Paper 2 Periodic Table MCQ Practice
10 multiple-choice questions on the periodic table for IGCSE Chemistry Paper 2. Covers groups, periods, trends, alkali metals, halogens, transition elements, and noble gases.
Published by IGCSEChemistry.com.my
Chemistry teaching team: K. S. Tan (15+ years teaching IGCSE Chemistry) and Ms Yash (10+ years teaching IGCSE Chemistry) and Ms Kartini (15+ years teaching IGCSE Chemistry).
Mapped to Cambridge IGCSE Chemistry 0620 (2026–2028). Last updated 2026-08-19.
Ten multiple-choice questions in the style of IGCSE Chemistry Paper 2. Choose the best answer for each, then check the mark scheme.
Question 1
Elements in the same group of the periodic table have similar chemical properties because they have:
A. the same number of electron shells B. the same number of outer-shell electrons C. the same number of neutrons D. the same atomic mass
Answer
B
Elements in the same group have the same number of electrons in their outer shell. It is the outer electrons that are involved in bonding and chemical reactions, so elements with the same outer electron configuration react in similar ways. Elements in the same period (not group) have the same number of electron shells.
Question 2
Going down Group I (the alkali metals), the reactivity:
A. decreases B. stays the same C. increases D. first increases then decreases
Answer
C
Reactivity increases down Group I. As you go down the group, atoms get larger with more electron shells. The outer electron is further from the nucleus and is shielded by more inner electrons, so it is lost more easily. Caesium is more reactive than sodium.
Question 3
Which element is in Group VII of the periodic table?
A. Sodium B. Neon C. Chlorine D. Calcium
Answer
C
Chlorine is a Group VII element (a halogen). Group VII elements have 7 outer electrons. Sodium is in Group I, neon is in Group VIII/0 (noble gases), and calcium is in Group II.
Question 4
Going down Group VII, the boiling points of the halogens:
A. decrease B. increase C. remain constant D. increase then decrease
Answer
B
Boiling points increase down Group VII. The molecules get larger with more electrons, so the intermolecular forces (van der Waals forces) become stronger and more energy is needed to separate them. Fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid at room temperature.
Question 5
Which statement about the noble gases (Group 0/VIII) is correct?
A. They are very reactive non-metals. B. They have incomplete outer electron shells. C. They exist as diatomic molecules. D. They are unreactive because they have full outer electron shells.
Answer
D
Noble gases have full outer electron shells (stable electron configurations), so they have no tendency to gain, lose, or share electrons. This makes them very unreactive. They exist as single atoms (monatomic), not diatomic molecules. Examples include helium (2), neon (2,8), and argon (2,8,8).
Question 6
Transition elements, compared with Group I metals, typically:
A. are softer and less dense B. have higher melting points and form coloured compounds C. are more reactive with water D. have lower melting points and are better conductors
Answer
B
Transition elements (such as iron, copper, and zinc) typically have higher melting points, higher densities, and greater hardness than Group I metals. They also form coloured compounds (e.g. CuSO₄ is blue) and can act as catalysts. Group I metals are soft, low density, and very reactive.
Question 7
What happens when chlorine water is added to potassium bromide solution?
A. No reaction occurs. B. The solution turns orange/brown as bromine is displaced. C. Chlorine gas is produced. D. Potassium chloride is deposited as a solid.
Answer
B
Chlorine is more reactive than bromine (higher in Group VII), so it displaces bromine from potassium bromide solution. The solution turns orange/brown due to the presence of bromine: Cl₂ + 2KBr → 2KCl + Br₂. A more reactive halogen displaces a less reactive one.
Question 8
Which property increases across a period from left to right?
A. Atomic radius B. Metallic character C. Number of outer-shell electrons D. Reactivity with water
Answer
C
Across a period, each successive element has one more proton and one more electron. The number of outer-shell electrons increases from 1 (Group I) to 8 (Group 0). Atomic radius decreases across a period (greater nuclear charge pulls electrons closer). Metallic character also decreases left to right.
Question 9
Lithium, sodium, and potassium all react with water to produce:
A. a metal oxide and hydrogen B. a metal hydroxide and hydrogen C. a metal hydroxide and oxygen D. a metal chloride and hydrogen
Answer
B
All Group I metals react with water to form a metal hydroxide and hydrogen gas. For example: 2Na + 2H₂O → 2NaOH + H₂. The hydroxide solution is alkaline, which is why Group I elements are called the alkali metals.
Question 10
Which property is typical of transition elements but not Group I metals?
A. They conduct electricity. B. They can have variable oxidation states. C. They react vigorously with cold water. D. They are stored under oil.
Answer
B
Transition elements commonly show variable oxidation states. For example, iron can be Fe²⁺ or Fe³⁺, and copper can be Cu⁺ or Cu²⁺. Group I metals always form +1 ions. Both conduct electricity. Group I metals (not transition elements) react vigorously with water and are stored under oil.
Studying this yourself? Tutoring arrangements are normally made by a parent or guardian. Message us for the details to share with them, or send them this page.