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GCSE Chemistry > Groups In The Periodic Table > Flashcards

Groups In The Periodic Table Flashcards

1
Q

What are the names and symbols of all the metals in group 1?

A

Lithium Li
Sodium Na
Potassium K
Rubidium Rb
Caesium Cs
Francium Fr

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2
Q

What is the appearance of lithium

A

dark grey solid

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3
Q

What is the appearance of sodium

A

pale grey solid

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4
Q

What is the appearance of potassium

A

dark grey solid

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5
Q

What happens to lithium when freshly cut

A

shiny

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6
Q

What happens to sodium when freshly cut

A

shiny

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7
Q

What happens to potassium when freshly cut

A

shiny

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8
Q

How hard is lithium to cut

A

it can be cut but is a bit tough

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9
Q

How hard is sodium to cut

A

easier to cut than lithium

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10
Q

How hard is potassium to cut

A

easier to cut than sodium

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11
Q

Why are group 1 metals stored in oil

A

to stop them reacting with oxygen in the air

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12
Q

Order of hardness of lithium

A

sodium

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13
Q

Observations when lithium reacts with water

A

effervescence

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14
Q

Observations when sodium reacts with water

A

effervescence

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15
Q

Observations when potassium reacts with water

A

effervescence

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16
Q

Observation when gas from lithium reaction is tested with a lit splint

A

a squeaky pop is heard

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17
Q

Observation when gas from sodium reaction is tested with a lit splint

A

a squeaky pop is heard

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18
Q

Observation when gas from potassium reaction is tested with a lit splint

A

a squeaky pop is heard

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19
Q

General equation for Group 1 metal reaction with water

A

metal + water → metal hydroxide + hydrogen

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20
Q

Word equation for lithium reaction with water

A

lithium + water → lithium hydroxide + hydrogen

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21
Q

Balanced symbol equation for lithium reaction with water

A

2Li(s) + 2H₂O(l) → 2LiOH(aq) + H₂(g)

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22
Q

Word equation for sodium reaction with water

A

sodium + water → sodium hydroxide + hydrogen

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23
Q

Balanced symbol equation for sodium reaction with water

A

2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g)

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24
Q

Word equation for potassium reaction with water

A

potassium + water → potassium hydroxide + hydrogen

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25
Q

Balanced symbol equation for potassium reaction with water

A

2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g)

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26
Q

Order of reactivity of lithium

A

sodium

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27
Q

Trend in reactivity as you go down Group 1

A

reactivity increases

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28
Q

Reason for increased reactivity down Group 1

A

outer electron is further from the nucleus and more easily lost

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29
Q

Will rubidium and cesium be more reactive or less reactive than potassium

A

more reactive

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30
Q

Why are Group 1 metals called alkali metals

A

they form alkaline solutions in water

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31
Q

What does “homonuclear” mean?

A

Molecules with the same type of atom.

32
Q

What does “diatomic” mean?

A

A molecule made up of two atoms.

33
Q

What is the definition of a molecule?

A

Two or more non-metal atoms covalently bonded.

34
Q

What is the appearance of fluorine at room temperature?

A

Yellow gas.

35
Q

What is the appearance of chlorine at room temperature?

A

Green gas.

36
Q

What is the appearance of bromine at room temperature?

A

Brown liquid.

37
Q

What is the appearance of iodine at room temperature?

A

Dark grey solid.

38
Q

What is the predicted appearance of astatine?

A

Dark grey solid.

39
Q

What is the trend in boiling points of halogens?

A

Boiling points increase as you go down the group.

40
Q

Why do boiling points increase in halogens?

A

Molecules get larger

41
Q

What is the trend in reactivity of halogens?

A

Reactivity decreases as you go down the group.

42
Q

Why does reactivity decrease in halogens?

A

Electrons are further from the nucleus

43
Q

What is the definition of a compound?

A

A substance with two or more different types of atoms chemically bonded.

44
Q

What happens when chlorine reacts with iron wool?

A

Iron glows brightly and reacts vigorously.

45
Q

What happens when bromine reacts with iron wool?

A

Iron glows and produces brown vapors

46
Q

What happens when iodine reacts with iron wool?

A

Least vigorous reaction

47
Q

What is the order of reactivity of halogens?

A

Chlorine > Bromine > Iodine.

48
Q

Why does reactivity decrease down the halogen group?

A

The outer electron shell is further from the nucleus

49
Q

What does the reaction between iron and chlorine produce?

A

Iron(III) chloride (FeCl₃).

50
Q

What does the reaction between iron and bromine produce?

A

Iron(III) bromide (FeBr₃).

51
Q

What does the reaction between iron and iodine produce?

A

Iron(III) iodide (FeI₃).

52
Q

What is the balanced equation for iron and chlorine?

A

2Fe(s) + 3Cl₂(g) → 2FeCl₃(s).

53
Q

What is the balanced equation for iron and bromine?

A

2Fe(s) + 3Br₂(g) → 2FeBr₃(s).

54
Q

What is the balanced equation for iron and iodine?

A

2Fe(s) + 3I₂(g) → 2FeI₃(s).

55
Q

What happens when fluorine reacts with hydrogen?

A

Fluorine and hydrogen produce hydrogen fluoride.

56
Q

What is the word equation for fluorine and hydrogen?

A

Hydrogen + Fluorine → Hydrogen fluoride.

57
Q

What is the balanced equation for fluorine and hydrogen?

A

H₂(g) + F₂(g) → 2HF(g).

58
Q

What does the dot-and-cross diagram for hydrogen fluoride look like?

A

Fluorine shares one pair of electrons with hydrogen in a single covalent bond.

59
Q

How does fluorine’s reactivity compare to chlorine?

A

Fluorine is more reactive because it has fewer electron shells.

60
Q

Why are Group 1 metals more reactive than Group 7 elements?

A

Group 1 elements lose electrons easily

61
Q

What is the reactivity trend in Group 1 and Group 7?

A

Reactivity increases down Group 1 but decreases down Group 7.

62
Q

Why does reactivity increase in Group 1?

A

The outer electron is further from the nucleus and is lost more easily.

63
Q

Why does reactivity decrease in Group 7?

A

Increased distance from the nucleus makes it harder to attract electrons.

64
Q

How does reactivity change down Groups 1 and 2?

A

Reactivity increases as you go down the groups.

65
Q

Why does reactivity increase down Groups 1 and 2?

A

Outer electrons are further from the nucleus due to more electron shells

66
Q

How does reactivity change down Group 7?

A

Reactivity decreases as you go down the group.

67
Q

Why does reactivity decrease down Group 7?

A

The number of electron shells increases

68
Q

What happens to the outer electron in Group 7 elements as you go down?

A

The outer electron is further from the nucleus and experiences weaker attraction

69
Q

Where are the noble gases located on the periodic table?

A

In Group 0.

70
Q

Why are noble gases unreactive?

A

They have full outer electron shells

71
Q

Why are noble gases placed in Group 0 instead of Group 8?

A

Helium has only two electrons

72
Q

What are the uses of helium?

A

Helium is used as a coolant

73
Q

What are the uses of neon?

A

Neon is used in vacuum tubes and neon signs.

74
Q

What are the uses of argon?

A

Argon is used in lightbulbs to prevent oxidation of the filament.

75
Q

What are the uses of krypton?

A

Krypton is used in bright lights like airport runway lamps and lasers.

76
Q

How does the reactivity of Group 0 change down the group?

A

Reactivity slightly increases as the atomic size increases

77
Q

Why do noble gases not readily gain/lose/share electrons?

A

Their outer shells are full, making them stable and unreactive.

GCSE Chemistry (8 decks)

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