Structure

Question 1

Ionic Structures

Answer 1

Lattice Structure (3D) - Arrays/Layers of positive negative Ions (Always alternating)

Ionic Bonds - High melting point - Strong bonds = takes more heat to break

Higher Ionic charge means more heat needed to break

Question 2

Simple Covalent Bonds

Answer 2

Small molecules restricted to atoms in its molecular formula e.g H2O has only 3 atoms

Buckminster fullerene is restricted to 60 carbon atoms

Type - Simple Covalent
Strength - Weak intermolecular forces
Energy - Not much energy needed to overcome

Question 3

Giant Covalent (1)

Answer 3

Diamond:

Giant covalent structure, many strong bonds, lot of energy needed to break bonds - Same for SiO2 (Sand)

Conduction - Doesnt conduct as electrons not free to move (Localised)

Arrangement - Tetrahedral structure with 4 Bond

Question 4

Giant Covalent (2)

Answer 4

Graphite:

Structure - Layered, 1 electron between layers

High melting point - G.C.S , Many strong bonds, takes alot to break bonds

Conductivity - Can conduct as 1 electron between layers in delocalised (free to move)
Explain Graphite a lubricant - weak I.M bonds and is layered so layers can slide over 1 another so can be a lubricant

Question 5

Metallic Structures

Answer 5

-Positive cations surrounded in a lattice structure by a sea of delocalised electrons. Electrons can move so can conduct electricity

• Type: Metallic - sea of delocalised electron
• Strength: Positive attracted to negative in strong bond
• Energy - Lots of energy required to break Bonds

Question 6

Structure Q’s Mark scheme

Answer 6

Type - Simple Covalent, G.C., Ionic, Metallic
Strength or how many - Strong bonds , weak I.M.F
Energy needed - Lots, Not much

Can conduct when Electrons free to move - Sea of delocalised electron