Name: Fran Yu Partner: Natasha Karatzas Date: 26 /05/2014
Introduction:
Bond types
Properties
Relation
Observations
Ionic
Poor conductors of electricity in solid state
Ions are fixed in place in the lattice.
It is cannot conduct electricity. (E.g. when it connects with a bulb, it cannot lighten the bulb)
Good conductors of electricity in liquid state and when in solution
Ions are now free to move through liquid or solution.
It is can conduct electricity well. (E.g. when it connects with a bulb, it can lighten the bulb)
High melting point
Strong electrostatic attraction between cations and anions.
We have to heat it in a high temperature for long time to melt it.
Brittle
If the lattice is disrupted, cations are forced next to cations, anions next to anions resulting in repulsions that break the crystal apart.
When we use a hammer to smash a substance, the big piece of it will become to be many small particles.
Metallic
Good conductors of electricity in any states
Mobile electrons in the sea of delocalized valence electrons.
It is can conduct electricity well. (E.g. when it connects with a bulb, it can lighten the bulb)
Malleable/Ductile
Lattice of cation is still hold together by sea of electrons even if the lattice is distracted.
Your can easily band it without break it.
Mid high melting/boiling point
Strong electrostatic attraction between cations and electrons.
We have to heat it in a high temperature for a well to melt it.
Covalent molecular – polar
Low and lower melting point
Relatively weak bonding
It is easy to melt it OR it is a liquid in room temperature.
Poor conductors of electricity in any states
There are no free-moving electron particles through it.
It is cannot conduct electricity. (E.g. when it connects with a bulb, it cannot lighten the bulb)
Soluble in water
Polar substances mix with each other. Non-polar substances mix with each other. Polar substance and non-polar substance don’t mix with each other.
Water is a polar-bonding covalent molecular substance. So it can mix with water.
Bond types
Properties
Relation
Observations
Covalent molecular – non-polar
Lower still melting point
Relatively weakest bonding
It is easy to melt it OR it is a liquid in room temperature.
Poor conductors of electricity in any states
There are no free-moving electron particles through it.
It is cannot conduct electricity. (E.g. when it connects with a bulb, it cannot lighten the bulb)
Insoluble in water
Polar substances mix with each other. Non-polar substances mix with each other. Polar substance and non-polar substance don’t mix with each other.
Water is a polar-bonding covalent molecular substance, not non-polar, so it cannot mix with water.
Covalent layer lattice
Very high melting/boiling point
Strong electrostatic attraction between cations and anions.
We have to heat it in a high temperature for long time to melt it. Mostly, we can’t melt it in the lab.
Good conductors of electricity in solid states
Good conductor of electricity within a layer but not between
It is can conduct electricity well. (E.g. when it connects with a bulb, it can lighten the bulb)
Layers slide over each other
Between layers only weak dispersion forces apply and the distance between layers is greater than atomic separation within layers.
When your rub the substance, you will feel that it is slide over each other and there will be some residues on your fingers.
Brittle
Layers slide past one another easily.
When we use a hammer to smash a substance, the big piece of it will become to be many small particles.
Covalent network lattice
Very very high melting/boiling point
Strong electrostatic attraction between cations and anions.
We can’t melt it in the lab because we can’t provide such a high temperature.
