C3 - Structure and Bonding

Question 1

What are the 3 states of matter?

Answer 1

• Solid, liquid and gas.

Question 2

What are the particles like in a solid?

Answer 2

• Packed closely together.

- Vibrate around fixed positions.

Question 3

What are the particles like in a liquid?

Answer 3

• Also close together.

- Can slip and slide over each other in random motion.

Question 4

What are the particles like in a gas?

Answer 4

• Lots of space between them and zoom around randomly.

Question 5

What happens in melting and boiling in the states of matter?

Answer 5

• Energy is transferred from the surroundings to the substance.

Question 6

What happens in freezing and condensing in the states of matter?

Answer 6

• Energy is transferred from the substance to the surroundings.

Question 7

How do elements form to create compounds?

Answer 7

• By gaining or losing electrons or by sharing electrons.

Question 8

What happens in a reaction between group 1 elements and group 7 elements (halogens)?

Answer 8

• Atoms of group 1 elements can lose one electron to gain the stable electronic structure of a noble gas.
• The electron can be given to an atom from group.7 which will also now have the electronic structure of a noble gas.

Question 9

What ions do group 1 form?

Answer 9

• 1+ ions.

Question 10

What ions do group 2 form?

Answer 10

• 2+ ions.

Question 11

What ions do group 3 form?

Answer 11

• 3+ ions when they form ions as opposed to sharing electrons.

Question 12

What ions do group 4 form?

Answer 12

• They do not form ions; however, led and tin form ions at the bottom of the group.

Question 13

What ions do group 5 form?

Answer 13

• 3- ions when they form ions as opposed to sharing electrons.

Question 14

What ions do group 6 form?

Answer 14

• 2- ions when they form ions as opposed to sharing electrons.

Question 15

What ions do group 7 form?

Answer 15

• 1- ions when they form ions as opposed to sharing electrons.

Question 16

What ions do group 0 form?

Answer 16

• Never form ions in compounds.

Question 17

How are ionic compounds held together?

Answer 17

• Strong forces of attraction between their oppositely charged ions
• This is called ionic bonding.

Question 18

What ions can form ionic compounds?

Answer 18

• Group 1 and group 7.

- Group 2 and group 6.

Question 19

Features of strong ionic bonds.

Answer 19

• Operate in all different directions holding a giant ionic lattice together, therefore ionic compounds have high melting points; they are all solid at room temperature.

Question 20

Features of ionic compounds.

Answer 20

• Conduct electricity when molten or dissolved in water.; their ions can then become mobil and carry charge through the liquid.

Question 21

What is a covalent bond?

Answer 21

• When non-metals are bonded together.

Question 22

How are covalent bonds formed?

Answer 22

• When atoms of non metals share pairs of electrons together.
• Each shared pair of electrons is a covalent bond.

Question 23

What do many substances with covalent bonds have?

Answer 23

• Consist of simple molecules but have some giant covalent structures.

Question 24

What are the boiling points of simple molecule substances likely to have?

Answer 24

• Low melting and boiling points.

Question 25

What are the forces of simple molecules like?

Answer 25

• They are weak; the weak intermolecular forces explain why substances made of simple molecules have low melting and boiling points.

Question 26

What is the charge like in simple molecules?

Answer 26

• No overall charge, therefore they cannot carry electrical charge.
• Substances of simple molecules cannot conduct electricity.

Question 27

Why are models used to show bonding?

Answer 27

• To help the understanding of its bonding but each models has its limitations in representing reality.

Question 28

What are giant covalent structure substances’ boiling points like?

Answer 28

• Very high - melting and boiling points.

Question 29

What are the giant covalent bonds like in graphite?

Answer 29

• Giant layers of covalently bonded carbon atoms.
• No covalent bonds between the layers.
• They can slide over each other, making graphite soft and slippery.
• Carbon atoms in diamond have a rigid giant covalent structure making it a very hard structure.

Question 30

Can graphite conduct electricity?

Answer 30

• Yes.

- Also can conduct thermal energy because of the delocalised electrons that can move along its layers.

Question 31

What are fullerenes?

Answer 31

• As well as diamond and graphite, carbons also exists in fullerenes, which can form large cage-like structures and tubes, based on hexagonal rings of carbon atoms.

Question 32

What are fullerenes being used for?

Answer 32

• Finding uses as a transport mechanism for drugs to specific sites in the body, as catalysts, and as a reinforcement for composite materials.

Question 33

What is graphene and what properties does it possess?

Answer 33

• A single layer of graphite and so is just one atom thick.
• Its properties: excellent electrical conductivity; will help create new developments in the electronics industry in the future.

Question 34

What are the atoms like in metals?

Answer 34

• Closely packed together and arranged in regular layers.

Question 35

How can you think of metallic bonding?

Answer 35

• Positively charged metal ions held together by electrons from the outermost shell of each metal atom.
• These delocalised electrons are free to move throughout the giant metal lattice.

Question 36

What are metals like in a giant metallic structure?

Answer 36

• Can be bent or shaped because the layer of atoms (or positively charged ions) can slide over each other.

Question 37

Why are alloys harder than pure metals?

Answer 37

• Regular layers in a pure metal are distorted by atoms of different sizes in an alloy.

Question 38

What delocalised electrons in metals do?

Answer 38

• Enable electricity and thermal energy to be transferred through metal easily.