Structure and Bonding

Question 1

What is the name of the structure that ionic compounds form?

Answer 1

Giant Ionic lattice

Question 2

What charge do metal ions have?

Answer 2

Positive

Question 3

What charge do non-metal ions have?

Answer 3

Negative

Question 4

What charge do Group 1 ions have?

Answer 4

1+

Question 5

What charge do group 2 ions have?

Answer 5

2+

Question 6

What charge Group 3 ions have?

Answer 6

3+

Question 7

What charge do group 5 ions have?

Answer 7

3-

Question 8

What charge do Group 6 ions have?

Answer 8

2-

Question 9

What charge do Group 7 ions have?

Answer 9

1-

Question 10

Are the attractions between positive and negative ions in an ionic lattice strong or weak?

Answer 10

Strong

Question 11

What are the strong attractions between the +ve and -ve ions in an ionic lattice called?

Answer 11

Strong electrostatic forces

Question 12

Why do ionic compounds have high melting and boiling points?

Answer 12

Because they have strong electrostatic forces which require a great deal of thermal energy to break.

Question 13

Why can’t ionic compounds conduct electricity when they are solids?

Answer 13

Because the ions cannot move as they are locked in place by the strong electrostatic forces of attraction, meaning they cannot carry the charge.

Question 14

Why can ionic compounds conduct electricity when molten or dissolved in water?

Answer 14

They are no longer locked in place by electrostatic forces and therefore the ions can move and carry a charge.

Question 15

What is an ion?

Answer 15

A charged particle

Question 16

True or False: The non-metal atom gains an electron in an ionic bond.

Answer 16

True - The non-metal atom gains the electron

Question 17

Ions have a full …

Answer 17

Outer shell

Question 18

Covalent bonds are formed between two…

Answer 18

Non-metal atoms

Question 19

What do covalently bonded atoms share with each other?

Answer 19

Their electrons

Question 20

Small covalent molecules usually have __ melting and boiling points

Answer 20

low

Question 21

Small covalent molecules are usually what state at room temp?

Answer 21

gas or liquid

Question 22

What are intermolecular forces?

Answer 22

The forces between molecules

Question 23

What are intramolecular forces?

Answer 23

The forces between atoms in a molecule.

Question 24

Why do small covalent molecules have low melting and boiling points ?

Answer 24

Because they have weak intermolecular forces which don’t take much energy to break.

Question 25

True or false: Small covalent molecules conduct electricity

Answer 25

False

Question 26

Why do small covalent molecules not conduct electricity?

Answer 26

Because the molecules do not have an overall electric charge.

Question 27

Diamond is an allotrope of … ?

Answer 27

Carbon

Question 28

What state are giant covalent molecules at room temperature ?

Answer 28

Solid

Question 29

Why do giant covalent molecules have high melting and boiling points?

Answer 29

Because they have millions of strong covalent bonds which take lots of energy to break.

Question 30

Why can’t diamond conduct electricity?

Answer 30

There are no delocalised electrons to carry the charge.

Question 31

List two properties of graphite.

Answer 31

- High melting and boiling point - Soft & slippery - Excellent conductor of electricity -Excellent conductor of heat

Question 32

Why does graphite have a high melting and boiling point?

Answer 32

It has many strong covalent bonds and it takes a lot of energy to break these bonds.

Question 33

Why is graphite slippery?

Answer 33

Graphite is arranged in layers. There are no covalent bonds between these layers so they can slide over each other.

Question 34

Why is graphite a good conductor of heat and electricity?

Answer 34

Because it has delocalised electrons that can move and conduct heat and electricity.

Question 35

Where do the delocalised electrons in graphite come from?

Answer 35

Each carbon atom forms a covalent bond with 3 other carbon atoms. Since carbon has 4 electrons in its outer shell, this leaves 1 electron not in a covalent bond. This electron is released from the atom and is now delocalised.

Question 36

What is Graphene?

Answer 36

Graphene is a single layer of graphite. It is one atom thick

Question 37

Can graphene conduct electricity? Why?

Answer 37

Yes because it has delocalised electrons

Question 38

List two properties of Graphene

Answer 38

- Excellent conductor of electricity - Extremely strong

Question 39

What are fullerenes?

Answer 39

Molecules of carbon atoms with hollow shapes

Question 40

List two uses of fullerenes

Answer 40

- Pharmaceutical delivery - Lubricants - Catalysts

Question 41

List two properties of carbon nanotubes

Answer 41

- They have a high tensile strength - Excellent conductors of heat and electricity

Question 42

How are polymers made?

Answer 42

By joining together thousands of small identical molecules called monomers.

Question 43

Why do polymers have a high melting point?

Answer 43

Because the intermolecular forces of attraction between polymer molecules are relatively strong.

Question 44

What is a metallic bond?

Answer 44

The strong electrostatic attractions between the negative delocalised electrons and the positive metal ions in a metal.

Question 45

Why do metals have high melting and boiling points?

Answer 45

Because a great deal of thermal energy is required to break the strong metallic bonds

Question 46

What makes metal good conductors of heat and electricity?

Answer 46

They have delocalised electrons that can move and carry a charge or thermal energy.

Question 47

Why can metals be bent and shaped?

Answer 47

Because the layers of atoms can slide over each other.

Question 48

What is an alloy?

Answer 48

An alloy is a mixture of metals

Question 49

Why are alloys harder than pure metals?

Answer 49

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

Question 50

What happens to the surface area to volume ratio if you decrease the size of a particle by ten times?

Answer 50

It increases by ten times

Question 51

Why do we only need a small amount of nanoparticles in comparison to normal particles we would need?

Answer 51

Because they have a large surface area to volume ratio

Question 52

How do you calculate the surface area to volume ratio?

Answer 52

surface area / volume

Question 53

How do you calculate the surface area of a cube?

Answer 53

base x height x no. of faces (6)

Question 54

How do you calculate the volume of a cube?

Answer 54

base x width x height

Question 55

List two uses of nanoparticles:

Answer 55

• Medicines • Suncreams • Cosmetics • Deodorants • Electronics •Catalysts

Question 56

State a possible risk of nanoparticles

Answer 56

It’s possible that nanoparticles can be absorbed into the body and enter our cells.