Which type of orbitals overlap with each other in benzene?

Why does the type of overlap shown in the following figure not result in bond formation? Explain.

Which of the following types of orbital overlapping results in the formation of a $\pi$ bond?

Considering the $x$-axis as the internuclear axis,which of the following will not form a sigma $(\sigma)$ bond and why?
$(a)$ $1s$ and $1s$
$(b)$ $1s$ and $2p_{x}$
$(c)$ $2p_{y}$ and $2p_{y}$
$(d)$ $1s$ and $2s$

The number of sigma $(\sigma)$ and pi $(\pi)$ bonds present in benzene respectively are:

Number of $\sigma$ (sigma) and $\pi$ (pi) bonds in aspirin are respectively . . . . . . .