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The Metallic Model · Paper 1 — Free Chemistry SL Practice Questions

What this topic covers

Every property question IB throws at you — why does this melt higher, why does that conduct here but not there — traces back to one of three bonding models: ionic, covalent, or metallic. This topic asks you to build each model from its electrostatic basics, then use it to predict and explain real behaviour: melting point, conductivity in different states, shape, solubility, malleability. The exam almost never tests the model in isolation — it tests whether you can name the right structural detail (coordination number, electron domain count, number of delocalized electrons) and explain why that detail produces the observed property. Vocabulary without mechanism gets you nowhere on the mark scheme.

Read the full Structure: Models of Bonding and Structure lesson notes →

1FoundationMCQMetallic bonding and electron sea model1 markPaper 1~2 min

Which statement best describes the electron sea model of metallic bonding?

Solutions

2FoundationMCQMetallic bonding and electron sea model1 markPaper 1~2 min

In the metallic bonding model, the strength of the bond depends on the charge density of the metal cations and the number of delocalised electrons. Sodium (Group 1) melts at 98 °C, while magnesium (Group 2) melts at 650 °C. Which statement best explains why magnesium has a significantly higher melting point than sodium?

Solutions

3FoundationMCQMetallic bonding and electron sea model1 markPaper 1~2 min

According to the electron sea model, which statement best explains why metals are both malleable and ductile?

Solutions

4MasteryMCQMetallic bonding and electron sea model1 markPaper 1~2 min

Copper wire carries a large current without melting or breaking. Which statement correctly explains both the electrical conductivity and the ductility of copper in terms of its bonding and structure?

Solutions

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