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year 10 mock exam revision > chemistry topic 1 periodic table > Flashcards

chemistry topic 1 periodic table Flashcards

1
Q

where is the nucleus and what does it contain?

A

its in the middle of the atom and contains the protons and neutrons

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2
Q

what’s the overall charge of the nucleus?

A

positive because of the protons

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3
Q

where are the electrons and what charge are they?

A

they are around the nucleus in shells and are negatively

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4
Q

what’s the relative mass if a proton?

A

1

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5
Q

what’s the relative mass of a neutron?

A

1

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6
Q

what’s the relative mass of an electron?

A

very small

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7
Q

what is the relative charge of a proton ?

A

+1

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8
Q

what is the relative mass of a neutron?

A

0

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9
Q

what is the relative mass of an electron?

A

-1

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10
Q

what are atoms overall?

A

neutral ( no charge)

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11
Q

what is charge like in an ion?

A

the number of protons isn’t equal to the number of electrons

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12
Q

what does the atomic number tell you?

A

how many protons and electrons there are

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13
Q

what does the mass number of an element tell us?

A

the total number of protons and neutrons in the atom

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14
Q

how do you get the number of neutrons in an atom?

A

subtract the atomic number from the mass number

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15
Q

what is an element ?

A

a substance made up of atoms that all have the same number of protons in their nucleus

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16
Q

if a substance only contains atoms with the same number of protons its call what?

A

element

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17
Q

what is an 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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18
Q

how do you work out the relative atomic mass of an element?

A

sum of (isotope abundance x isotope mass number)/ sum of abundance of all isotopes

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19
Q

what are compounds?

A

substances formed from two or more elements , the atoms of each are in fixed proportions throughout the compound and are chemically bonded together

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20
Q

what does making bonds involve?

A

giving away, taking or sharing electrons

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21
Q

what is a compound that consists of metal and non metal?

A

an ion

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22
Q

what does the opposite charges in an ion mean?

A

they are strongly attracted to each other

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23
Q

what does a compound consist of when it has got non metals in it?

A

molecules

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24
Q

what type of bonding Is it called when non metals share electrons in a compound?

A

a covalent bond

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25
Q

just like elements are shown as symbols what are compounds shown as?

A

formulas

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26
Q

`what is the formula for carbon dioxide?

A

CO 2

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27
Q

what is the formula for ammonia?

A

NH 3

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28
Q

what is the formula for water?

A

H2O

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29
Q

what is the formula for sodium chloride?

A

NACL

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30
Q

what is the formula for carbon monoxide?

A

CO

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31
Q

what is the formula for hydrochloric acid?

A

HCL

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32
Q

what is the formula for calcium carbonate?

A

CACL2

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33
Q

what is the formula for sodium carbonate?

A

NA2CO3

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34
Q

what is the formula for sulphuric acid?

A

H2SO4

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35
Q

in a mixture there is no what?

A

chemical bond between the different parts of the mixture

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36
Q

how can mixtures be separated?

A

by physical methods

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37
Q

what happens during chromatography?

A

draw a little line of pencil then a dot of ink. place in water without the ink touching or it will dissolve the different inks will separate and move up the paper

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38
Q

what is filtration used for?

A

to separate solids from liquids

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39
Q

what two methods can separate soluble solids from solutions?

A

evaporation and crystallisation

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40
Q

what happens in evaporation?

A

heat the solution under a Bunsen burner until crystals start to form ( the solvent has evaporated) and keep heating until dry crystals have fully formed

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41
Q

what happens in crystallisation?

A

heat them the same as in evaporation however when crystals start to form stop heating the dish and leave it cool. Then filter the crystals out and leave them in a warm place to dry

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42
Q

what 4 steps separate rock salt?

A

grinding, dissolving, filtering and evaporation

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43
Q

what is simple distillation used for?

A

to separate a liquid from a solution

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44
Q

what happens in simple distillation?

A

the solution is heated and the part of the solution with the lowest boiling point evaporates, the vapour condenses and is collected

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45
Q

what is the problem with simple distillation ?

A

you can only separate things with very different boiling points because if the temperature is higher than the highest boiling point they will mix again

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46
Q

what is fractional distillation?

A

a more complicated type of distillation used when liquids have similar boiling points

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47
Q

in a fractional column where is the coolest and where is the hottest?

A

the coolest is at the top and the hottest Is at the bottom

48
Q

what happens to the liquid with the lowest boiling point in fractional distillation ?

A

it evaporates first

49
Q

what happens in fractional distillation when the temperature matches the boiling point of the different solutions?

A

it will reach the top of the column

50
Q

what happens to liquids with higher boiling points in fractional distillation?

A

they start to evaporate but will condense and run back down until the temperature is increased to its boiling point

51
Q

what did John Dalton describe atoms as ?

A

atoms where solid spheres and different spheres made up the different elements

52
Q

when did John Dalton come up with his theory?

A

at the start of the 19th century

53
Q

what did JJ Thompson conclude about atoms?

A

his measurements of charge and mass showed that an atom must contain even smaller, negatively charged particles- electrons

54
Q

when did JJ Thompson come up with his theory?

A

1897

55
Q

what was the sphere ideology replaced with?

A

the plum pudding model

56
Q

what does the plum pudding model show?

A

the atom as a ball of positive charge with electrons stuck in it

57
Q

who showed that the plum pudding model was wrong and when?

A

ernest Rutherford in 1909

58
Q

what did ernest ruthorford do?

A

scatter positively charged alpha particles at a thin sheet of gold

59
Q

what did ernest ruthorford expect from the ideas of the plum pudding model?

A

he expected the particles to pass straight through the sheet of gold or only be slightly deflected

60
Q

why did Rutherford expect this ?

A

because the plum pudding model explained that the positive charge was thought to be spread out in each atom

61
Q

what actually happened when Rutherford fired the particles at the sheet of gold?

A

some deflected more than expected and some deflected backwards

62
Q

what theory did Rutherford then come up with?

A

the nuclear model. any particles that came near the nucleus in the middle would be deflected otherwise they would pass through an empty space between the electrons

63
Q

what did Niels Bohr suggest?

A

he suggested that electrons were contained in shells

64
Q

what did James Chadwick discover?

A

evidence that there was neutral particles in the nucleus - neutrons

65
Q

how many electrons are aloud in the first shell and the rest?

A

2 in the first and 8 in the rest

66
Q

in the early 1800’s what were elements arranged in?

A

atomic mass

67
Q

what two ways did scientists categorise elements in the periodic table?

A

their physical/ chemical properties and their relative atomic mass

68
Q

what happened when they were arranged in order of atomic mass?

A

some were placed in the wrong group

69
Q

what did Mendeleev do in 1869?

A

he arranged the table in atomic mass but switched them if properties were similar, he also left gaps for undiscovered elements

70
Q

where are metals on the periodic table?

A

left

71
Q

where are non metals on the periodic table?

A

right

72
Q

what are vertical columns called in the periodic table?

A

groups

73
Q

what does the group number tell us?

A

how many electrons are in the outer shell

74
Q

what happens to reactivity as you go down the group?

A

reactions become more vigorous

75
Q

in group 7, what happens to reactivity as you go down?

A

it decreases

76
Q

what are the rows called in the periodic table?

A

periods

77
Q

what does the period tell us?

A

how many shells an element has got

78
Q

when metals react what do they form?

A

positively charged ions

79
Q

where are non metals found?

A

at the far right and top

80
Q

how do metals to the left react?

A

they don’t have many electrons to remove

81
Q

how do metals towards the bottom of the periodic table react?

A

the outer electrons are far away from the nucleus so the electrostatic attraction is weak

82
Q

what does it mean when there is a weak attraction to the nucleus?

A

not much energy is needed to remove the electrons and form positively charged ions

83
Q

why is it hard to form positively charged ions in non metals?

A

non metals tend to have lots of electrons to remove In order to get a full outer shell or there outer shell is close to the nucleus therefore there is a strong attraction

84
Q

what is it easier for non metals to do?

A

gain electrons and become negatively charged ions

85
Q

what is the bonds called between two metals?

A

metallic bonding

86
Q

all metals are strong but malleable, what does malleable mean?

A

they can be bent or hammered into shape

87
Q

do all metals have a high or low boiling and melting point ?

A

high

88
Q

what do transition metals normally good at being?

A

being catalysts

89
Q

what are group one elements known as ?

A

alkali metals

90
Q

what do alkali metals have to be stored in since they are very reactive?

A

oil

91
Q

what properties do the alkali metals have ?

A

they are soft with low density

92
Q

as the alkali metals go down what happens to their reactivity?

A

the reactivity increases

93
Q

why does the reactivity increase as you go down the alkali metals ?

A

the outer electron is more easily lost as the attraction between the nucleus and the electron decreases because the electron becomes further away the further down the group you go

94
Q

what do all alkali metals have regarding melting and boiling points ?

A

lower melting and boiling points

95
Q

what do alkali metals have a high of?

A

a high relative atomic mass

96
Q

what ions do the alkali metals form easily?

A

1+ ions

97
Q

what is produced when alkali metals react with water?

A

they produce metal hydroxides and hydrogen

98
Q

the amount of energy released from the alkali metals reacting does what as you go down the group?

A

increase

99
Q

what happens when group 1 metals react vigorously when heated in chlorine gas ?

A

they form metal chloride salts

100
Q

what happens when the alkali metals react with oxygen?

A

they from different types of metal oxide

101
Q

what happens when lithium reacts with oxygen?

A

lithium oxide

102
Q

what are the differences between transition metals and alkali metals?

A

group 1 metals are more reactive, less dense, hard and strong compared to transition metals and group 1 metals have lower boiling points

103
Q

what are the group 7 elements known as ?

A

the halogens

104
Q

what happens as you go down the group 7 halogens?

A

they become less reactive

105
Q

why does reactivity go down throughout the halogens ?

A

because its harder to gain an extra electron, because the outer shell is further away from the nucleus

106
Q

as you go down the halogens what happens to their melting and boiling points?

A

they get higher

107
Q

what happens to the relative atomic mas as you go down the halogens?

A

they get higher

108
Q

to achieve a full outer shells what do the halogens do?

A

they share electrons with other non metals via covalent bonding

109
Q

what do more reactive halogens do to less reactive ones?

A

displace them

110
Q

what are group 0?

A

the noble gases

111
Q

why don’t noble gases react with much at all?

A

they all already have a full outer shell

112
Q

noble gases are single atoms not bonded together, whats the name for this?

A

monatomic gases

113
Q

what are all elements in group 0 like at room temperature?

A

colourless gases

114
Q

are noble glasses flammable?

A

no

115
Q

what happens to the boiling point and relative atomic mass of the noble gases as you go down?

A

they get higher

116
Q

what is the increase in boiling point due to?

A

the increase in number of electrons leads to greater intermolecular forces that need to be overcome

117
Q

what order do the noble gases?

A

helium, neon, argon, krypton, xenon, radon

year 10 mock exam revision (26 decks)

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