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C4 Flashcards

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1
Q

What are atoms?

A

Tiny particles of matter that make up everything in the universe

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2
Q

At the start of the 19th century what did John Dalton describe atoms as?

A

Solid spheres and the different spheres made up the different elements

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3
Q

In 1897 what did J J Thomson conclude from his experiment?

A

That atoms weren’t solid spheres. His measurements of charge and mass showed that an atom must contain even smaller, negatively charged particles - electrons.
This was known at the plumb pudding model.

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4
Q

Who showed that the ‘plumb pudding model’ was wrong?

A

Ernest Rutherford, and his students Hans Geiger and Ernest Marsden.
They conducted the famous gold foil experiment.

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5
Q

What is the famous gold foil experiment?

A

They fired positively charged particles at an extremely thin sheet of gold. From the plumb pudding model, they were expecting most of the particles to be deflected by the positive ‘pudding’ that made up most of the atom. In fact, most of the particles passed straight through the gold atoms, and a very small number were deflected backwards. so the plumb pudding model couldn’t be right.

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6
Q

What new theory did Rutherford come up with?

A

The theory of the nuclear atom.
In this there’s a tiny, positively charged nucleus at the centre, surrounded by a ‘cloud’ of negative electrons - most of the atom is empty space.

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7
Q

Most scientists realised that the ‘cloud’ around the atom would be attracted to the nucleus causing the atom to collapse. What did Bohr decide instead?

A

That the electrons can only exist in fixed orbits, or shells, and not anywhere between. Each shell had a fixed energy.
It contained a nucleus in the middle and was pretty close to the structure we have today.

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8
Q

Give 4 facts about the nucleus

A

It’s in the middle of the atom
It contains protons and neutrons
It has a positive charge because of the protons
Almost the whole mass of the atom is concentrated in the nucleus

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9
Q

Give 5 facts about electrons

A

They move around the nucleus in electron shells
They’re negatively charged
They’re tiny, but they cover a lot of space
The volume of their orbits determines the size of the atom
Electrons have virtually no mass

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10
Q

What are protons?

A

Heavy and positively charged

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11
Q

What are neutrons?

A

They are heavy and neutral

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12
Q

What are electrons?

A

Tiny and negatively charged

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13
Q

What is the number of protons equal to in an atom?

A

Electrons

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14
Q

What charge do neutral atoms have?

A

No charge

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15
Q

Wanna hear a joke…? :P

A

A neutron walks into a bar and asks how much for a drink.

The bar man says, “For you, no charge.”

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16
Q

Why are atoms neutral?

A

The charge on the electrons is the same size as the charge on the protons but opposite - so the charges cancel out

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17
Q

What is ‘The Mass Number’?

A

The top number next to the symbol on the periodic table.

It is the total number of protons and neutrons in the atom

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18
Q

What is ‘The Atomic Number’?

A

The bottom number next to the symbol on the periodic table.

It is the number of protons in the atom

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19
Q

How can you get the number of neutrons in an atom?

A

By subtracting the atomic number from the mass number

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20
Q

Which number is always the biggest number when looking at an atom on the periodic table?

A

The mass number

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21
Q

What is the ‘relative atomic mass’?

A

The mass number, the top number when looking at an atom on the periodic table

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22
Q

What are elements?

A

Substances made up of only one type of atom.

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23
Q

How many elements are there?

A

100 ish, more are still being discovered

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24
Q

What does the modern periodic table show the elements in order of?

A

Ascending atomic number

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25
Q

What do all of the atoms in the same columns share?

A

Similar properties

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26
Q

What are the vertical columns in the periodic table called?

A

Groups

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27
Q

What does the group of an atom correspond with?

A

The number of electrons on its outer shell

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28
Q

How many electrons do group 1 elements have on their outer shell?

A

1

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29
Q

How many electrons do group 7 elements have on their outer shell?

A

7

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30
Q

What are rows in the periodic table called and what does each new row represent?

A

Periods, each new period represents another full shell of electrons

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31
Q

What are isotopes?

A

Different forms of the same element, which have the same number of protons but a different number of neutrons.

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32
Q

What are the similarities and differences between atomic numbers and mass numbers in isotopes?

A

Isotopes have the same atomic number but different mass numbers

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33
Q

Give an example of a popular pair of isotopes

A

Carbon-12 and carbon-14

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34
Q

In the 1800’s what was the only thing they could measure?

A

Relative atomic mass

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35
Q

What did Dobereiner do to try and organise the elements?

A

Put them in groups of three called triads. The average relative atomic mass of the top and bottom one was equal to the relative atomic mass of the middle one

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36
Q

What was the first good effort of trying to organise the atoms called?

A

Newlands’ Law of Octaves

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37
Q

Give some problems of Newlands’ Law of Octaves

A

The pattern broke down on the third row
He left no gaps for the elements that were yet to be discovered
His groups contained elements that didn’t have similar properties
He mixed up metals and non metals

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38
Q

Who’s theory do we still use for our periodic table today?

A

Dmitri Mendeleev, he left gaps where he thought elements should be and when new ones were found they fitted the pattern. Yay!

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39
Q

What are the three electron shell rules?

A

Electrons always occupy shells
The lowest energy levels are always filled first
Only a certain number of electrons are allowed in each shell.

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40
Q

How many electrons are allowed in the first shell?

A

2

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41
Q

How many electrons are allowed in the first and second shells?

A

8 in each

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42
Q

What is electron configuration?

A

How the electrons occupy the shells around an atom

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43
Q

What is the electron configuration for nitrogen if the atomic number is 7?

A

2.5

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44
Q

What is the electron configuration for aluminium if the atomic number is 13?

A

2.8.3

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45
Q

What can you use electron configuration to work out?

A

The period, group and atomic number of an element

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46
Q

What is an ion?

A

An atom which has lost or gained electrons causing it to become positively or negatively charged

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47
Q

What happens in ionic bonding?

A

Atoms lose or gain electrons to form charged particles (or ions) which are then strongly attracted to one another (because of the attraction of opposite charges, + and - )

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48
Q

How many electrons to the group 1 elements have on their outer shells and why does this make them very reactive?

A

They only have one, the main aim for an atom is to have a full outer shell so they are keen to get rid of that extra electron and turn into a positive ion.

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49
Q

What do positive ions want to bond to?

A

Negative ions

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50
Q

What do group 6 or 7 elements want to do?

A

Gain one or two electrons

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51
Q

What do group 7 elements become when they gain an extra electron?

A

A negative ion

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52
Q

What do ionic compounds form?

A

Giant ionic lattices

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53
Q

Give 3 properties of ionic compounds

A

The ions are closely packed together
The ions are not free to move meaning they don’t conduct electricity in solid form
There are very strong chemical bonds between all the ions

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54
Q

Give two names of giant ionic structures

A

Magnesium oxide

Sodium chloride

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55
Q

Give two properties of both magnesium oxide and sodium chlordie

A

They both have high melting points

They both have high boiling points

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56
Q

Why do magnesium oxide and sodium chloride both have high melting and boiling points?

A

Because they have very strong attractions between oppositely charged ions in the giant structures

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57
Q

Which has a higher melting point:
Mg2+ + O2-
or
Na+ + Cl-

A

Mg2+ + O2-
This is because the forces are double the strength of the other one, so the attraction between them is harder to overcome
Also the O2- ions are smaller than Cl- ions, so the ions in MgO can pack together more closely, this also makes the attraction between them harder to overcome.

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58
Q

What happens when MgO melts?

A

The ions are free to move and they’ll conduct electricity

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59
Q

When metals form ions what do they do?

A

They lose electrons to form positive ions

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60
Q

When non-metals form ions what do they do?

A

They gain electrons to form negative ions

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61
Q

K+ + Cl- —> ?

A

KCl

62
Q

2K+ + O2- —> ?

A

K(little 2) O

63
Q

What are covalent bonds?

A

When two atoms share electrons so that their outer shells are complete

64
Q

How many more electrons do hydrogen atoms need to have a complete outer shell? Because of this, how many covalent bonds do they need to form?

A

one more

This means they only need to form one covalent bond between them to become H2

65
Q

How many electrons do chlorine atoms need to complete their outer shells, how many covalent bonds do they form with other atoms and what does it form after?

A

one
one
Cl2

66
Q

How many electrons are on the outer shell of a carbon atom, how many covalent bonds form with it and what does it form after?

A

4
4
Methane, CH4

67
Q

How many more electrons does an oxygen atom need on its outer shell, how many covalent bonds does it from with other atoms and what does it make after?

A

2
2
H2O

68
Q

How many more electrons does a carbon atom need on its outer shell, how many covalent bonds does it form with oxygen and what does it create afterwards?

A

4
2 - because oxygen shares two electrons per covalent bond
CO2

69
Q

What do substances formed from covalent bonds usually have?

A

simple molecular structures
This is because the atoms within the molecules are held together by very strong covalent bonds, but in contrast the forces of attraction between these molecules are very weak

70
Q

What is a result of feeble intermolecular forces?

A

The melting and boiling points are very low, this is because the molecules are very easily parted form each other

71
Q

What are most molecular substances in the form of at room temperature?

A

Gases or liquids

72
Q

Why don’t most molecular substances conduct electricity?

A

There are no free electrons or ions

73
Q

What are group 7 elements called?

A

Halogens

74
Q

What is group 7 made up of?

A 
Fluorine
Chlorine
Bromine
Iodine
Astatine
75
Q

What happens as you go down group 7 in the periodic table?

A

They become less reactive
This is because there’s less inclination to gain the extra electron to fill the outer shell when its further out from the nucleus.
Also the melting points and boiling points of them increase as you go down the group 7 elements

76
Q

What is chlorine like at room temperature?

A

Fairly reactive
Poisonous
Dense green gas
Low boiling point

77
Q

What is bromine like at room temperature?

A

Dense
Poisonous
Orange liquid

78
Q

What is iodine like at room temperature?

A

A dark grey crystalline solid

High boiling point

79
Q

What is reduction?

A

The gain of electrons

80
Q

What does a halogen molecule turn into when it gains electrons?

A

A halide ion

81
Q

Halogens react vigorously with alkali metals to form what?

A

Salts called ‘metal halides’

82
Q

2Na + Cl2 —> ?

Sodium + Chlorine —> ?

A

2NaCl

Sodium chloride

83
Q

2K + Br2 —> ?

Potassium + Bromine —> ?

A

2KBr

Potassium bromide

84
Q

What can more reactive halogens do?

A

Displace less reactive ones

85
Q

What can chlorine displace?

A

Bromine and iodine from a solution of bromide or iodide

86
Q

What can bromine displace?

A

Iodine

87
Q

Chlorine + Potassium iodide —>

A

Iodine + Potassium chloride

88
Q

Chlorine + Potassium bromide —>

A

Bromine + Potassium chloride

89
Q

What are the group 1 metals called?

A

Alkali metals

90
Q

What happens as you go down group 1?

A

They become more reactive

91
Q

What are the physical properties of the group 1 elements?

A

Low melting point
Low boiling point
Low density
Very soft

92
Q

What bonds to group 1 elements from?

A

Ionic ones only

93
Q

What is oxidation?

A

The loss of electrons

94
Q

What happens when you put group 1 elements in the water?

A

They react very vigorously and produce hydrogen gas

95
Q

What do sodium and potassium do in the heat of the reaction?

A

Melt

96
Q

What are the first 5 group 1 elements?

A 
Lithium
Sodium
Potassium
Rubidium
Caesium
97
Q

2Na H2O —> ?

Sodium + water —> ?

A

2NaOH H2

Sodium hydroxide + Hydrogen

98
Q

What do all the alkali metals form when they react with water?

A

Their symbol and then OH
Lithium produces LiOH
Potassium forms KOH
(they also all produce H2 as a product too)

99
Q

How can you test to see which alkali metal you have?

A

Dip a wire loop into some hydrochloric acid to clean and moisten it
Put the loop into a powdered sample of the compound to be tested, then place the end in a blue bunsen flame
Alkali metal ions will give pretty coloured flames - the colour of the flame tells you which alkali metal is present.

100
Q

What colour flame does lithium produce?

A

Red

101
Q

What colour flame does sodium produce?

A

Yellow/orange

102
Q

What colour flame does potassium produce?

A

Lilac

103
Q

What structure do all metals have?

A

A crystal structure

104
Q

What are metallic bonds?

A

The bonds allow the outer electron(s) of each atom to more freely. This creates a ‘sea’ of delocalised electrons throughout the metal.

105
Q

Give ___ properties of metals?

A 
Very hard, dense and lustrous (shiny)
They have a high tensile strength
They're malleable
High melting points and boiling points
Good conductors of heat and electricity
106
Q

In what conditions does the strength of a metallic bond decrease?

A

When the atomic radius increases

107
Q

Give the properties of a saucepan and the metal that they are made from

A

Good conductor of heat, doesn’t rust easily

Stainless steel - its cheap too

108
Q

Give the properties of electrical wiring and the metal that is used for them

A

Good conductor of electricity, easily bent

Copper. One of the best conductors around

109
Q

Give the properties of aeroplanes and the metal used for them

A

Low density, strong, doesn’t corrode

Aluminium. Titanium is sometimes used, but it’s a lot more expensive

110
Q

Give the properties of bridges and the metal used for them

A

Strong

Steel - this is mostly iron, but it’s got a little bit of carbon in it, which makes it a lot less brittle

111
Q

At what temperatures are some metals super conductors?

A

Very low temperatures

112
Q

What is electrical resistance?

A

Where metals that conduct electricity have the draw backs of losing their power through heat as they are used

113
Q

Do superconductors have electrical resistance?

A

NO

114
Q

What can you make using super conductors?

A

Power cables that transmit electricity without any power loss
Really strong electromagnets that don’t need a constant power source
Electronic circuits that work really fast, because there’s no resistance to slow them down

115
Q

What’s the catch of superconductors?

A

They only start superconducting at less than -265 degrees C

Getting things what cold is very hard and very expensive

116
Q

What are scientists trying to do regarding super conductors?

A

They are trying to develop them to work at room temperature. So far they’ve got up to -135 degrees C which is much cheaper but the ideal is 20 degrees C

117
Q

What are the metals in the middle of the periodic table?

A

Transition metals

118
Q

What do transition metals make?

A

Googd catalysts

119
Q

What is an iron catalyst used for?

A

Making ammonia in the Haber process

120
Q

What is a nickel catalyst used for?

A

The hydrogenation of alkenes (e.g. to make margerine)

121
Q

What colours are Iron (II) compounds usually?

A

Light green

122
Q

What colours are Iron (III) compounds usually?

A

Orange/brown

123
Q

What colours are copper compounds usually?

A

Blue

124
Q

What is thermal decomposition?

A

The breaking down of something with heat

125
Q

Can transition metals thermally decompose?

A

Yes

126
Q

What do transition metal carbonates always include some of?

A

CO3

127
Q

What do transition metal oxides break down into when they are thermally decomposed?

A

They make a metal oxide and carbon dioxide.

This usually results in a colour change

128
Q

Give the word and symbol equation for the thermal decomposition of copper (II) carbonate

A

Copper(II) carbonate —> Copper oxide + carbon dioxide

CuCO3 CuO CO2

129
Q

What is a precipitation reaction?

A

Where two solutions react and an insoluble solid forms in the solution

130
Q

What do transition metal compounds form when they react with sodium hydroxide?

A

An insoluble hydroxide with then precipitates out

131
Q

CuSO4 + 2NaOH —> ?

copper(II) sulphate + sodium hydroxide —> ?

A

Cu(OH)2 Na2SO4

copper(II) hydroxide + sodium sulphate

132
Q

What is the ionic equation for the precipitation reaction of coper sulphate and sodium hydroxide?

A

Cu2+ + 2OH- —> Cu(OH)2

133
Q

How can you test for transition metal ions?

A

Using precipitation reactions

134
Q

What transition metal hydroxide produces a blue solid?

A

Copper (II) hydroxide

135
Q

What transition metal hydroxide produces a grey/green solid?

A

Iron (II) hydroxide

136
Q

What transition metal hydroxide produces a orange/brown solid?

A

Iron (III) hydroxide

137
Q

What happens if you add sodium hydroxide to an unknown soluble salt?

A

The colour that is produced is an indicator of what the unknown soluble salt is. (if its orange/brown the salt will be iron (III) hydroxide)

138
Q

Where do we get our water from in the UK?

A

Surface water: lakes, rivers and reservoirs (artificial lakes) But these start to run dry during the summer months.
Groundwater: aquifers (rocks that trap water underground)

139
Q

What are water resources limited by?

A

Annual rainfall

140
Q

What are the three stages of water purification?

A

Filtration - a wire mesh screens out large twigs and then gravel and sand beds filter out any other solid bits
Sedimentation - iron sulphate or aluminium sulphate is added to the water, which makes fine particles clump together and settle at the bottom
Chlorination - chlorine gas is bubbled through to kill harmful bacteria and other microbes

141
Q

What various pollutants are still in our tap water?

A

Nitrate residues (from excess fertiliser ‘run off’ into rivers and lakes
Lead compounds from old lead pipes
Pesticide residues from spraying too near to rivers and lakes

142
Q

What is wrong with water distillation?

A

It needs lots of energy
It’s really expensive
Not practical for producing large quantities of fresh water

143
Q

How can you test for sulphate ions in water?

A

Using Barium Chloride

  1. add some dilute hydrochloric acid to the test sample
  2. Then add 10 drops of barium chloride solution
  3. If you see a white precipitate, there are sulphate ions in the sample
144
Q

Give an example of where potassium sulphate is present in the sample of water

A

barium chloride + potassium sulphate —> barium sulphate + potassium chloride
(BaCl2 + K2SO4 —> BaSO4 + 2KCl)

145
Q

How can you test for halide ions in water?

A

Using silver nitrate

  1. add some dilute nitric acid to the test sample
  2. then add 10 drops of silver nitrate solution
  3. if halide ions are present a precipitate will form
146
Q

When testing for chloride ions in water what colour precipitate will form?

A

white

147
Q

When testing for bromide ions in water what colour precipitate will form?

A

cream

148
Q

When testing for iodide ions in water what colour precipitate will form?

A

pale yellow

149
Q

Silver nitrate + sodium chloride —> ?

AgNO3 NaCl

A

Silver chloride + sodium nitrate

AgCl NaNO3

150
Q

Silver nitrate + sodium bromide —> ?

AgNO3 NaBr

A

Silver bromide + Sodium nitrate

AgBr NaNO3

151
Q

Silver nitrate + sodium iodide —> ?

AgNO3 NaI

A

Silver iodide + sodium nitrate

AgI NaNO3

Chemistry (3 decks)

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