Quantum Numbers Class 11 Chemistry

Quantum Numbers Class 11 Chemistry
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Quantum numbers are sets of numerical values that describe the unique quantum state of an electron in an atom. These numbers arise from the solutions to the Schrödinger equation for the hydrogen atom and define the properties of atomic orbitals and the electrons in those orbitals. There are four quantum numbers:
1. Principal Quantum Number (n):
- Symbol: n
- Description: Determines the energy level and size of the orbital. It can take positive integer values (1, 2, 3, ...).
- Example: For n = 1 , the electron is in the first energy level (closest to the nucleus).
2. Angular Momentum Quantum Number (l):
- Symbol: l
- Description: Determines the shape of the orbital. It can take integer values from 0 to n-1 .
- Example: For n = 3 , l can be 0, 1, or 2, corresponding to s, p, and d orbitals, respectively.
3. Magnetic Quantum Number (m):
- Symbol: m
- Description: Determines the orientation of the orbital in space. It can take integer values from -l to +l, including zero.
- Example: For l = 1 (p orbital), m_l can be -1, 0, or +1.
4. Spin Quantum Number (s):
- Symbol: s
- Description: Determines the spin orientation of the electron. It can take values of +1/2 or -1/2.
- Example: An electron in an orbital can have a spin of +1/2 (spin-up) or -1/2 (spin-down).
These quantum numbers are essential in quantum mechanics to describe the position and energy of electrons in atoms, and they follow the Pauli exclusion principle, which states that no two electrons in an atom can have the same set of all four quantum numbers.
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