Question

question 6
1 pts
which of the following incorrectly assigns a dipole moment to a bond?
( ^{d+} b r-b r^{d-} )
( ^{d+} s i-s^{d-} )
( ^{d+} h-f^{d-} )
( ^{d+} h-c l^{d-} )

Explanation:

• For a bond to have a dipole moment, there must be a difference in electronegativity between the two atoms forming the bond.
• In the case of \(Br - Br\), both atoms are the same (bromine). Atoms of the same element have the same electronegativity. So, there is no separation of charge (\(\delta+\) and \(\delta-\)) across the \(Br - Br\) bond.
• For \(Si - S\), sulfur (\(S\)) is more electronegative than silicon (\(Si\)), so \(Si\) has a \(\delta+\) and \(S\) has a \(\delta-\).
• For \(H - F\), fluorine (\(F\)) is more electronegative than hydrogen (\(H\)), so \(H\) has a \(\delta+\) and \(F\) has a \(\delta-\).
• For \(H - Cl\), chlorine (\(Cl\)) is more electronegative than hydrogen (\(H\)), so \(H\) has a \(\delta+\) and \(Cl\) has a \(\delta-\).

Answer:

\(\ce{^{\delta +}Br - Br^{\delta -}}\)