Covalent Bonding
- Created by: Chloe Smith
- Created on: 16-04-13 20:18
View mindmap
- Covalent Bonding
- Simple
- Can be polar
- Small
- Low boiling and melting point
- tend to be gases at room temperature
- except water
- Strong intermolecularbonds
- Hydrogen bonding (strongest)
- Permanent dipole-permanent dipole
- Instantaneousdipole-induced dipole (weakest)
- Strong intermolecularbonds
- Solubility
- In polar solvents e.g. water
- polar substances can be soluble
- In non polar solvents e.g. hexane
- non polar substances can be soluble
- In polar solvents e.g. water
- Giant
- High melting point
- High boiling point
- insoluble
- non-discrete
- Three allotropes of carbon
- Graphite
- delocalised electrons
- layers that can slide past each other
- good conductor of electricity
- good lubricant
- Diamond
- each carbon is joined tetrahedrally to four other carbon atoms, by strong covalent bonds
- the very strong C-C bonds and highly symmetrical network structure make diamond the hardest naturally occuring substance.
- Fullerenes
- C60
- buckyballs
- Graphite
- Period 2 elements
- N2 (g) is diatomic with a triple bond and 2 lone pairs
- O2 (g) is diatomic with a double bond and 4 lone pairs
- F2(g) is diatomic with a single bond and 6 lone pairs
- Period 3 elements
- P4 (s)
- S8(s)
- CO2 and SiO2
- CO2
- molecular structure with 3 atoms bonded in a linear arrangement,
- weak intermolecularbonds so little energy is needed to pull the molecules about therefore low boiling/melting points
- polar intramolecularbonds so dissolves in water easily
- SiO2
- Si atoms are larger than C and have more electrons so are unable to make double bonds.
- has a giant network structure which needs a lot of energy to overcome these intramolecularbonds
- has high melting and bioling point and doesnt dissolve in water
- CO2
- Simple
Comments
No comments have yet been made