giant covalent structures

Question 1

name the type of bonding in diamond

Answer 1

covalent

Question 2

name the atoms diamond is made from

Answer 2

carbon

Question 3

how many atoms in each carbon atom in diamond bonded to?

Answer 3

4

Question 4

state two properties of diamond and why

Answer 4

•high melting/boiling point (more intermolecular forced, more energy to break)
•hard (many covalent bonds, requires a lot of energy to break)
•poor electricity conductivity (no delocalised electrons)

Question 5

state two uses of diamond

Answer 5

•drills
•glass cutting

Question 6

name the bonding of graphite

Answer 6

covalent

Question 7

name the atoms graphite is made from

Answer 7

carbon

Question 8

how many atoms is each carbon atom in graphite bonded to?

Answer 8

3

Question 9

state the uses of graphite

Answer 9

•pencil
•lubricant

Question 10

explain why graphite can be using in pencil?

Answer 10

layers with weak bonds, require little energy to break.

Question 11

graphite is a hood conductor of thermal energy and electricity. why?

Answer 11

it has delocalised electrons which means they can move freely through the structure.

Question 12

can solid ionic compounds conduct electricity? why/why not?

Answer 12

no
the ions are fixed in a giant lattice so the ions cannot move or carry charge, only vibrate.

Question 13

can molten ionic compounds conduct electricity? why/why not?

Answer 13

yes
the giant lattice is broken so the ions are free to move and are able to carry charge

Question 14

can dissolved ionic compounds conduct electricity? why/why not?

Answer 14

yes
the giant lattice is broken so the ions are free to move and can carry charge

Question 15

can dissolved ionic compounds conduct electricity? why/why not?

Answer 15

yes
the giant lattice is broken so the ions are free to move and can carry charge