Quantum Numbers, Atomic Orbitals, and Electron Configurations

What does the principal quantum number (n) primarily describe for an electron in an atom?

• The shape of the electron's orbital.

• The orientation of the electron's orbital in space.

• The energy level and average distance of the electron from the nucleus.

• The spin direction of the electron.

If an electron has a principal quantum number (n) of 3, which of the following is a possible value for its angular momentum quantum number (l)?

• 3

• 4

• 2

• -1

How many d orbitals are present in a given energy level?

• 1

• 3

• 5

• 7

What is the maximum number of electrons that can occupy a single atomic orbital, and what must be true about their spin quantum numbers?

• One electron, with a spin of +1/2.

• Two electrons, with the same spin quantum number.

• Two electrons, with opposite spin quantum numbers.

• Three electrons, with varying spin quantum numbers.

Which of the following represents the correct order of filling atomic orbitals according to the Aufbau principle?

• 1s, 2s, 2p, 3s, 3p, 3d, 4s

• 1s, 2s, 2p, 3s, 3p, 4s, 3d

• 1s, 2s, 3s, 2p, 3p, 4s, 3d

• 1s, 2s, 2p, 3p, 3s, 4s, 3d

What does Hund's Rule state regarding the filling of degenerate orbitals?

• Each orbital in a subshell must be singly occupied with electrons of the same spin before any one orbital is doubly occupied.

• Electrons must occupy the lowest energy orbitals first.

• No two electrons in an atom can have the same set of four quantum numbers.

• Electrons fill orbitals in order of increasing energy.

Which block on the periodic table corresponds to the filling of d-orbitals?

• s-block

• p-block

• d-block

• f-block

An atom is considered paramagnetic if its orbital diagram shows which characteristic?

• All electrons are paired.

• It has at least one unpaired electron.

• It has a full outer shell.

• It is not affected by a magnetic field.