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GCSE - Chemistry > Topic 6 - Groups In Periodic Table > Flashcards

Topic 6 - Groups In Periodic Table Flashcards

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1
Q

How are elements arranged in the periodic table?

A

Ordered by increasing atomic number
Elements in same group(column) = same no of outer shell electrons
Elements in same period(row) = same no of electron shells

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2
Q

How many electrons are in the outer shell of a group 1 element?

A

1

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3
Q

Why do elements in the same group have similar chemical properties?

A

Have same no of electrons in outer shell

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4
Q

What group of the periodic table are the alkali metals?

A

Group 1

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5
Q

List 2 properties of alkali metals

A

Relatively low melting pts

Soft

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6
Q

Why are group 1 elements called the alkali metals?

A

They react with water to form alkaline solutions (pH bigger than 7)

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7
Q

What are the products of the reaction between lithium and water?

A

Lithium hydroxide and hydrogen

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8
Q

Write a balanced symbol equation for the reaction of sodium with water

A

2Na + 2H₂O -> 2NaOH + H₂

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9
Q

Why should alkali metals be stored in oil?

A

To prevent them reacting with water vapour and oxygen in the air

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10
Q

What would be observed when lithium reacts with water?

A

Slowest reaction of alkali metals
Bubbles of hydrogen produced
Doesn’t melt (highest melting pt of alkali metals)

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11
Q

What would be observed when sodium reacts with water?

A

Faster reaction than lithium
Floats on surface (less dense than water)
Bubbles of hydrogen produced - cause sodium to whizz around surface
Melts as enough energy is given out to meet melting pt

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12
Q

What would be observed when potassium reacts with water?

A

More violent reaction than sodium
Bubbles of hydrogen produced - cause potassium to whizz round surface
Melts into shiny ball
Burns with lilac flame

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13
Q

What is the order of reactivity of the first 3 alkali metals with water?

A

Lithium (least)
Sodium
Potassium (most)

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14
Q

Using the reactions of the first 3 alkali metals with water, predict the reactivity trend down group 1

A

Reactivity increases down group 1

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15
Q

Why does reactivity increase down group 1?

A

No of electron shells increases down the group so there is more electron sheilding.
Is weaker attraction between + nucleus and outer electron shell.
Means is easier to remove outer shell electron to form + metal ion

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16
Q

Which group 1 element would you expect to react most violently with water?

A

Reactivity increases down the group so francium will react most violently with water

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17
Q

What group are the halogens in? Why?

A

Group 7 - they have 7 outer shell electrons

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18
Q

What is the colour and state of chlorine at room temp?

A

Pale green gas

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19
Q

What is the colour and state of bromine at room temp?

A

Red-brown liquid

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20
Q

What is the colour and state of iodine at room temp?

A

Black solid

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21
Q

Why are the halogens at different states at room temp? What is the trend down the group?

A

They have different melting and boiling pts.

As you go down the group, they increase

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22
Q

What state would you expect the halogens flourine and astatine to be at room temp?

A

Flourine is above chlorine so should have a boiling pt lower than it. Means it would be a gas at room temp.
Astatine is below iodine in group 7 so should have a higher melting pt. Can predict that is would be a solid at room temp.

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23
Q

Why does melting and boiling pt increase down group 7?

A

Molecules get bigger down the group - more intermolecular forces to overcome during melting/boiling - more energy required

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24
Q

What is the chemical test for chlorine?

A

Damp litmus paper placed into test tube of gas

If chlorine present, litmus paper will turn red then white die to bleaching effect of chlorine

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25
Q

Halogens are diatomic. What does this mean?

A

They form molecules consisting of 2 atoms

Cl₂ Br₂

26
Q

What charge does a halide ion carry? Why?

A

-1

They gain one electron to have a stable electron configuration

27
Q

What is produced when a halogen reacts with a metal?

A

Metal halide salt

28
Q

Write a balanced symbol equation for the reaction between bromine and sodium

A

Br₂ + 2Na -> 2NaBr

29
Q

Write a balanced symbol equation for the reaction between chlorine and calcium

A

Cl₂ + Ca -> CaCl₂

30
Q

Predict the product of the reaction between magnesium and fluorine

A

Magnesium fluoride (MgF₂)

31
Q

Write a work equation for the reaction between iodine and potassium

A

Iodine + potassium -> potassium iodide

32
Q

Describe the trend in reactivity of the halogens. How does this affect the rate of reaction?

A

Reactivity decreases down group 7

Rate of reaction decreases down group 7

33
Q

What is formed when hydrogen reacts with a halogen?

A

Hydorgen halides

HCl, HBr

34
Q

Chlorine reacts with hydrogen in the presence of sunlight but bromine requires a flame. Why?

A

Reactivity decreases down the group so bromine requires more energy for the reaction to occur

35
Q

What is formed when a hydrogen halide dissolves in water?

A

An acidic solution. Hydrogen ions dissociate, making the solution acidic

36
Q

Write a balanced symbol equation for the reaction between hydrogen and chlorine

A

H ₂ + Cl ₂ -> 2HCl

37
Q

Predict the product of the reaction between hydrogen and fluorine

A

Hydrogen fluoride

38
Q

When does a halogen displacement reaction occur?

A

When a more reactive halogen displaces a less reactive halogen from an aqueous solution of its halide

39
Q

Why will halogen A only be displaced by halogen B if B is above A in group 7?

A

The more reactive halogen (B) will displace the less reactive one to become part of the ionic compound. Reactivity increases as you go up the group so B must be higher to be more reactive than A

40
Q

Which halogens can chlorine displace from an aqueous ionic solution?

A

Chlorine can displace any halogens below it in group 7. It will displace iodine and bromine.

41
Q

Which halogens cant be displaced from an aqueous ionic solution by bromine?

A

Bromine cant displace any halogens above it in group 7. These are chlorine and fluorine.

42
Q

Why cant iodine displace chlorine or bromine from an aqueous ionic solution?

A

Because reactivity decreases down the group and iodine is below chlorine and bromine in group 7.

43
Q

Write the word equation for the reaction between chlorine and potassium bromide

A

Chlorine + potassium bromide -> potassium chloride + bromine

44
Q

Write the word equation for the reaction between bromine and calcium chloride

A

No reaction will occur because bromine is less reactive than chlorine so chlorine wont be displaced

45
Q

Write the balanced symbol equation for the reaction that takes place netween bromine and potassium iodide

A

Br ₂ + 2Kl -> I ₂ + 2KBr

46
Q

Which halogens would you expect astatine to be able to displace?

A

None. Its at bottom of group 7 so has lowest reactivity

47
Q

Why does reactivity decrease down group 7?

A

Outer shell is further from nucleus as go down group
Electron sheilding increases
Attraction between nucleus and outer electrons decreases so is harder for atom to gain an electron - reactivity decreases

48
Q

What colours are solutions of chlorine, bromine and iodine?

A

Chlorine water - colourless
Bromine water - orange
Iodine solution - brown

49
Q

What would you observe when chlorine is added to potassium bromide?

A

Cl ₂ + 2KBr -> Br ₂ + 2KCl

Colour change from colourless to orange

50
Q

What is a redox reaction?

A

Reaction where oxidation and reduction take place at same time

51
Q

Are halogen displacement reactions redox reactions? Explain your answer.

A

Yes

  • halide ion is oxidised (loses an electron) to form a halogen atom
  • halogen is reduced (gains an electron) to form a halide ion
52
Q

Write 2 half equations for the reaction between chlorine and potassium bromide, state which is reduction/oxidation

A

Reduction: Cl₂ + 2e⁻ -> 2Cl⁻
Oxidation: 2Br⁻ -> Br₂ + 2e⁻

53
Q

Bromine reacts with potassium iodide.

What is reduced and what is oxidised?

A

Bromine is reduced to bromide ions

Iodide ions are oxidised to iodine

54
Q

What name is used to describe the elements in group 0 of the periodic table?

A

Noble gases

55
Q

How many electrons do the noble gases have in their outer shell?

A

8

Have no incomplete shells of electrons

56
Q

What does chemically inert mean?

A

Not chemically active

57
Q

Why are the noble gases chemically inert?

A

Have full outer electron shells. This is a very stable electron configuration + means elements are very unreactive

58
Q

What properties of helium makes it suitable for use in balloons?

A

Is less dense than air and doesnt burn

59
Q

Why is argon used to fill electric light bulbs?

A

Very chemically inert so wont react when bulb gets hot. Is non flammable

60
Q

Why is argon used for welding?

A

Provides an inert welding atmosphere

Argon is more dense than air so keeps air away from metal

61
Q

What is the trend down group 0 in boilings pts?

A

Boiling pt increases down group 0 because the relative atomic mass increases so there are more intermolecular forces between atoms

62
Q

What is the trend in density down group 0?

A

Increases down group
Helium least dense
Radon most dense

GCSE - Chemistry (8 decks)

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