Bonding

Question 1

Metallic

Answer 1

-Between two metals
-Delocalised electrons move freely throughout giant metallic lattice
-Giant structure

Question 2

Ionic

Answer 2

Between a metal and non-metal.
High melting and boiling points; strong electrostatic attraction, so takes more energy to break down bonds.

Question 3

Covalent

Answer 3

-Between two non-metals
-Low melting and boiling points.
-Weak intermolecular forces to it requires less energy to break down bonds.

Question 4

Giant covalent

Answer 4

-Example: graphite
-Made from layers of atoms.
-Delocalised electrons can move through the layers easily.
-Layers slide over each other, because no covalent bonds between layers, making graphite soft/slippery.

Question 5

Giant ionic

Answer 5

-Takes a lot of energy to break strong bonds acting in all directions, that hold lattice together.
-High melting points, solids at room temp.
-Conduct electricity when molten or dissolved in water, because ions can become mobile and carry charge through liquid.

Question 6

Fullerenes

Answer 6

-Can form large case-like structures based on hexagonal rings of carbon atoms.
-Used as catalysts

Question 7

Graphene

Answer 7

-Single layer of graphite
-One atom thick
-Conducts electricity

Question 8

Alloys

Answer 8

-Harder than pure metals
-Mixture of two or more elements, at least one of which is a metal
-Different sized atoms from different elements, making harder for the layers to slide over each other.

Question 9

Simple molecules

Answer 9

-Low melting/boiling point
-weak intermolecular forces
-no overall charge