$s$-character, $75\, \%\,p$-character $sp ^2=33 \,\%\, s$-character, $66 \,\% \,p$-character $sp =50\, \%\, p -$ character. The more $s$-character a bond has, the stronger and shorter the bond is. Hence the bond length decrease with increase in $s$ character. An $sp-sp$ bond is strongest and $s p ^3- sp ^3$ bond is weakest.

The bond angle of $sp ^3$ is $109.5, sp ^2$ is $120$ and $sp$ is $180$ . An $sp$ orbital is half $s$ character, $sp ^2$ is $1 / 3 s$ character and $sp ^3$ is $1 / 4 s$ character, so increasing the s character corresponds to increasing the bond angle.

The size of the orbital depends upon the value of principal quantum number$(n)$. Greater the value of $n$, larger is the size of the orbital and lesser the $s$-character