Cambridge IGCSE 0620Paper 4 · Exam ModeTotal: 39 marks

8.6 Periodic Table Masterclass

Synthesis & Comparison · 15 Questions · Sections A, B & C

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Section A

Group I vs Transition Elements

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Section B

Group I vs Group VII Trends

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Section C

Full Periodic Table Logic

Section A

Group I vs Transition Elements

11 marks

Q1[3 marks]

State three ways in which the physical properties of transition elements differ from those of Group I (alkali metals).

💡 Examiner Tip: Each point must be a clear COMPARISON. Don't just describe transition metals — contrast them against Group I.

Q2[2 marks]

State two ways in which the chemical properties of transition elements differ from those of Group I metals.

💡 Examiner Tip: These are chemical properties — not physical. Look for oxidation states, coloured compounds, and catalysis.

Q3[2 marks]

Iron(III) chloride solution is orange-brown. Explain, in terms of ions, what this tells us about the nature of transition metal compounds.

💡 Examiner Tip: Link the colour observation to the concept of transition metal ions.

Q4[3 marks]

The table shows properties of lithium (Li) and iron (Fe). Suggest values and explain the trends. Li: Melting point 181°C, Density 0.53 g/cm³ Fe: Melting point 1538°C, Density 7.87 g/cm³ Explain why iron has a much higher melting point than lithium.

💡 Examiner Tip: This is a metallic bonding question. Think about the strength of the metallic bond.

Q5MCQ[1 mark]

Which of the following is a property of transition elements but NOT of Group I metals? A) They conduct electricity B) They react vigorously with cold water C) They can act as catalysts D) They form ionic compounds

💡 Examiner Tip: Eliminate: A and D apply to both. B is Group I. C is the answer.

Section B

Group I vs Group VII Trends

12 marks

Q6[4 marks]

Compare the trend in reactivity down Group I (alkali metals) with the trend in reactivity down Group VII (halogens). In each case, state the trend and explain it in terms of electronic structure.

💡 Examiner Tip: This is a 4-mark compare question. State the trend + explain for EACH group = 4 marks.

Q7[2 marks]

Chlorine water is added to potassium iodide solution. State the observation and write an ionic equation for the reaction.

💡 Examiner Tip: Displacement reaction: a more reactive halogen displaces a less reactive one.

Q8[3 marks]

Sodium reacts with chlorine to form sodium chloride. (a) Write a balanced equation with state symbols. (b) Describe what you would observe. (c) State the type of bonding in the product.

💡 Examiner Tip: Three separate parts — don't merge them. Each earns a mark.

Q9[2 marks]

Explain why the boiling point of the halogens increases down Group VII (F₂ → I₂).

💡 Examiner Tip: Link molecular mass → intermolecular forces → boiling point.

Q10MCQ[1 mark]

A student adds bromine water to sodium iodide solution and to sodium chloride solution. Which result is correct? A) Both solutions decolourise the bromine water B) NaI turns brown; NaCl has no visible change C) NaCl turns brown; NaI has no visible change D) Both solutions turn brown

💡 Examiner Tip: Bromine is more reactive than iodine, but less reactive than chlorine.

Section C

Full Periodic Table Logic

16 marks

Q11[3 marks]

Element Z has proton number 18. Use its position in the periodic table to predict its chemical reactivity, and explain why.

💡 Examiner Tip: Identify the group first from the proton number (electron configuration: 2,8,8). Then reason from electron structure.

Q12[4 marks]

Elements A, B, and C have proton numbers 11, 17, and 20 respectively. (a) Identify the group each element belongs to. (b) Predict whether each element is a metal or non-metal. (c) Write the formula of the compound formed between A and C.

💡 Examiner Tip: Work out electron configurations first: 11→2,8,1; 17→2,8,7; 20→2,8,8,2. Groups follow from outer shell electrons.

Q13[2 marks]

A student claims 'all metals are on the left side of the periodic table.' Evaluate this claim.

💡 Examiner Tip: Think about the position of metalloids and transition metals. Where is the dividing line?

Q14[3 marks]

The period 3 elements Na, Mg, Al, Si, P, S, Cl, Ar show a trend in type of oxide formed. (a) State the trend in acid-base character of oxides from Na to Cl. (b) Write an equation showing Na₂O reacting with water. (c) Write an equation showing SO₃ reacting with water.

💡 Examiner Tip: Metal oxides → basic/alkaline. Non-metal oxides → acidic. This is a classic P4 pattern.

Q15[4 marks]

[Extended Writing — 4 marks] A student is given an unknown element X. They observe: it is a shiny solid at room temperature, it conducts electricity, and it reacts slowly with dilute hydrochloric acid to produce bubbles of gas. (a) Suggest which region of the periodic table element X belongs to, and justify your reasoning. (b) Identify the gas produced. Write an ionic equation for the reaction with HCl.

💡 Examiner Tip: This is a 'detective' question — use each observation as a clue to narrow the region.

📊 Session Score Tracker

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Section A

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Section B

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Section C

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Total Marks

🔁 Review Required

Key Examiner Keywords

Full outer electron shell · Variable oxidation states · Coloured ions · Delocalized electrons · Electrostatic attraction · State symbols

Top 3 Traps in This Paper

1. Confusing physical vs chemical properties. 2. Forgetting state symbols in equations. 3. Misidentifying Group VII trend direction.

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