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AQA GCSE Chemistry > 2. Bonding, Stucture and The Properties of Matter > Flashcards

2. Bonding, Stucture and The Properties of Matter Flashcards

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1
Q

How do elements react?

A

They form bonds with each other after they’ve reacted, share electrons, or gain/lose outer electrons.

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2
Q

What do ionic compounds contain?

A

Metal and non-metal atoms

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3
Q

What do covalent compounds contain?

A

non-metal atoms only

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4
Q

What is an ionic bond?

A

Attraction between oppositely charged ions

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5
Q

What is a covalent bond?

A

Two shared electrons between two atoms

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6
Q

Why do ionic compounds conduct when molten or as a solution?

A
  • They’re liquids so ions can move freely

* They have charged particles which pass on the energy

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7
Q

Why do elements react together?

A

Because they gain or lose outer electrons to get a full outer shell

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8
Q

Why do ionic compounds have high melting/boiling points?

A

Because there’s a strong bond between ions and need a lot of energy to be broken

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9
Q

What properties do particles need to have to conduct electricity?

A
  • particles must be able to move freely

* particles must have a charge

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10
Q

Why don’t simple covalent substances conduct electricity?

A

Because they don’t lose/gain electrons - only share them - so there are no charged particles to conduct the energy

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11
Q

Why do simple covalent substances have low melting/ boiling points?

A

Because the intermolecular forces are weak even though covalent bonds are strong

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12
Q

What are macromolecules?

A

Giant covalent structures

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13
Q

Does diamond conduct?

A

No because there are no charged particles to carry the charge

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14
Q

What are diamond’s melting and boiling points like?

A

High because they have covalent bonds only which are hard to break

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15
Q

How many carbon atoms is each one covalently bonded to in diamond?

A

4

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16
Q

Why is diamond hard to break?

A

Because they are all covalent bonds - no intermolecular forces

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17
Q

Does graphite conduct?

A

Yes because there is one free electron which is free to move per molecule

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18
Q

What is graphite’s boiling and melting point like?

A

High because it has covalent bonds and intermolecular forces

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19
Q

Which has a lower melting point, graphite or diamond? Why?

A

Graphite because it only has 3 covalent bonds per atom (diamond has 4 per molecule)

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20
Q

Why is diamond the hardest substance on earth?

A

It has all covalent bonds

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21
Q

Why is graphite soft and slippery?

A

Because the layers can glide over each other because the weak intermolecular forces are easily broken

22
Q

Formula of buck minster fullerene?

A

C60

23
Q

How are the carbon atoms bonded in buck minster fullerene?

A

Each carbon atom bonds to 3 others with two forming single bonds and one a double bond

24
Q

What does silicon dioxide have a similar structure to?

A

Diamond

25
Q

What structure do diamond and silicon dioxide have?

A

tetrahedral

26
Q

Particles in ionic compounds?

A

Ions

27
Q

Particles in metallic compounds (metallic bonding)?

A

Positive ions and delocalised electrons

28
Q

Particles in giant covalent compounds?

A

Atoms

29
Q

Particles in simple molecular covalent compounds?

A

Molecules

30
Q

What bonds atoms together in metals?

A

The strong electro-static attraction between negatively charged electrons and positively charged atoms

31
Q

How are the ions arranged in a metal?

A

In regular layers

32
Q

Properties of metals?

A
  • Shaped because the layers slide over each other
  • Conducts as outer electrons are delocalised
  • High melting point as thee are strong bonds between ions and electrons
33
Q

What are alloys?

A

Mixtures where other atoms are added to metals

34
Q

Why are alloys stronger than pure metal?

A

The layers are irregular so it’s harder for atoms to slide over eachother

35
Q

What is ethane an example of?

A

A monomer

36
Q

What is polyethane an example of?

A

A polymer

37
Q

What are monomers?

A

Small molecules

38
Q

What are polymers?

A

Large molecules

39
Q

How do polymer chains slide past each other?

A

Due to weak intermolecular forces

40
Q

What is graphene?

A

A thin layer of carbon

41
Q

What do several layers of graphene form?

A

Graphite

42
Q

What are fullerenes?

A

Larges molecules of allotropes of carbon arranged in balls, cages or tubes

43
Q

What was the first fullerene discovered?

A

Buckminster Fulllerene

44
Q

What are fullerenes used for?

A
  • drug delivery systems
  • lubricants
  • catalysts
  • sports equipment
45
Q

An example of a fullerene?

A

Carbon nanotubes

46
Q

Properties of carbon nanotubes?

A

High electrical conductivity and are strong and flexible

47
Q

How big are nanoparticles?

A

Between 1 and 100nm

atom radius = 0.1nm

48
Q

Advantages of nanoparticles?

A
  • high sa/v ratio so can react quickly
  • make materials stronger and lighter
  • save lives
  • antibacterial properties
  • target specific cells
49
Q

Disadvantages of nanoparticles?

A
  • could be toxic
  • could enter blood stream and cause harm
  • speed up reactions in unpredictable ways
  • physical handling is hard in liquid or dry forms
50
Q

Uses of nanoparticles?

A
  • sports equipment- tennis rackets, golf clubs, shoes
  • clothing - silver nanoparticles added to socks to absorb smell
  • sunscreens - offer protection and can be rubbed in so no white marks
  • cosmetics - some contain ‘liposmos’ (fatty nanoparticles)
  • house paint and certain candy-coated chocolates - titanium dioxide are so small they don’t reflect visible light
51
Q

What state is a substance at melting point or above?

A

Liquid

52
Q

What state is a substance at boiling point or above?

A

Gas

AQA GCSE Chemistry (10 decks)

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