Question

1st attempt
part 1 (1 point)
the overall (net) dipole of this compound is pointed in which direction?
choose one:
a
b
c there is no dipole.
part 2 (1 point)
based on vsepr and electronegativity differences, predict whether this ion is ionic, polar, or nonpolar.
choose one:
a ionic
b. polar
c. nonpolar

Explanation:

Part 1

Step1: Analyze electronegativity

Electronegativity of \(S = 2.58\), \(C=2.55\), \(N = 3.04\). The bond \(C - S\) has a small electronegativity difference (\(\Delta\chi=2.58 - 2.55=0.03\)), and the bond \(C\equiv N\) has \(\Delta\chi = 3.04 - 2.55 = 0.49\). The dipole moment direction is from less electronegative to more electronegative atom. So the net dipole is towards \(N\) (direction \(A\)).

Part 2

Step1: Check VSEPR and polarity

The ion \([S - C\equiv N]^{-}\) has a linear shape (VSEPR, as central \(C\) has two electron - group (one single bond and one triple bond)). There is a net dipole moment (from \(C\) to \(N\) as \(N\) is more electronegative). So it is polar.

Answer:

Part 1: A.
Part 2: B.