Question

Draw the structure of d-orbital.

Answer 1

Hint: The answer here is dependent on the basic concept of chemistry that deals with the atomic structures and the orbitals in it where the electrons are accommodated and their respective structure based on its number of orientations that is in d – orbital has five orientations.

Complete answer:
The concepts of general chemistry that deals with the atom and its structure and also the atomic orbitals of various elements with their orientations are familiar to us.
Let us now see in detain once again about the structure of d – orbital.
To start with, the orbitals are designated as s, p, d and f that hold the electrons in atoms.
- These orbitals have different shapes and energies and the electronic configurations are written in terms of these notations like 1s, 2s 2p, 3s 3p 3d and so on.
- Since the orbitals have different shapes, among them d – orbital have five orientations that are ${{d}_{xy}},{{d}_{yz}},{{d}_{xz}},{{d}_{{{z}^{2}}}}$and${{d}_{{{x}^{2}}-{{y}^{2}}}}$
Thus, these five orientations have different shapes and thus they are shown below,

For the d – orbital, azimuthal quantum number is i = 2 and the magnetic quantum number is m = -2, -1, 0, +1, +2.
Therefore, this is the reason that d – orbital have five orientations in the space and corresponds to four double dumb-bell shape $\left( {{d}_{xy}},{{d}_{yz}},{{d}_{xz}},{{d}_{{{x}^{2}}-{{y}^{2}}}} \right)$ and one dum-belled with dough nut shape $\left( {{d}_{{{z}^{2}}}} \right)$.

Note:
Do not be confused about the terms s, p, d and f configuration and K, L, M and N configuration as KLMN configuration is the method which is based on electron shells and only indicates the number of electrons an atom has with each principal quantum number and spdf configuration subdivides each shell into its subshells.