Question

Hydrogen has an electronegativity value between boron and carbon and is identical to phosphorus. With this in mind, rank the following bonds in order of decreasing polarity: P-H, O-H, N-H, F-H, C-H.

Short answer

Answer:

Step-by-step solution

of 1: Check the group or period of the elements to which they belong. 

The more strongly an atom attracts the electron in its bonds, the larger its electronegativeity, Electrons in a polar covalent bond are shifted toward the more electronegative atom; thus the more electronegative atom is the one with the partial negative charge . The greater the difference in electronegativity, the more polarised the electron distribution and the larger the partial charge of the atom.

Step 2.: Here F, O, N, C belong to the same period and P and N belong to the same group.

The electronegativities increase in a period and decrease in a group. The ∆EN of F- 4.0, O- 3.5, N- 3.0, C- 2.5, P- 2.1.

Then the rank of the Polarity of bond in decreasing order is F-H > O-H > N-H > C-H > P-H