If uncertainty in the position of an electron is zero the uncertainty in its momentum will be:
1. <h/4
2. >h/4
3. zero
4. infinite
Which one is the wrong statement?
1. | de-Broglie's wavelength is given by λ =h/mv where m = mass of the particle, v = group velocity of the particle |
2. | The uncertainty principle is |
3. | Half-filled and fully filled orbitals have greater stability due to greater exchange energy, greater symmetry and more balanced arrangement |
4. | The energy of 2s-orbital is less than the energy of 2p-orbital in case of hydrogen like atoms. |
If uncertainty in position and momentum are both equal, then uncertainty in velocity will be:
1.
2.
3.
4.
The measurement of the electron position is associated with an uncertainty in momentum which is equal to 1x10-18 g cm s-1. The uncertainty in velocity of the electron will be:
(mass of an electron is 9 x 10-28 g)
1. 1 x 109 cm s-1
2. 1 x 106 cm s-1
3. 1 x 105 cm s-1
4. 1 x 1011 cm s-1
Given: The mass of electron is 9.11 x 10-31 kg
Planck constant is 6.626 x 10-34 Js
the uncertainty involved in the measurement of velocity within a distance of 0.1 is:
(a) 5.79 x 106 ms-1 (b) 5.79 x 107 ms-1
(c) 5.79 x 108 ms-1 (d) 5.79 x 105 ms-1
For a subatomic particle, the uncertainty in position is same as that of uncertainty in its momentum. The
least uncertainty in its velocity can be given as-
1.
2.
3.
4.
Which of the following does not represent the mathematical expression for the Heisenberg uncertainty principle?
1.
2.
3.
4.
Uncertainty in position of a and He is similar. If uncertainty in momentum of is , then uncertainty in momentum of He will be:
1. | 32×105 | 2. | 16×105 |
3. | 8×105 | 4. | None of the above |
If the position of the electron were measured with an accuracy of +0.002 nm, the uncertainty in the momentum of the electron would be:
1. 5.637 × 10–23 kg m s–1
2. 4.637 × 10–23 kg m s–1
3. 2.637 × 10–23 kg m s–1
4. 3.637 × 10–23 kg m s–1