Question detail
How does the structure of a metal contribute to its malleability?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Bonding
Question
- A. The rigid structure prevents deformation
- B. Layers of atoms can slide over each other
- C. Strong ionic bonds hold the structure together
- D. Delocalised electrons are fixed in place
Answer
Layers of atoms can slide over each other
Explanation
Metals are malleable because their structure allows layers of atoms to slide over one another without breaking the metallic bond. This sliding ability is due to the delocalised electrons that maintain the bond while allowing movement.
Common mistake
Misunderstanding Metallic Bonding Strength
Students often confuse the strength of metallic bonding with the melting point of metals, thinking that all metals have high melting points due to strong metallic bonds without considering the structure.
To correctly relate metallic bonding strength to melting point, remember that the melting point is influenced by the arrangement of metal ions and the number of delocalised electrons. Use the formula: 'Higher charge and smaller ionic radius lead to stronger metallic bonds, resulting in higher melting points.' For example, consider magnesium (Mg) with a higher charge compared to sodium (Na); thus, Mg has a higher melting point due to stronger metallic bonding.
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