C3

Question 1

What is graphene?

Answer 1

A single layer of graphite and has properties that make it useful in electronics and conmposites a

Question 2

What are the properties of graphene?

Answer 2

• excellent conductor of electricity and thermal energy
• very low density
• most reactive form of carbon
• pieces of it are incredible strong for its mass

Question 3

What are fullerenes?

Answer 3

Molecules made of carbon atoms with hllow shapes . The structure of fullerenes is based on hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms.

Question 4

What was the first fullerene to be discovered?

Answer 4

Buckminsisterfullerene c60 which had a speherical shape

Question 5

What are carbon nanotubes?

Answer 5

Cylindrical fullerenes with very high length to dimater ratios. Their properties make them useful for nanotechnology, electronics and materials.

Question 6

What are the molecular forces like between buckministerfullerene?

Answer 6

Weak intermolecular forces between molecules

-slippery and low melting point

Question 7

What are the states of matter?

Answer 7

• solids
• liquid
• gases

Question 8

What is the difference between the volume and shape of the three states of matter?

Answer 8

• solids have fixed shape and volume
• liquids have a fixed volume but can change their shape
• gases have no fixed shape or volume , they can be compressed easily

Question 9

What does particle theory describe?

Answer 9

• movment of particles

- average distance between particles

Question 10

How close are the state of matters particles together?

Answer 10

• solids particles touch
• liquids particles touch but move around aswell
• gas particles do not touch

Question 11

What is needed for a solid to become a base?

Answer 11

Heat which will break bonds between atoms and increase the energy making particles move around faster and increase collisions between particles making them move around rapidly

Question 12

What takes place at the maelting point?

Answer 12

Melting and freezing

Question 13

What takes place at the boiling point?

Answer 13

Boiling and condensing

Question 14

What is the reason for a substance having a high boiling or melting point?

Answer 14

Strong forces between particles.

Question 15

What are the three types of bonding?

Answer 15

Ionic , covalent and metallic

Question 16

What compounds does ionic bonding occur in?

Answer 16

Metal and non metal

Question 17

What compound does covalent bonding occur in?

Answer 17

Non metal and non metal

Question 18

What does metallic bonding occur in?

Answer 18

Metallic elements and alloys

Question 19

How do atoms gain a stable valence shell?

Answer 19

• ionic bonding

- covalent bonding

Question 20

What happens during ionic bonding?

Answer 20

Metal atom loses electron to become positively charge ion or a non metal gains an electron to become a negatively charged ipn

Question 21

What is an ionic compound?

Answer 21

A giant structure of ions

Question 22

What holds ionic compounds toegther?

Answer 22

Strong electrostatic forces between oppositkey charged ions. These forces act in all directions in a lattice structure, this is ionic bonding.

Question 23

What is covalent bonding?

Answer 23

When atoms shair pairs of electrons , froming bonds that are strong

Question 24

What may covalently bonded substances consist off?

Answer 24

Small molcules

Question 25

What covalently bonded substances have very large molecules?

Answer 25

Polymers

Question 26

What are examples of giant covalent structures?

Answer 26

Diamond | Silicon dixoide

Question 27

What is metallic bonding?

Answer 27

Two metals reacting , forming bonds

Question 28

What do metals atoms consist off?

Answer 28

A giant structure of atoms in a regular repeating pattern

Question 29

What is the electrons configuration for metallic bonding?

Answer 29

Electrons in the outer shell are delocalised and so are free to move through the structure.

Question 30

What are the properties of ionic compounds?

Answer 30

- high melting points | - high boiling points, because large amount of energy needed to break bonds

Question 31

How do you make ionic compounds conduct electricity ?

Answer 31

Melt it or dissolve it in water. This frees up the so ions charge can flow .

Question 32

What state are small Covalent molecules usually found in?

Answer 32

Gases or liquids

Question 33

What are the melting points of small covalent molecules?

Answer 33

Low melting and boiling points

Question 34

How strong are small Covalent molecules intermolecular forces?

Answer 34

- weak intermolecular forces | - overcome when melted or boiled

Question 35

What happens as molecules get bigger?

Answer 35

Intermolecular forces increase so larger molecules have high melting and boiling points

Question 36

Do small Covalent molecules conduct electricity ?

Answer 36

No because they have no overall electric charge

Question 37

Properties of polymers?

Answer 37

- very large molecules - atoms in polymer molecules are linked to other atoms by strong covalent bonds - intermolecular forces are strong - solids at room temperature

Question 38

What are giant covalent structures?

Answer 38

Substances that are solids with very high melting points, covalently bonded.

Question 39

What is bonding like in giant covalent structures?

Answer 39

All atoms linked by strong covalent bonds

Question 40

How to melt or boil a giant covalent strcutre?

Answer 40

Overcome the strong covlent bonds .

Question 41

Properties of metals and alloys?

Answer 41

Metals have a giant structure of atoms with strong metallic bonding. Means most metals have high melting and boiling points

Question 42

What is the structure and properties of a pure metal?

Answer 42

- atoms are arranged in layers - can be bent and shaped - soft

Question 43

What are alloys?

Answer 43

Metals mixed together . They are harder than just a pure metal

Question 44

Are metals good conductors of electricity?

Answer 44

Yes, because delocalised electrons carry electrical charge through the metal. Metals are good conductors of thermal energy because energy is transferred by the delocalised electrons.

Question 45

What are the properties of diamond?

Answer 45

- formed from carbon - each carbon atoms forms four covalent bonds with other carbon atoms in a giant covalent structure - diamond is very hard - has a very high melting point - does not conduct electricity

Question 46

Properties of graphite?

Answer 46

- made of carbon - each carbon atom forms three covalent bonds with three other atoms, forming layers of hexagonal rings which have no covalent bonds between layers

Question 47

Are graphite electrons delocalised?

Answer 47

Graphite has 1 delocalised electrons

Question 48

Why can metals be bent and shaped?

Answer 48

Metal ions can slide over each other

Question 49

How are metals structured?

Answer 49

-strong electrostatic attraction between sea of delocalised negative electrons and positive metal ions

Question 50

Why can delocalised electrons carry a current?

Answer 50

Because they are charged

Question 51

Why are alloys harder?

Answer 51

Mixture of metals. The different sizes of atoms distorts the layers , making it more difficult for them to slide over each other