Shape of Orbitals - Practice Questions & MCQ

$\mathrm{d}_{\mathrm{xy}}, \mathrm{d}_{\mathrm{yz}}, \mathrm{d}_{\mathrm{zx}}$

$\mathrm{d}_{\mathrm{x}^2-\mathrm{y}^2}, \mathrm{~d}_{\mathrm{z}^2}$

$\mathrm{d}_{\mathrm{x}^2-\mathrm{y}^2}, \mathrm{~d}_{\mathrm{xy}}$

$\mathrm{d}_{\mathrm{z}^2}, \mathrm{~d}_{\mathrm{yz}}, \mathrm{d}_{\mathrm{zx}}$

Spherical with zero nodes

Spherical with one nodes

Dumble with one node

Dumble with zero node

Double dumble along Y and Z axis 

Double dumble along X and Y axis 

Single dumble along Z axis 

One dumble along Z - axis and a ring in XY plane.

1s and 2s orbitals are spherical in shape.
 

The probability of finding the electron is maximum near the nucleus.
 

The probability of finding the electron at a given distance is equal in all directions.
 

The probability density of electrons for 2s orbital decreases uniformly as distance from the nucleus increases.