The elements nitrogen and chlorine have the same electronegativity value, 3.0.

Which of the following claims are likely to be true?

Check all that apply.

A. The nitrogen-chlorine bond is polar covalent.
B. The nitrogen-chlorine bond is ionic.
C. The nitrogen-chlorine bond has weak ionic character.
D. The nitrogen-chlorine bond is unstable.
E. A molecule with this bond will have a partial negative charge on the Cl atom.
F. The nitrogen-chlorine bond is stable.
G. A molecule with this bond will have a partial negative charge on the N atom.
H. The nitrogen-chlorine bond is non-polar covalent.
I. The nitrogen-chlorine bond has no ionic character.
J. The nitrogen-chlorine bond has strong ionic character.

Given that nitrogen and chlorine have the same electronegativity value (3.0), it implies that they have a non-polar covalent bond. Here are the likely true claims:

1. **The nitrogen-chlorine bond is non-polar covalent.**

- True, because non-polar covalent bonds occur when two identical atoms (or atoms with the same electronegativity) share electrons equally.

2. **A molecule with this bond will have no partial negative charge on the N or Cl atom.**

- True, in a non-polar covalent bond, there is no significant difference in electronegativity, so there are no partial charges.

3. **The nitrogen-chlorine bond is stable.**

- True, non-polar covalent bonds are generally stable.

Therefore, the likely true claims are:

- The nitrogen-chlorine bond is non-polar covalent.

- A molecule with this bond will have no partial negative charge on the N or Cl atom.

- The nitrogen-chlorine bond is stable.