Embibe Experts Solutions for Chapter: Structure of Atom, Exercise 4: Exercise 4

If the photon of wavelength $150 \mathrm{pm}$ strikes an atom and one of its inner bound electron is ejected out with a velocity of $1.5\times {10}^7 \mathrm{m}/\mathrm{s}$, what is the energy with which it is bound to the nucleus?

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

The total number of atomic orbitals in fourth energy level of an atom is

If $\mathrm{n}=6,$ the correct sequence for filling of the electrons will be:

The number of $\mathrm{d}-$electrons retained in ${\mathrm{Fe}}^{2+}$ (atomic number of $\mathrm{Fe}=26$) ion is

The frequency of light emitted for the transition $\mathrm{n}=4$ to $\mathrm{n}=2$ of ${\mathrm{He}}^{+}$ is equal to the transition in $\mathrm{H}$ atom corresponding to which of the following

Energy of an electron is given by
$\mathrm{E}=-2.178\times {10}^{-18}\mathrm{J}\left[\frac{{\mathrm{Z}}^2}{{\mathrm{n}}^2}\right]$ 
Wavelength of light required to excite an electron in an hydrogen atom from level $\mathrm{n} = 1$ to $\mathrm{n} = 2$ will be:
$(\mathrm{h}=6.64\times {10}^{-34}\mathrm{Js}$ and $\mathrm{c}=3.0\times {10}^8{\mathrm{ms}}^{-1})$)?

Which of the following is the energy of a possible excited state of hydrogen?: