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प्रश्न
Explain the anomalous behaviour of chromium.
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उत्तर
- Chromium (Cr) has atomic number 24.
- Its expected electronic configuration is 1s2 2s2 2p6 3s2 3p6 4s2 3d4.
- The 3d orbital is less stable, as it is not half-filled.
- Due to inter-electronic repulsion forces, one 4s electron enters into the 3d orbital. This makes the 4s and 3d orbitals half-filled, which gives extra stability, and the electronic configuration of Cr becomes 1s2 2s2 2p6 3s2 3p6 4s1 3d5.
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संबंधित प्रश्न
Using s, p, d notations, describe the orbital with the following quantum numbers n = 3; l =1.
Define the term Electronic configuration.
State Hund’s rule of maximum multiplicity with a suitable example.
State the order of filling atomic orbitals following Aufbau principle.
Write condensed orbital notation of electronic configuration of the following element:
Silicon (Z = 14)
Write condensed orbital notation of electronic configuration of the following element:
Chlorine (Z = 17)
Write condensed orbital notation of electronic configuration of the following element:
Calcium (Z = 20)
If n = 3, what are the quantum number l and m?
The electronic configuration of oxygen is written as 1s2 2s2 \[\ce{2p^2_{{x}}}\] \[\ce{2p^1_{{y}}}\] \[\ce{2p^1_{{z}}}\] and not as 1s2 2s2 \[\ce{2p^2_{{x}}}\], \[\ce{2p^2_{{y}}}\] \[\ce{2p^0_{{z}}}\], Explain.
The principal quantum number (n) and magnetic quantum number (ml) for the valence electrons of rubidium atom (Z = 37) are ____________ respectively.
Which mineral among the following contains vanadium in it?
The designation of a subshell with n = 6 and l = 2 is ____________.
How many electrons in 19K have n = 3, l = 1?
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.
How many electrons can fit in the orbital for which n = 4 and l = 2?
The number of radial nodes for 3p orbital is ______.
The pair of ions having same electronic configuration is ______.
Which of the following sets of quantum numbers are correct?
| `n` | `l` | `m_l` | |
| (i) | 1 | 1 | +2 |
| (ii) | 2 | 1 | +1 |
| (iii) | 3 | 2 | –2 |
| (iv) | 3 | 4 | –2 |
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) \[\ce{N3-, Cl-}\]
Which of the following statements concerning the quantum numbers are correct?
(i) Angular quantum number determines the three dimensional shape of the orbital.
(ii) The principal quantum number determines the orientation and energy of the orbital.
(iii) Magnetic quantum number determines the size of the orbital.
(iv) Spin quantum number of an electron determines the orientation of the spin of electron relative to the chosen axis.
Calculate the total number of angular nodes and radial nodes present in 3p orbital.
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Based upon the above information, arrange the following orbitals in the increasing order of energy.
4s, 3s, 3p, 4d
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, arrange the following orbitals in the increasing order of energy.
5p, 4d, 5d, 4f, 6s
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?
4d, 4f, 5s, 5p
The electronic configuration of valence shell of Cu is 3d104s1 and not 3d94s2. How is this configuration explained?
Choose the INCORRECT statement
Which of the following is not the permissible arrangement of electrons in an atom?
In assigning R - S configuration, which among the following groups has highest priority?
What are the possible values of magnetic quantum number for p orbital?
