Question

The bonding of chlorine with each of the Period 3 elements shows a change in bonding type from ionic through polar covalent to nonpolar covalent. Select the properties that reflect this change in bonding character.

A. There is a general decrease in ΔEN moving from left to right across the period.
B. At room temperature, the Period 3 covalently bonded molecules of chlorine are all liquids.
C. Electron density relief maps show a steady increase in electron sharing from NaCl to Cl2.
D. Electrical conductivity at the melting point is high only for chlorides of Group 1A(1) and Group 2A(2).
E. Melting point increases as the bonding character changes from ionic to covalent.

Answer 1

The bonding of chlorine with Period 3 elements shows a change in bonding type from ionic through polar covalent to nonpolar covalent. Properties A, B, and C reflect this change in bonding character.

Step-by-step explanation:

The bonding of chlorine with each of the Period 3 elements shows a change in bonding type from ionic through polar covalent to nonpolar covalent. To reflect this change in bonding character, the following properties are observed:

1. There is a general decrease in electronegativity difference (ΔEN) moving from left to right across the period.
2. At room temperature, the Period 3 covalently bonded molecules of chlorine are all gases, not liquids.
3. Electron density relief maps show a steady increase in electron sharing from NaCl to Cl2.

Therefore, properties A, B, and C reflect the change in bonding character.