Question

1.) which of the following is the correct order of filling the orbitals?
(1 point)
1s, 2s, 2p, 3s
1s, 2s, 3s, 3p
1s, 2s, 2p, 2f
1s, 2s, 2p, 2d
2.)
in the orbital diagram above, which of the following does it violate?
pauli exclusion principle
aufbau principle
hund’s rule
3.) a single f-orbital can accommodate up to ______ electrons with opposite spin. (1 point)
all of the answers
14
10
2

Explanation:

Question 1

Step1: Recall orbital filling rules

The Aufbau principle states that electrons fill orbitals in order of increasing energy. The energy order for orbitals is \(1s < 2s < 2p < 3s < 3p < 4s < 3d \dots\) Also, \(f\) orbitals start at \(n = 4\) (\(4f\)) and \(d\) orbitals start at \(n = 3\) (\(3d\)). So \(2f\) and \(2d\) don't exist. And \(3s\) comes after \(2p\), not \(3s\) before \(2p\) related steps.

Step2: Evaluate each option

• Option 1: \(1s, 2s, 2p, 3s\) follows the energy order ( \(1s\) filled, then \(2s\), then \(2p\), then \(3s\) as energy increases).
• Option 2: \(1s, 2s, 3s, 3p\) is wrong because \(2p\) (lower energy than \(3s\)) should be filled before \(3s\).
• Option 3: \(2f\) doesn't exist ( \(f\) orbitals start at \(n = 4\)), so invalid.
• Option 4: \(2d\) doesn't exist ( \(d\) orbitals start at \(n = 3\)), so invalid.

Step1: Recall electron filling principles

• Pauli Exclusion Principle: No two electrons in an orbital have same spin (max 2 electrons with opposite spins per orbital).
• Aufbau Principle: Electrons fill lowest energy orbitals first.
• Hund’s Rule: Electrons fill degenerate (same energy) orbitals singly with parallel spins before pairing.

Step2: Analyze the orbital diagram

The \(2p\) orbitals are degenerate. In the diagram, one \(2p\) orbital has paired electrons while another is not filled singly first. This violates Hund’s Rule (which says electrons should occupy degenerate orbitals singly first).

Step1: Recall orbital capacity

A single orbital (regardless of type: \(s, p, d, f\)) can hold a maximum of 2 electrons with opposite spins (Pauli Exclusion Principle). An \(f\) subshell has 7 orbitals, so total 14 electrons for \(f\) subshell, but a single \(f\)-orbital holds 2.

Step2: Evaluate options

• "All of the answers" is wrong.
• 14 is for the \(f\) subshell (7 orbitals), not a single orbital.
• 10 is for \(d\) subshell (5 orbitals, 2 each: \(5\times2 = 10\)), not \(f\) orbital.
• 2: A single orbital (including \(f\)-orbital) can hold 2 electrons with opposite spins.

Answer:

1s, 2s, 2p, 3s

Question 2