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प्रश्न
Indicate the number of unpaired electron in:
Cr (Z = 24)
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उत्तर
Cr (Z = 24): 1s2 2s2 2p6 3s2 3p6 4s1 3d5
Orbital diagram:
| ↑↓ | ↑↓ | ↑↓ | ↑↓ | ↑↓ | ↑↓ | ↑↓ | ↑↓ | ↑↓ | ↑ | ↑ | ↑ | ↑ | ↑ | ↑ |
| 1s | 2s | 2p | 3s | 3p | 4s | 3d | ||||||||
Number of unpaired electrons = 6
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संबंधित प्रश्न
Using s, p, d notations, describe the orbital with the following quantum numbers n = 3; l =1.
Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l =3.
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Define the term Electronic configuration.
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 4, l = 2
Write condensed orbital notation of electronic configuration of the following element:
Calcium (Z = 20)
Write a note on ‘Principal Quantum number.
Indicate the number of unpaired electrons in \[\ce{Si}\] (Z = 14).
The designation of a subshell with n = 6 and l = 2 is ____________.
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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.
The probability density plots of 1s and 2s orbitals are given in Figure:
The density of dots in a region represents the probability density of finding electrons in the region.
On the basis of above diagram which of the following statements is incorrect?
Number of angular nodes for 4d orbital is ______.
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4s, 3s, 3p, 4d
What is the difference between the terms orbit and orbital?
Match the following species with their corresponding ground state electronic configuration.
| Atom / Ion | Electronic configuration |
| (i) \[\ce{Cu}\] | (a) 1s2 2s2 2p6 3s2 3p6 3d10 |
| (ii) \[\ce{Cu^{2+}}\] | (b) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 |
| (iii) \[\ce{Zn^{2+}}\] | (c) 1s2 2s2 2p6 3s2 3p6 3d10 4s1 |
| (iv) \[\ce{Cr^{3+}}\] | (d) 1s2 2s2 2p6 3s2 3p6 3d9 |
| (e) 1s2 2s2 2p6 3s2 3p6 3d3 |
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 |
Match species given in Column I with the electronic configuration given in Column II.
| Column I | Column II |
| (i) \[\ce{Cr}\] | (a) [Ar]3d84s0 |
| (ii) \[\ce{Fe^{2+}}\] | (b) [Ar]3d104s1 |
| (iii) \[\ce{Ni^{2+}}\] | (c) [Ar]3d64s0 |
| (iv) \[\ce{Cu}\] | (d) [Ar] 3d54s1 |
| (e) [Ar]3d64s2 |
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?
In the case of R, S configuration the group having the highest priority is ______.
What are the possible values of magnetic quantum number for p orbital?
