Bonding: Practice Questions

Which statement best explains why metals are good conductors of electricity in terms of their bonding and structure?

Diamond and graphite are both allotropes of carbon with giant covalent structures.
Which of the following accurately compares their bonding and electronic properties?

Which of the following is a significant limitation of using a two-dimensional dot and cross diagram to represent a simple covalent molecule like methane, \(\text{CH}_4\)?

Nanoparticles have a very high surface area to volume ratio.
Consider a cube-shaped nanoparticle with a side length of \(10\text{ nm}\) and a larger cube of the same material with a side length of \(100\text{ nm}\).
What is the ratio of the surface area to volume ratio of the nanoparticle compared to the larger cube?

Explain why magnesium oxide (\(\text{MgO}\)) has a significantly higher melting point than water (\(\text{H}_2\text{O}\)) by comparing the types of bonds and the forces that must be overcome in each substance.

Diamond and graphite are both allotropes of carbon. Although they are made of the same element, their properties are very different.
a) Explain, in terms of structure and bonding, why diamond has a very high melting point.
b) Graphite is also a giant covalent structure but can conduct electricity. Explain why graphite is a conductor while diamond is an insulator.
c) Graphene is a more recently discovered form of carbon. Describe the relationship between the structure of graphene and graphite.