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Chemistry- Paper 1 > Atomic Structure And The Periodic Table > Flashcards

Atomic Structure And The Periodic Table Flashcards

1
Q

What are all substances made from?

A

Atoms

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2
Q

What is an atom?

A

The smallest part of an element that can exist

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3
Q

Atoms of each element are represented by what?

A

A chemical symbol

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4
Q

How many different elements are there and where are they shown?

A

There are about 100 different elements. Elements are shown in the periodic table

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5
Q

What are compounds formed from?

A

They are formed from elements by chemical reactions

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6
Q

What do chemical reactions always involve?

A

Chemical reactions always involve the formation of one or more new substances and often involve a detectable energy change

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7
Q

What do compounds contain?

A

Compounds contains two or more elements chemically combined in fixed proportions

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8
Q

How can compounds be represented?

A

Compounds can be represented by formulae using the symbols of the atoms from which they were formed

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9
Q

How can compounds be separated?

A

Compounds can only be separated into elements by chemical reactions

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10
Q

What does the nucleus in an atom contain?

A

It contains protons and neutrons

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11
Q

Why does the nucleus in an atom have a positive charge?

A

It has a positive charge because of the protons

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12
Q

How do the electrons move around the atom?

A

They move around the nucleus in electron shells

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13
Q

Are electrons positively or negatively charged?

A

They are negatively charged and tiny but they cover a lot of space

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14
Q

Do electrons have a mass?

A

They have virtually no mass

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15
Q

Where is almost all of the mass of an atom?

A

In the nucleus

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16
Q

What does the sum of the protons and neutrons in an atom create?

A

Its mass number

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17
Q

Atoms of the same element can have different numbers of neutrons. What are these atoms called?

A

Isotopes of that element

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18
Q

Is the mass number the top number or bottom number?

A

The top number

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19
Q

Is the atomic number the top number or the bottom number?

A

The bottom number

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20
Q

What is the relative mass of a proton?

A

1

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21
Q

What is the relative mass of a neutron?

A

1

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22
Q

What is the relative mass of an electron?

A

Very small

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23
Q

What is a proton’s relative charge?

A

+1

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24
Q

What is a neutron’s relative charge?

A

0

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25
Q

What is an electron’s positive charge?

A

-1

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26
Q

In an atom what is the number of electrons is equal to?

A

The number of electrons is equal to the number of protons in the nucleus

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27
Q

Do you atoms have an overall electrical charge?

A

No

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28
Q

What does the atomic number represent?

A

The number of protons in an atom

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29
Q

Why do atoms not have an overall electrical charge?

A

Because they have the same number of protons as electrons

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30
Q

What does the mass number represent?

A

The mass number represents the total number of protons and neutrons in the atom

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31
Q

How do you work out the number of neutrons in an atom?

A

Subtract the atomic number from the mass number

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32
Q

Why does the charge cancel out in an atom?

A

Because 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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33
Q

Why do ions have an overall charge?

A

Because in an ion the number of protons doesn’t equal the number of electrons

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34
Q

What is an ion?

A

An ion is an atom or group of atoms that have lost or gained electrons

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35
Q

How big is the radius of a nucleus in an atom?

A

1×10 to the power of -14

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36
Q

The radius of the nucleus is less than how much of that of the atom?

A

1 out of 10,000

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37
Q

What are isotopes?

A

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

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38
Q

Isotopes of the same except for what?

A

Extra neutrons

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39
Q

Isotopes have the same atomic number but different what?

A

Different mass numbers

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40
Q

What do mixtures consist of?

A

A mixture consists of two or more elements or compounds not chemically combined together

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41
Q

The chemical properties of each substance in the mixture are what?

A

Unchanged

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42
Q

How can mixtures be separated?

A

Physical processes such as filtration, crystallisation, simple distillation, fractional distillation and chromatography

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43
Q

When mixtures are separated by physical processes it does not involve chemical reactions so are any new substances made?

A

There are no new substances made

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44
Q

Unlike in a compound, there’s no what between the different parts of a mixture?

A

There is no chemical bond

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45
Q

What were atoms thought to be like before the discovery of the electron?

A

Atoms were thought to be tiny spheres that could not be divided

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46
Q

What did the discovery of the electron lead to?

A

It led to the plum pudding model of the atom

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47
Q

The plum pudding model suggests that the atom is a ball of positive charge with what embedded in it?

A

Negative electrons

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48
Q

The results from what experiment led to the conclusion that the mass of an atom was concentrated at the nucleus and that the nucleus was charged?

A

Alpha particle scattering experiment

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49
Q

What replaced the plum pudding model?

A

The nuclear model

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50
Q

Who adapted the nuclear model?

A

Niels Bohr

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51
Q

How did Niels Bohr adapt the nuclear model?

A

By suggesting that electrons orbit the nucleus at specific distances

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52
Q

What did later experiments lead to? What was the name of the particles?

A

The idea that the positive charge of any nucleus could be subdivided into a whole number of smaller particles, each particle having the same amount of positive charge. The name proton was given to these particles

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53
Q

The experimental work of who provided the evidence to show the existence of what within the nucleus

A

James Chadwick provided the evidence to show the existence of neutrons within the nucleus

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54
Q

At the start of which century did who describe atoms as solid spheres and said that different spheres made up the different elements?

A

At the start of the 19th century John Dalton

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55
Q

In 1897 who concluded from his experiments that atoms weren’t solid spheres?

A

JJ Thomson

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56
Q

JJ Thompson’s measurements of charge and mass showed that an atom must contain what?

A

Even smaller, negatively charged particles- electrons

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57
Q

Who conducted the famous alpha particle scattering experiment in 1909?

A

Ernest Rutherford and his student Ernest Marsden

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58
Q

How did Ernest Rutherford and Ernest Marsden conduct the alpha particle scattering experiment?

A

They fired positively charged alpha particles at an extremely thin sheet of gold

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59
Q

Why couldn’t the plum pudding model be right?

A

Because while most of the particles went straight through the gold sheet, some were deflected more than expected, and a small number were deflected backwards

60
Q

Scientists realised that electrons in a ‘cloud’ around the nucleus of an atom would be attracted to the what causing the atom to collapse

A

Nucleus

61
Q

Niels Bohr’s nuclear model of the atom suggested that all electrons are contained in what?

A

Contained in shells

62
Q

What did Bohr propose about electrons?

A

That electrons orbit the nucleus in fixed shells and aren’t anywhere in between. Each shell is a fixed distance from the nucleus

63
Q

What is relative atomic mass?

A

The relative atomic mass of an element is an average value that takes account of the abundance of the isotopes of the element

64
Q

What is the formula to work out the relative atomic mass of an element

A

Relative atomic mass= sum of (isotope abundance x isotope mass number) divided by the sum of abundances of all the isotopes

65
Q

In an atom what occupies the lowest available energy levels?

A

The electrons

66
Q

How can the electronic structure of an atom be represented?

A

By numbers or a diagram

67
Q

What do you electrons always occupy?

A

Shells

68
Q

Which energy levels are always filled first?

A

The lowest energy levels are always filled first and are the ones closest to the nucleus

69
Q

How many electrons are allowed in the first shell?

A

2

70
Q

How many electrons are allowed in the second shell?

A

8

71
Q

How many electrons are allowed in the third shell?

A

8

72
Q

What does the atom want to do when the outer shell is not full?

A

React to fill it

73
Q

When are atoms happy?

A

When they have full electron shells

74
Q

Before the discovery of protons, neutrons as electrons, how did scientists attempt to classify the elements?

A

By arranging them in order of their atomic weight

75
Q

What was wrong with the early periodic tables?

A

They were incomplete

76
Q

Why were some elements placed in the wrong groups in early periodic tables?

A

Because the strict order of atomic weights had been followed

77
Q

How did Mendeleev overcome some of the problems in the early periodic table?

A

By leaving gaps for elements that he thought had not been discovered and in some places changed the order based on atomic weights

78
Q

What made it possible to explain why the order based on atomic weight was not always correct?

A

Knowledge of isotopes

79
Q

How are elements in the periodic table arranged?

A

In order of atomic number and so that the elements with similar properties are in columns known as groups

80
Q

Why is the table called the periodic table?

A

Because similar properties occur at regular intervals

81
Q

What gives elements in the same group similar chemical properties?

A

They have the same number of electrons in their outer shell

82
Q

What do elements with similar properties form?

A

Columns

83
Q

What are vertical columns called in the periodic table?

A

Groups

84
Q

What does the group number tell you? Except group 0

A

How many electrons there are in the outer shell

85
Q

How do the elements react in group 1?

A

The elements react more vigourously as you go down the group

86
Q

How do the elements in group 7 react?

A

Reactivity decreases as you go down the group

87
Q

What are the horizontal rows called?

A

Periods

88
Q

What does each new period represent?

A

Another full set of electrons

89
Q

Until quite recently what with the two obvious ways to categorise elements?

A

Physical and chemical properties and their relative atomic mass

90
Q

What are elements that react to form positive ions?

A

Metals

91
Q

What are elements that do not form positive ions?

A

Non-metals

92
Q

Where are metals found in the periodic table?

A

To the left and towards the bottom

93
Q

Where are non-metals found in the periodic table?

A

Towards the right and the top

94
Q

What do metals form when they react?

A

Positive ions

95
Q

What don’t generally form positive ions when they react?

A

Non-metals

96
Q

Metals to the left of the periodic table don’t have many what to remove?

A

Electrons

97
Q

Metals towards the bottom of the periodic table have outer electrons which are a long way from the nucleus so feel what?

A

A weaker attraction

98
Q

Why is it more difficult for non-metals to form positive ions?

A

Because they are either to the right of the periodic table- where they have lots of electrons to remove or towards the top- where the outer electrons are close to the nucleus so feel a strong attraction

99
Q

What are the elements in group 0 called?

A

The noble gases

100
Q

Are elements in group 0 unreactive?

A

Yes

101
Q

Why do elements in group 0 not easily form molecules?

A

Because the atoms have stable arrangements of electrons

102
Q

How many electrons do the noble gases have in their outer shell

A

The noble gases have eight electrons in their outer shell except for helium which has only two

103
Q

How does the boiling point of the noble gases change

A

The boiling points of the noble gases increase with increasing relative atomic mass (going down the group)

104
Q

What are the noble gases?

A

Helium, neon, argon, krypton, xenon and radon

105
Q

Why does the boiling points increase as you go down group 0 (noble gases)?

A

It is due to an increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome

106
Q

As the outer shells of group 0 elements are energetically stable, they don’t need to give up or gain electrons to become more stable this means they are what?

A

This means they are more or less inert- which means they don’t react with much at all

107
Q

What do group 0 elements exist as?

A

They exist as monatomic gases- single atoms not bonded to each other

108
Q

At room temperature what are all the elements?

A

Colourless gases

109
Q

Why are the noble gases non-flammable?

A

Because they are inert.

110
Q

What are the elements in group 1 known as?

A

Alkali metals

111
Q

Why do group 1 elements have characteristic properties?

A

Because of the single electron in their outer shell

112
Q

In group 1, how does the reactivity of the elements change?

A

The reactivity of the elements increases going down the group

113
Q

What do the group 1 elements look like?

A

They are silvery solids that have to be stored in oil as they are very reactive

114
Q

What are the alkali metals?

A

Lithium, sodium, potassium, rubidium, caesium, francium

115
Q

In which group are the elements all soft and have low densities?

A

Group 1- alkali metals

116
Q

The first three elements in group 1 are less dense than what?

A

Water

117
Q

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

A

They all have one electron in their outer shell which makes them very reactive and give them similar properties

118
Q

What are the trends of alkali metals as you go down the group?

A

Increasing reactivity, lower melting and boiling points and higher relative atomic mass

119
Q

It’s so easy for alkali metals to lose their outer electron that they only ever react to form what?

A

To form ionic compounds. These compounds are usually white solids that dissolve in water to form colourless solutions

120
Q

What happens when group 1 metals are put in water?

A

They react vigourously to produce hydrogen gas and metal hydroxides—salts that dissolve in water to produce alkaline solutions

121
Q

The more reactive (lower down the group) an alkali metal is the more what the reaction?

A

The more violent the reaction

122
Q

The amount of what given out by the reaction increases down the group?

A

Energy-the reaction with potassium releases enough energy to ignite hydrogen

123
Q

What happens when group 1 metals react with chlorine?

A

Group 1 metals react vigorously when heated in chlorine gas to form white metal chloride salts.

124
Q

Why will the reaction with chlorine get more vigorous as you go down the group 1 elements?

A

Because reactivity increases

125
Q

What happens when group 1 elements react with oxygen?

A

The group 1 elements can react with oxygen to form a metal oxide. Different types of oxide will form depending on the group 1 metal.

126
Q

Why do group 1 metals tarnish in the air?

A

Because group 1 metals react with oxygen in the air to form a full metal oxide layer.

127
Q

What are the group 7 elements known as?

A

The halogens

128
Q

Why do group 7 elements (halogens) have similar reactions?

A

They all have seven electrons in their outer shell.

129
Q

Are the halogens metals or non-metals?

A

Non-metals

130
Q

The group 7 elements consist of molecules made of what?

A

Molecules made of pairs of atoms

131
Q

How does the reactivity change as you go down the group 7 elements?

A

The reactivity decreases going down the group

132
Q

In group 7, the further down the group an element is the higher the what?

A

The higher it’s relative molecular mass, melting point and boiling point

133
Q

A more reactive halogen can displace a less reactive halogen from what solution?

A

From an aqueous solution of its salt

134
Q

The halogens are non-metals with what vapours ?

A

Coloured vapours

135
Q

What is fluorine?

A

A very reactive, poisonous yellow gas

136
Q

What is chlorine?

A

A fairly reactive, poisonous dense green gas

137
Q

What is bromine?

A

A dense, poisonous, red-brown volatile liquid

138
Q

What is iodine?

A

A dark grey crystalline solid or purple vapour

139
Q

The halogens all exist as what which are pairs of atoms?

A

They all exist as molecules which are pairs of atoms

140
Q

Why is it harder to gain an extra electron as you go down group 7?

A

Because as you go down, the elements become less reactive so it’s harder to gain an extra electron because the outer shell’s further from the nucleus

141
Q

Halogen atoms can share electrons via what?

A

Via covalent bonding with other non-metals to achieve a full outer shell

142
Q

Halogens can form what sort of compounds?

A

Molecular compounds

143
Q

What sort of bonds do halogens form with metals?

A

Ionic bonds

144
Q

Halogens form -1 Iona called?

A

Halides (F-,Cl-,Br- and I-)

145
Q

The compounds that halogens form have what sort of structure?

A

Ionic structures

146
Q

More reactive halogens will do what to less reactive ones?

A

Displace them

Chemistry- Paper 1 (2 decks)

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