Giant Covalent/Metallic Bonds

Question 1

Explain two propeties that both graphie and diamonds have.

Answer 1

Diamond and graphite have giant covalent structures.
Diamond and graphite both consist only of carbon atoms.

Question 2

Is graphite a good conductor? Explain your answer.

Answer 2

Graphite is a good conductor electricity because it contains delocalised electrons which can move through its structure.

Question 3

Define metallic bonding.

Answer 3

A force of attraction between a metal cation ion and a delocalised electron. It results in a sea of delocaliased electrons, that aren’t bound to a single atom.

Question 4

Define lattice.

Answer 4

A regular arrangement of atoms or molecules within a larger amount of a solid substance.

Question 5

Compare the melting points of metals and their ionic bonds.

Answer 5

The melting point of metals are lower than the melting points of the same metal in an ionic bond. For example, the melting point of sodium is only 98 °C, whereas the melting point of sodium chloride is 801 °C.

Question 6

Is the electrostatic force of attraction between positive and negative ions have higher or lower forces of attraction when compared to the sea of delocalised electrons.

Answer 6

The electrostatic forces of attraction between positive and negative ions must be a lot higher than the forces of attraction between positive ions and the sea of delocalised electrons.

Question 7

Define malleability.

Answer 7

Easily bent and shaped. A property of metals.

Question 8

Metals can be described as a lattice of positive ions in a sea of electrons. This is described as a metallic bond (not ionic bond). They conduct electricity because the electrons (not the ions) are free to move. They are malleable because the layers can slide over each other.

Answer 8

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