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IB Chemistry HL 2.3 The Metallic Model Questions

Explore how positive-ion lattices and delocalized electrons explain metallic bonding, conductivity and malleability; compare bond-strength and melting-point trends in transition metals.

Syllabus
First assessment 2025
Course
Chemistry HL
Level
HL

Exam points

  • Describe metallic bonding as electrostatic attraction between a lattice of positive metal ions and delocalized electrons.
  • Explain electrical and thermal conductivity using mobile delocalized electrons, and malleability by sliding layers of positive ions without breaking non-directional metallic bonding.
  • Compare metallic bond strength using metal-ion charge, radius and the attraction to delocalized electrons.
  • Explain melting-point trends in s- and p-block metals by relating ion charge and radius to metallic bond strength.
  • Compare transition-element melting points using evidence about metal-ion radius and available valence electrons.

Covered syllabus points

2.3.1—Metallic bonding2.3.2—Bond strength2.3.3 (HL)—Transition elements

Question 1

[Maximum number: 3]

Titanium and vanadium are consecutive elements in the first transition metal series.

Question (a)

(a)

Describe the bonding in metals.

[ 2 ]

Question (b)

(b)

Suggest why the melting point of vanadium is higher than that of titanium.

[ 1 ]

Question 2

[Maximum number: 1]

Which combination causes the strength of metallic bonding to increase?

Table for Question 2 — IB Chemistry HL
A

Charge on cations: smaller; ionic radius: smaller.

B

Charge on cations: larger; ionic radius: larger.

C

Charge on cations: smaller; ionic radius: larger.

D

Charge on cations: larger; ionic radius: smaller.

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