Match the quantum numbers with the information provided by them:
Quantum number | Information provided | ||
A. | Principal quantum number | 1. | Orientation of the orbital |
B. | Azimuthal quantum number | 2. | Energy and size of orbital |
C. | Magnetic quantum number | 3. | Spin of electron |
D. | Spin quantum number | 4. | Shape of the orbital |
A | B | C | D | |
1. | 2 | 4 | 1 | 3 |
2. | 1 | 2 | 3 | 4 |
3. | 1 | 4 | 3 | 2 |
4. | 4 | 1 | 3 | 2 |
Match the ensuing rules with the corresponding statements:
Rules | Statements | ||
A. | Hund’s Rule | 1. | No two electrons in an atom can have the same set of four quantum numbers. |
B. | Aufbau Principle | 2. | Half-filled and completely filled orbitals have extra stability. |
C. | Pauli's Exclusion Principle | 3. | Pairing of electrons in the orbitals belonging to the same subshell does not take place until each orbital is singly occupied. |
D. | Heisenberg’s Uncertainty Principle | 4. | It is impossible to determine the exact position and exact momentum of a subatomic particle simultaneously. |
5. | In the ground state of atoms, orbitals are filled in the order of their increasing energies. |
A | B | C | D | |
1. | 3 | 5 | 1 | 2 |
2. | 1 | 2 | 3 | 4 |
3. | 3 | 5 | 1 | 4 |
4. | 4 | 5 | 3 | 2 |
Match the following:
Column I | Column II | ||
A. | X-rays | 1. | |
B. | Ultraviolet wave (UV) | 2. | |
C. | Long radio waves | 3. | |
D. | Microwave | 4. |
A | B | C | D | |
1. | 4 | 1 | 3 | 2 |
2. | 1 | 4 | 2 | 3 |
3. | 1 | 4 | 3 | 2 |
4. | 4 | 3 | 1 | 2 |
Assertion (A): | All isotopes of a given element show the same type of chemical behaviour. |
Reason (R): | The chemical properties of an atom are controlled by the number of electrons in the atom. |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True but (R) is False. |
4. | (A) is False but (R) is True. |
A 25-watt bulb emits monochromatic yellow light with a wave length of 0.57µm. The rate of emission of quanta per second would be :
1. 7.17 × 10–19 s–1
2. 4.13 × 1016 s–1
3 . 7.17 × 1019 s–1
4 . 1.26 × 1020 s–1
The wavelength of light emitted when the electron in a H atom undergoes the transition from an energy level with n = 4 to an energy level with n = 2, is :
1. 586 mm
2. 486 nm
3. 523 nm
4. 416 pm
The wave number for the longest wavelength transition in the Balmer series of atomic hydrogen would be :
\(1 . 1 . 52 \times 10^{6} m^{- 1}\)
\(2 . 3 . 14 \times 10^{6} \left(cm\right)^{- 1}\)
\(3 . 15 . 2 \times 10^{6} m^{- 1}\)
\(4 . 1 . 52 \times 10^{6} \left(cm\right)^{- 1}\)
If the photon detector receives a total of 3.15 J from the radiation of 600 nm, the number of photons received by the detector would be:
If the velocity of the electron is 1.6 × 106 . The de Broglie wavelength associated with this electron is:
Match the following species with their corresponding ground state electronic configuration.
Atom/Ion | Electronic configuration | ||
A. | Cu | 1. | |
B. | Cu2+ | 2. | |
C. | Zn2+ | 3. | |
D. | Cr3+ | 4. | |
5. |
A | B | C | D | |
1. | 4 | 2 | 5 | 1 |
2. | 3 | 4 | 1 | 5 |
3. | 3 | 2 | 1 | 4 |
4. | 4 | 2 | 1 | 3 |