Advertisements
Advertisements
Question
Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l =3.
Solution
For n = 4 and l = 3
The orbital is 4f.
APPEARS IN
RELATED QUESTIONS
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 -
Explain the anomalous behaviour of copper.
Explain the anomalous behaviour of chromium.
Write condensed orbital notation of electronic configuration of the following element:
Carbon (Z = 6)
Draw shapes of 2p orbitals.
The designation of a subshell with n = 6 and l = 2 is ____________.
Total number of orbitals associated with third shell will be ______.
Orbital angular momentum depends on ______.
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.
4s, 3s, 3p, 4d
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?
In the case of R, S configuration the group having the highest priority is ______.
Which one of the following laws will represent the pairing of electrons in a subshell after each orbital is filled with one electron?
