C2: Bonding, Structure and the Properties of Matter

What is an ion?

A charged particle

Why do atoms lose or gain electrons to form ions?

To get a full outer electron shell

What is a cation?

A positively charged ion

What is an anion?

A negatively charged ion

What type of bonding involves the transfer of electrons?

Ionic

What are ions attracted to in an ionic bond?

Oppositely charged ions

What forces hold together ions in an ionic compound?

Strong electrostatic forces of attraction

How many electrons does a group 1 element need to lose to get a full outer shell?

1

How many electrons does a group 2 element lose to get a full outer shell?

2

How many electrons does a group 7 element need to gain to get a full outer shell?

1

How many electrons does a group 6 element need to gain to get a full outer shell?

2

What type of diagrams show the arrangement of electrons in an atom or ion?

Dot and cross diagram

What structure do ionic compounds have?

Giant ionic lattice

Why do ionic compounds have high melting and boiling points?

Lots of energy is needed to break the strong electrostatic forces of attraction holding the ions together

In what state can ionic compounds conduct electricity?

Aqueous

Why can't ionic compounds conduct electricity when solid?

The ions are held in place so cannot move to carry electrical charge

What type of bonding occurs between non-metals?

Covalent

What are the electrostatic forces attracted between in covalent bonds?

The positive nuclei and shared pairs of negative electrons

What is the name of a substance made up of molecules containing a few atoms joined together by covalent bonds?

Simple Molecular Substances

What forces hold together the atoms WITHIN molecules of molecular substances?

Strong covalent bonds

What forces hold together molecules in a simple molecular substance?

Weak intermolecular forces

Why do simple molecular substances have low melting and boiling points?

Little energy is needed to break the weak intermolecular forces holding the molecules together

Why don't molecular substances conduct electricity?

They aren't charged, so there are no free electrons or ions

What is a polymer?

A large chain of small repeating units joined together by strong covalent bonds

What are the small repeating units in polymers called?

Monomers

What forces are between polymer molecules?

Weak intermolecular forces

Why DON'T most giant covalent structures conduct electricity?

They dont contain any charged particles

How are atoms held together in giant covalent structures?

Strong covalent bonds

How many covalent bonds does each atom form in diamond?

4

What shape is the layers in graphite?

Hexagonal

How many covalent bonds does each atom form in graphite?

3

Define allotrope.

Different structural forms of the same element

Why is diamond very hard?

Each carbon atom forms 4 covalent bonds

Why is graphite soft?

They layers formed in graphite can slide over eachother because there are no covalent bonds between them

Why can graphite conduct electricity?

Each carbon atom forms 3 covalent bonds, so each atom has a delocalised electron that can carry electrical charge

What is graphene?

A single layer of graphite

Give 1 use of diamond

Cutting materials

Give 1 use of graphite

Lubricant

Give 1 use of graphene

Electronics

T or F: Graphene cannot conduct electricity.

F - graphene can conduct electricity because it contains delocalised electrons

What is a fullerene?

Hollow molecules of carbon

What is the name of the fullerene with the molecular formula C60?

Buckminsterfullerene

What shape of BMfullerene?

A hollow sphere

Give 1 use of BMfullerene.

Drug delivery

What is the name given to small carbon fullerene cylinders?

Nanotubes

What is the name of technology that uses very small particles?

Nanotechnology

What is the name of bonding that occurs between metals?

Metallic

Why can metals conduct electricity?

Electrons in the outer shell are delocalised, so they are free to carry electrical charge

Why are most metals solid at room temperature?

The electrostatic forces between the metal atoms and electrons are really strong so lots of energy is needed to break them

This means they have very high melting and boiling points so they are usually solid

Why are most metals malleable?

Layers of atoms in a metal can slide over eachother

Define alloy.

A mixture of two or more elements where at least one is a metal

Why are alloys harder than pure metals?

In alloys, layers are distorted because different elements have different sized atoms, so the layers cannot slide over eachother

What are the 3 states of matter?

Solid

Liquid

Gas

How do forces between particles affect state of matter?

Stronger forces = solid

Weak forces = liquid

Very weak forces = gas

Describe the arrangement of particles in a solid

Regular arrangement

Vibrate in fixed positions

Describe the arrangement of particles in a liquid

Irregular arrangement

Always touching

Can move around eachother / flow

Describe the arrangement of particles in a gas

Irregular arrangement

Far apart - never touching

Move randomly

What is the change of state between a solid and a liquid?

Melting

What is the change of state between a liquid and a gas?

Evaporation / Boiling

What is the change of state between a gas and a liquid?

Condensing

What is change of state between liquid and solid?

Freezing

What state does the state symbol 'aq' refer to?

Aqueous

How big are coarse particles?

Between 2500nm and 10 000nm

How big are fine particles?

Between 100nm and 2500nm

How big are nanoparticles?

Between 1nm and 100nm

What is the formula to calculate surface area to volume ratio?

Surface area / volume

Why could nanoparticles help make new catalysts?

They have a high surface area to volume ratio

T or F: nanoparticles are used in cosmetics.

T