Metallic Bonding
Chemistry ⇒ Chemical Bonding and Structure
Metallic Bonding starts at 9 and continues till grade 12.
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Describe how metallic bonding explains the high density of most metals.
Describe how the structure of an alloy differs from that of a pure metal.
Describe the difference between metallic bonding and ionic bonding.
Describe the effect of adding a small amount of carbon to iron to form steel, in terms of metallic bonding.
Describe the role of metallic bonding in the formation of alloys.
Explain why mercury is a liquid at room temperature, while most other metals are solid.
Explain why metals are good conductors of electricity.
Explain why metals are malleable and ductile, while ionic solids are brittle.
Explain why the melting point of group 1 metals decreases down the group.
Explain why transition metals often have higher melting points than s-block metals.
In the context of metallic bonding, what is meant by 'delocalized electrons'?
A sample of pure copper is alloyed with a small amount of zinc. Predict and explain the effect this has on the malleability of the resulting alloy compared to pure copper.
Compare the metallic bonding in sodium (Na) and aluminum (Al), and explain why aluminum has a much higher melting point than sodium.
Consider two metals, X and Y. Metal X has a higher number of delocalized electrons per atom and a smaller ionic radius than metal Y. Which metal would you expect to have a higher melting point? Explain your reasoning.
Explain, in terms of metallic bonding, why the electrical conductivity of a metal decreases as its temperature increases.
