Does anyone understand hybrid orbitals?

draw for yourself the energy-level diagram showing the hybrid orbitals formed in the c atom when it bonds. [ done ]
now look at those hybrid orbitals and those of the n atom, and describe how the bonding with a n atom will differ with the bonding that occurs with a c atom, even though both atoms have four hybrid orbitals oriented in a tetrahedral shape

N has a lone pair... the lone pair-bond pair repulsion is greater than the bond pair-bond pair repulsion so the tetrahedral geometry of N will be distorted.

The answer options is d

For cyclohexane compounds drawn in a chair conformation:   -axial bonds are vertical  -equatorial bonds are parallel to two bonds within the ring.  thus, as i assume the chair conformation is drawn:   -the x group is in an axial position, as are the five other vertical bonds.  -three axial bonds are on the top face of the ring  -the other three axial bonds are on the bottom face  the position of the second substituent on each ring carbon is equatorial.  gauche groups must be on an adjacent carbon such as carbon 6 and carbon 2, and also gauche groups are rotated by 60 degrees relative to each other.  drawing the newman projections for c1–c2 and c1–c6 aids in visualizing the groups that are gauche to the y group on c1.  click this link and watch some academic videos that may you more understand the topic