Topic 2

Question 1

What is ionic bonding

Answer 1

Metal + non metal

Question 2

What’s the ionic bonding between group 1 and group 7

Answer 2

G1 metal loses 1 electron to form positive ion
G7 non metal gain 1 electron to form negative ion

Question 3

What happens when a group 2 metal reacts with a group 6 non metal

Answer 3

G2 metal loses 2 electrons to form 2+ ion
G6 non metal gains electron to form 2- ion

Question 4

What do ionic compounds form

Answer 4

Giant ionic lattices

Question 5

What are the properties of giant ionic lattices

Answer 5

Every p+ ion surrounded by n- ions
3D structures
Very strong forces of attraction between ions ( electrostatic forces of attraction)

Question 6

What are melting and boiling points like in ionic compounds

Answer 6

High
As strong electrostatic forces of attraction
Requires great deal of energy to break

Question 7

Why can’t ionic compounds conduct electricity when solid + when can they conduct electricity

Answer 7

As ions are locked in place by strong forces of attraction
Can conduct when molten or dissolved in water (can move and carry electrical charge)

Question 8

What’s covalent bonding between

Answer 8

2 non metals

Question 9

What happens when 2 hydrogens bond covalently

Answer 9

2 hydrogen atoms overlap and share electrons to achieve full out energy level (H-H)

Question 10

What happens when 2 hydrogens bond covalently

Answer 10

2 hydrogen atoms overlap and share electrons to achieve full out energy level (H-H)

Question 11

What happens when 2 chlorine atoms covalently bond (7 electrons in outer energy leve)

Answer 11

Requires one more electron
Overlap outer energy levels form a single covalent bond (Cl^2)

Question 12

Why do small covalentl molecules have low melting and boiling points

Answer 12

Atoms held by strong covalent bond and weak intermolecular forces
Which don’t require a lot of energy to break

Question 13

What if we increase temp of small covalent molecules

Answer 13

Vibrations increase
Breaks weak intermolecular forces
Molecules turn to a gas (boil)
Therefore doesn’t require a lot of energy to break bonds

Question 14

Why don’t small covalent molecules conduct electricity

Answer 14

As they don’t have an overall charge

Question 15

What’s graphene

Answer 15

Single layer of graphite

Question 16

Why is graphene a good conductor of electricity

Answer 16

Has delocalised electrons which are free to carry charge -> so useful in electronics

Question 17

Why do graphene have high M+ b points

Answer 17

Large number of covalent bonds
Useful in producing new materials

Question 18

What are diamond and silicon dioxide examples of

Answer 18

Giant covalent substances

Question 19

Why do diamond and silicon dioxide have high M B points

Answer 19

Must break the millions of covalent bonds
Requires a lot of energy

Question 20

What are properties of diamon

Answer 20

Lots of carbon atoms joined by covalent bonds so very hard
Cannot conduct electricity as all outer electrons are in covalent bonds (no free electrons to carry charge)
High m b points

Question 21

Silicon dioxide properties

Answer 21

Huge number of covalent bonds
Very high melting and boiling points

Question 22

What are properties of graphite

Answer 22

Soft and slippery
High m b point
Good conductor of electricity and heat

Question 23

How many atoms do graphite bond to

Answer 23

3

Question 24

What do graphite form + what is the arrangement + what does this mean

Answer 24

Hexagonal rings (6 carbon atoms)
Arranged into layers with no covalent bonds
So layers can slide over each other (can be used as lubricants)

Question 25

Why can graphite conduct electricity

Answer 25

Delocalised electron
That can move and carry electric current

Question 26

What are properties of fullerene

Answer 26

Hollow shapes
Hexagonal rings of carbon atoms

Question 27

What is buckminsterfullerene used for

Answer 27

60 carbon atoms
Use to deliver drugs in body + lubricants (due to hollow shape)

Question 28

What are carbon nanotubes + uses

Answer 28

Fullerenes shaped into long cylinders with small diameter
High tensile strength + delocalised electrons
So useful in reinforcing materials

Question 29

How are polymers made

Answer 29

Joining together thousands of monomers

Question 30

Why do polymers high m and b points

Answer 30

Strong Intermolecular forces of attraction between molecules
Lots of energy to break

Question 31

What do metals consist of

Answer 31

Giant structure of atoms arranged in regular layers
Have sea of delocalised electrons
So strong electrostatic forces of attraction between delocalised electrons and positive ions

Question 32

How are metallic bonds formed

Answer 32

the sea of delocalised electrons and positive metal ions
have Strong electrostatic forces of attraction = metallic bond (strong)

Question 33

Why do metals have high m b points

Answer 33

Have to break strong metallic bonds
Requires lots of energy

Question 34

Why do metals have high m b points

Answer 34

Have to break strong metallic bonds
Requires lots of energy

Question 35

Why are metals good conductors of heat and electricity

Answer 35

Delocalised electrons can move
And can carry electric current and thermal energy

Question 36

Why are metals good conductors of heat and electricity

Answer 36

Delocalised electrons can move
And can carry electric current and thermal energy

Question 37

Properties of metals

Answer 37

Can be bent and shaped as layers of atoms can slide over each other

Question 38

Why are alloys useful

Answer 38

Mixture of metals
The different sizes of atoms distort the layers
Making it more difficult to slide over each other
Making alloys harder than pure metals

Question 39

Why are alloys useful

Answer 39

Mixture of metals
The different sizes of atoms distort the layers
Making it more difficult to slide over each other
Making alloys harder than pure metals