If `E_(1)^(delta-) -E_(2)^(delta+)` bond has given polarity, which of the following is/are correct about polarity? (Electronegativity of `E_(1) = 2.4, Q = 3.1, R = 2.6` respectively)

Options

A. `E_(1)^(delta)-Q^(delta+)`
B. `Q^(delta-)-R^(delta+)`
C. `R^(delta+)-E_(2)^(delta-)`
D. `Q^(delta+)-E_(2)^(delta-)`

Answer

B

Explanation

More electronegative element always contain negative charge as compared to less electronegative element so tha polarity will be `Q^(del-) -R^(del+)` while as per given information `E_(2)` is less electronegative than E.