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Chemistry paper 2 > Topic 6 > Flashcards

Topic 6 Flashcards

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1
Q

How are elements arranged in the periodic table.

A

Groups
Periods
increasing atomic number

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2
Q

What group of the periodic table are alkali metals in?

A

Group 1

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3
Q

Two properties of alkali metals

A

Soft

Relatively low melting points

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4
Q

Why are they called alkali metals?

A

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

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5
Q

Products of lithium and water?

A

Lithium hydroxide + hydrogen

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6
Q

Balanced equation of sodium and water

A

2Na + 2H2O -> 2NaOH + H2

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7
Q

What would we see when lithium reacts with water.

A

Slowest reaction of alkali metals
Bubbles of hydrogen are produced
Doesn’t melt.

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8
Q

Order of reactivity of first 3 alkali metals with water.

A

Lithium < Sodium < Potassium

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9
Q

Trend of reactivity in group 1

A

Reactivity increases down group 1

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10
Q

Why does reactivity increase down group 1?

A

Number of electron shells increase down the group so more electron shielding. weaker attraction between electron and nucleus, so easier to remove outer shell electron to positive ion.

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11
Q

What group are halogens in?

A

Group 7, as they have 7 outer shell electrons

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12
Q

Colour and state of chlorine at room temp?
Colour and state of Bromine at room temp?
Colour and state of Iodine at room temp?

A

Pale green and gas
Red brown liquid
Black solid

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13
Q

What is the trend of melting and boiling point of halogens?

A

As you go down the group, melting an boiling point increases

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14
Q

Why does melting and boiling point increase down group 7?

A

Molecules get bigger down the group, more intermolecular forces to overcome melting/boiling point, more energy required.

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15
Q

Chemical test for chlorine

A

Damp litmus paper placed in tube of gas, if chlorine present, litmus paper turns red then white due to the bleaching effect of chlorine.

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16
Q

Halogens are diatomic, what does that mean?

A

Form molecules consisting of 2 atoms.

E.g Cl2 O2 and Br2

17
Q

What is produced when a halogen reacts with a metal?

A

Metal halide salt

18
Q

Balanced symbol equation of reaction between bromine and sodium.

A

Br2 + 2Na -> 2NaBr

19
Q

Word equation for reaction between iodine and potassium.

A

Iodine + potassium -> Potassium Iodide

20
Q

Describe trend of reactivity of halogens

A

Reactivity decreases down group 7

21
Q

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

A

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

22
Q

What happens when a hydrogen halide dissolves in water?

A

An acidic solution, hydrogen ions dissociate, making solution acidic

23
Q

When does halogen displacement occur?

A

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

24
Q

Word equation of reaction between chlorine and potassium bromide.

A

Chlorine + potassium bromide -> potassium chloride + bromine

25
Q

Why does reactivity decrease down group 7

A

Further down outer shell is further away from nucleus, electron shielding increases, attraction between nucleus and outer electrons decreases so harder for atom to gain electron so reactivity decreases.

26
Q

What colours are solutions of chlorine bromine and iodine?

A

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

27
Q

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

A

Colour change from colourless to orange

Cl2 + 2KBr -> Br2 + 2KCL

28
Q

What is a redox reaction?

A

A reaction where oxidation and reduction take place at same time.

29
Q

Are halogen displacement reactions redox reactions? Explain.

A

Yes as the halide ion is oxidised (loses and electron) to from halogen atom while the halogen atom is reduced gains an electron) to become a halide ion.

30
Q

Write 2 half equations for reaction of chlorine and potassium bromide. tell me which is reduction and which is oxidation.

A

Overall equation:
Cl2 + 2KBr -> Br2 + 2KCl

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

31
Q

What names describe group 0 in periodic table?

A

Noble gases

32
Q

How many electrons do noble gases have in outer shell?

A

0

They have no incomplete shells of electrons.

33
Q

What does chemically inert mean?

A

Not chemically active.

34
Q

Why are noble gases chemically inert.

A

Because they have a full outer shell of electrons. So its very stable and means the elements are very unreactive.

35
Q

What properties of helium make it suitable for use in balloons.

A

less dense than air and does not burn.

36
Q

Why is argon useful to fill electric light bulbs.

A

Very chemically inert so doesn’t react when bulb gets hot and non flammable.

37
Q

Why is argon used for welding

A

It provides inert welding atmosphere. Argon is more dense than air so it keeps air away from metal.

38
Q

Trend in boiling points down group 0?

A

Boiling point increases down group 7 because relative atomic mass increases so there is more intermolecular forces between atoms.

39
Q

Trend of density down group 0

A

Density increases down the group.

Chemistry paper 2 (3 decks)

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