Pearson Edexcel GCSE Combined Science · C6

Groups in the periodic table

50 revision questions with answers for C6 Groups in the periodic table in Pearson Edexcel GCSE Combined Science (spec 1SC0). Practise with flashcards, a topic quiz, a random quiz across the course, 5 crosswords, or read every question and answer below.

All 50 questions and answers

Question 1 · Spec C6.1
Where are alkali metals, halogens and noble gases in the periodic table?
Answer:
Groups 1, 7 and 0, respectively.
Question 2 · Spec C6.2
State two physical properties of alkali metals.
Answer:
They are soft and have relatively low melting points compared with many other metals.
Question 3 · Spec C6.5
How many outer-shell electrons do Group 1 atoms have?
Answer:
One.
Question 4 · Spec C6.5
Why do alkali metals normally form +1 ions?
Answer:
They lose their single outer-shell electron to obtain a stable full outer shell.
Question 5 · Spec C6.3
What are the products of an alkali metal reacting with water?
Answer:
A metal hydroxide and hydrogen.
Question 6 · Spec C6.3
Describe lithium reacting with water.
Answer:
It floats, fizzes and moves slowly as hydrogen and lithium hydroxide form.
Question 7 · Spec C6.3
Describe sodium reacting with water.
Answer:
It floats, fizzes vigorously and usually melts into a ball as sodium hydroxide and hydrogen form.
Question 8 · Spec C6.3
Describe potassium reacting with water.
Answer:
It reacts more vigorously than sodium and may ignite with a lilac flame.
Question 9 · Spec C6.3
Balance sodium's reaction with water.
Answer:
2Na + 2H₂O → 2NaOH + H₂.
Question 10 · Spec C6.3
Why is the resulting water solution alkaline?
Answer:
The metal hydroxide releases hydroxide ions into the solution.
Question 11 · Spec C6.4
How does Group 1 reactivity change down the group?
Answer:
It increases; potassium reacts more vigorously than sodium, which reacts more vigorously than lithium.
Question 12 · Spec C6.5
Why does alkali-metal reactivity increase down the group?
Answer:
The outer electron is farther from the nucleus and more shielded, so it is lost more easily.
Question 13 · Spec C6.4
Predict rubidium's reaction with water compared with potassium.
Answer:
It should be more vigorous because rubidium is lower in Group 1.
Question 14 · Spec C6.3
How is the gas from an alkali-metal-water reaction identified?
Answer:
It gives a squeaky pop with a lighted splint.
Question 15 · Spec C6.4
Why compare similar small amounts and conditions when judging reactivity?
Answer:
Unequal size or conditions can change reaction vigour independently of the element.
Question 16 · Spec C6.6
State chlorine's colour and physical state at room temperature.
Answer:
A pale green or green-yellow gas.
Question 17 · Spec C6.6
State bromine's colour and physical state at room temperature.
Answer:
A red-brown liquid.
Question 18 · Spec C6.6
State iodine's appearance and physical state at room temperature.
Answer:
A dark grey solid; its vapour is purple.
Question 19 · Spec C6.7
How do halogen melting and boiling points change down the group?
Answer:
They increase from chlorine to bromine to iodine.
Question 20 · Spec C6.7
Predict astatine's state at room temperature.
Answer:
Solid, based on the increasing melting and boiling points down Group 7.
Question 21 · Spec C6.9
What is a metal halide?
Answer:
A compound of a metal with a halogen, such as sodium chloride.
Question 22 · Spec C6.9
What forms when sodium reacts with chlorine?
Answer:
Sodium chloride: 2Na + Cl₂ → 2NaCl.
Question 23 · Spec C6.9
What formula results from magnesium reacting with bromine?
Answer:
MgBr₂: one Mg²⁺ ion requires two Br⁻ ions.
Question 24 · Spec C6.9
How can halogen reaction patterns predict a less familiar metal halide?
Answer:
Use the metal ion's charge and the halide's -1 charge to obtain a neutral formula.
Question 25 · Spec C6.10
What forms when hydrogen reacts with a halogen?
Answer:
A hydrogen halide, such as hydrogen chloride.
Question 26 · Spec C6.10
Why is hydrogen chloride gas different from hydrochloric acid?
Answer:
Hydrochloric acid is hydrogen chloride dissolved in water, where it produces hydrogen ions.
Question 27 · Spec C6.10
Predict the effect of dissolving hydrogen bromide in water.
Answer:
It forms an acidic solution.
Question 28 · Spec C6.8
What is the chemical test for chlorine?
Answer:
It bleaches damp litmus paper white.
Question 29 · Spec C6.8
Why use damp rather than dry litmus for chlorine?
Answer:
Water enables the reactions responsible for the indicator change and bleaching.
Question 30 · Spec C6.11
Order chlorine, bromine and iodine by reactivity.
Answer:
Chlorine is most reactive, then bromine, then iodine.
Question 31 · Spec C6.11
What happens when chlorine is added to bromide solution?
Answer:
Chlorine displaces bromine: Cl₂ + 2Br⁻ → 2Cl⁻ + Br₂.
Question 32 · Spec C6.11
What happens when bromine is added to iodide solution?
Answer:
Bromine displaces iodine because bromine is more reactive.
Question 33 · Spec C6.11
Can iodine displace chlorine from chloride solution?
Answer:
No. Iodine is less reactive than chlorine.
Question 34 · Spec C6.12 · Higher only
In chlorine-bromide displacement, which substance is reduced?
Answer:
Chlorine gains electrons to form chloride ions.
Question 35 · Spec C6.12 · Higher only
Write the oxidation half equation for bromide ions.
Answer:
2Br⁻ → Br₂ + 2e-.
Question 36 · Spec C6.13
Why does halogen reactivity decrease down the group?
Answer:
Greater shielding and distance weaken attraction for an incoming electron.
Question 37 · Spec C6.11
Predict astatine's ability to displace iodine from iodide.
Answer:
It should not displace iodine because astatine is predicted to be less reactive.
Question 38 · Spec C6.7
Why do larger halogen molecules generally have higher boiling points?
Answer:
Stronger intermolecular attractions require more energy to overcome.
Question 39 · Spec C6.14
Why are noble gases relatively inert?
Answer:
Their outer electron shells are full, giving stable electronic configurations.
Question 40 · Spec C6.14
How is helium's full shell different from neon's?
Answer:
Helium's first shell is full with two electrons; neon's outer shell has eight.
Question 41 · Spec C6.14
Why do noble gases rarely gain or lose electrons?
Answer:
Their full outer shells are stable, so forming ions is energetically unfavourable under ordinary conditions.
Question 42 · Spec C6.16
How does noble-gas density generally change down the group?
Answer:
It increases as atomic mass increases.
Question 43 · Spec C6.16
How do noble-gas boiling points generally change down the group?
Answer:
They increase, although they remain low compared with many solids and liquids.
Question 44 · Spec C6.16
Predict krypton's boiling point compared with argon's.
Answer:
Higher, because krypton lies below argon.
Question 45 · Spec C6.15
Why is helium suitable for balloons?
Answer:
It has low density and is non-flammable.
Question 46 · Spec C6.15
Why is helium safer than hydrogen for lifting balloons?
Answer:
Both are light gases, but helium is non-flammable while hydrogen is flammable.
Question 47 · Spec C6.15
Why can argon protect a hot lamp filament?
Answer:
Its chemical inertness reduces reactions between the hot filament and surrounding gas.
Question 48 · Spec C6.15
Why can argon be used around hot metal during welding?
Answer:
It provides an unreactive atmosphere that limits oxidation.
Question 49 · Spec C6.15
Which properties matter most for a gas shielding hot materials?
Answer:
Chemical inertness and non-flammability, rather than simply low cost or low density.
Question 50 · Spec C6.5
Compare Group 1 and Group 7 electron changes during reaction.
Answer:
Group 1 atoms lose an electron; Group 7 atoms gain one.

← C4 Extracting metals and equilibria C7 Rates of reaction and energy changes →

Groups in the periodic table

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