IB DP Chemistry - Structure 2.3 The metallic model - IB Style Questions For HL Paper 1A -FA 2025

IBDP Chemistry HL Paper 1A & 1B - All Chapters

Question

Which option arranges the metals in order from strongest to weakest metallic bonding?
(A) \( \text{Al} > \text{Mg} > \text{Na} > \text{K} \)
(B) \( \text{Al} > \text{Mg} > \text{K} > \text{Na} \)
(C) \( \text{Na} > \text{K} > \text{Mg} > \text{Al} \)
(D) \( \text{K} > \text{Na} > \text{Mg} > \text{Al} \)
▶️ Answer/Explanation
Detailed solution

Metallic bond strength increases with higher charge density (smaller atomic radius and greater charge).
Al³⁺ (Al) > Mg²⁺ (Mg) > Na⁺ (Na) > K⁺ (K)
✅ Answer: (A)

Question

Zinc metal contains metallic bonding. Which is the best description of a metallic bond?
A. The electrostatic attraction between a pair of electrons and positively charged nuclei.
B. The electrostatic attraction between oppositely charged ions.
C. The electrostatic attraction between a lattice of positive ions and delocalized electrons.
D. The bond formed when one atom provides both electrons in a shared pair.
▶️ Answer/Explanation
Detailed solution

In a metal such as zinc, atoms lose their outer (valence) electrons. These electrons become delocalized and move freely throughout the structure, forming a “sea of electrons”.

The metal atoms become positive ions (cations), arranged in a regular lattice. The key feature of a metallic bond is the electrostatic attraction between this lattice of positive ions and the delocalized electrons.

Therefore, option C correctly describes a metallic bond as “the electrostatic attraction between a lattice of positive ions and delocalized electrons”.

✅ Answer: (C)

Question

Which series shows the correct order of metallic bond strength from strongest to weakest?
(A) \( \text{Na} > \text{K} > \text{Rb} > \text{Mg} \)
(B) \( \text{Mg} > \text{Rb} > \text{K} > \text{Na} \)
(C) \( \text{Rb} > \text{K} > \text{Na} > \text{Mg} \)
(D) \( \text{Mg} > \text{Na} > \text{K} > \text{Rb} \)
▶️ Answer/Explanation
Detailed solution

Metallic bond strength increases with higher charge and smaller ionic radius. Magnesium forms \( \text{Mg}^{2+} \), giving stronger bonding than the Group 1 metals, which form \( \text{M}^+ \) ions.

In Group 1, metallic bond strength decreases down the group: \( \text{Na} > \text{K} > \text{Rb} \).

Therefore, the order from strongest to weakest is:

✅ Answer: (D) \( \text{Mg} > \text{Na} > \text{K} > \text{Rb} \)

More DP Chemistry HL Paper 1 Questions..
Scroll to Top