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प्रश्न
Write condensed orbital notation of electronic configuration of the following element:
Carbon (Z = 6)
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उत्तर
| Element | Condensed orbital notation |
| Carbon (Z = 6) | [He] 2s2 2p2 |
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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 = 2.
Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l =3.
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 Heisenberg uncertainty principle.
State and explain Pauli’s exclusion principle.
State Hund’s rule of maximum multiplicity with a suitable example.
Explain the anomalous behaviour of chromium.
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:
Oxygen (Z = 8)
Write condensed orbital notation of electronic configuration of the following element:
Silicon (Z = 14)
Write a note on ‘Principal Quantum number.
Indicate the number of unpaired electron in:
Cr (Z = 24)
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 of the following has a greater number of electrons than neutrons?
(Mass number of Mg, C, O and Na is 24, 12, 16 and 23 respectively).
The number of radial nodes for 3p orbital is ______.
Number of angular nodes for 4d orbital is ______.
Total number of orbitals associated with third shell will be ______.
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 |
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.
1s, 2s, 3s, 2p
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
The electronic configuration of valence shell of Cu is 3d104s1 and not 3d94s2. How is this configuration explained?
What is the difference between the terms orbit and 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 |
Choose the INCORRECT statement
Which of the following is not the permissible arrangement of electrons in an atom?
