Advertisements
Advertisements
Question
Write condensed orbital notation of electronic configuration of the following element:
Carbon (Z = 6)
Advertisements
Solution
| Element | Condensed orbital notation |
| Carbon (Z = 6) | [He] 2s2 2p2 |
APPEARS IN
RELATED QUESTIONS
Using s, p, d notations, describe the orbital with the following quantum numbers n = 4; l = 2.
Choose the correct option.
Principal Quantum number describes -
State Heisenberg uncertainty principle.
State Hund’s rule of maximum multiplicity with a suitable example.
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 2, l = 1
Write orbital notations for the electron in orbitals with the following quantum numbers.
n = 3, l = 2
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:
Oxygen (Z = 8)
Write condensed orbital notation of electronic configuration of the following element:
Chlorine (Z = 17)
If n = 3, what are the quantum number l and m?
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 electron in:
Cr (Z = 24)
Which mineral among the following contains vanadium in it?
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.
Which of the following options does not represent ground state electronic configuration of an atom?
Which of the following orbitals are degenerate?
3dxy, 4dxy 3dz2, 3dyz, 4dyz, 4dz2
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
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 not the permissible arrangement of electrons in an atom?
In the case of R, S configuration the group having the highest priority is ______.
Which of the following element do not follow Aufbau principle?
Which one of the following laws will represent the pairing of electrons in a subshell after each orbital is filled with one electron?
