The value of Planck's constant is 6.63 × 10^–34 Js. The speed of light is 3 × 10¹⁷ nm s^–1. Which value is closest to the wavelength in nanometer of a quantum of light with frequency of 6 × 10¹⁵ s^–1 ?

 

1. 25
2. 50
3. 75
4. 10

Based on equation E = –2.178 × 10^–18J, $\frac{{\mathrm{Z}}^2}{{\mathrm{n}}^2}$ certain conclusions are written. Which of them is not correct ?
1. Larger the value of n, larger is the orbit radius.
2. Equation can be used to calculate the change in energy when the electron changes orbit.
3. For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit.
4. The negative sign in equation simply means that the energy of electron bound to the nucleus is lower than what it would be if the electrons were at an infinite distance from the nucleus.

Maximum number of electrons in a sub shell with l = 3 and n = 4 is

1. 14

2. 16

3. 10

4. 12

The correct set of four quantum numbers for the valence electron of a rubidium atom (Z =37) is 

1. $5,1,1,+\frac{1}{2}$

2. $6,0,0,+\frac{1}{2}$

3. $5,0,0,+\frac{1}{2}$

4. $5,1,0,+\frac{1}{2}$

The energies E₁ and E₂ of two radiations are 25 eV and 50 eV respectively. The relation between their wavelenghs i.e., ${\mathrm{\lambda }}_1$ and ${\mathrm{\lambda }}_2$ will be

1.  ${\mathrm{\lambda }}_1=2{\mathrm{\lambda }}_2$

2.  ${\mathrm{\lambda }}_1=4{\mathrm{\lambda }}_2$

3.  ${\mathrm{\lambda }}_1=\frac{1}{2}{\mathrm{\lambda }}_2$

4.  ${\mathrm{\lambda }}_1={\mathrm{\lambda }}_2$

If n = 6, the correct sequence for the filling of electrons will be

1. $\mathrm{ns} \stackrel{}{\to } \left(\mathrm{n}-1\right) \mathrm{d} \stackrel{}{\to } \left(\mathrm{n}-2\right) \mathrm{f} \stackrel{}{\to } \mathrm{np}$

2. $\mathrm{ns} - \left(\mathrm{n}-2\right) \mathrm{f} \stackrel{}{\to } \mathrm{np} \stackrel{}{\to } \left(\mathrm{n}-1\right) \mathrm{d}$

3. $\mathrm{ns} - \mathrm{np} \stackrel{}{\to } \left(\mathrm{n}-1\right)\mathrm{d} \stackrel{}{\to } \left(\mathrm{n}-2\right) \mathrm{f}$

4. $\mathrm{ns} \stackrel{}{\to } \left(\mathrm{n}-2\right) \mathrm{f} \stackrel{}{\to } \left(\mathrm{n}-1\right) \mathrm{d} \stackrel{}{\to } \mathrm{np}$

The rule used to determine the maximum number of electrons in a subshell of an atom is

1. 4l+2

2. 2l+1

3. 4l-2

4. 2n²

The incorrect set of quantum numbers among the following is
1. n= 4, l= 0, m= 0, s= -1/2
2. n= 5, l= 3, m= 0, s= +1/2
3. n= 3, l= 2, m= -3, s= -1/2
4. n= 3, l= 2, m= 2, s= -1/2