ionic, covalent and metallic bonding

what is ionic bonding

electrostatic force of attraction between oppositely charged ions formed by electron transfer

structure of ionic bonding

giant lattice

properties of ionic bonding

Brittle

High melting point

Hard

Non-Conductive

What is covalent bonding?

sharing of electrons

what is a molecule

A small group of covalently bonded atoms

properties of covalent bonding

- Low melting and boiling points- weak intermolecular forces

- Do not conduct electricity

how are atoms held together in covalent bonding?

by the electrostatic attraction between nuclei and shared electrons

single vs double covalent bonds in terms of strength

a single covalent bond is weaker than a double covalent bond as less electrons are being shared so weaker electrostatic attraction between nuclei and covalent bond

what is dative (coordinate) covalent bonding?

shared pair of electrons in the covalent bond come from only one of the bonding atoms

what is metallic bonding?

electrostatic force of attraction between the positive metal ions and the delocalised electrons

what factors affect the strength of a metallic bond?

1. Number of protons/ Strength of nuclear attraction.

2. Number of delocalised electrons per atom

3. Size of ion.

how does number of protons affect strength of metallic bond?

more protons = stronger bond

how does the number of delocalised electrons per atoms affect the strength of metallic bonding

more delocalised electrons = greater charge = stronger bond

how does size of an ion affect strength of metallic bonding?

smaller= stronger

how does metallic bonding explain malleability/ductility

atoms in layers which can slide over each other without breaking