As the % s-character of hybrid orbitals increases :

The bond angle in a hybrid orbital grows as the s-character does. The majority of the time, the s-orbitals overlap one another from end to end, increasing the bond angle.
In $s{p}^3$: s- character is 25%, p-character is 75% and bond angle is ${109}^{\circ }{28}^{\text{'}}.$
In $s{p}^2$: s-character is 33.33%, p-character is 77.67% and bond angle is 120 degree. 
In $\mathrm{sp}$: s-character is 50%, p-character is 50% and bond angle is 180 degree.
So, when the % s-character of hybrid orbitals increases bond angle increases.

Hence, the option B is correct