If the binding energy of the electron in a hydrogen atom is 13.6 eV, the energy required to remove the electron from the first excited state of ${\mathrm{Li}}^{++}$ is 

(1) 122.4 eV       

(2) 30.6 eV

(3) 13.6 eV         

(4) 3.4 eV

Which state of triply ionised Beryllium $\left({\mathrm{Be}}^{+++}\right)$ has the same orbital radius as that of the ground state of hydrogen

(1) n = 4                 

(2) n = 3

(3) n = 2                 

(4) n = 1

The ratio of areas within the electron orbits for the first excited state to the ground state for hydrogen atom is

1. 16 : 1             

2. 18 : 1

3. 4 : 1               

4. 2 : 1

Taking Rydberg’s constant ${\mathrm{R}}_{\mathrm{H}}=1.097\times {10}^7 \mathrm{m}$ first and second wavelength of Balmer series in hydrogen spectrum is

(1) 2000 Å, 3000 Å                 

(2) 1575 Å, 2960 Å

(3) 6529 Å, 4280 Å                 

(4) 6552 Å, 4863 Å

The kinetic energy of electron in the first Bohr orbit of the hydrogen atom is 

(1) – 6.5 eV               

(2) – 27.2 eV

(3) 13.6 eV               

(4) – 13.6 eV

In Bohr’s model of hydrogen atom, which of the following pairs of quantities are quantized 

(1) Energy and linear momentum

(2) Linear and angular momentum

(3) Energy and angular momentum

(4) None of the above

The energy of the highest energy photon of Balmer series of hydrogen spectrum is close to
(1) 13.6 eV             

(2) 3.4 eV

(3) 1.5 eV               

(4) 0.85 eV

Which one of the relation is correct between time period and number of orbits while an electron is revolving in a orbit

(1) ${\mathrm{n}}^2$             

(2) $\frac{1}{{\mathrm{n}}^2}$

(3) ${\mathrm{n}}^3$             

(4) $\frac{1}{\mathrm{n}}$

An electron changes its position from orbit n = 4 to the orbit n = 2 of an atom. The wavelength of the emitted radiation’s is (R = Rydberg’s constant)

(1) $\frac{16}{\mathrm{R}}$             

(2) $\frac{16}{3\mathrm{R}}$

(3) $\frac{16}{5\mathrm{R}}$             

(4) $\frac{16}{7\mathrm{R}}$

If the energy of a hydrogen atom in nth orbit is ${\mathrm{E}}_{\mathrm{n}}$, then energy in the nth orbit of a singly ionized helium atom will be 

(1) 4${\mathrm{E}}_{\mathrm{n}}$             

(2) ${\mathrm{E}}_{\mathrm{n}}$/4

(3) 2${\mathrm{E}}_{\mathrm{n}}$             

(4) ${\mathrm{E}}_{\mathrm{n}}$/2