Question

explain diagrammatically the boundary surfaces for three 2P orbitals and five 3d orbitals?

Answer 1

Answer:

$\huge{\textbf{\textsf{{\color{navy}{An}}{\purple{sw}}{\pink{er}} {\color{pink}{:}}}}}$

Explanation:

The boundary surface diagrams are drawn in space for an orbital where the probability density is the maximum.

The p-orbital has 2 lobes and d-orbital has 4 lobes.

Refer to the attachment as well..!

“Hope it helps you”

Answer 2

$\fbox\blue{1}$ $\sf\underline\red{ Shape~of~2p-orbital}$ :

• Shape of p-orbital is dumbbell.
• There are three 2p-orbitals.
• They are ${2p}_{x}$ , ${2p}_{y}$ & ${2p}_{z}$ orbitals.
• Each orbital has two lobes.
• These lobes are oriented along their respective axes.
• Each p orbital has one nodal plane.

$\fbox\pink{2}$ $\sf\underline\green{Shape~of~3d-orbital}$ :

• d-orbital has double dumbbell shape.
• There are five d-orbitals.
• They are ${d}_{xy}$ , ${d}_{yz}$ , ${d}_{zx}$ , ${d}_{x²~-y²}$ & ${d}_{z²}$ .
• Each d orbital has 4 lobes.
• In ${d}_{xy}$ orbital, the lobes are placed in between the x & y axes.
• Similar in the case with other orbitals ${d}_{yz}$ , ${d}_{zx}$
• In ${d}_{x²~-~y²}$ orbital the lobes lie along x & y axes.
• Each d orbital has two nodal planes.
• In ${d}_{z²}$ orbital, two lobes lie along z axis & there is a ring of electrons - cloud around the centre.