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Chemistry Paper 1 > Bonding, Structure, And The Properties Of Matter > Flashcards

Bonding, Structure, And The Properties Of Matter Flashcards

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1
Q

What are the 3 types of chemicam bonds?

A

Ionic, covalent and metallic

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2
Q

What is involved inionic bonding?

A

A metal and non-metal

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3
Q

What happens in ionic bonding?

A

The outer electrons from metal atoms are transferred to the outer electron shell of a non-metal atom.

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4
Q

What is the force of attraction of ionic bonds?

A

Oppositely charged bonds

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5
Q

What is involved in covalent bonding?

A

Non-metals

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6
Q

What are the 3 types of substances with covalent bonds exist as molecules?

A
  1. Small structures
  2. Very large molecules
  3. Giant covalent structures.
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7
Q

What do covalent bonds share?

A

An pair of electrons.

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8
Q

What are the forces of attraction in covalent bonding?

A

Nuclei of two atoms and a shared pair on electrons

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9
Q

How are covalent moleucles represented?

A

Structural formula
E.g. methane:

         H
         |
  H  - C - H
         | 
         H
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10
Q

What is involved in metallic bonding?

A

Metals

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11
Q

What are the forces of attraction in metallic bonding?

A

Nuclei of atoms and delocalised electrons

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12
Q

What aes giant structures in metallic bonding?

A

Metal atoms are arranged in a regular pattern of many layers. 2-D diagrams often show just one layer.

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13
Q

What is a delocalised electron?

A

An electron in an atom, ion or compound that isn’t connected to a single atom or bond.

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14
Q

When do positively charged ions form?

A

When electrons permanently leave the atom.

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15
Q

What structure do ionic compounds have?

A

Giant ionic lattice

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16
Q

What is a giant ionic lattice structure

A
  1. Lattice - large structure
  2. Ionic - structure that consists of ions with ionic bonding.
  3. Giant - regular structure that repeats many times.
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17
Q

How can you represent ionic structures?

A

Ball and stick diagrams, space- filling diagrams and dot and cross diagrams.

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18
Q

What are the limitations and benefits of using a dot and cross diagram?

A

Limitations:
Doesn’t show the relative size of atoms
Doesn’t show the shape of the lattice

Benefits:
Shows bonding in detail

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19
Q

What are the limitations and benefits of using a ball and stick diagram?

A

Limitations:
Inaccurate size of atoms

Benefits:
Shows the shape of the lattice
Shows bonds as lines

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20
Q

What are the limitations and benefits of using a space-filling diagram?

A

Limitations:
Doesn’t show bonds

Benefits:
Shows the relative size of atoms and shape of lattice.

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21
Q

What are the two main rules for dot and cross diagrams?

A
  1. Only the outer shell of electrons are shown
  2. Dots or crosses represent electrons.
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22
Q

What are the 3 states of matter

A

Solid, liquid, gas

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23
Q

What are the arrangement of particles, distance between particles and motion of particles in a solid?

A

Arrangement: Regular
Distance: close
Motion: vibrate about fixed positions

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24
Q

What are the arrangement of particles, distance between particles and motion of particles in a liquid?

A

Arrangement: random
Distance: close
Motion: move around each other

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25
What are the arrangement of particles, distance between particles and motion of particles in a gas?
Arrangement: random Distance: far apart Motion: move quickly in all directions
26
Solid Liquid Gas --------------------------------------------------------> ______ energy
Increasing
27
When does melting and boiling occur?
Melting: when some forces are overcome Boiling: when all forces are overcome
28
Annotate: 1》 2》 Solid -----> liquid ------> gas 《4 《3
1: melting 2: evaporating 3: condensing 4: freezing
29
What does the state of an object being solid mean?
It is below the melting point
30
What are the forces overcome, the strength of forces and MP and BP of small molecules?
Forces overcome: intermolecular Strength: weak MP+BP: low
31
What are the forces overcome, the strength of forces and MP and BP of large molecules?
Forces overcome: intermolecular Strength: medium to strong MP+BP: Medium to high
32
What are the forces overcome, the strength of forces and MP and BP of Giant ionic compounds?
Forces overcome: ionic Strength: Strong MP+BP: high
33
What are the forces overcome, the strength of forces and the MP and BP of Giant Covalent bonds?
Forces overcome; covalent Strength: covalent MP+BP: High
34
What are the forces overcome, the strength of forces and MP and BP of metals?
Forces overcome: metallic Strength: strong MP+BP: high
35
What is a bulk property of a substance?
A bulk property of a substance is one of its observable or measurable features. Eg. Melting and boiling points.
36
What structure do ionic compounds have?
Giant ionic lattice structure
37
What is the name of the forces in a giant ionic lattice structure and what is it between?
Electrostatic forces of attraction between oppositely charges ions.
38
What must be transferred for the electrostatic bonds in ionic compounds to be overcome?
Large amounts of energy.
39
What 2 things determine if a substance can conduct electricity?
1. It contains charged particles 2. The particles are free to move
40
In ionic compounds, when can it conduct electricity?
When the ions are free to move in the liquid state.
41
What are the atoms in small molecules held together by?
Strong covalent bonds.
42
What is a polymer?
A large molecule that is formed by linking together many smaller molecules called monomers, through covalent bonds.
43
Polymer molecules are attracted to each other by...
Intermolecular forces
44
Explain why polypropene is a solid at room temperature
It consists of large molecules and the intermolecular forces are overcome by melting. These are relatively strong because the molecules are large so they need more energy to overcome.
45
Giant covalent structures have a lattice structure in which: (2)
1. The atoms are linked by covalent bonds 2. The regular lattice structure is repeated many times.
46
What must be transferred to melt or boil a giant covalent structure?
A lot of energy.
47
What are two examples of Giant covalent structures?
Diamond and graphite.
48
What are metals good conductors of? (2)
Electricity and thermal energy
49
What two properties can metals have and what do they mean?
Malleable- bent or hammered without breaking. Ductile- can be pulled to make wires without snapping.
50
Why are pure metals malleable and ductile?
Because the layers of atoms can slide over each other when forces are applied.
51
What is an alloy.
A mixture of a metal element with at least one other element, usually another metal.
52
Why are some alloys more useful than pure metals?
They are harder
53
Give examples of alloys
Steel- iron and carbon.
54
Why is steel harder than iron.
The carbon atoms distort the regular lattice structure, making it more difficult for the layers to slide over each other.
55
What substances can conduct electricity?
Substances with charged particles and if the particles are free to move.
56
What bonds are in a diamond
Covalent
57
How many atoms are bonded to each carbon atom in a diamond structure?
4
58
Does a diamond structure contain layers?
No
59
Are the forces strong or weak between the layers in a diamond structure?
Strong
60
Does a diamond structure contain delocalised electrons?
No
61
What bonds are in a graphite sturcture
Covalent
62
How many atoms are bonded to each carbon atom in a graphite structure?
3
63
Does a graphite structure contain layers?
Yes. Hexagonal rings of atoms
64
Are the forces strong or weak between the layers in a graphite structure?
Yes
65
Does a graphite structure contain delocalised electrons?
Yes
66
Why do diamonds have high melting and boiling points?
Because of the many strong covalent bonds. The bonds require a lot of energy to break
67
Why don't diamonds conduct electricity?
They don't contain any delocalised electrons or any other charged particles that are free to move
68
Why is graphite slippery?
The weak intermolecular forces between the layers of atoms.
69
What are graphene and fulleners?
Different forms of carbon.
70
What are the properties of graphene? (3)
1. Single layer of graphite - doesn't have a layered structure so it's flexible. 2. Delocalised electrons so jt conducts electricity 3. Carbon atoms joined by covalent bonds so it's strong
71
What was the first fllerene discovered?
Buckministerfullerene. C 60
72
How many carbon atoms are in buckminsterfullerene?
60

Chemistry Paper 1 (5 decks)

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