Bonding, Structure and Properties of Matter

Question 1

What are the three types of bonding?

Answer 1

Ionic Bonding, Covalent Bonding and Metallic Bonding.

Question 2

What is Ionic Bonding?

Answer 2

The bonding of metals and non-metals. Involves the transfer of electrons.

Question 3

What happens to the metal atoms in an ionic bond?

Answer 3

The metal atoms lose electrons to form positively charged ions.

Question 4

What happens to the non-metal atoms in an ionic bond?

Answer 4

The non-metal atoms gain the electrons lost by the metal atoms to form negatively charged ions.

Question 5

How does the group a metal is in effect how it bonds?

Answer 5

The group of a metal tells us how many electrons it will gain or lose. eg. Mg (Group 2), becomes +2 ions.

Question 6

What are some properties of Ionic Compounds?

Answer 6

high melting & boiling points and can conduct electricity in a solution or when melted.

Question 7

What is Covalent Bonding?

Answer 7

Bonding between two non-metals.

Question 8

What do dot and cross Diagrams show us?

Answer 8

Show how electrons rearranged in an atom or ion. Each electron is represented by a dot or a cross.

Question 9

What is covalent bonding?

Answer 9

The bonding of non-metals and non-metals. Atoms share electrons to form two full outer shells.

Question 10

What is a molecular formula?

Answer 10

A molecular formula describes the atoms present in a molecule, eg. H2O (2xH) (1XO)

Question 11

What are two examples of giant covalent structures?

Answer 11

Diamond: each carbon atom is bonded to 4 other carbon atoms (tetrahedral structure).
Graphite: each carbon atom is bonded to 3 other carbon atoms (layers of hexagonal rings)

Question 12

What are some properties of Graphite structures?

Answer 12

• Has some delocalised electrons
• Forces between layers are weak. (lubricant)

Question 13

What is Metallic Bonding?

Answer 13

The bonding of metals and metals. The electrons are delocalised and are free to move.

Question 14

Why can Metallic Bonds conduct electricity?

Answer 14

Because the electrons are delocalised and free to move.

Question 15

What are Alloys?

Answer 15

Mixtures of different metals.

Question 15

What are the three states of matter?

Answer 15

Solid, liquid and gas

Question 16

Describe the particles in each of the states of matter?

Answer 16

Solid: particles all touching, neat rows, can vibrate to move.
Liquid: particles touching each other and their container, not in rows, particles can move past each other.
Gas: particles moving freely, not touching each other but can collide.

Question 17

Name for the change of matter in:
liquid -> solid
solid -> liquid
liquid -> gas
gas -> liquid

Answer 17

freeze
melt
evaporate
condense

Question 18

What are some properties of Diamond structures?

Answer 18

Very Hard, high melting points

Question 19

What is the structure of Ionic Compounds? Describe what this means.

Answer 19

Giant ionic lattice structures where ions are packed in a regular structure with strong electrostatic forces between oppositely charged ions.

Question 20

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

Answer 20

Weak intermolecular forces.

Question 21

Why do small covalent molecules not conduct electricity?

Answer 21

They do not have an overall electric charge.

Question 22

What are the seven diatomic molecules?

Answer 22

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine and iodine.

Question 23

What are the three main examples of Giant Covalent Structures?

Answer 23

Diamond, Graphite and Silicon Dioxide.

Question 24

Why do Giant Covalent Structures have high melting/boiling points?

Answer 24

Strong intermolecular forces.

Question 25

What element is Diamond formed from?

Answer 25

Carbon

Question 26

Do Diamond Structures conduct electricity? Explain your answer.

Answer 26

No, because all of the outer electrons are in covalent bonds and so there are no free electrons to carry an electrical charge.

Question 27

What are some of the key properties of Graphite? (3)

Answer 27

Soft and slippery.
High melting and boiling point.
Conductor of electricity and heat.

Question 28

What element is Graphite formed from?

Answer 28

Carbon

Question 29

Why is Graphite soft and slippery?

Answer 29

Carbon atoms bond with three other carbon atoms, forming layers of hexagonal shapes. These layers have no covalent bonds between them, so they can slide over each other.

Question 30

Why does Graphite conduct heat and electricity?

Answer 30

Carbon atoms have four electrons in their outer shell. In graphite, each carbon atom bonds with three other carbon atoms, leaving one electron. These electrons are delocalised and so can move and conduct electricity.

Question 31

What is Graphene?

Answer 31

A single layer of graphite (one atom thick)

Question 32

What are the properties of Graphene? (3)

Answer 32

• Conducts electricity (delocalised electrons)
• Strong
• High Melting/Boiling Points

Question 33

What are Fullerenes?

Answer 33

Molecules of Carbon forming spheres or tubes.

Question 34

What is Buckminsterfullerene?

Answer 34

The first fullerene to be discovered.

Question 35

What are Allotropes?

Answer 35

Structures made of the same element but arranged differently.