C2-Bonding,structure and properties of matter

Topic 2a

What is ionic bonding? 

When a metal and a non-meta react together,  a metal atom LOSES electrons and a non-metal atom GAINS electrons

What are the properties of an ionic compound? (6) 

• Giant regular lattice

• STRONG ionic bonds

• Strong electrostatic forces of attraction

• High melting and boiling points (Lots of energy to over come attraction) 

• Can't conduct electricity when solid (ions can't move) 

• Can conduct electricity when liquid (ions can move) 

Why do ionic compounds have high melting points? 

Strong electrostatic attractions between ions require lots of energy to overcome. 

Why do ionic compounds conduct when dissolved in water? 

The ions are free to move and carry charge.  (Delocalized)

What structure do ionic compounds form? 

A giant ionic lattice 

Why do ionic compounds conduct when dissolved in water?

The ions are free to move and carry charge 

What is covalent bonding?

When a non-metal and a non-metal react together they share pairs of elecrons

What are the types of covalent bonding?

• Giant covalent bond

• Simple covalent bond

Are the covalent bonds broken when a simple molecular substance melts? 

No, only the weak intermolecular forces are overcome. 

Why does a simple molecular substance have a low boiling point? 

Weak intermolecular forces are easily overcome. 

Explain why magnesium chloride has a high melting point.

Strong electrostatic attractions between oppositely charged ions require lots of energy to overcome. 

What is the key difference between ionic and simple covalent substances? 

Ionic bonding shows the transfer of electrons whereas SIMPLE covalent substances shows shring electrons.

What are the properties of a SIMPLE covalent bond?

• Strong covalent bond

• Weak intermolecular forces between molecules

• Can't conduct electricity (no free particles) 

• Low melting and boiling point

• Made of a few atoms

Explain why chlorine gas has a low boiling point. 

Chlorine molecules have weak intermolecular forces that require little energy to overcome.

What are the properties that all 3 giant covalent structure share?

• Giant

• Strong covalent bond

• Lots of energy to overcome (don't conduct electricity except graphite)

What are the properties of diamond? (6) 

• Each carbon has 4 bonds

• Tetreheadral shape

• Very hard

• Useful for cutting

• Doesnt conduct electricity becasuse there is no delocalized electrons

What are the properties of graphite? (5)

• Each carbon has 3 atoms

• forms layers of hexagonal rings, creating layers

• Weak forces between layers which can slide over eachother making it useful as a lubricant

• Each carbon atom has one delocalized electron which moves through the structure carry charge and electricity.

What are the allotropes of carbon?

• Diamond

• Graphite

• Graphene

• Fullerenes

What is graphene?

• One layer of graphite

• Strong and lightweight- composite materials

• Contains delocalised electrons so can conduct electricity and be used in electronics

What is properties of buckminster fullerene?

• Sphereical shape

• Transports drugs around body

• High surface area:vloume ratio (used as catalyst)

• good lubricant, can roll

Properties of carbon nanotubes?

• Conduct heat and electricity

• High tensile strenght, pull weights

• graphene rolled into cylindrical shape