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Chemistry GCSE AQA > Topic 1 - Atomic Structure And The Periodic Table > Flashcards

Topic 1 - Atomic Structure And The Periodic Table Flashcards

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1
Q

What are all substances made of?

A

Atoms

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2
Q

What is the radius of an atom?

A

0.1 manometers

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3
Q

What type or particles are in the nucleus?

A

Protons and neutrons

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4
Q

What type of particles are found in shells outside of the nucleus?

A

Electrons

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5
Q

What is the charge of an electron?

A

Negative

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6
Q

What is the charge of a proton?

A

Positive

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7
Q

What is the charge of a neutron?

A

None

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8
Q

What is the relative mass of an electron?

A

0

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9
Q

What is the relative mass of a proton?

A

1

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10
Q

What is the relative mass of a neutron?

A

1

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11
Q

The number of protons in an atom is equivalent to what?

A

The number of electrons

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12
Q

What is the overall charge of an atom?

A

Neutral

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13
Q

What does the atomic number of a nuclear symbol tell you?

A

How many protons (and therefore electrons) an atom has

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14
Q

What does the mass number of a nuclear symbol tell you?

A

The relative atomic mass of the atom

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15
Q

How do you figure out the number of electrons from a nuclear symbol?

A

Mass number - atomic number

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16
Q

What is an element?

A

A substance made up of atoms that are all the same

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17
Q

What determines what type of atom and atom is?

A

The number of protons

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18
Q

What are isotopes?

A

Different forms of the same element with just a different number of neutrons

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19
Q

Atoms and their corresponding isotopes have the same _____ number.

A

Atomic

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20
Q

Atoms and there corresponding isotopes have different _____ numbers.

A

Mass

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21
Q

What is the relative atomic mass of an element?

A

How much that element weighs depending on the types of isotopes it contains

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22
Q

Relative atomic mass of an element =

A

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

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23
Q

What is a compound?

A

A mix of elements

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24
Q

How are compounds formed?

A

When elements react

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25
Q

When stones combine to form compounds, how are they held together?

A

Chemical bonds

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26
Q

What happens to electrons when bonds are made?

A

They are given, taken or shared

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27
Q

A compound of a metal and a non-metal will form what type of bonds?

A

Ionic bonding

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28
Q

What happens to metals in ionic bonding?

A

They lose electrons and become positive ions

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29
Q

What happens to non-metals in ionic bonding?

A

They gain electrons to become negative ions

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30
Q

A compound of non-metals will form what kind of bonds?

A

Atoms share electrons

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31
Q

Are properties of compounds usually similar or different to the elements from which they came from?

A

No

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32
Q

How can we represent compounds?

A

With formulas

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33
Q

If a symbol has a small number after and slightly below it, what does that mean?

A

There are that many of that specific element in the compound proportionally.

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34
Q

If a formula has a large number before it, what does that mean?

A

You would work out the smaller numbers first. Then double all the elements that are listed in the formula

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35
Q

What does it mean if there is a small number after brackets?

A

Multiply all the elements within the brackets by that number

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36
Q

What is the formula of ammonia?

A

NH3

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37
Q

What is the formula of sulphuric acid?

A

H2SO4

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38
Q

What are the two types of chemical equations?

A

Word and symbol

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39
Q

What are the molecules on the left hand side of an equation called?

A

Reactants

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40
Q

What are the molecules on the right hand side of an equation called?

A

Products

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41
Q

What do you have to do to symbol equations?

A

Balance them

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42
Q

What are you allowed to add to an equation to balance it?

A

Big numbers in front of formulas

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43
Q

What is the difference between a compound and a mixture?

A

Mixtures have no chemical bonds

44
Q

What is the most common mixture?

A

Air

45
Q

Do mixtures have the same properties of the elements they contain?

A

Yes

46
Q

Who created a theory of atomic structure in the early 19th century?

A

John Dalton

47
Q

What was John Dalton’s theory?

A

That atoms were solid spheres, and different spheres made different elements

48
Q

Who created a theory of atomic structure in 1897?

A

JJ Tomson

49
Q

What was JJ Thomson’s theory?

A

The plum pudding model: atoms were balls of positive charge containing negative electrons

50
Q

What did Rutherford prove?

A

That the plum pudding model was wrong

51
Q

What was Rutherford’s experiment?

A

Firing positively charged alpha particles at a thin sheet of gold foil

52
Q

What results was Rutherford expecting based on the plum pudding model?

A

Particles to pass straight through with some rare slight deflection

53
Q

What results did Rutherford get?

A

Most particles passed through, but a lot were deflected more than expected and a few even deflected backwards

54
Q

What was Rutherford’s theory of atomic structure?

A

In the centre of an atom was a tiny positive nucleus. Around this was a cloud of electrons and a lot of empty space.

55
Q

What alteration did Bohr make to Rutherford’s atomic structure?

A

He realised electrons had to be fixed else they’d be attracted to the nucleus, so he proposed they were in fixed shells a certain distance from the nucleus

56
Q

What did Rutherford later prove about atomic structure?

A

The nucleus could be divided into smaller, positive particles: protons

57
Q

What did James Chadwick prove about the atomic structure?

A

The nucleus also contained neutral particles: neutrons

58
Q

Which shells are filled first in atoms?

A

Those closest to the nucleus

59
Q

How many electron fit into the first shell?

A

2

60
Q

How many electron fit into the 2nd shell onwards?

A

8

61
Q

How many electrons do atoms want in their outermost shells?

A

The most possible, 2 or normally 8

62
Q

Which elements have full outer shells?

A

The noble gases

63
Q

How were elements originally arranged?

A

By atomic mass

64
Q

What did Dmitri Mendeleev do?

A

Left gaps, predicted elements and swapped elements around depending on their properties

65
Q

How are elements organised in the modern periodic table?

A

Atomic number

66
Q

Columns of elements have similar properties, what are they called?

A

Groups

67
Q

What does the group number tell you about an atom’s electronic structure?

A

How many electrons are in the outer shell

68
Q

Each new row means another full shell in the atom, what are these rows called?

A

Periods

69
Q

Which side of the periodic table do metals lie on?

A

Left

70
Q

Which side of the periodic table do non-metals lie?

A

Right

71
Q

What type of ions do metals form?

A

Positive

72
Q

What type of ions do non-metals typically form?

A

Negative

73
Q

Why do atoms react?

A

To form full outer shells

74
Q

Why do metals form positive ions?

A

The number of electrons in their outer shell makes it easier to lose than gain. They are lower in the table so their outer shells are further from the nucleus and have weaker forces of attraction.

75
Q

Why do non-metals form negative ions?

A

The number of electrons in their outer shells make it easier to gain than lose. They are higher in the table so their outer shells are closer to the nucleus and have stronger forces of attraction

76
Q

A compound of metals will form what type of bonds?

A

Metallic

77
Q

What are four main properties of metals?

A

Strong, malleable, conductive, high melting and boiling points

78
Q

What are five main properties of non-metals?

A

Brittle, not always solids at room temp, full, not conductive, lower densities

79
Q

What are transition metals?

A

Typical metals, found between groups 2 and 3

80
Q

What are the three specific properties found in transition metals?

A

More than one ion, coloured, good catalysts

81
Q

What are Group 1 metals known as?

A

Alkali metals

82
Q

What are the first three alkali metals?

A

Lithium, sodium, potassium

83
Q

How many electrons do alkali metals have in their outer shells?

A

1

84
Q

Do alkali metals increase reactivity going up or down the column and why?

A

Down, because there are more shells therefore weaker forces of attraction therefore the 1 outer electron is more easily lost

85
Q

Going down the column, do alkali metals’ MP and BP increase or decrease?

A

Decrease

86
Q

How do alkali metals react with water?

A

Vigorously, producing hydrogen gas and sometimes enough energy to ignite the hydrogen gas

87
Q

How do alkali metals react with chlorine?

A

Vigorously, producing metal chloride salts

88
Q

How do alkali metals react with oxygen?

A

Producing metal oxide

89
Q

What are Group 7 elements also known as?

A

Halogens

90
Q

What are the first four halogens?

A

Fluorine, chlorine, bromine, iodine

91
Q

What does fluorine look like?

A

Yellow gas

92
Q

What does chlorine look like?

A

Green gas

93
Q

What does bromine look like?

A

Red-brown liquid

94
Q

What does iodine look like?

A

Grey solid or purple gas

95
Q

What do all the halogen molecules do?

A

Pair up

96
Q

What happens to reactivity as you go down the halogen column and why?

A

Decreases, because the outer shell gets further from the nucleus therefore the forces of attraction are weaker therefore it’s harder to gain an electron.

97
Q

How many electrons do the halogens have in their outer shells?

A

7

98
Q

What types of bonding can halogens do?

A

Covalent and ionic

99
Q

What happens when a halogen salt reacts with a more reactive halogen?

A

The more reactive halogen will displace the other

100
Q

What are Group 0 elements also known as?

A

Noble gases

101
Q

What are the first three noble gases?

A

Helium, neon, argon

102
Q

How many electrons do noble gases have on their outer shells?

A

8, or 2 in helium’s case

103
Q

What are they called because of their reactivity?

A

Inert - barely react with anything

104
Q

What do all noble gases look like?

A

Colourless gases

105
Q

Are noble gases flammable?

A

No

106
Q

Do the BPs and MPs increase or decrease going down the column?

A

Increase

Chemistry GCSE AQA (2 decks)

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