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Chemistry > C2 - Bonding > Flashcards

C2 - Bonding Flashcards

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1
Q

What is metallic bonding?

A

The bonding between metals

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2
Q

How does metallic bonding occur?

A

Lattice structure of positive ions surrounded by sea of delocalised electrons. They attract each other as they are oppositely charged

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3
Q

Why can metals conduct electricity and heat?

A

Electrons are free to move THROUGH the structure to carry a charge

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4
Q

What is ionic bonding?

A

Bonding between metals and non-metals

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5
Q

How does ionic bonding occur?

A

Metal atoms donate electrons to form positive ions. Non-metal takes electron to form negative ions

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6
Q

How can we show ionic bonding?

A

Dot and Cross diagram

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7
Q

What do the charges of all ions have to add up to in an ionic compound?

A

0

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8
Q

Structure of ionic structures

A

Lattice of repeating units positive and negative ions which form a crystal

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9
Q

Properties of ionic structures

A

-High melting and boiling point due to strong electrostatic forces
-Conduct electricity when molten or dissolved because ions are free to move and carry charge
-

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10
Q

Formula for hydroxide ions

A

OH-

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11
Q

Formula for sulphate ions

A

(SO4)2-

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12
Q

Formula for carbonate ions

A

(CO3)2-

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13
Q

Formula for nitrate ions

A

(NO3)-

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14
Q

Formula for ammonium ion

A

(NH4)+

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15
Q

What are ionic compounds also known as?

A

Salts. e.g. sodium chloride

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16
Q

Positive ions are known as…

A

Cations

17
Q

Negative ions are known as…

A

Anions

18
Q

What is covalent bonding?

A

Bonding between non metals

19
Q

In covalent bonding are electrons shared or transferred

A

Shared

20
Q

In ionic bonding are electrons shared or transferred

A

Transferred

21
Q

What are simple covalent structures?

A

Covalent molecules with a small number of atoms

22
Q

Properties of small covalent structures

A

-Low melting and boiling points, weak electrostatic forces
-Can’t conduct electrical

23
Q

What is a giant covalent structure? Give an example

A

Structures that consist of repeating units of atoms, essentially creating giant molecules
- diamond, silicon dioxide

24
Q

What is a giant covalent structure?

A

Structures that consist of repeating units of atoms, essentially creating giant molecules

25
Q

Properties of a giant covalent structure

A
  • Very high melting and boiling points as you have to break the strong COVALENT bonds
26
Q

Properties of diamond

A

-Very hard
-High melting and boiling point as you have to break very strong covalent bonds
- Can’t conduct electricity
- Each carbon is bonded to 4 other carbons

27
Q

What is an allotrope?

A

Structures made of the same element but structured differently

28
Q

Describe the structure of graphite

A

-Layers of carbon with 3 bonds each
- Layers can slide over each other
- Delocalised electrons form weak bonds between layers, so can conduct electricity

29
Q

Can graphite conduct electricity?

A

Yes

30
Q

What is graphene?

A

A singular layer of graphite

31
Q

Why are metal alloys stronger than pure metals?

A

Different size atoms disrupt the lattice, so layers cannot slide over each other as easily - strong!

32
Q

What are fullerenes/nanotubes? Name an example

A

3d structures of carbon atoms
- Buckminster Fullerene (made of 60 carbon atoms)

33
Q

Uses of fullerenes/nanotubes

A

-Electronics
-Composites
- Medical purposes (delivering drugs into body)

34
Q

How many nanometres (nm) are there in a nanoparticle?

A

1-100 nm

35
Q

Size of fine particles in nm

A

100-2500 nm

36
Q

Size of coarse particles e.g. dust

A

> 2500 nm

37
Q

Why are fullerenes useful? In terms of surface area: volume ratio

A

High surface area to volume ratio, so fewer are needed for purpose

Chemistry (5 decks)

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