AssessmentExam Bank

Structure 3.1: Assessment Bank

Test your understanding with Paper 1 (MCQ) and Paper 2 (Structured) style questions.

Section A: Paper 1 Style (MCQ)

Which series is arranged in order of decreasing ionic radius?

Mg^{2+} > Na^+ > F^- > O^{2-}

O^{2-} > F^- > Na^+ > Mg^{2+}

P^{3-} > S^{2-} > Cl^- > K^+

K^+ > Cl^- > S^{2-} > P^{3-}

Which equation represents the First Ionization Energy of Calcium?

Ca(s) \to Ca^+(g) + e^-

Ca(g) \to Ca^+(g) + e^-

Ca^+(g) \to Ca^{2+}(g) + e^-

Ca(g) \to Ca^{2+}(g) + 2e^-

Why is the First Ionization Energy of Oxygen lower than Nitrogen?

A. Oxygen has a higher nuclear charge.

B. Oxygen removes an electron from a 2s orbital.

C. Repulsion between paired electrons in the 2p orbital of Oxygen.

D. Nitrogen has a stable octet.

Which oxide reacts with water to form a solution with pH < 2?

Na_2O

MgO

Al_2O_3

P_4O_{10}

HL Only

Which ion is colorless in aqueous solution?

Fe^{3+}

Cu^{2+}

Sc^{3+}

Co^{2+}

Which property is NOT characteristic of transition metals?

A. Formation of colored compounds.

B. Variable oxidation states.

C. Fixed oxidation states of +1.

D. Catalytic behavior.

Why does $Al$ have a lower First IE than $Mg$ ?

A. Removal from 3p vs 3s.

B. Removal from 3s vs 3p.

C. Al has lower nuclear charge.

D. Spin-pair repulsion.

Identify the element with Successive IEs (kJ/mol): 738, 1450, 7730, 10540.

A. Na

B. Mg

C. Al

D. Si

Section B: Paper 2 Style (Structured)

Q1: Explaining Trends (Reasoning) [3 marks]

Prompt: Explain why the First Ionization Energy of Sulfur is lower than that of Phosphorus, despite Sulfur having a higher nuclear charge.

Q2: Oxide Chemistry (Equations) [3 marks]

Prompt: State the formula of the oxide of Phosphorus (V). Write a balanced equation for its reaction with water and state the approximate pH of the resulting solution.

Q3: Transition Metal Complexes [4 marks]

Prompt: Explain, using the Crystal Field Theory, why $[Ti(H_2O)_6]^{3+}$ is colored, whereas $Sc^{3+}$ is colorless.