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Chemistry IGCSE CIE Extended > Chapter 12 - The Periodic Table > Flashcards

Chapter 12 - The Periodic Table Flashcards

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1
Q

What is the purpose of the periodic table?

A

Its a way of classifying the elements

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2
Q

In what order is the periodic table arranged?

A

Shows elements in order of their proton number

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3
Q

What is PERIODICITY?

A

When elements with similar properties appear at regular intervals

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4
Q

What are the columns called

A

groups

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5
Q

What are the rows called?

A

Periods

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6
Q

What does the group number correlate to?

A

Same as the number of outer-shell electrons

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7
Q

What are the outer-shell electrons called?

A

valency electrons

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8
Q

Why are valency electrons important?

A

They dictate how an element behaves

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9
Q

Why do elements in the same group have similar reactions?

A

have the same number of valency electrons

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10
Q

Do group 0/8 elements react?

Why?

A

NO

  • have a very stable electron arrangement
  • are unreactive
  • full outer electron shell
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11
Q

What does the period of an element tell you?

A

Tells you the number of electron shells the atom has

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12
Q

What is the nucleon number?

A

Total number of particles in the nucleus

protons + neutrons

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13
Q

Group 1 different name

A

alkali metals

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14
Q

Group 2 different name

A

alkaline earth metals

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15
Q

Group 7 different name

A

halogens

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16
Q

Group 8/0 different name

A

noble gases

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17
Q

What percentage of the elements are metals?

A

over 80%

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18
Q

Why is hydrogen alone in the periodic table?

Properties

A
  • has 1 valency electron
  • forms a positive ion (H+)
  • similar to group 1 metals but it is A GAS
  • reacts like a non-metal
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19
Q

Revise the properties of metals and non-metals

A

yes

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20
Q

What are artificial elements and why can they not be found in nature?

A
  • elements made in a lab

- are radioactive and their atoms break down very quickly

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21
Q

list the group 1 metals

A

lithium, sodium, potassium, rubidium, caesium, francium

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22
Q

list the physical properties of group 1 metals

4

A
  • good conductors of heat and electricity
  • softer than most other metals (can cut with a knife)
  • low density (float on water) ctom
  • low melting and boiling points ctom
    ctom - compared to other metals
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23
Q

trends in softness g1

A

softness increases going down the group

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24
Q

trends in density g/cm3 g1

A

density increases going down the group

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25
Q

trends in melting point g1

A

mp decreases going down the group

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26
Q

trends in reactivity g1

A

reactivity increases going down the group

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27
Q

lithium reaction with water

A

floats and fizzes

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28
Q

sodium reaction with water

A

shoots across the water

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29
Q

potassium reaction with water

A

melts with the heat of the reaction, hydrogen catches fire producing lilac flame

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30
Q

Overall description of group 1 metals with water

A

Alkali metals react vigorously with water.

Hydrogen bubbles off, leaving solutions of their hydroxides, which are alkalis.

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31
Q

chemical equation of lithium/sodium with water

A

2Na + 2H20 –> 2NaOH + H2
2Li + 2H2O –> 2LiOH + H2
etc

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32
Q

Overall description of group 1 metals with chlorine

A

If you heat the 3 metals and plunge them into gas jars of chlorine, they burst into flames.
Burn brightly forming chlorides

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33
Q

Overall equation for group 1 metals with chlorine

A

2Li + Cl2 –> 2LiCl

2Na + Cl2 –> 2NaCl

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34
Q

Overall description of group 1 metals with oxygen

A

Burst into flames when heated and plunged into gas jars of oxygen
Form oxides

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35
Q

Are group 1 oxides acidic or alkaline

A

alkaline

- dissolve in water to form alkaline solutions

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36
Q

Why are group 1 metals the most reactive?

A
  • have only 1 valency electron
  • strong drive to react with other elements and compounds, in order to give up this electron
  • lose electron to form ions
37
Q

What compounds do g1 metals make?

A

IONIC compounds

38
Q

What charge do all the ions in group 1 have?

A

+1

39
Q

What colour are group 1 compounds?

What colour do they form when they dissolve?

A

white solids

colourless solutions when dissolved in water

40
Q

Why does reactivity increase going down group 1?

A
  • in reactions, group 1 atoms lose their outer electron to gain a stable outer shell
  • the more shells there are, the further the valence electron is from the positive nucleus - easier to lose
  • easier the valence electron is to lose, more reactive a metal will be
41
Q

List group 7 elements

A

fluorine, chlorine, bromine, iodine

42
Q

3 properties of halogens

A
  • form coloured gases
  • are poisonous
  • for diatomic molecules (containing 2 atoms)
43
Q

What colour is … in gaseous form?

  • fluorine
  • chlorine
  • bromine
  • iodine
A
  • pale yellow
  • green
  • red
  • purple
44
Q

Trend for colour for halogens

A

colour gets deeper going down the group

45
Q

Trend for denisty for halogens

A

density increases going down the group

46
Q

Trend for bp for halogens

A

the boiling point increases going down the group

47
Q

Trend for reactivty for halogens

A

reactivity DECREASES going down the group

48
Q

Overall reaction for halogens with metals

A

React to form halides

49
Q

Fluorine reaction with iron wool

A

Iron wool bursts into flames

- no heating required

50
Q

chlorine reaction with iron wool

A

hot iron wool glows brightly

51
Q

bromine reaction with iron wool

A

hot iron wool glows, less brightly

52
Q

iodine reaction with iron wool

A

hot iron wool shows a faint red glow

53
Q

Why are the halogens so reactive?

A
  • need just one more electron to reach a stable outer shell
  • strong drive to react with other elements or compounds to gain this electron
  • they accept electrons (w/metals) / share them (w/non-metals)
54
Q

Why does reactivity decreases going down group 7?

A
  • halogen atoms react to gain or share an electron
  • positive nucleus of the atom attracts the electron
  • more outer shells there are, further, the outer shell is from the nucleus
  • attracting an electron becomes difficult
55
Q

Overall rule for halogen reactions with halides

A

A halogen will displace a less reactive halogen from a solution of its halids
Cl2 + 2KBr –> 2KCl + Br2

56
Q

Group 8/0 list elements

A

helium, neon, argon, krypton, xenon

57
Q

properties of noble gases (5)

A
  • non-metals
  • colourless gasses
  • occur naturally in air
  • MONOATOMIC - exist as single atoms
  • unreactive
58
Q

Why are noble gases monoatomic and unreactive?

A

Their elements already have a stable outer shell

59
Q

Where do we get the noble gases from?

A

Fractional distillation of liquid air

- helium is obtained from natural gas (it’s an impurity)

60
Q

trend in atoms for group 8

A

atoms increase in size and mass going down the group

61
Q

trend in density for group 8

A

density of gas increases going down the group

62
Q

trend in boiling point for group 8

A

the boiling points increase going down the group

63
Q

What does the increase in boiling points show?

A

A sign of increasing attraction between atoms

- harder to separate them to form a gas

64
Q

What happens when a current is passed through noble gases at a low pressure?

A

They glow

65
Q

Uses for helium

A
  • used to fill balloons and airships

- won’t catch fire and lighter than air

66
Q

Uses for argon

A
  • used to provide an inert atmosphere
  • as a filler in tungsten light bulbs
  • to protect metals that are being welded
67
Q

Uses for neon

A
  • used in advertising signs
  • glows red
  • colour can be changed by mixing with other gases
68
Q

uses for krypton

A
  • used in lasers

e. g eye surgery / car headlamps

69
Q

Uses for xenon

A
  • gives a bright light with a blue tinge
  • used in lighthouse lamps
  • lights for hospital operating rooms
  • car headlamps
70
Q

What are the transition elements?

A

Block of 30 elements in the middle of the periodic table.

71
Q

Physical properties of transition metals (5)

A
  • hard, tough and strong
  • high melting points (mercury is an exception)
  • malleable, ductile
  • good conductors of heat and electricity
  • high density
72
Q

which metal is the best conductor?

A

silver

and then copper

73
Q

Chemical properties of transition metals (6)

A
  • much less reactive than group 1 metals
  • show no clear trend in reactivity
  • most transition elements form coloured compounds
  • most can form ions with different charges
  • form more than one compound with another element
  • most can form complex ions
74
Q

In general, do transition elements corrode easily?

A

No

- iron is an exception - it rusts easily

75
Q

What is the name for elements that form many ions with different charges?

A

They have a VARIABLE VALENCY

76
Q

How do you make salt of a transition element?

A

react their oxide/hydroxide with acids

their oxides are basic and react with acids to form salts

77
Q

What do the roman numerals in brackets tell you? e.g (II)

A
  • how many electrons the metal atom has lost

- OXIDATION STATE

78
Q

Uses of the transition elements? (4)

A
  • used in structures such as bridges, buildings, cars.
  • used in making alloys
  • used as conductors of heat and electricity e.g copper for electric wiring
  • most act as catalysts e.g iron is used in making ammonia
79
Q

What transition element is most commonly used in making structures?

A

Iron is most widely used usually in the form of alloys called steels

80
Q

what is an alloy?

A

Small amounts of other substances are mixed with a metal to improve its properties

81
Q

What is used to create stainless steel?

A

chromium and nickel

82
Q

Trends across the periodic table (left to right)

2

A
  • go from metals to non-metals

- mp and bp rise to the middle of the period (IV), then fall to very low values on the right

83
Q

What type of conductors are metalloids known as?

A

Semi-conductors

84
Q

What does valency mean?

A

The valency of an element is the number of electrons its atoms lose, gain or share, to form a compound

85
Q

What does the valency match?

A
  • number of valency electrons (up to group IV)

- matches the charge on the ion, where an element forms ions

86
Q

Rules for electron transfer for metals and non-metals

A

metals - lose their outer electrons

non-metals - gain or share electrons

87
Q

trends in reactivity for non/metals

A
  • reactivity
    decreases across metals
  • reactivity increases for non-metals
    across the periods
88
Q

Why does reactivity decrease for metals across the period?

A

The more electrons a metal atom needs to lose, the more difficult it is (must have enough energy to overcome the pull of the nucleus)

89
Q

Why does reactivity increase for non-metals across the period?
(except group 0)

A

The fewer electrons a non-metal needs to gain, the easier it is to attract them

Chemistry IGCSE CIE Extended (15 decks)

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