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GCSE Chemistry Revision > C1-5 Obscure Content Flashcards > Flashcards

C1-5 Obscure Content Flashcards

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1
Q

What is the charge of a calcium ion

A

Ca 2+

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2
Q

What is the charge of a copper ion

A

Cu 2+

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3
Q

What is the charge of an aluminium ion

A

Al 3+

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4
Q

What is teh charge of a Magnesium ion

A

Mg 2+

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5
Q

What is the charge of a sodium ion?

A

Na +

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6
Q

What is the charge of sulfate?

A

SO4 = 2-

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7
Q

What is the charge of a carbonate ion

A

CO3 (2-)

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8
Q

What is teh charge of a nitrate ion?

A

NO3 (-)

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9
Q

What is the formula of nitric acid?

A

HNO3

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10
Q

What is teh formula of Sulfuric acid?

A

H2SO4

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11
Q

What is the charge of a zinc ion

A

2+

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12
Q

What is the charge of ammonium

A

NH4+

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13
Q

C1
What happens when sodium reacts with chlorine

A

Flame + smoke/clouds of white sodium chloride

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14
Q

What colour does fluorine turn when reacted with iron?

A

White

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15
Q

What colour does chlorine turn when reacted with iron?

A

Orange brown

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16
Q

What colour does bromine turn when reacted with iron?

A

Red brown

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17
Q

What colour does iodine turn when reacted with iron

A

Grey

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18
Q

What happens when fluorine reacts with hydrogen?

A

Explodes at room temp

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19
Q

What happens when chlorine is reacted with hydrogen

A

Explodes (with a flame or in sunlight)

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20
Q

What happens when bromine reacts with hydrogen

A

When warmed reacts vigorously

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21
Q

When iodine is reacted with hydrogen what happens?

A

Very slow reaction when heated allot

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22
Q

A more reactive halogen will _____ a less reactive halogen from its salt solution

A

Displace

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23
Q

As iodine forms in a solution it turns _____

A

Darker

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24
Q

What colour is chlorine?

A

Yellow

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25
Q

How reactive is fluorine? How dangerous?

A

Very
Poisonous

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26
Q

What colour is chlorine? How dangerous is it?

A

Dense green gas - poisonous

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27
Q

What colour is bromine? Is it poison?

A

Red brown liquid
Yes

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28
Q

What colour is iodine? State? What other colour can it be as a vapour?

A

Dark grey
Crystalline solid
Purple vapour

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29
Q

What is observed when a group 1 metal is exposed to air

A

Turns dull/white smoke seen
When heated with oxygen = burns

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30
Q

What happens when lithium is heated with oxygen
What does it form?

A

Red flame

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31
Q

What happens when sodium is heated with oxygen? What forms? (2 things)

A

Orange flame
Sodium oxide
Sodium peroxide (2 sodiums, 2 oxygens)

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32
Q

What happens when potassium is reacted with oxygen? What forms?

A

Lilac flame
Potassium peroxide (K2 O2)
Potassium superoxide (KO2)

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33
Q

What happens when lithium is reacted with chlorine?

A

Burns slowly with reddish flame
White solid produced

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34
Q

What happens when chlorine is reacted with sodium?

A

Burns brightly with yellow flame
White solid producd

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35
Q

What happens when potassium is reacted with chlorine

A

Burns brightly with purplish flame
White solid produced

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36
Q

What happens when lithium is reacted with water?

A

Fizzes
Gets smaller and smaller until it disappears

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37
Q

What happens when sodium reacts with water?

A

Fizzes allot, forms a ball then gets smaller and disappears

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38
Q

What happens when potassium reacts with water?

A

Burns violently with sparks and a lilac flame

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39
Q

Give 3 properties of group 1

A

Soft (can be cut with a knife)
Relatively low melting points
Low density

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40
Q

What has the lowest boiling point of any element?

A

Helium

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41
Q

Give 6 properties of transition metals

A

Strong
Good conductors (of heat and electricity
Highly dense
High melt points ]more than one oxidation state ]forms colourful compounds

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42
Q

Give 3 uses of transition metals as catalysts

A

Iron in haber process (to make ammonia)
Vanadium pentoxide in contact process to make Sulfuric acid
Nickel used in the hydrogenation of alkenes

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43
Q

Why is titanium (transition metal) so useful in medicine?

A

High biocompatibility
Only element that can bond with bones

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44
Q

Give 3 other applications of transition metals

A

Forming coloured compounds in:
Dyes
Paints
Stained glass
Jewellery
Anti corrosive materials

45
Q

Give the difference in reactivity with oxygen at room temperature of transition metals compared to group 1

A

Group 1 react quickly with oxygen
Transition metals react slowly or not at all with oxygen at room temperature

46
Q

Give difference in reactivity of group 1 and transition metals with cold water

A

Group 1elements react vigorously with cold water
Transition metals react Slowly or not at all with cold water
Group 1 elements react vigorously with halogens
Some transition metals also react with halogens

47
Q

Give difference in reactivity of group 1 metals and transition metals with halogens

A

Group 1 elements react vigorously with halogens
Some transition metals also react with halogens

48
Q

Give 4 differences between group 1 elements and transition metals

A

All of group 1 metals form +1 ions but transition metals have variable charges
Transition metals are harder, stronger and denser,
Higher melting points of transition metals than group1
Transition metals much less reactive than group 1

49
Q

How many years passed between the discovery of the nucleus and Chadwick discovering the existence of neutrons

A

20

50
Q

What is the radius of an atom

A

0.1 nm (1 x 10 ^-10 m)

51
Q

How much smaller is the radius of the nucleus compared to the radius of an atom

A

More than 10 000 x smaller

52
Q

Why is the periodic table called that?

A

Similar properties occur at regular intervals

53
Q

Knowledge of what explained why the order based on atomic weights sometimes put elements in the wrong place

A

Isotopes

54
Q

Why does it sometimes seem that mass is not conserved in reactions?

A

Reactant or product is a gas and its mass hasn’t been counted

55
Q

Give an example of a reaction where mass is seemingly not conserved

A

Metal oxide formation (metal oxide seems to have a mass greater than the metal )
Thermal decomposition of metal carbonates (CO2 produced and metal oxide is only solid product)

56
Q

What is the volume of 1 mol of any gas at room temperature?

A

24 dm3

57
Q

As pH decreases by 1 unit
Hydrogen ion concentration increases by a factor of

A

10

58
Q

Give 3 examples of weak acids

A

Ethanoic
Citric
Carbonic

59
Q

Give 3 examples of strong acids

A

Hydrochloric
Nitric
Sulfuric

60
Q

Are bases insoluble or soluble?

A

Insoluble

61
Q

Give the order of the reactivity series

A

Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
zinc
Iron
Lead
Hydrogen
Copper
Silver
Gold
Platinum

62
Q

What is reactivity in terms of ions

A

Tendency to form positive ions

63
Q

What is teh difference between a fuel cell and a normal chemical cell

A

Supplied by an external source of fuel (such as hydrogen or oxygen or air)
Fuel is oxidised electrochemically within cell to create potential difference

64
Q

What is the overall reaction in a hydrogen fuel cell?

A

Oxidation of hydrogen to produce water

65
Q

Give an example of a non rechargeable battery

A

Alkaline battery

66
Q

What does a non rechargeable cell mean

A

Reactions stop when one reactant has been used up

67
Q

What are batteries made of to provide greater voltage?

A

Multiple cells

68
Q

How can you easily make a simple cell

A

Connecting 2 different metals in contact with an electrolyte

69
Q

Give 3 examples of Exothermic reactions (chemical)

A

Combustion
Many oxidation reactions
Neutralisation

70
Q

Give 2 everyday examples of Exothermic reactions

A

Self heating cans
Hand warmers

71
Q

Give 2 examples of endothermic reactions

A

Thermal decomposition
Reaction of citric acid and sodium hydrogencarbonate

72
Q

Give 1 everyday example of an endothermic reaction

A

Injury packs

73
Q

Give 2 common examples of polymers

A

Polythene
Polyvinyl chloride (PVC)

74
Q

What is polythene used in

A

Plastic bags

75
Q

What is PVC used to make

A

Water pipes
Used industrially

76
Q

What are polymer atoms linked to other atoms by

A

Strong covalent bonds

77
Q

Why are polymers solids at room temperature?

A

The intermolecular forces between polymer molecules are relatively strong

78
Q

What shape does graphite make?

A

Hexagonal rings of carbon atoms

79
Q

Give 3 examples of giant covalent structures

A

Graphite
Diamond
Silicon dioxide (silica)

80
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes

81
Q

Give 3 possible numbers of carbon atoms per ring in a fullerene

A

6, 5, 7,

82
Q

What was the first fullerene to be discovered?

A

Buckminsterfullerene (C60)

83
Q

What is the shape of C60

A

Spherical

84
Q

What are carbon nanotubes?

A

Cylindrical fullerenes with very high length:diameter ratios

85
Q

Give 2 advantages of dot + cross

A

Shows electron transfer
Shows which atom bonding electrons come from

86
Q

Give 2 limitations of dot + cross

A

Not 3D\doesn’t show relative sizes of atoms

87
Q

Give 2 advantages of ball and stick model

A

3D
Useful to visualise molecule shape

88
Q

Give 2 limitations of the ball and stick model

A

Doesn’t show movement of electrons
Atoms shown as far apart but they are actually close

89
Q

Give 2 advantages of displayed formula

A

Simpler versions of ball and stick model
Show what atoms are in the molecule and how they are connected

90
Q

Give 2 limitations of displayed formula (2D)

A

Doesn’t show relative sizes of atoms
Doesn’t show shapes of atoms
Or what they look like in 3D

91
Q

Give 3 limitations of particle theory

A

Doesn’t show forces
Particles all represented as spheres
These spheres are seen as solid

92
Q

Do atoms themselves have bulk properties of materials

A

No

93
Q

What forces are overcome when a covalent molecule is boiled

A

Weak intermolecular forces
NOT strong covalent bonds intramolecular

94
Q

Why can metals be bent and shaped?

A

The ions are arranged in layers

95
Q

What are nanoparticles?

A

Structures 1-100nm in size (a few hundred atoms

96
Q

What are fine particles?

A

Diameters of 100 - 25 000nm

97
Q

What are coarse particles also known as?

A

Dust

98
Q

What are the diameters of coarse particles?

A

1 x 10 ^-5 m and 2.5 x 10 ^-6m

99
Q

If the side of a cube decreases by a factor of 10, by what factor does the surface area: volume ratio increase?

A

10

100
Q

Why do nanoparticles have different properties to the same materials in bulk?

A

They have a high surface area: volume ratio

101
Q

____ quantities of nanopartciles are needed to be effective for the same task than for materials with normal ____

A

Smaller
Sizes

102
Q

Give 2 uses of nanoparticles in medicine

A

Can deliver drugs right to cells where needed (as fullerenes are hollow, absorbed easily by body (be careful with talking about absorption as it’s not always accepted, + high surface area: volume ratio)

Silver nanoparticles have antibacterial properties (can be added to polymer fibres to make surgical masks + wound dressings)

103
Q

Give 1 use of nanopartciles in electronics

A

Some conductor and can be used in tiny electronic circuits in computer chips

104
Q

Give 1 use of nanopartciles in cosmetics

A

Improving moisturisers without making them oil]y

105
Q

Give 2 advantages of using nanoparticles in Sun creams

A

Better than usual ones at protecting from UV rays
Give better skin coverage than usual ones

106
Q

Give a reason for using nanopartciles in deodorants

A

Silver nanoparticles have anti bacterial properties

107
Q

Give 1 reason nanopartciles are used as catalysts

A

You need less to cover same stuff
As high surface area: volume ratio

108
Q

Give 4 risks of nanopartciles

A

We don’t know long term health impacts
Effects haven’t been investigated properly
Many argue products so should be clearly labelled so consumers can choose whether or not to use them
Could get into body and potentially damage cells
when washed away could damage environment

GCSE Chemistry Revision (13 decks)

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