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AQA GCSE Chemistry > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

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1
Q

Describe the arrangement of particles in Solids [3]

A
  1. Regular arrangement
  2. Are very close together
  3. Vibrate about fixed positions
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2
Q

Describe the arrangement of particles in Liquids [3]

A
  1. Random arrangement
  2. Close together
  3. Flow around each other
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3
Q

Describe the arrangement of particles in Gases [3]

A
  1. Much more random arrangement
  2. Much further apart
  3. Move very quick in random directions
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4
Q

What are three limitations of the Particle Model?

A

Doesn’t take into account:

  1. Forces between the particles
  2. Volume of the particles
  3. Space between the particles
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5
Q

Melting point

A

The temperature at which a certain substance will always melt or freeze

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6
Q

Boiling point

A

The temperature at which a certain substance will always boil or condense

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7
Q

What is the factor that affects the melting and boiling points of a substance?

A

The amount of energy required to overcome the forces of attraction between the particles

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8
Q

Describe what happens when forces of attraction are stronger? [2]

A
  1. Greater energy required to overcome them

2. Therefore higher melting and boiling points will be

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9
Q

Explain how forces of attraction affects melting and boiling points in simple substances [3]

A
  1. Bonds are strong covalent between molecules
  2. Forces of attraction are much weaker
  3. Only a little amount of energy is required to overcome the forces of attraction here
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10
Q

What are ions?

A

Atoms that have gained or have losed an electron

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11
Q

Describe the structure of Ions

A

They have complete outer shells of electrons, similar to noble gasses

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12
Q

Describe an Ionic Bond [2]

A
  1. Strong ELECTROSTATIC force of attraction

2. Between positive metal ion and negative non-metal ion

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13
Q

Sodium forms an ionic compound with chlorine

Describe what happens when two atoms of sodium react with one molecule of chlorine

Give your answer in terms of electron transfer [6]

A
  1. Sodium belongs to group 1=> 1 outer shell electron
  2. Chlorine belongs to group 7=> 7 outer shell electron
  3. One chlorine molecule=2 atoms
  4. Each sodium transfers 1 electron to one chlorine atom each
  5. All atoms now have 8 outer shell electrons
  6. The atoms are Na+ and CL-, with the compound sodium chloride, NACL
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14
Q

Describe the structure of ionic compounds [2]

A
  1. Giant structures of ions

2. Held by strong electrostatic forces of attraction in all directions between oppositely charged ions

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15
Q

Describe the properties of ionic compounds [3]

A
  1. Have high melting and boiling points
  2. Do NOT conduct electricity when solid as they cannot move
  3. Do conduct when Colten or in solution=> charged ions can move about and carry charge
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16
Q

Why do ionic compounds have high melting and boiling points? [2]

A
  1. Ionic bonds are very strong

2. Takes a lot of energy to overcome them

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17
Q

In which 2 places do metallic bonding occur?

A
  1. In metals

2. In Alloys

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18
Q

What is a metallic bond?

A

The attraction between positive ions and delocalised negatively charged electrons

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19
Q

Describe the structure of metals [3]

A
  1. Electrons in the outer shells are delocalised
  2. Produces a lattice of positive ions
  3. Held by electrostatic attraction to delocalised electrons
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20
Q

Why do metals make good construction materials? [2]

A
  1. Very strong

2. High melting and boiling points

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21
Q

Why are metals good thermal and electrical conductors?

A

Delocalised electrons can move freely and transfer electricity

22
Q

Describe the advantages of structure of atoms in pure metals [2]

A
  1. Layers can slide over each other easily

2. This makes them easily bent and shaped

23
Q

Why is copper used to make water pipes? [2]

A
  1. It is very unreactive=> doesn’t react with metal

2. Easily shaped for tubing

24
Q

Why is gold good to use for jewellery? [2]

A
  1. Ductile

2. Shiny

25
Q

Alloy

A

A mixture that contains a metal and at least one other element

26
Q

What the properties of alloys in comparison to pure metals?

A

They are much harder

27
Q

Why are alloys harder and stronger than most metals? [2]

A
  1. Added element disturbs regular arrangement of atoms

2. So layers do not slide over eachother as easily

28
Q

Describe the production of Steel [3]

A
  1. Iron oxide REDUCED in a BLAST FURNACE to produce iron
  2. Impurities are removed from the iron to make it pure
  3. MIXED with small amount of carbon or other metal
29
Q

Why is molten iron obtained from a blast furnace not very useful? [2]

A
  1. Contains many impurities

2. => Very brittle

30
Q

How does the amount of other elements in Steel determine its properties? [3]

A
  1. Steel with a high carbon content is hard and strong
  2. Steel with a low carbon content is soft and easily shaped
  3. Stainless steel contains chromium and nickel=> resistant to corrosion
31
Q

What does the carat system show?

A

The amount of gold in an alloy

32
Q

What is 24 carat gold?

A

100% gold

33
Q

What is a covalent bond?

A

A shared pair of electrons between atoms

34
Q

At what 2 places do covalent bonds occur?

A
  1. Non metallic elements like 02

2. Compounds of non metals

35
Q

How does a chlorine atom (7 outer shell electrons) form a bond with another? [3]

A
  1. An electron between each atom is shared
  2. This gives each chlorine atom eight electrons in their outer shell
  3. Each atom now has a complete outer shell
36
Q

What do simple molecules contain? [2]

A
  1. A relatively small amount of non-metal atoms

2. Joined together by covalent

37
Q

What happens when the size of molecules increase?

A

The stronger the intermolecular forces become

38
Q

Why do elements further down group 7 have a higher melting/ boiling point? [3]

A
  1. Their molecule size increases
  2. Therefore so does the strength of their intermolecular forces
  3. And so more energy is required to overcome them
39
Q

Why do giant covalent structures have high melting and boiling points? [2]

A
  1. All atoms are linked by strong covalent bonds

2. These bonds must be broken for the substance to melt or boil

40
Q

Describe the structure and properties of Diamond [3]

A
  1. Giant, rigid covalent structure of carbon (lattice)
  2. Each carbon atom forms four strong covalent bonds with other carbon atoms
  3. These mean that it is a very hard substance with a very high melting point
  4. There are no charged particles/ delocalised electrons=> does not conduct electricity
41
Q

Describe the structure and properties of Graphite [6]

A
  1. Giant covalent structure of carbon=> High melting point
  2. Each carbon atom forms three covalent bonds with other atoms
  3. Creates a layered hexagonal structure
  4. Layers are held together by weak intermolecular forces
  5. => Layers can slide past each other=> soft and slipper
  6. One electron per carbon is delocalised=> conduct heat and electricity
42
Q

Describe the structure of Silica [2]

A
  1. Each oxygen atom joined to two silicon atoms

2. Each silicon atom joined to four oxygen atoms

43
Q

What is graphene?

A

A form of carbon that is a single layer of graphite

44
Q

What are the properties of graphene? [3]

A
  1. Strong
  2. Good thermal and electrical conductor
  3. Nearly transparent
45
Q

What are the shape of fullerenes?

A

They have hollow shapes, like tubes and cages

46
Q

Describe the structure and properties of Buckministerfullerene

A
  1. Consists of 60 carbon atoms
  2. Joined together in a series of hexagons and pentagons
  3. It is the most symmetrical and so stable fullerene
47
Q

What are the uses of Fullerenes?

A
  1. To deliver drugs in the body
  2. As catalysts
  3. For reinforcing materials=> e.g. frames of tennis rackets=> strong but lightweight
  4. As lubricants
48
Q

How are atoms In polymers held together?

A

Covalent bonds

49
Q

Why are polymers solid at room temperature

A

The intermolecular forces between large polymer molecules are strong

50
Q

What is the range of diameters for nanoparticles?

A

Between 1 and 100nm

51
Q

What does the small diameters of nanoparticles mean? [3]

A
  1. They have a large SA:V ration

2. This is important for catalysts as it makes them more effective

52
Q

What is research into nanoparticles leading to the development of? [4]

A
  1. New drug delivery systems
  2. Synthetic skin for burn victims
  3. Computers and technology
  4. Stronger and lighter construction material

AQA GCSE Chemistry (10 decks)

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