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1
Q

What is the mass number

A

The total number of protons and neutrons in an atom

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2
Q

What is an isotope

A

An atom with the same number of protons but a different number of neutrons

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3
Q

What is the atomic number

A

The amount of protons in the atom

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4
Q

Which one is the mass number

A

The top number

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5
Q

Which one is the atomic number

A

The bottom number

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6
Q

How do you find out how many neutrons there are in an atom

A

Mass number-atomic number

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7
Q

What is an isotope

A

An atom with the same amount of protons and electrons but with a different number of neutrons

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8
Q

What is the only diferance that can exist between two isotopes

A

One being radioactive and the other not

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9
Q

How do you work out relative atomic mass

A

(%of isotope 1Xmass of isotope1)+(%of isotope2Xmass of isotope 2)

Ans/100

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10
Q

Who invented the law of octaves

A

John newlands

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11
Q

Give an example of issues Mendeleev had with putting attoms in order of their atomic mass

A

Iodine had a lower atomic mass than tellurium so it should come before tellurium. To get iodine in order with other elements with similar property’s he had to put it after tellurium, breaking his own rules

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12
Q

How did Henry Mosley propose to solve problems caused by ordering atoms by atomic mass

A

Using atomic number instead

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13
Q

What is the ordering value used along the rows of the periodic table

A

Atomic mass

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14
Q

What is eh period number in the periodic table

A

The vertical number from lithium down to francium

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15
Q

What does the period number show

A

The number of shells used up by the electrons

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16
Q

How do you draw out the electronic structure

A

Have how many electrons on each shell with commas between them

Don’t confuse with dot and cross diagrams

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17
Q

Why are ions

A

Electrically charged particles formed when atoms lose or gain electrons

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18
Q

What sort of ions do metals form

A

Positive

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19
Q

What sort of ions do non metals form

A

Negative

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20
Q

What are the strong electrostatic forces between oppositely charged ions called

A

Ionic bonds

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21
Q

What are the forces that hold ionic bonds together called

A

Electrostatic forces

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22
Q

How so you work out the charge of a metal ion

A

It is equal to the group number it is in

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23
Q

How do you work out the charge on a non metal ion

A

The group number minus eight

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24
Q

What does it mean if there is an ide at the end of the compound

A

There are only the atoms in the compound present

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25
Q

What does it mean if there is an ate at the end of the compounds name

A

There is an oxygen present

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26
Q

In what structure are ionic compounds arranged

A

Lattice

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27
Q

What does a lattice structure result in the formation of

A

A crystal

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28
Q

What do the strong ionic bonds in a crystal lattice cause

A

Very strong compounds and high boiling points

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29
Q

Why can solid ionic compounds not conduct electricity

A

The ions are held firmly in place

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30
Q

Why can molten ionic compounds move

A

Because the charged ions are free to move

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31
Q

Can a solution of ionic compounds conduct electricity

A

Yes

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32
Q

What is sodium chlorides melting point

A

800degrees Celsius

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33
Q

What is magnesium oxides melting point

A

2800 degrees c

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34
Q

What makes nacl a weaker bond than Mgo

A

Mgo has two pos and two neg charges where as nacl only has one of each

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35
Q

What is an example of a precipitation reaction

A

AgNO3+NaCL->AgCL+NaNO3

Silver nitrate(soluble)+sodium chloride(soluble)-> silver chloride(insoluble) + sodium nitrate soluble

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36
Q

A use for an insoluble salt

A

Barium sulphate-to show up on X-rays

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37
Q

Why does barium sulphate not kill people when they ingest it

A

It is toxic but is also insoluble so can not enter the blood stream

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38
Q

Steps of doing a flame test

Four

A

Dip a clean flame test loop in the sample solution

Hold a flame test loop at the edge of a Bunsen burner flame

Observe the changed colour of the flame and decide which metal it indicates

Clean the loop in acid and rinse with water, then repeat steps 1 to 3 with a new sample

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39
Q

Barium a flame test colour

A

Pale green

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40
Q

Calcium a flame test colour

A

Yellow red

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41
Q

Coppers flame test colour

A

Green blue

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42
Q

Lithiums flame test colour

A

Red

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43
Q

Sodium a flame test colour

A

Orange

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44
Q

Potassium flame test colour

A

Lilac

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45
Q

What are the uses of a flame test

A

Confirming the results of a precipitation test

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46
Q

What is an anion test

A

Detecting ions present in water through precipitation reactions

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47
Q

What is the colour of the precipitate formed by a soul fire ion and barium chloride

A

Barium sulphate is formed, it is white and insoluble

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48
Q

What do you use to test for halide ions in water

A

Silver nitrate, all halide ions form precipitates

49
Q

What colour precipitates do

Chlorine bromine and iodine ions when in a precipitation reaction with silver nitrate

A

Silver chloride white precipitate

Silver bromide cream precipitate

Silver iodide pale yellow precipitate

50
Q

How do you test for carbonates

A

Acid is added to the carbonate

If carbonate carbon dioxide will bubble off, test this by running it through lime water

51
Q

What is spectroscopy

A

When atoms are heated they all give off light, a proximity is used to split this light into a spectrum. Each element has it’s own distinctive light spectrum

52
Q

What is the process in which the light given off by an unknown element is analysed

A

Spectroscopy

53
Q

How was helium discovered

A

By studying the kin spectra emitted by the sun

54
Q

Which elements could not have been discovered without the use of spectroscopy

A

Rubidium
Caesium
Helium

55
Q

What happens to the group one metals melting point as you go down the group

A

The melting point decreases

56
Q

What happens to the density of group one elements as you go down the group

A

They become more dense

57
Q

in which direction do group one metals change their reaction speed

A

Speed and violence of the reaction increases as you go down the group

58
Q

What happens to lithium in a cold water reaction

A

It floats, it fizzes and becomes smaller until it disappears

59
Q

What is the word and letter equation of a lithium reaction with water

A

Lithium+water->lithium hydroxide+ hydrogen

2Li+2H2O->2LiOH+H2

60
Q

Describe the reaction sodium has with cold water

A

Fizzes rapidly

Melts to form a ball

Hydrogen produced May burn with an orange flame before the sodium disappears

61
Q

What are the word equation and letter plus number equations of the reaction between water and sodium

A

2Na+2H2O->2NOH+H2

Sodium+water->sodium hydroxide+hydrogen

62
Q

Describe the reaction between potassium and water

Five

A

The metal melts and floats

It moves around very quickly on the water

The hydrogen ignites immediately

The metal is set on fire with a lilac flame and sparks

There is sometimes a small explosion at the end of the reaction

63
Q

What is the word equation and letter plus number equation between potassium and cool water

A

Potassium+water->potassium hydroxide+water

2k+2H2O->2KOH+H2

64
Q

Why does the reactivity go up as you go down the group of alkaline metals

A

The number of electron shells increases so increases distance between the single outer electron and the nucleus the attraction from the positive nucleus to the negative electron is less making it easier to remove the outer electron to form an ionic bond

65
Q

What happens to the halogens boiling temp as you go down the group

A

Their boiling temp increases

66
Q

What is the trend in the state of group 7 matter as you go down the group

A

They move from solid liquid then gas

67
Q

What happens to the colour of the halogens as you go down the group

A

They get darker

68
Q

What happens to the reactivity of halogens as you go down the group

A

It reduces

69
Q

What is the product of a halogen reacting with a metal

A

A metal halide

70
Q

Uses of halogens

A

They are bleaching agents
Chlorine is used to bleach wood pulp white for paper

They kill bacteria, chlorine is added to drinking water to make it safe to drink

71
Q

What happens in a displacement reaction

A

a more reactive element replaces a less reactive element in a compound

72
Q

Give an example of a displacement reaction

A

When chlorine is added to sodium bromide solution the chlorine replaces the bromine

The solution turns brown due to the excess bromine in the mixture

73
Q

What is the word for chemically unreactive

A

Inert

74
Q

What Are five things noble/inert gases have in common

A

Non metals

Unreactive

Colourless

Are monatomic-exist as single atoms

75
Q

Uses for helium

1

A

Balloons and airships

Less dense than air so it causes stuff to float

76
Q

One use for neon

A

Used in advertising signs

It glows when electricity is passed through it, different coloured neon lights can be made by filling the inside tube with different chemicals

77
Q

Use for argon one

A

Used in light bulbs

The oxygen in air would burn the filament if it where filled with air

78
Q

What’s the name for a reaction that takes heat from the surroundings

A

Endothermic

79
Q

What’s the name for a reaction that releases heat into the environment

A

Exothermic

80
Q

What is an example of an Exothermic reaction

A

Neutralisation reactions

Combustion

81
Q

Give two examples of an endothermic reaction

A

Electrolysis

Photosynthesis

82
Q

What sort of energy process is bond breaking

A

Endothermic

83
Q

What sort of energy process is bond making

A

Exothermic

84
Q

What makes the difference between a reaction being Exothermic or endothermic

A

If more bonds are made than broken it is Exothermic

If more bonds are broken than made it is endothermic

85
Q

What is the equation for the calculating the energy transferred

A

Energy transferred=mass of water heated x specific heat capacity of water x temperature rise

86
Q

What are the two ways to measure the rate of reaction

A

Measure the rate in which the reactant is used up

Measure the rate in which the product is formed

87
Q

Things to measure in a rate of reaction equation

Prior
Two

A

The mass of substance

The volume of gas

88
Q

What is the equation for rate of reaction

A

Rate of reaction=amount of reactant or product/time taken

89
Q

What are the five things that increase the rate of reaction

A

The temperature envreasing

The concentration of a dissolved reactant being increased

The pressure of a reactant gas being increased

Solid reactants being broken into smaller pieces

A catalyst being used

90
Q

What is the minimum energy required for particles to react called

A

The activation energy

91
Q

Why are catalysts important in industry

A

They reduce costs

92
Q

How do catalysts work

A

They lower the activation energy needed

93
Q

Which catalyst is used in an nitrogen+hydrogen->ammonia reaction

A

Iron or platinum

94
Q

Which catalyst is used to make dilutive acid

A

Vanadium oxide

95
Q

What do catalytic converters do

A

Increase rate of reaction between carbon monoxide and unburnt fuel from exhaust gases with oxygen in the air using catalysts (platinum)

96
Q

How do you work out the relative formula mass of a compound

A

Add their relative atomic mass together

97
Q

What is the relationship between the mass of reactants and the mass of products

A

Mass of reactants=mass of products

98
Q

How to calculate relative atomic mass

A

(%Of isotope 1 x mass of isotope 1) + (%of isotope 2 x mass of isotope 2)

99
Q

Two property’s of simple molecular bonds

A

Low melting and boiling points because the weak inter molecular forces break down easily

Non conductive they don’t have any free electrons

100
Q

Property’s of giant molecular bonds

A

Very high melting points because a lot of strong covalent bonds must be broken

Variable conductivity diamond does not conduct electricity silicon is semi conductive graphite contains free electrons so it does conduct

101
Q

What are the three allotropes of carbon

A

Diamond graphite and buckminsterfullerene

102
Q

What are the uses if diamond and why

A

Hard and high melting point so is used in cutting tools

Shines so is used in jewellery

103
Q

Uses of graphite and why

A

Pencil leads
Graphite is in layers which slip off of the lead and onto the paper very easily

Component of many lubricants

Has a high melting point and is insoluble in water and is conductive so it makes it suitable as an anode and cathode in electrolysis

104
Q

How many bonds does carbon form in a diamond

A

4

105
Q

How many bonds does graphite form

A

Three

106
Q

What piece of equipment can be used to deprecate two im miscible liquids like oil and water

A

A separation funnel

The liquids are left to separate then a tap at the bottom is run until the lower liquid has left the mixture

107
Q

How are miscible liquids seep rated

A

Fractional distillation

108
Q

How air is seep rated into different fractions through cooling

Four steps

A

Water vapour condenses and is removed using absorbent filters

Carbon dioxide freezes at minus seventy nine degrees

Oxygen liquified at minus one hundred and eighty three degrees

Nitrogen liquifies at 196 degrees centigrade

Nitrogen and oxygen are then separated through fractional distillation

109
Q

What is chromatography

A

The separation of liquids on a piece of paper

This is suitable for dyes and food colouring

110
Q

How do you find out the rf value of a chemical

A

Rf can be identified by the equation

Distance moved by compound/distance moved by solvent

111
Q

What sort of bond holds together metals

A

Metallic bonds

112
Q

What do the transition metals all have in common

Seven

A

They form coloured compounds

They are good conductors of heat and electricity

They are are malleable

They are less reactive than alkaline metals

They have high melting points except for mercury

They are usually hard and tough

They have high densities

113
Q

How do you work out the percentage by mass of a component in a compound

A

(Mass number of element/mass number of whole molecule) x 100

114
Q

Formula for calculating percentage yield

A

(Actual yield/theoretical yield) * 100

115
Q

What are the three things that cause a non on hundred percent yield

A

Incomplete reactions

Losses during the practical

Unwanted by~products being produced

116
Q

What are three problems with waste products

A

Have no commerce benefits

Are difficult either socially or environmentally to dispose of

Are expensive to dispose of

117
Q

What does a reaction that is economically favourable have

A

High percentage yield

By products are commercially useful and are sold

The reaction occurs are a suitable rate

118
Q

What is an example of an economically favourable reaction

A

The production of ammonia

N2+3H2->2nh3

Chem (9 decks)

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