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प्रश्न
Match the quantum numbers with the information provided by these.
| Quantum number | Information provided |
| (i) Principal quantum number | (a) orientation of the orbital |
| (ii) Azimuthal quantum number | (b) energy and size of orbital |
| (iii) Magnetic quantum number | (c) spin of electron |
| (iv) Spin quantum number | (d) shape of the orbital |
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उत्तर
| Quantum number | Information provided |
| (i) Principal quantum number | (b) energy and size of orbital |
| (ii) Azimuthal quantum number | (d) shape of the orbital |
| (iii) Magnetic quantum number | (a) orientation of the orbital |
| (iv) Spin quantum number | (c) spin of electron |
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संबंधित प्रश्न
Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l = 2.
Choose the correct option.
“No two electrons in the same atoms can have identical set of four quantum numbers”. This statement is known as -
Choose the correct option.
Principal Quantum number describes -
State Hund’s rule of maximum multiplicity with a suitable example.
State the order of filling atomic orbitals following Aufbau principle.
Explain the anomalous behaviour of copper.
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 3, l = 2
Write condensed orbital notation of electronic configuration of the following element:
Carbon (Z = 6)
Write condensed orbital notation of electronic configuration of the following element:
Oxygen (Z = 8)
Draw shapes of 2p orbitals.
Which one of the following orders is CORRECT in case of energy of the given subshells?
P: n = 4; l = 3
Q: n = 5; I = 1
R: n = 5; l = 0
S: n = 4; l = 2
The three electrons have the following set of quantum numbers:
X = 6, 1, −1, `+1/2`
Y = 6, 0, 0, `+1/2`
Z = 5, 1, 0, `+1/2`
Identify the CORRECT statement.
Which one of the following is NOT possible?
In which of the following pairs, the ions are iso-electronic?
(i) \[\ce{Na^{+}, Mg^{2+}}\]
(ii) \[\ce{Al3^{+}, O-}\]
(iii) \[\ce{Na+ , O2-}\]
(iv) \[\ce{N3-, Cl-}\]
The arrangement of orbitals on the basis of energy is based upon their (n + l) value. Lower the value of (n + l), lower is the energy. For orbitals having same values of (n + l), the orbital with lower value of n will have lower energy.
Based upon the above information, solve the questions given below:
Which of the following orbitals has the lowest energy?
5p, 5d, 5f, 6s, 6p
Which of the following is the correct plot for the probability density ψ2 (r) as a function of distance 'r' of the electron from the nucleus for 2s orbitals?
Which of the following is not the permissible arrangement of electrons in an atom?
Which one of the following laws will represent the pairing of electrons in a subshell after each orbital is filled with one electron?
