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Year 9 Science > Chemistry - Atomic structure and the periodic table > Flashcards

Chemistry - Atomic structure and the periodic table Flashcards

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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

What is the radius of an atom

A

0.1 nm (nanometres) (1 x 10-10m), it is very small

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4
Q

What is the radius of the

nucleus

A

1 x 10-14 m (1/10000th of the radius of an atom)

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5
Q

Where is most of the mass in an

atom located

A

In the nucleus

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6
Q

What can elements be

represented as

A

Symbols

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7
Q

How many elements are there

A

About 100

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8
Q

Where are elements shown

A

The periodic table

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9
Q

What is a compound

A

Two or more different types of atoms chemically joined together in fixed proportions

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10
Q

How can compounds be separated into their elements

A

By chemical reactions

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11
Q

Are the properties of a
compound the same as the
elements they are made from

A

No

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12
Q

What is a mixture

A

Two or more different types of elements or compounds not chemically bonded together, the chemical properties of each substance in the mixture are unchanged

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13
Q

5 ways to separate a mixture

A

Crystilisation, simple distillation, fractional distillation, chromatography and filtration

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14
Q

Why are the techniques used to
separate mixtures described as
physical processes

A

As mixtures contain two or more elements or compounds not chemically combined

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15
Q

Why is a lid used

chromatography

A

Stops solvent evaporating

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16
Q

How does filtration work

A

Pass through filter paper, liquid passes through, insoluble particles get caught by the filter paper

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17
Q

How do you carry out

crystallisation

A

Evaporation dish and heat source. Filter crystals out of the solution

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18
Q

How can you get sand and salt

from a mixture of the two

A

Dissolve in water, salt is soluble, sand isn’t. Filter to remove sand, then use crystallisation

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19
Q

What two processes are involved

in distillation

A

Evaporation and condensation

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20
Q

Where is the hottest part in

fractional distillation

A

The bottom

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21
Q

What property must the mixture
have to be able to separate by
fractional distillation

A

Each part of the mixture must have different boiling points

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22
Q

What is an element

A

A substance made up of only one type of atom

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23
Q

What is a molecule

A

Two or more atoms joined together e.g. O2, Cl2, H2O, CO2

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24
Q

Where are the reactants found

in an equation

A

Left side

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25
Q

Where are the products found in

an equation

A

Right hand side

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26
Q

What is distillation

A

The separating of a liquid using evaporation and then

condensation

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27
Q

A method used to separate two

or more liquids

A

Fractional distillation

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28
Q

A method used to separate the
coloured compounds in a
mixture

A

Chromatography

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29
Q

A method used to separate an insoluble solid from a liquid

A

Filtration

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30
Q

What is crystallisation

A

A way to separate a dissolved solid from a solution by evaporation to leave crystals of the solid

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31
Q

Before electrons were
discovered, was it thought that
atoms could be divided

A

no

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32
Q

Before electrons were
discovered, atoms were thought
to be what

A

Tiny spheres

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33
Q

What model did the discovery of

the electron lead to

A

Plum pudding model

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34
Q

What was the plum pudding

model

A

That the atom was a ball of positive charge with negative

electrons embedded in it

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35
Q

What model replaced the plum

pudding model

A

Nuclear model

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36
Q

What experiment led to idea
that mass of the atom was
concentrated in the centre

A

Alpha scattering experiment

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37
Q

What would happen with the
alpha particle experiment if the
plum pudding model was correct

A

Expect particles to pass straight through or slightly deflected

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38
Q

What was observed in the alpha

scattering experiment

A

Most of the particles passed through
Some deflected more than expected
Very few deflected backwards

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39
Q

What charge are alpha particles?

A

Positively charged

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40
Q

Explain the observations of the alpha scattering experiment

A

Most of the particles passed through = atom is mostly empty space
Some deflected more than expected = alpha particles hit a positively charged centre and repelled
Very few deflected backwards = alpha particles hit a concentrated mass

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41
Q

Describe the nuclear model

A

has a positively charged nucleus, most of the atom is empty space

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42
Q

What sub atomic particle was

discovered first

A

Electron

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43
Q

Who led to the idea that

electrons are in orbitals/shells

A

Niels Bohr

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44
Q

What order where the sub

atomic particles discovered

A

Electron, proton the neutron

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45
Q

Who provided evidence for the
existence of neutrons within the
nucleus

A

Chadwick (about 20 years after the nucleus idea was

accepted)

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46
Q

What are the differences
between the plum pudding
model and the nuclear model

A

Plum - single ball of positive charge spread throughout,
electrons in embedded, no nucleus, no neutrons
nuclear - positive centre/nucleus, electrons in fixed positions, has a nucleus, has neutron

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47
Q

What did Bohr suggest about the arrangement and movement of electrons

A

Electrons orbit the nucleus in shells that are a fixed distance
from the nucleus. Electrons can only be found in these shells

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48
Q

What particle was discovered as the nucleus was found to be

positive

A

Proton

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49
Q

Name the three sub atomic particle

A

Proton, neutron & electron

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50
Q

What is the relative charge of a

proton

A

1+

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51
Q

What is the relative charge of a

neutron

A

0

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52
Q

What is the relative charge of an

electron

A

-1

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53
Q

Why do atoms have no overall
electrical charge (are neutral)

A

The number of positive proton equals the number of negative electrons so charges cancel out

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54
Q

What does the atomic number

tell you

A

number of protons

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55
Q

What makes an atom of an

element the element it is

A

The protons, e.g. If an atom has 8 protons, it must be oxygen

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56
Q

What makes atoms of elements different to each other

A

different amount of protons

57
Q

What is the relative mass of a

proton

A

1

58
Q

What is the relative mass of a

neutron

A

1

59
Q

What is the relative mass of an

electron

A

Very small

60
Q

What is mass number

A

The sum of the protons and neutrons in an atom

61
Q

What is an isotope?

A

The same element but with the same number of protons but different numbers of neutrons

62
Q

Why is the relative atomic mass of chlorine not a whole number

A

Has more than one isotope

63
Q

How do the chemical properties of an isotope differ

A

Doesn’t - has have the same number of electrons

64
Q

How do you work out the number of protons

A

Use the atomic (proton) number

65
Q

How do you work out the number of electrons in an atom

A

Same as the protons

66
Q

How do you work out the number of neutrons

A

Mass number - atomic number

67
Q

What is relative atomic mass

A

The average value that takes account of the abundance of the isotopes of an element

68
Q

What do the electrons occupy in

an atom

A

lowest energy available

69
Q

How many electrons are there found in shells 1, 2 & 3

A

2,8,8

70
Q

What sub atomic particle is involved in bonding (chemical

reactions)

A

electrons

71
Q

What holds atoms of elements

together in compounds

A

Chemical bonds

72
Q

What holds atoms of elements

together in compounds

A

Chemical bonds

73
Q

How were early periodic tables

arranged (Newland and Mendeleev)

A

By atomic weights (as protons, neutron and electrons were not discovered)

74
Q

What did Newland do wrong

A

Put more than one element in a box

Followed a strict order of atomic weight

His pattern eventually broke down

He didn’t leave any gaps for undiscovered elements which led to elements being place in inappropriate groups

75
Q

What is the name of the

scientist who first published the periodic table

A

Dmitri Mendeleev

76
Q

What did Mendeleev do to solve

the problem of elements not in the correct groups

A

He left gaps for undiscovered elements
He was able to predict the properties of these AND was
correct

77
Q

How is the modern periodic

table ordered?

A

In order of atomic number (protons)

78
Q

What are elements with similar

properties place in

A

Groups (columns)

79
Q

What do all elements in the

same group have in common?

A

The same number of electrons in their outer shell

80
Q

How is the modern periodic

table arranged

A

Atomic number (protons) with elements in the same group as their outer number of electrons

81
Q

What is the name given to the

columns on the periodic table

A

Group

82
Q

rows of the periodic table

A

Periods

83
Q

What does the group number of

an element tell you

A

The number of electron in its outer shell/ energy level

84
Q

What does the period number of an element tell you

A

Number of energy levels the atom has

85
Q

How many groups are there on the periodic table

A

8

86
Q

How are the metals and non-metals arranged in the periodic table

A

Metals are on the left hand side and metals on the right

87
Q

What is an ion

A

A charged particle

88
Q

What types of ions do metals

form

A

Positive, as they lose electrons to get a full outer shell

89
Q

What types of ions do non-

metals form

A

Negative, as they gain electrons to get a full outer shell

90
Q

What elements are founds in the
block of the periodic table
between groups 2&3

A

Transition metals

91
Q

What are the elements in group

0 called

A

Noble gases

92
Q

Why are Noble gases unreactive/inert

A

As they have a full outer shell so their atoms have stable
electron arrangements (He-2, all others-8)

93
Q

What happens to the boiling
point of the Noble gases as you
go down the group

A

Increases, as relative atomic mass increases so stronger

intermolecular forces

94
Q

What does monoatomic mean

Noble gases

A

Exist as atoms

95
Q

What are the elements in group

1 called

A

Alkali metals

96
Q

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

A

1

97
Q

Why do the metals in group 1

have similar properties

A

All have 1 electron in their outer shell

98
Q

What happens to the melting

point as you down group 1

A

Decreases

Due to metallic bonds becoming weaker as go down the group

99
Q

What happens to the reactivity
of the group 1 metals as you go
down the group

A

Increases

100
Q

Why do the alkali metals
become more reactive as you go
down the group

A

Increase in number of electrons/electron shells,
outer electron is further from the nucleus
so is less attracted to the positive nucleus
so easier to lose an electron

101
Q

Give three characteristics of

alkali metals

A

Metals, soft, highly reactive

102
Q

What are the products when a
group 1 metals reacts with
water

A

Metal hydroxide and hydrogen

103
Q

What is the word equation for
the reaction of sodium with
water

A

Sodium + water  sodium hydroxide + hydrogen

104
Q

What is the balanced symbol equation of sodium with water

A

2Na + 2H2O —> 2NaOH + H2

105
Q

What observations do you see
when an alkali metal reacts with
water?

A

Alkali metals float on water = less dense than water
alkali metals fizz = hydrogen gas released

universal indicator (if added) goes purple = alkali produced aka metal hydroxide

metal dissolves = metal reacting to produce metal hydroxide (aq)
Reactions become more vigorous as go down group 1

106
Q

What is observed when lithium

reacts with water

A

Floats, moves on the surface, fizzes

107
Q

What is observed when sodium

reacts with water

A

Floats, forms a ball, moves on the surface, fizzes, can see a yellow flame

108
Q

What is observed when

potassium reacts with water

A

Floats, forms a ball, moves on the surface, fizzes, a lilac

flame

109
Q

What is formed when alkali

metals react with oxygen

A

Metal oxide

110
Q

What is the word equation for
the reaction of sodium with
oxygen

A

Sodium + oxygen  sodium oxide

111
Q

What is the symbol equation for the reaction of sodium with oxygen

A

4Na + O2 —> 2Na2O

112
Q

What observations do you see
when lithium reacts with
oxygen?

A

Red-tinged flame
Bright flame in oxygen
White solid formed

113
Q

What observations do you see
when sodium reacts with
oxygen?

A

Yellow-orange flame
Brighter flame in oxygen
White solid formed

114
Q

What observations do you see
when potassium reacts with
oxygen?

A

Lilac flame
Even brighter flame in oxygen
White solid formed

115
Q

What is formed when alkali

metals react with chlorine

A

A metal halide is formed e.g. Sodium chloride

116
Q

What is the word equations for
the reaction of sodium with
chlorine

A

Sodium + chlorine  sodium chloride

117
Q

What is the symbol equation for
the reaction of sodium with
chlorine

A

2Na + Cl2  2NaCl

118
Q

What observations do you see
when group 1 elements react
with chlorine?

A

Bright flame

White solid

119
Q

What are the elements in group

7 called

A

Halogens

120
Q

How many electrons do all
groups 7 elements have on their
outer shell

A

7

121
Q

What state is chlorine at room

temperature and its colour?

A

Yellow/ green gas

122
Q

What state is bromine at room

temperature and its colour?

A

Brown liquid

123
Q

What state is iodine at room

temperature and its colour?

A

Purple solid

124
Q

Three properties of the halogens are

A

Non-metals,
very reactive,
diatomic (exist as molecules),
melting points and boing points increase down the group
(links with change of states as go down the group)

125
Q

What is the charge on a halide

ion

A

-1, as lose one electron to get a full outer shell

126
Q

What happens to the reactivity
of the group 7 halogens as you
go down the group

A

Decreases

127
Q

Why do the halogens become
less reactive as you go down the
group

A

Increase in number of energy levels,
outer shell of electrons are further from the nucleus
so less attraction between outer electrons and nucleus
so harder to gain and attract a new electron

128
Q

What sort of compounds do
halogens form with other non
metals

A

Covalent

129
Q

What sort of compounds do

halogens form with metals

A

Ionic

130
Q

What sort of molecules do all

halogen form

A

Diatomic, go round in pairs

131
Q

What is a displacement reaction

A

When a more reactive element displaces (kicks out) a less reactive element, so more reactive halogen (higher up the group) can kick out a less reactive halogen from an aqueous solution of its salt

132
Q

A word equation to show the
displacement reaction between
chlorine and sodium bromide

A

Chlorine + sodium bromide  bromine + sodium chloride

133
Q

A symbol equation to show the
displacement reaction between
chlorine and sodium bromide

A

Cl2 + 2NaBr  Br2 + 2NaCl

134
Q

where are the transition metals found in the periodic table

A

in the centre, between groups 2 and 3

135
Q

Compare properties of transition metals to alkali

A

higher melting point,
higher density,
stronger,
harder

136
Q

how does the reactivity of the transition metals compare to the reactivity of alkali metals

A

less reactive

137
Q

what are the properties of transition metals

A

can form different charged ions
form coloured compounds
useful as catalysts

138
Q

what property of transition metals is an important industrial use

A

used as catalysts to speed up reactions

Year 9 Science (5 decks)

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