Question

Are the following compounds likely to be ionic or not ionic based on the properties described?

1.) Compound A is solid at room temperature with poor conductivity. However, when it is in liquid form, it is able to conduct electricity.
2.) Compound B has a low melting point and is a poor conductor of electricity.

Answer 1

Based on the properties described, Compound A is likely an ionic compound that is able to conduct electricity in its liquid form. Compound B is likely a molecular compound with a low melting point and poor conductivity.

Step-by-step explanation:

The compounds described in the question are likely to be:

1.) Compound A: Based on the properties described, Compound A is likely an ionic compound. It is solid at room temperature with poor conductivity, but when it is in liquid form, it is able to conduct electricity. This suggests that the ions in Compound A are unable to move freely in the solid state, but can move freely in the liquid state, allowing for conductivity.

2.) Compound B: Based on the properties described, Compound B is likely a

molecular compound

. It has a low melting point and is a poor conductor of electricity. Molecular compounds generally have lower melting points than ionic compounds and do not conduct electricity well.