In the Hydrogen atom, the energy of the first excited state is – 3.4 eV. Then find out K.E(kinetic energy) of the same orbit of the Hydrogen atom:

1. + 3.4 eV

2. + 6.8 eV

3. – 13.6 eV

4. + 13.6 eV

The value of Planck's constant is 6.63 × 10^–34 J s. The velocity of light is 3.0 × 10⁸ m s^–1. The closest value to the wavelength in nanometers of a quantum of light with a frequency of $8\times {10}^{15}$ ${\mathrm{s}}^{-1}$ is:

1. $2\times {10}^{-25}$

2. $5\times {10}^{-18}$

3. $4\times {10}^1$

4. $3\times {10}^7$

The mass and charge of one mole of electrons are, respectively:

1. 5.48 × ${10}^{-7}$ kg, 9.65 C, 
2. 5.48 × ${10}^{-7}$ C, 1.098 × 10²⁷
3. 5.48 × ${10}^{-7}$ kg, 9.65 × ${10}^4$ C
4. 9.65 × ${10}^4$ C, 1.098 × 10²⁷

The period in the modern periodic table indicates the value of :

1. Atomic number

2. Atomic mass

3. Principal quantum number

4. Azimuthal quantum number.

The number of orbitals indicated by the following set of quantum numbers, n = 3, l = 2, m =+2 is:

1.  1

2.  2

3.  3

4.  4

The maximum number of neutrons are present in the nuclei of:

$1.$ ${\mathrm{O}}_8^{16}$
$2.$ ${\mathrm{Mg}}_{12}^{24}$
$3.$ ${\mathrm{Fe}}_{26}^{56}$
$4.$ ${\mathrm{Sr}}_{38}^{88}$

The complete symbol for the atom with the given atomic number (Z) and atomic mass (A) would be, respectively :

1.  ${}_4{}^9\mathrm{Be}$   ${}_{92}{}^{233}\mathrm{U}$     ${}_4{}^9\mathrm{Be}$

2.  ${}_{17}{}^{35}\mathrm{Cl}$    ${}_{92}{}^{233}\mathrm{U}$    ${}_4{}^9\mathrm{Be}$

3.  ${}_4{}^9\mathrm{Be}$    ${}_{17}{}^{35}\mathrm{Cl}$     ${}_{92}{}^{233}\mathrm{U}$

4. ${}_{92}{}^{233}\mathrm{U}$    ${}_4{}^9\mathrm{Be}$    ${}_{17}{}^{35}\mathrm{Cl}$

Yellow light emitted from a sodium lamp has a wavelength (λ) of 580 nm. The frequency (ν) and wave number of this yellow light would be, respectively:

1. 517 × 10¹⁴ s^–1 , 172 × 10⁶ m^–1

2. 6.17 × 10¹⁴ s^–1 , 1.72 × 10⁶ m^–1

3. 4.17 × 10¹⁴ s^–1 , 2.72 × 10⁶ m^–1

4. 5.17 × 10¹⁴ s^–1 , 1.72 × 10⁶ m^–1

The energy of the photon with a frequency of 3 × 10¹⁵ Hz is:

1. 1.988 × ${10}^{-18}$ J
2. 1.588 × ${10}^{-18}$ J
3. 1.288 × ${10}^{-18}$ J
4. 2.988 × ${10}^{-18}$ J

A photon of wavelength 4 × 10^–7 m strikes a metal surface, the work function of the metal being 2.13 eV.  The kinetic energy of emission would be: