Bondings
1. Ionic bond
- electrostatic force of attraction between oppositely charged ions
- between metals and non- metals
2. Covalent bond
- Electrostatic force of attraction between negative shared electron pairs and
positive nucleus
- does not consist of charged particles
- only between non- metals
3. Metallic bond
- electrostatic attraction between a lattice of positively charged ions surrounded
by a ‘sea’ of delocalised electrons
- only between metals
, Simple Molecular Structure
Structure
- Gas, liquid, solid
- Atoms are held by very strong covalent bonds
Properties
- Low mp, low bp
(intermolecular forces are weak ----> little energy is needed to overcome)
- Does not conduct electricity
(does not consist of delocalised electrons or mobile ions -----> does not have an
overall charge)
Giant Ionic Structure
Structure
- Ionic lattice of alternating cations and anions -----> form crystals
Properties
- High mp, high bp
(held by strong ionic bonds ---> lots of energy needed to separate ions/ break the
bonds)
- Cannot conduct electricity at solid state, but can conduct electricity at liquid state or
in aqueous solution
(at solid state; ions are immobile; bonded together in a lattice)
(at liquid state or in aqueous solution; ions are mobile and free to move through)
- Brittle
(when layer of ions is shifted, ions of the same charge line up and they repel against
each other)
1. Ionic bond
- electrostatic force of attraction between oppositely charged ions
- between metals and non- metals
2. Covalent bond
- Electrostatic force of attraction between negative shared electron pairs and
positive nucleus
- does not consist of charged particles
- only between non- metals
3. Metallic bond
- electrostatic attraction between a lattice of positively charged ions surrounded
by a ‘sea’ of delocalised electrons
- only between metals
, Simple Molecular Structure
Structure
- Gas, liquid, solid
- Atoms are held by very strong covalent bonds
Properties
- Low mp, low bp
(intermolecular forces are weak ----> little energy is needed to overcome)
- Does not conduct electricity
(does not consist of delocalised electrons or mobile ions -----> does not have an
overall charge)
Giant Ionic Structure
Structure
- Ionic lattice of alternating cations and anions -----> form crystals
Properties
- High mp, high bp
(held by strong ionic bonds ---> lots of energy needed to separate ions/ break the
bonds)
- Cannot conduct electricity at solid state, but can conduct electricity at liquid state or
in aqueous solution
(at solid state; ions are immobile; bonded together in a lattice)
(at liquid state or in aqueous solution; ions are mobile and free to move through)
- Brittle
(when layer of ions is shifted, ions of the same charge line up and they repel against
each other)
