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

Bonding, Structure and Properties of Matter Flashcards

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
Alloy
A mixture that contains a metal and at least one other element
26
What the properties of alloys in comparison to pure metals?
They are much harder
27
Why are alloys harder and stronger than most metals? [2]
1. Added element disturbs regular arrangement of atoms | 2. So layers do not slide over eachother as easily
28
Describe the production of Steel [3]
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
Why is molten iron obtained from a blast furnace not very useful? [2]
1. Contains many impurities | 2. => Very brittle
30
How does the amount of other elements in Steel determine its properties? [3]
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
What does the carat system show?
The amount of gold in an alloy
32
What is 24 carat gold?
100% gold
33
What is a covalent bond?
A shared pair of electrons between atoms
34
At what 2 places do covalent bonds occur?
1. Non metallic elements like 02 | 2. Compounds of non metals
35
How does a chlorine atom (7 outer shell electrons) form a bond with another? [3]
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
What do simple molecules contain? [2]
1. A relatively small amount of non-metal atoms | 2. Joined together by covalent
37
What happens when the size of molecules increase?
The stronger the intermolecular forces become
38
Why do elements further down group 7 have a higher melting/ boiling point? [3]
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
Why do giant covalent structures have high melting and boiling points? [2]
1. All atoms are linked by strong covalent bonds | 2. These bonds must be broken for the substance to melt or boil
40
Describe the structure and properties of Diamond [3]
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
Describe the structure and properties of Graphite [6]
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
Describe the structure of Silica [2]
1. Each oxygen atom joined to two silicon atoms | 2. Each silicon atom joined to four oxygen atoms
43
What is graphene?
A form of carbon that is a single layer of graphite
44
What are the properties of graphene? [3]
1. Strong 2. Good thermal and electrical conductor 3. Nearly transparent
45
What are the shape of fullerenes?
They have hollow shapes, like tubes and cages
46
Describe the structure and properties of Buckministerfullerene
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
What are the uses of Fullerenes?
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
How are atoms In polymers held together?
Covalent bonds
49
Why are polymers solid at room temperature
The intermolecular forces between large polymer molecules are strong
50
What is the range of diameters for nanoparticles?
Between 1 and 100nm
51
What does the small diameters of nanoparticles mean? [3]
1. They have a large SA:V ration | 2. This is important for catalysts as it makes them more effective
52
What is research into nanoparticles leading to the development of? [4]
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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