C3 Structure and Bonding Flashcards Preview

Combined Chemistry - Paper 1 > C3 Structure and Bonding > Flashcards

Flashcards in C3 Structure and Bonding Deck (35)
Loading flashcards...
1
Q

What is ionic bonding?

A

When an atom transfers electrons to another atom to form ions

2
Q

What type of elements form ionic bonds between them?

A

A metal and a non-metal

3
Q

What force holds ions together in ionic compounds?

A

Electrostatic forces

4
Q

What type of structure do ionic compounds form?

A

Giant lattices

5
Q

What is the charge on a Group 1 metal ion?

A

+1

6
Q

What is the charge on a Group 6 element’s ion?

A

-2

7
Q

How many electrons are in the outer shell of an ion?

A

Full outer shell (e.g. 8 or if the first shell 2)

8
Q

Draw the dot and cross diagram for a sodium ion.

A

Full outer shell of 8 electrons, square brackets, +1 charge outside the brackets.

9
Q

Do ionic compounds have high or low melting and boiling points?

A

High

10
Q

Why do ionic compounds have high melting and boiling points?

A

Strong ionic bonds (electrostatic forces) need a lot of energy to break them.

11
Q

When do ionic compounds conduct electricity?

A

Molten (melted) or in solution

12
Q

Why do ionic compounds conduct electricity when molten and in solution?

A

The ions are free to move

13
Q

What is covalent bonding?

A

Sharing of electrons

14
Q

What type of elements form covalent bonds between them?

A

Non-metals

15
Q

What type of structure do covalent compounds such as chlorine, water and methane form?

A

Simple covalent molecules

16
Q

Draw the dot and cross diagram for a chlorine molecule.

A

Two overlapping shells (circles). 2 electrons in the bond, 6 more in each shell.

17
Q

Do small molecules have high or low melting and boiling points?

A

Low

18
Q

Why do small molecules have low melting and boiling points?

A

Weak intermolecular forces (forces between the small molecules)

19
Q

Do larger molecules have higher or lower melting and boiling points?

A

Higher

20
Q

Do small covalent molecules conduct electricity?

A

No

21
Q

Why don’t small molecules conduct electricity?

A

No charged particles

22
Q

Why are polymers solid at room temperature?

A

Relatively strong intermolecular forces

23
Q

What is the bonding in a polymer?

A

Covalent

24
Q

Do giant covalent structures have high or low melting and boiling points?

A

High

25
Q

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

A

It is the covalent bonds that are broken and they are strong so need a lot of energy to break them.

26
Q

Why is diamond hard?

A

Strong covalent bonds (4 per carbon)

27
Q

Can diamond conduct electricity? Explain why.

A

No. No free (delocalised) electrons.

28
Q

Why is graphite a solid at room temperature?

A

Strong covalent bonds (3 per carbon)

29
Q

Why can graphite be used as a lubricant?

A

Layers can slide over each other (weaker intermolecular forces between layers

30
Q

Can graphite conduct electricity? Explain why.

A

Yes. Free (delocalised) electrons can move and carry charge.

31
Q

What is graphene?

A

Single layer of graphite

32
Q

What properties make graphene useful?

A

Very good conductor of electricity, strong.

33
Q

What is metallic bonding?

A

Attraction between delocalised (free) electrons and positive ions

34
Q

Why can metals conduct electricity and thermal energy?

A

Delocalised (free) electrons can move and carry charge

35
Q

Why are alloys harder than pure metals?

A

Different sized metal atoms so the layers can’t slide over each other.