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IB Chemistry SL 2.3 The Metallic Model Questions

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

Syllabus
First assessment 2025
Course
Chemistry SL
Level
SL

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.

Covered syllabus points

2.3.1—Metallic bonding2.3.2—Bond strength

Question 1

[Maximum number: 1]

Iron may be extracted from iron (II) sulfide, FeS.

Outline why metals, like iron, can conduct electricity.

Question 2

[Maximum number: 1]

Which series shows the correct order of metallic bond strength from strongest to weakest?

A

Na>K>Rb>Mg

B

Mg>Rb>K>Na

C

Rb>K>Na>Mg

D

Mg>Na>K>Rb

Question 3

[Maximum number: 2]

Titanium is a transition metal.

Describe the bonding in metals.

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