Advertisements
Advertisements
Question
Write electronic configurations of \[\ce{Fe, Fe2+, Fe3+}\].
Advertisements
Solution
| Species | Orbital notation |
| \[\ce{Fe}\] | 1s2 2s2 2p6 3s2 3p6 4s2 3d6 OR [Ar] 4s23d6 |
| \[\ce{Fe2+}\] | 1s2 2s2 2p6 3s2 3p6 3d6 OR [Ar] 3d6 |
| \[\ce{Fe3+}\] | 1s2 2s2 2p6 3s2 3p6 3d5 OR [Ar] 3d5 |
APPEARS IN
RELATED QUESTIONS
Using s, p, d notations, describe the orbital with the following quantum numbers n = 3; l =1.
Choose the correct option.
p-orbitals are _________ in shape.
Choose the correct option.
“No two electrons in the same atoms can have identical set of four quantum numbers”. This statement is known as -
State Heisenberg uncertainty principle.
State and explain Pauli’s exclusion principle.
State Hund’s rule of maximum multiplicity with a suitable example.
Write condensed orbital notation of electronic configuration of the following element:
Lithium (Z = 3)
Write condensed orbital notation of electronic configuration of the following element:
Calcium (Z = 20)
Draw shapes of 2p orbitals.
Write a note on ‘Principal Quantum number.
Using the concept of quantum numbers, calculate the maximum numbers of electrons present in the ‘M’ shell. Give their distribution in shells, subshells, and orbitals.
Indicate the number of unpaired electrons in \[\ce{Si}\] (Z = 14).
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
Which one of the following is NOT possible?
The number of radial nodes for 3p 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 orbitals are degenerate?
3dxy, 4dxy 3dz2, 3dyz, 4dyz, 4dz2
Calculate the total number of angular nodes and radial nodes present in 3p orbital.
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 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 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 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 |
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?
