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C1 > C2 > Flashcards

C2 Flashcards

1
Q

What are 3 states of matter

A

Liquid
Solid
Gas

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2
Q

What is the melting point

A

The temperature at which a solid changes into a liquid

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3
Q

What is the boiling point

A

The temperature at which the particles gain enough energy to change from a liquid to a gas

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4
Q

What does the amount of energy needed to break bonds to change state depend on?

A

Strength of forces between particles of substance

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5
Q

The stronger the forces between particles…

A

The higher the m.p. and b.p. of substance

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6
Q

What does (aq) stand for

A

Aqueous solution

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7
Q

(g) meanning

A

Gas

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8
Q

(l) meanning

A

Liquid

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9
Q

(s) meanning

A

Solid

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10
Q

Describe properties of gas particles

A
  • widely spaced
  • movement of particles: in random directions at random speed
  • collisions are frequent and elastic
  • weak forces between particles
  • have highest energy
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11
Q

Describe properties of liquid particles

A
  • closely spaced but still in constant motion
    -therefore constantly colliding
  • forces between particles are weaker than in solid
  • randomly arranged
  • move around eachother
  • can flow and take shape of container
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12
Q

Describe solid particles

A

Solid particles can only vibrate in a fixed position
- low energy
- regular pattern
- cannot be compressed

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13
Q

How do you turn: solid into liquid

A

Melting

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14
Q

How do you turn: liquid into gas

A

Evaporating/ boiling

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15
Q

How do you turn: gas into liquid

A

Condensing

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16
Q

How do you turn: liquid into solid

A

Freezing

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17
Q

How do you turn: gas to solid or solid to gas

A

Sublimation

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18
Q

Example of sublimation

A

Solid carbon dioxide ( dry ice) and Iodine

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19
Q

How do substances change state

A

Energy must be transferred

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20
Q

How do substances melt. Explain in terms of energy

A
  • particles gain energy- heating
  • bonds are broken between particles
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21
Q

What happens when a substance boils or evaporates.

A

Forces of attraction between particles are overcome

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22
Q

The stronger the forces of attraction…

A

The more energy Is required to overcome forces

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23
Q

What happens to particles during condensation and freezing

A
  • Energy is transferred from substance to surroundings
  • This is because the forces of attraction between the particles get stronger
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24
Q

How do you know if a substance is solid when given its temperature

A

Given temperature < melting point

= solid

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25
Q

How do you if a substance is liquid when given the temperatures of its b.p. and m.p.

A

Given temperature is between melting and boiling points

=liquid

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26
Q

How do you know if a substance is gas when given its temperature

A

Given temperature > boiling point

= gas

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27
Q

What are limitations of particles model

A
  • particles are not solid they are mostly empty space
  • many particles are not spherical
  • no forces between spheres
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28
Q

What does the particle model show

A

Particles are solid spheres with no forces between them

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29
Q

How can you distinguish a pure substance when given the time and temperature it takes for it to melt and boil

A
  • pure substance will melt or boil at a fixed temperature (flat horizontal line)
  • mixture will melt over a range of temperatures and not sharp melting point
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30
Q

Define ion

A
  • charged atom
  • when an atom loses or gains electrons to obtain full outer shell
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31
Q

In what compounds does ionic bonding occur between

A

Metals combined with non- metals

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32
Q

What ions do metal atoms form in ionic bonding

A

Positively charged ions- lose electron

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33
Q

What ions do non metal atoms form in ionic bonding

A

Negatively charged ions- gain electron

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34
Q

How are positive metal ions formed in ionic bonding

A

-When metal reacts with non-metal and loses electron from outer shell -it becomes fully stable
- positive because there is more protons than electrons

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35
Q

How do non metals become negatively charged ions in ionic bonding

A

-they gain electron
-to get fully stable outer shell
- becomes negatively charged because there is more electrons than protons

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36
Q

Group 1 always forms ..

A

1+ ions

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37
Q

Group 2 always forms..

A

2+ ions

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38
Q

Group 6 always form..

A

2- ions

39
Q

Group 7 always form..

A

1- ions

40
Q

What does a dot and cross diagram represent

A

Electron transfer during formation of ionic compound

41
Q

What is ionic bond

A

Force of attraction between oppositely charged ions

42
Q

Describe electron transfer between potassium oxide

A
  • potassium atom loses electron and forms 1+ potassium ion
  • oxygen gains 2 electrons and forms 2- oxide ion

2 potassium atoms react with 1 oxygen atom

43
Q

For sodium chloride the ions are Na+ and Cl- . What is the formula of compound

A

NaCl 1+ charge cancels out 1 - charge

44
Q

Magnesium fluoride the ions are Mg 2+ and F - . What is the formula of compound

A

MgF₂
We need 2 F- ions to cancel out the 2+ charge on Mg

45
Q

Lithium oxide the ions are Li+ and O2- . What is the formula of compound

A

Li₂O
We need 2 lithium ions to cancel out the 2- charge on O

46
Q

What are ionic compounds held together by

A

Strong electrostatic forces of attraction between oppositely charged ions

47
Q

Properties of ionic substances

A
  • high m.p. and b.p.
  • in solid form they do not conduct electricity
48
Q

Why do ionic substances have high melting and boiling point

A

because of large amounts of energy needed to break many strong electrostatic forces of attraction between oppositely charged ions

49
Q

Why can ionic substances not conduct electricity in solid form

A

Because ions are in fixed position

50
Q

How can ionic compounds conduct electricity

A

When melted or in aqueous solution because ions are free to move therefore can carry charge

51
Q

what words to always use when describing ionic structures and their properties

A

Ions

52
Q

what words to never use when describing ionic structures and their properties

A
  • delocalised electrons
  • molecules
  • intermolecular forces
53
Q

What is an ionic lattice

A

When ions have a regular repeating arrangement

54
Q

What does the ball and stick diagram present in ionic bonding

A

Ions are arranged close seperated by sticks to eachother
- but in reality there is no gaps or sticks between ions

55
Q

What is empirical formula

A

Simplest ratio of ions in compound

56
Q

Ions with higher charge will…

A

have stronger forces of attraction between them, so will need more energy in order to overcome these forces

57
Q

Covalent bonding occurs in what compounds?

A

Compounds of non- metals

58
Q

What happens in covalent bonding

A

Atoms share pairs of electrons

59
Q

Limitations of models showing covalent bonds

A
  • none are to scale
  • some do not show 3 dimensional arrangement in space
  • some do not show electrons or all the shells
60
Q

Properties of covalent substances

A

These substances:
- consist of small molecules - are usually gases or liquids that have low m.p. b.p.

  • do not conduct electricity because molecules do not have overall electrical charge
61
Q

What happens to forces when covalent substance heated

A
  • weak intermolecular forces between molecules are overcome- when substance melts or boils- these require little energy to break
  • STRONG COVALENT BONDS DO NOT BREAK
62
Q

Explain the effect of the size of molecule on intermolecular forces

A
  • intermolecular forces increase with size of molecule
  • larger molecules need more energy to break intermolecular forces and so have higher m.p. + b.p.
  • this explains why melting and boiling point Increases down group 7
63
Q

What is the only word you should be using to describe covalent bonding

A

Intermolecular forces

64
Q

What is a polymer

A

Very large covalent compound with many repeating units

65
Q

Polymer- structure, properties and explanation

A
  • lines show covalent bonds
  • solid
  • intermolecular forces between polymer molecules are relatively strong
66
Q

What does n represent in polymers

A

A large number

67
Q

Giant covalent structures properties

A

Solids with very high melting and boiling points
Atoms joined together by strong covalent bond
These bonds must be overcome in order to melt or boil substance

68
Q

Examples of giant covalent substances

A

Diamond and graphite (forms of carbon)
Silicon dioxide (silica)

69
Q

Diamond- structures, properties and explanations

A

● doesn’t conduct electricity= no delocalised electrons to cary charge

●very hard = strong covalent bond to form lattice

● very high melting point= each carbon atom forms 4 covalent bonds with other carbon atoms
large amount of energy is needed to overcome all these bonds
-

70
Q

What is graphene

A

Single layer of graphite so one atom thick

71
Q

Graphene properties

A

○ very strong
○ able to conduct electricity due to delocalised electrons

72
Q

Graphene uses

A
  • Electronics
  • Composites
73
Q

Describe the structure of fullerene

A

Hallow shaped, hexagonal rings of carbon atoms

74
Q

Example of fullerene

A

Buckminsterfullerene (C ⁶⁰)

75
Q

Describe Properties of fullerenes

A

Very strong
Hallow so can contain other other chemicals within it

76
Q

Uses of fullerene

A

Drug delivery, lubricants

77
Q

Describe structure of Carbon nanotubes

A

Cylindrical tubes of carbon atoms that are very long compared to their diameter

78
Q

Uses of carbon nanotubes

A

Nanotechnology, electronics, reinforcing (e.g. tennis rackets)

79
Q

Properties of carbon nanotubes

A

●Very strong, light and flexible
● Able to conduct electricity due to delocalised electrons

80
Q

Describe structure of graphite

A
  • each carbon forms 3 bonds to other carbon atoms
  • forming layers of hexagonal rings
81
Q

Why can graphite conduct electricity

A

Conducts electricity= 1 carbon only forms 3 bonds so one electron is delocalised
These electrons are free to move and can carry charge through the structure conducting thermal energy and electricity

82
Q

Why is graphite soft and slippery

A

Arranged in layers with weak intermolecular forces between layers so layers can easily slide due to no covalent bonds present

83
Q

What is a pure metal

A

● Sea of delocalised electrons with positive metal ions
● Ions are tightly packed and arranged in rows

84
Q

What is an alloy

A

Presence of other elements between positive metal ions and delocalised electrons- distorts layers and prevents them from sliding over eachother

85
Q

How are delocalised electrons and metal ions bonded together

A

Strong electrostatic force of attraction between positive metal ions and negatively charged electrons

86
Q

Properties of metals

A
  • have high m.p. b.p. = lots of energy needed to break strong metallic bonds between positive ions and delocalised electrons
  • good conductors of electricity- delocalised electrons free to carry charge
  • same with thermal energy- good conductors
  • malleable- layers can slide over eachother, bent, shaped, attraction between ions and electrons prevents metal from shattering
87
Q

Benefits of alloys

A

Different sizes of atoms in alloy distorts layers in structure of metal making it more difficult for them to slide over eachother so are harder

88
Q

Nanoparticles have a …

A

High surface area to volume ratio

89
Q

Risks of nanoparticles

A
  • so small so can be inhaled through lungs and because if large s.a. to volume ratio they can initiate harmful reactions and toxic substances can bind to them
90
Q

What charge is a cation

A

Positive

91
Q

What charge is an ion

A

Negative

92
Q

What charge is cathode

A

Negative electrode

93
Q

What charge in annode

A

Positive

C1 (5 decks)

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