Giant Structures

Question 1

What state are giant ionic structures at room temperature?

Answer 1

solid

Question 2

Why are ionic bonds hard to break?

Answer 2

Because a lot of energy is needed to break the ionic bond due to the strong electrostatic forces

Question 3

Why do some ionic substances dissolve in water?

Answer 3

Because water molecules can split up the lattice

Question 4

What bond are atoms in a molecule held together by?

Answer 4

covalent bonds

Question 5

How high is the attraction inbetween simple molecules?

Answer 5

low because the covalent bond only acts between the atom and the molecule

Question 6

What is the melting point of simple molecules like?

Answer 6

Low because of the weak force of attraction

Question 7

Why do molecules not carry electrical charges?

Answer 7

Because they have no overall charge

Question 8

What are the forces inbetween molecules called?

Answer 8

intermolecular

Question 9

How strong are intermolecular forces?

Answer 9

weak

Question 10

What state is a molecule with very weak intermolecular forces?

Answer 10

gas at room temp

Question 11

What size do molecules with weak intermolecular forces tend to be?

Answer 11

small

Question 12

What are larger molecules with stronger intermolecular forces at room temperature?

Answer 12

liquid

Question 13

What happens when atoms with several covalent bonds join together?

Answer 13

They form giant covalent structures

Question 14

What else is a giant covalent structure known as?

Answer 14

A macromolecule

Question 15

What happens to the atoms in giant covalent structures?

Answer 15

They join together

Question 16

Why do giant covalent structures have high melting points?

Answer 16

Because it takes a lot of energy to break down the lattice

Question 17

What is diamond?

Answer 17

A form of carbon

Question 18

What is the structure of diamond like?

Answer 18

regular and 3D

Question 19

How many carbon atoms are covalently bonded to one in a diamond

Answer 19

One carbon atom is covalently bonded to 4 others

Question 20

What makes diamond hard and transparent?

Answer 20

one carbon atom being covalently bonded to 4 others

Question 21

What has a similar structure to diamond?

Answer 21

Silicon dioxide (silica)

Question 22

What is graphite?

Answer 22

A form of carbon

Question 23

How many carbon atoms are covalently bonded to one in graphite?

Answer 23

three

Question 24

What is the structure of graphite like?

Answer 24

flat and 2D layers of covalently bonded carbon atoms

Question 25

Why can the 2D layers in graphite slide over one and other?

Answer 25

Because the layers aren’t covalently bonded to one and other

Question 26

What makes graphite slippery and grey?

Answer 26

The fact that the layers can slide over one and other

Question 27

Why can graphite conduct heat and electricity?

Answer 27

Because one electron from each carbon atom is delocalised

Question 28

What are the intermolecular forces between the layers of graphite like?

Answer 28

Weak

Question 29

What are fullerenes?

Answer 29

Large molecules formed from hexagonal rings of carbon atoms

Question 30

How do the hexagonal rings of carbon atoms join in fullerenes?

Answer 30

They join together to form cage like shapes

Question 31

Can fullerenes be nanosized?

Answer 31

Yes

Question 32

Why are metals easy to shape?

Answer 32

Because their layers can slide over one and other without breaking

Question 33

How are metal atoms arranged?

Answer 33

In layers

Question 34

Why are alloys harder than pure metals?

Answer 34

Because the different sized atoms distort the layers

Question 35

Why is it easy for metals to conduct?

Answer 35

Because it is easy and quick to transfer energy throughout the lattice