MCQ Detailed View

In atomic theory, quantum numbers are used to describe the unique state of an electron in an atom. They are numerical values that specify the energy, shape, and orientation of electron orbitals. There are four main quantum numbers: principal (n), azimuthal or angular momentum (l), magnetic (m), and spin (s).

The principal quantum number (n) determines the energy level and distance of the electron from the nucleus. The azimuthal quantum number (l) defines the shape of the orbital (s, p, d, f). The magnetic quantum number (m) indicates the orientation of the orbital in space. The spin quantum number (s) specifies the spin direction of the electron, either +½ or -½.

Quantum numbers are essential for understanding electron configurations, chemical bonding, and periodic properties of elements. They help predict how electrons fill orbitals according to the Pauli Exclusion Principle and Hund’s Rule.

Other options are incorrect. Quantum numbers are not simply arithmetical, geometric, or logical values—they are numerical values that represent electron properties quantitatively. Their numerical nature allows chemists to calculate energy levels, orbital shapes, and electron arrangements precisely.

Understanding quantum numbers is fundamental in inorganic chemistry and atomic structure studies. They provide insight into chemical reactivity, spectral properties, and magnetic behavior of atoms. By using numerical quantum numbers, students can explain patterns in the periodic table, orbital diagrams, and the behavior of electrons in molecules.

Thus, quantum numbers are numerical values that describe the energy, shape, orientation, and spin of electrons, making them a key concept in atomic theory and inorganic chemistry.