C2 Bonding Structure and Properties Flashcards

1
Q

What is ionic bonding?

A

When an atom transfers electrons to another atom to form ions

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2
Q

What type of elements form ionic bonds between them?

A

A metal and a non-metal

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3
Q

What force holds ions together in ionic compounds?

A

Electrostatic forces (strong)

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4
Q

What type of structure do ionic compounds form?

A

Giant lattices

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5
Q

What is the charge on a Group 1 metal ion?

A

1

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6
Q

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

A

-2

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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)

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8
Q

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

A

High

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9
Q

Why do ionic compounds have high melting and boiling points?

A

Strong ionic bonds need a lot of energy to break them.

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10
Q

When do ionic compounds conduct electricity?

A

Molten (melted) or in solution

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11
Q

Why can ionic compounds only conduct electricity when molton or in solution?

A

The ions are free to move

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12
Q

What is covalent bonding?

A

Sharing of electrons

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13
Q

What type of elements form covalent bonds between them?

A

Non-metals

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14
Q

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

A

Simple covalent molecules

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15
Q

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

A

Low

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16
Q

Why do small molecules have low melting and boiling points?

A

Weak intermolecular forces (forces between the small molecules)

17
Q

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

A

Higher

18
Q

Do small covalent molecules conduct electricity?

A

No

19
Q

Why don’t small covalent molecules conduct electricity?

A

No charged particles

20
Q

Why are polymers solid at room temperature?

A

Relatively strong intermolecular forces

21
Q

What is the bonding in a polymer?

A

Covalent

22
Q

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

A

High

23
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.

24
Q

Why is diamond hard?

A

Strong covalent bonds (4 per carbon)

25
Q

Can diamond conduct electricity? Explain why.

A

No. No free (delocalised) electrons.

26
Q

Why is graphite a hard, solid at room temperature?

A

Strong covalent bonds (3 per carbon)

27
Q

Why can graphite be used as a lubricant?

A

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

28
Q

Can graphite conduct electricity? Explain why.

A

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

29
Q

What is graphene?

A

Single layer of graphite

30
Q

What properties make graphene useful?

A

Very good conductor of electricity, strong.

31
Q

What is metallic bonding?

A

Attraction between delocalised (free) electrons and positive ions

32
Q

Why can metals conduct electricity and thermal energy?

A

Delocalised (free) electrons can move and carry charge

33
Q

Why are alloys harder than pure metals?

A

Different sized metal atoms so the layers can?t slide over each other.

34
Q

Draw a sodium ion.

A
35
Q

Draw a chlorine molecule.

A