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Abi Science 2017 > The Periodic Table > Flashcards

The Periodic Table Flashcards

1
Q

What is the Periodic Table?

A

A collection of all known elements

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2
Q

What order is the Periodic Table arranged in?

A

Ascending atomic number from left to right

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3
Q

What are groups on the Periodic Table?

A

The vertical columns

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4
Q

What are periods on the Periodic Table?

A

The horizontal rows

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9
Q

How can the electron configuration of an element be determined?

A

By its position on the Periodic Table

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10
Q

What is the special name given to elements in group 1 (I)?

A

Alkali metals

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11
Q

What special name is given to elements in group 2 (II)?

A

Alkaline earth metals

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12
Q

What special name is given to elements in group 17 (VII)?

A

Halogens

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13
Q

What is the special name given to elements in group 18 (VIII)?

A

Noble gases

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14
Q

What is a diatomic element?

A

An element which, in its elemental state, bonds to itself

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15
Q

Which elements are diatomic?

A

The halogens
Nitrogen
Oxygen
Hydrogen

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16
Q

What kind of ions do metals usually form?

A

They generally lose electrons easily

So they form positive ions

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17
Q

How many valence electrons do metals have?

A

Generally they have few valence electrons

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18
Q

Where are metals found?

A

Left hand side of the Periodic Table (except H)

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19
Q

Where are non-metals found?

A

On the right hand side of the periodic table

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20
Q

How many valence lecterns do non-metals have?

A

Generally, they have many valence electrons

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21
Q

Which elements are stable?

A

The noble gases

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22
Q

Why are noble gases stable?

A

All of their energy levels are filled

They do not have any unpaired electrons

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23
Q

What do all atoms try to do?

A

Become stable

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24
Q

How do atoms attempt to become stable?

A

They try to match the electron configuration of the stable elements
i.e They try to have all of their energy levels filled

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25
Q

How do atoms make all of their electrons filled?

A

By gaining or losing electrons (forming ions)

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26
Q

What charge will elements in group I try to form?

A

A positive charge of one

i.e they will try to lose an electron

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27
Q

What charge will elements in group II try to form?

A

A positive charge of two

i.e they will try to lose two electrons

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28
Q

What charge will elements in group III try to form?

A

A positive charge of three

i.e. They will try to lose three electrons

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29
Q

What kind of charge will elements in group IV try to form?

A

Either positive or negative charges of four, depending

i.e they will either try to lose or gain four electrons

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30
Q

What kind of charge will elements in group V try to form?

A

A negative charge of three

i.e They will try to gain three electrons

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31
Q

What kind of charge will elements in group VI try to form?

A

A negative charge of two

i.e they will try to gain two electrons

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32
Q

What kind of charge will elements in group VII try to form?

A

A negative charge of one

i.e they will try to gain one electron

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33
Q

What causes the gradually changing properties of elements in a given period?

A

The gradually changing valence electron configuration

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34
Q

What is atomic radius?

A

The distance from the centre of the nucleus to the outermost electron

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35
Q

What happens to atomic radius as you move from the left of a period to the right?

A

It decreases

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36
Q

Why does atomic radius decrease as you move from left right on the Periodic Table?

A

There are more protons
The attractive force on the lecterns is also greater
The electrons move closer to the nucleus
The radius decreases

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37
Q

What happens to atomic radius as you move down the groups on the Periodic Table?

A

It increases

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38
Q

Why does atomic radius increase as you move down the groups on the Periodic Table?

A

Energy levels are added

The electrons are therefore further away from the nucleus

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39
Q

What is density?

A

Mass per unit volume

How heavy something is in relation to the amount of space it occupies

40
Q

Are metals or non-metals generally more dense?

A

Metals

41
Q

What happens to the density of metals as you move from left to right on the Periodic Table?

A

Increases

42
Q

In which groups does moving from left to right increase melting and boiling points?

A

Groups 1-14

43
Q

What is the general melting and boiling point for elements in groups 15-18?

A

Low

44
Q

As you move down in group 1 and 2, what happens to the melting and boiling points?

A

Decrease

45
Q

As you move down in group 17 and 18, what happens to the melting and boiling points?

A

Increase

46
Q

What does ionisation energy concern?

A

The formation of cations

47
Q

What is ionisation energy?

A

The energy required to remove an electron from a single atom in the gaseous phase

48
Q

What is first ionisation energy?

A

The energy required to remove one electron

49
Q

What is second ionisation energy?

A

The energy required to remove the second electron

50
Q

What happens to first ionisation energy as you move from left to right?

A

It increases

51
Q

What happens to first ionisation energy as you move down a group?

A

Decreases

52
Q

Why does first ionisation energy increase as you move across a period?

A

More protons means a greater force of attraction on the electrons
Need more energy to overcome this force

53
Q

Why does first ionisation energy decrease as you move down a group?

A

More energy levels
Force of attraction is weaker
Less energy required to break it

54
Q

What does electrons affinity concern?

A

The formation of anions

55
Q

What is electron affinity?

A

The amount of energy liberated (released) when an electron is added to a single atom in the gaseous phase

56
Q

What happens to electron affinity when you move across a period?

A

Increases

57
Q

What happens to electron affinity when you move down a group?

A

Decreases

58
Q

Why does electron affinity increase as you move across a period?

A

The attraction for an electron is greater

59
Q

Why does electron affinity decrease when you move down a group?

A

The attraction for an electron decreases

60
Q

What does electron negativity concern?

A

The formation of shared electron pairs (covalent bonds)

61
Q

What is electron negativity?

A

The attractive force that an atom has on a shared electron pair

62
Q

How is electronegativity measured?

A

On a scale of 1-4

63
Q

What happens to electronegativity as you move across a period?

A

It increases

64
Q

What happens to electronegativity as you move down a group?

A

It decreases

65
Q

Why does electronegativity increase as you move across a period?

A

More protons

Greater force can be exerted on the electron pair

66
Q

Why does electronegativity decrease when you move down a group?

A

Extra energy level
The electron pair is further from the nucleus
Can’t exert as great a force

67
Q

Which element has the greatest electronegativity?

A

Fluorine

68
Q

Why does Fluorine have the greatest electronegativity?

A

It has the most protons in its period, but the fewest energy levels in its group

69
Q

Which group is the most reactive?

A

Group I

Alkali Metals

70
Q

Why is Group I the most reactive?

A

All the elements in this group only have one valence electron
It is eager to give up this electron, so chemical reactions happen easily

71
Q

Where are alkali metals naturally found?

A

In compounds

72
Q

How are the elemental forms of alkali metals stored?

A

In inert liquids, to prevent reactions from occurring

73
Q

How do alkali metals react with cold water?

A

They produce hydrogen and a hydroxide

74
Q

What happens to the reactivity of group I as you move down the group?

A

Increases

75
Q

What does the group number of an element tell us?

A

The number of valence electrons an element has (except He)

76
Q

Which two groups have their valence electrons in s-Orbitals?

A

I and II

77
Q

Which groups have their valence electrons in p-Orbitals?

A

III to VIII (except He)

78
Q

What tells us the number of energy levels that an element has?

A

The period number

79
Q

What do the alkali metals look like?

A

Soft and grey

80
Q

What are the alkali earth metals like?

A

Very similar to alkali metals

Just slightly less reactive

81
Q

What do alkali earth metals do when in contact with cold water?

A

Except for Be, they form a hydroxide and hydrogen

82
Q

What do alkali earth metals look like?

A

Apart form Be, they are light grey and soft

83
Q

What is the reactivity of the halogens like?

A

High

84
Q

Why is the reactivity of halogens high?

A

They only need one electron to reach the ‘stable’ state

85
Q

What do the halogens form when reacting with metals?

A

Salts

86
Q

What happens to the reactivity of the halogens as you move down the group?

A

Decreases

87
Q

Why does the reactivity of the halogens decrease as you move down the group?

A

The atomic radius increase

The force of attraction on the electrons decreases

88
Q

What are the melting points of the halogens like?

A

Low

89
Q

What is the reactivity of group 18 like?

A

Very low

90
Q

Why are the elements in group 18 called the noble gases?

A

They don’t tend to bond with anything

They are all gases at room temperature

91
Q

How are the charges of atoms shown?

A

With a superscript number in the top right hand corner of the chemical symbol
The number of the charge is shown, as well as the type (+ / -)

Abi Science 2017 (18 decks)

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