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.

Subtopic:  Bohr's Theory |
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Maximum number of electrons in a sub shell with l = 3 and n = 4 is

1. 14

2. 16

3. 10

4. 12

Subtopic:  Quantum Numbers & Schrodinger Wave Equation |
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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. $5,1,0,+\frac{1}{2}$

Subtopic:  Quantum Numbers & Schrodinger Wave Equation |
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The total number of atomic orbitals in fourth energy level of an atom is

1.  16
2.  32
3.  4
4.  8

Subtopic:  Bohr's Theory |
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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.  ${\mathrm{\lambda }}_{1}={\mathrm{\lambda }}_{2}$

Subtopic:  Bohr's Theory |
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If n = 6, the correct sequence for the filling of electrons will be

1.

2.

3.

4.

Subtopic:  AUFBAU Principle |
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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

Subtopic:  Shell & Subshell |
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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

Subtopic:  Quantum Numbers & Schrodinger Wave Equation |
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If uncertainty in position and momentum are equal, then uncertainty in velocity is:

1.  $\frac{1}{2\mathrm{m}}\sqrt{\frac{\mathrm{h}}{\mathrm{\pi }}}$

2.  $\sqrt{\frac{\mathrm{h}}{2\mathrm{\pi }}}$

3.  $\frac{1}{\mathrm{m}}\sqrt{\frac{\mathrm{h}}{\mathrm{\pi }}}$

4.  $\sqrt{\frac{\mathrm{h}}{\mathrm{\pi }}}$

Subtopic:  Heisenberg Uncertainty Principle |
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The measurement of the electron position is associated with uncertainty in momentum, which is equal to 1 x 10-18 g cm s-1. The uncertainty in electron velocity will be (mass of an electron is 9 x 10-28 g)-

1. 2 x 109 cm s-1
2. 1 x 109 cm s-1
3. 1 x 105 cms-1
4. 1 x 1011 cm s-1

Subtopic:  Heisenberg Uncertainty Principle |
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