised electrons
Lattice structure
Electricity → free charged particles (electrons or ions) carry current or charge
- Ionic compounds = brittle
1. Small displacement causes contact of ions of same charge
2. Which repel and structure shatters
Can dissolve in water (polar solvents) as delta+ H attracted to polar non-metal and delta- oxygen
attracted to polar metal
- Covalent → within molecules (intramolecular), held together by electrostatic forces of
attraction between nuclei and shared electrons
- Dative covalent → lone pair →electron deficient (empty orbital)
Common is ammonia, H3O+ , F3BNH3
Coordinate bonds are of same strength and length as ordinary
covalent bonds
Simple molecular substances
Most covalent molecules stay as
molecules when dissolved in water
and will not conduct electricity. - Metallic bonding outer main levels of atoms merge so outer
Hydrogen chloride (HCl) reacts with electrons no longer associated with any one particular atom.
water to form ions → will conduct Giant structures as metallic bonding spreads throughout metal
electricity Electricity – an electron from -ve terminal join electron sea at
𝐻𝐶𝑙(𝑔) + 𝑎𝑞 → 𝐻 + (𝑎𝑞) + 𝐶𝑙 − (𝑎𝑞) one end of the wire as a different electron leaves wire at
positive terminal.
Also ethanoic acid in water
Strength of metals depends on charge and size
Electronegativity – F is 4.0 on Pauling scale F—O—N/Cl—Br
Generally, bond is non-polar if electronegativity difference is less than 0.4
Depends on 1. Nuclear charge 2. Atomic radius 3. shielding
Electron density – electron charge clouds in non-polar bonds, there is uniform distribution due to
same or very similar electronegativities.
