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Abi Science 2017 > The Periodic Table > Flashcards

The Periodic Table Flashcards

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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
What kind of charge will elements in group IV try to form?
Either positive or negative charges of four, depending | i.e they will either try to lose or gain four electrons
30
What kind of charge will elements in group V try to form?
A negative charge of three | i.e They will try to gain three electrons
31
What kind of charge will elements in group VI try to form?
A negative charge of two | i.e they will try to gain two electrons
32
What kind of charge will elements in group VII try to form?
A negative charge of one | i.e they will try to gain one electron
33
What causes the gradually changing properties of elements in a given period?
The gradually changing valence electron configuration
34
What is atomic radius?
The distance from the centre of the nucleus to the outermost electron
35
What happens to atomic radius as you move from the left of a period to the right?
It decreases
36
Why does atomic radius decrease as you move from left right on the Periodic Table?
There are more protons The attractive force on the lecterns is also greater The electrons move closer to the nucleus The radius decreases
37
What happens to atomic radius as you move down the groups on the Periodic Table?
It increases
38
Why does atomic radius increase as you move down the groups on the Periodic Table?
Energy levels are added | The electrons are therefore further away from the nucleus
39
What is density?
Mass per unit volume | How heavy something is in relation to the amount of space it occupies
40
Are metals or non-metals generally more dense?
Metals
41
What happens to the density of metals as you move from left to right on the Periodic Table?
Increases
42
In which groups does moving from left to right increase melting and boiling points?
Groups 1-14
43
What is the general melting and boiling point for elements in groups 15-18?
Low
44
As you move down in group 1 and 2, what happens to the melting and boiling points?
Decrease
45
As you move down in group 17 and 18, what happens to the melting and boiling points?
Increase
46
What does ionisation energy concern?
The formation of cations
47
What is ionisation energy?
The energy required to remove an electron from a single atom in the gaseous phase
48
What is first ionisation energy?
The energy required to remove one electron
49
What is second ionisation energy?
The energy required to remove the second electron
50
What happens to first ionisation energy as you move from left to right?
It increases
51
What happens to first ionisation energy as you move down a group?
Decreases
52
Why does first ionisation energy increase as you move across a period?
More protons means a greater force of attraction on the electrons Need more energy to overcome this force
53
Why does first ionisation energy decrease as you move down a group?
More energy levels Force of attraction is weaker Less energy required to break it
54
What does electrons affinity concern?
The formation of anions
55
What is electron affinity?
The amount of energy liberated (released) when an electron is added to a single atom in the gaseous phase
56
What happens to electron affinity when you move across a period?
Increases
57
What happens to electron affinity when you move down a group?
Decreases
58
Why does electron affinity increase as you move across a period?
The attraction for an electron is greater
59
Why does electron affinity decrease when you move down a group?
The attraction for an electron decreases
60
What does electron negativity concern?
The formation of shared electron pairs (covalent bonds)
61
What is electron negativity?
The attractive force that an atom has on a shared electron pair
62
How is electronegativity measured?
On a scale of 1-4
63
What happens to electronegativity as you move across a period?
It increases
64
What happens to electronegativity as you move down a group?
It decreases
65
Why does electronegativity increase as you move across a period?
More protons | Greater force can be exerted on the electron pair
66
Why does electronegativity decrease when you move down a group?
Extra energy level The electron pair is further from the nucleus Can't exert as great a force
67
Which element has the greatest electronegativity?
Fluorine
68
Why does Fluorine have the greatest electronegativity?
It has the most protons in its period, but the fewest energy levels in its group
69
Which group is the most reactive?
Group I | Alkali Metals
70
Why is Group I the most reactive?
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
Where are alkali metals naturally found?
In compounds
72
How are the elemental forms of alkali metals stored?
In inert liquids, to prevent reactions from occurring
73
How do alkali metals react with cold water?
They produce hydrogen and a hydroxide
74
What happens to the reactivity of group I as you move down the group?
Increases
75
What does the group number of an element tell us?
The number of valence electrons an element has (except He)
76
Which two groups have their valence electrons in s-Orbitals?
I and II
77
Which groups have their valence electrons in p-Orbitals?
III to VIII (except He)
78
What tells us the number of energy levels that an element has?
The period number
79
What do the alkali metals look like?
Soft and grey
80
What are the alkali earth metals like?
Very similar to alkali metals | Just slightly less reactive
81
What do alkali earth metals do when in contact with cold water?
Except for Be, they form a hydroxide and hydrogen
82
What do alkali earth metals look like?
Apart form Be, they are light grey and soft
83
What is the reactivity of the halogens like?
High
84
Why is the reactivity of halogens high?
They only need one electron to reach the 'stable' state
85
What do the halogens form when reacting with metals?
Salts
86
What happens to the reactivity of the halogens as you move down the group?
Decreases
87
Why does the reactivity of the halogens decrease as you move down the group?
The atomic radius increase | The force of attraction on the electrons decreases
88
What are the melting points of the halogens like?
Low
89
What is the reactivity of group 18 like?
Very low
90
Why are the elements in group 18 called the noble gases?
They don't tend to bond with anything | They are all gases at room temperature
91
How are the charges of atoms shown?
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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