Shapes and Energies of Orbitals

In hydrogen atom, the degeneracy of the level with energy $\frac{-{\mathrm{R}}_{\mathrm{H}}}{9}$ is

Which of the following elements contain non-spherical electron density?

The five $\mathrm{d}$-orbitals are designated as ${\mathrm{d}}_{\mathrm{x}\mathrm{y}},\mathrm{}{\mathrm{d}}_{\mathrm{y}\mathrm{z}},\mathrm{}{\mathrm{d}}_{\mathrm{x}\mathrm{z}},\mathrm{}{\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}$ and ${\mathrm{d}}_{{\mathrm{z}}^2}.$ Choose the correct statement.

For a multi-electron atom, the highest energy level among the following is

Which of the following shell have maximum $32$ electrons?

$0.53 A^{\circ }$ is Bohr's radius of the first orbit. In the light of the wave mechanical model, it suggests that 

Which of the following statements is/are correct?

For which one of the following sets of four quantum numbers, an electron will have the highest energy?

The order of filling of electrons in the orbitals of an atom will be

The electrons, identified by quantum numbers $n and l \left(i\right)n=4, l=1 \left(ii\right)n=4, l=0 \left(iii\right)n=3, l=2 \left(iv\right)n=3, l=1$ can be placed in order of increasing energy, from the lowest to highest, as

The orbitals are called degenerate when

In general, the $\mathrm{d}$ -orbital involved in ${\mathrm{s}\mathrm{p}}^3$ $\mathrm{d}$ hybridisation is

Identify the transition element.

The degeneracy of hydrogen atom that has energy equal to $-\frac{{\text{R}}_{\text{H}}}{9}$    (where R_H is Rydberg constant) is

Which of the following orbitals are degenerate?

${\text{3d}}_{\text{xy}}{\text{, 4d}}_{\text{xy}}{\text{, 3d}}_{{\text{z}}^2}{\text{, 3d}}_{\text{yz}}{\text{, 5d}}_{{\text{z}}^2}$

Which of the following statements in relation to the hydrogen atom is correct?

Which of the given statements concerning the hydrogen atom is correct?

In a multi-electron atom, which of the following orbitals described by the three quantum numbers will have the same energy in the absence of magnetic and electric fields?

$$\begin{gathered} \left(\mathrm{i}\right) \mathrm{n}=1, \mathrm{l}=0, \mathrm{m}=0 \\ \left(\mathrm{ii}\right) \mathrm{n}=2, \mathrm{l}=0, \mathrm{m}=0 \\ \left(\mathrm{iii}\right) \mathrm{n}=2, \mathrm{l}=1, \mathrm{m}=1 \\ \left(\mathrm{iv}\right) \mathrm{n}=3, \mathrm{l}=2, \mathrm{m}=1 \\ \left(\mathrm{v}\right) \mathrm{n}=3, \mathrm{l}=2, \mathrm{m}=0 \end{gathered}$$

What is the probability at the second site, if the electrons were in a ${\mathrm{p}}_{\mathrm{z}}$ orbital. The nucleus of an atom is located at $\mathrm{x}=\mathrm{y}=\mathrm{z}=0$. If the probability of finding an s-orbital electron in a tiny volume around $\mathrm{x}=\mathrm{a}, \mathrm{y}=\mathrm{z}=0$ is $1\times {\text{10}}^{-\text{5}}$.

The nucleus of an atom is located at $\mathrm{x}=\mathrm{y}=\mathrm{z}=0$. If the probability of finding an s-orbital electron in a tiny volume around $\mathrm{x}=\mathrm{a}, \mathrm{y}=\mathrm{z}=0$ is $1\times {\text{10}}^{-\text{5}}$, what is the probability of finding the electron in the same sized volume around $\mathrm{x}=\mathrm{z}=0, \mathrm{y}=\mathrm{a}$?