NET Chemistry MCQs

A d subshell contains five orbitals.
At two electrons per orbital, it holds ten electrons.

The Aufbau principle guides ground-state configurations.
Actual filling order follows orbital energies.

Hund's rule minimizes electron repulsion in degenerate orbitals.
Unpaired electrons have parallel spins before pairing.

The principle limits each orbital to two opposite-spin electrons.
It is fundamental to electron configuration.

The ground state is the most stable configuration.
Energy absorption can promote electrons to excited states.

Excited atoms can return to lower levels by emitting energy.
Atomic spectra arise from these transitions.

First ionization energy removes the first electron from a neutral gaseous atom.
Successive ionization energies remove additional electrons.

Thomson's cathode-ray experiments revealed negatively charged particles.
He proposed an early model with electrons in positive matter.

Chadwick identified the neutral nuclear particle in 1932.
Neutrons explain isotopic mass differences.

Quantum mechanics describes electron probability distributions.
An orbital can hold up to two electrons with opposite spins.

The Pauli exclusion principle allows two electrons per orbital.
They must have opposite spin quantum numbers.

An s subshell contains one orbital.
It can hold a maximum of two electrons.