General Characteristics of Quantum Numbers
Quantum numbers are fundamental to understanding the behavior of electrons within atoms. They provide a complete “address” of an electron, defining its energy, location, and properties. Together, they explain the arrangement of electrons in atoms, chemical bonding, and periodic trends. General Characteristics of Quantum Numbers
Key Characteristics of Quantum Numbers
- Pauli Exclusion Principle: No two electrons in an atom have the same set of four quantum numbers.
- Quantization: Quantum numbers take only discrete values, explaining defined electron energy levels.
- Principal Quantum Number (n): Defines the main energy level/shell.
- Azimuthal Quantum Number (l): Determines orbital shape (s, p, d, f).
- Magnetic Quantum Number (m): Specifies orbital orientation in space.
- Spin Quantum Number (s): Indicates electron spin (+½ or –½).
- Energy & Stability: Lower n and l values fill first (Aufbau principle).
Illustration of Quantum Numbers
Figure: Representation of quantum numbers and orbital shapes
MCQs. General Characteristics of Quantum Numbers
- The azimuthal quantum number (l) determines:
a) Energy level
b) Orbital shape ✅
c) Orbital orientation
d) Electron spin - The magnetic quantum number (m) ranges between:
a) 0 to n
b) –l to +l ✅
c) –n to +n
d) +½ or –½ - Which principle states no two electrons can have the same set of quantum numbers?
a) Hund’s Rule
b) Aufbau Principle
c) Pauli Exclusion Principle ✅
d) Bohr’s Postulate
FAQs General Characteristics of Quantum Number
Q1: What is the principal quantum number?
Ans: It defines the main energy level of an electron. Higher n means higher energy.
Q2: How does l affect orbital shape?
Ans: l determines orbital shape: s (spherical), p (dumbbell), d (cloverleaf), f (complex).
Q3: Why is spin quantum number important?
Ans: Spin affects magnetic properties and how electrons pair within orbitals.
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