Question

part d - rules of electron configurations
what rule is being violated in each electron configuration below? explain your answer for each.
(1)
↑↓
1s
↑↓
2s
↑↓
2p
——
(2)
↑↓
1s
↑↓
2s
↑↓
↑↓
↑↓
2p
——
3s
↑↓
↑↓
↑
3p
(3)
↑↓
1s
↑↓
2s
↑↓
↑↓
↑↓
↑
2p
↑↓
3s
↑↓
↑↓
↑↓
↑
3p
(4)
↑↓
1s
↑↓
2s
↑↓
↑↓
↑↓
↑↓
2p
↑↓
3s
↑↓
↑↓
↑↓
↑↓
3p
↑↓
↑↓
↑↓
↑↓
↑↓
3d

Explanation:

For Configuration (1):

The electron configuration for (1) has the 2p subshell with only 2 electrons (shown as two orbitals with paired electrons, but 2p should have 3 orbitals. The Aufbau principle (or filling order) and Hund's rule: 2p has 3 orbitals, electrons should fill singly first. Also, the 2p subshell here is not filled correctly in terms of orbital filling. Wait, more accurately, the 2p subshell has 3 orbitals. In (1), the 2p is shown with two orbitals (the lines) but 2p should have 3. Wait, no, looking at the diagram, (1) has 1s², 2s², and then 2p with two orbitals (each with paired electrons) but 2p has 3 orbitals. Also, the Pauli exclusion principle: each orbital can hold max 2 electrons (spin - paired). But the main issue here is the Aufbau Principle? No, wait, the 2p subshell: the correct filling is that 2p has 3 orbitals. In (1), after 2s², the 2p is not filled with electrons in all 3 orbitals (it has only 2 orbitals shown? Wait, the diagram for (1) shows 1s (filled), 2s (filled), then 2p with two lines (orbitals) but 2p has 3 orbitals. So the error is violating the Aufbau Principle (filling order) or more likely, the Hund's Rule? Wait, no, the 2p subshell: the number of orbitals. Wait, 2p has 3 orbitals. In (1), the 2p is drawn with two orbitals (the lines), which is wrong. Also, the electron count: 1s² (2), 2s² (2), 2p²? But 2p can have up to 6 electrons. Wait, maybe the problem is that the 2p subshell has electrons paired in orbitals before all orbitals have one electron (Hund's rule violation) or the Pauli exclusion (but Pauli is about spin). Wait, let's re - examine:

• Pauli Exclusion Principle: Each orbital can hold at most 2 electrons with opposite spins. In (1), the 1s and 2s are filled correctly (2 electrons each, opposite spins). But the 2p subshell: the diagram shows two orbitals (lines) with paired electrons, but 2p has 3 orbitals. So the error is that the 2p subshell is not using all 3 orbitals. Also, the electron configuration here might be missing the third 2p orbital. So the rule violated is the Aufbau Principle (filling orbitals in the correct subshell order) or more accurately, the Hund's Rule (electrons fill orbitals singly before pairing) and the correct orbital filling for 2p (3 orbitals). Wait, another approach: the 2p subshell has 3 orbitals. In (1), after 2s², the 2p electrons are placed in two orbitals (paired) instead of filling all three orbitals with one electron each first (Hund's rule). Also, the 3s and 3p are not present, but the main issue with (1) is that the 2p subshell has only 2 orbitals (lines) drawn, but 2p has 3 orbitals, so the orbital filling (Aufbau and orbital existence) is wrong. But more precisely, the Pauli Exclusion Principle is not violated here (each orbital has 2 electrons with opposite spins), but the Hund's Rule and the correct number of orbitals in 2p. Wait, maybe the key is that the 2p subshell should have 3 orbitals, and in (1) it's drawn with 2, so the rule violated is the Aufbau Principle (filling the correct subshell orbitals) or the orbital filling (number of orbitals in a subshell).

Wait, let's list the rules:

1. Aufbau Principle: Electrons fill the lowest - energy orbitals first.
2. Pauli Exclusion Principle: No two electrons in the same atom can have the same set of four quantum numbers (max 2 per orbital, opposite spins).
3. Hund's Rule: Electrons in degenerate (same energy) orbitals fill singly first, with parallel spins, before pairing.

For (1):

• The 2p subshell has 3 degenerate orbitals. In (1), the 2p is shown with…

Answer:

The electron configuration for (1) has the 2p subshell with only 2 electrons (shown as two orbitals with paired electrons, but 2p should have 3 orbitals. The Aufbau principle (or filling order) and Hund's rule: 2p has 3 orbitals, electrons should fill singly first. Also, the 2p subshell here is not filled correctly in terms of orbital filling. Wait, more accurately, the 2p subshell has 3 orbitals. In (1), the 2p is shown with two orbitals (the lines) but 2p should have 3. Wait, no, looking at the diagram, (1) has 1s², 2s², and then 2p with two orbitals (each with paired electrons) but 2p has 3 orbitals. Also, the Pauli exclusion principle: each orbital can hold max 2 electrons (spin - paired). But the main issue here is the Aufbau Principle? No, wait, the 2p subshell: the correct filling is that 2p has 3 orbitals. In (1), after 2s², the 2p is not filled with electrons in all 3 orbitals (it has only 2 orbitals shown? Wait, the diagram for (1) shows 1s (filled), 2s (filled), then 2p with two lines (orbitals) but 2p has 3 orbitals. So the error is violating the Aufbau Principle (filling order) or more likely, the Hund's Rule? Wait, no, the 2p subshell: the number of orbitals. Wait, 2p has 3 orbitals. In (1), the 2p is drawn with two orbitals (the lines), which is wrong. Also, the electron count: 1s² (2), 2s² (2), 2p²? But 2p can have up to 6 electrons. Wait, maybe the problem is that the 2p subshell has electrons paired in orbitals before all orbitals have one electron (Hund's rule violation) or the Pauli exclusion (but Pauli is about spin). Wait, let's re - examine:

• Pauli Exclusion Principle: Each orbital can hold at most 2 electrons with opposite spins. In (1), the 1s and 2s are filled correctly (2 electrons each, opposite spins). But the 2p subshell: the diagram shows two orbitals (lines) with paired electrons, but 2p has 3 orbitals. So the error is that the 2p subshell is not using all 3 orbitals. Also, the electron configuration here might be missing the third 2p orbital. So the rule violated is the Aufbau Principle (filling orbitals in the correct subshell order) or more accurately, the Hund's Rule (electrons fill orbitals singly before pairing) and the correct orbital filling for 2p (3 orbitals). Wait, another approach: the 2p subshell has 3 orbitals. In (1), after 2s², the 2p electrons are placed in two orbitals (paired) instead of filling all three orbitals with one electron each first (Hund's rule). Also, the 3s and 3p are not present, but the main issue with (1) is that the 2p subshell has only 2 orbitals (lines) drawn, but 2p has 3 orbitals, so the orbital filling (Aufbau and orbital existence) is wrong. But more precisely, the Pauli Exclusion Principle is not violated here (each orbital has 2 electrons with opposite spins), but the Hund's Rule and the correct number of orbitals in 2p. Wait, maybe the key is that the 2p subshell should have 3 orbitals, and in (1) it's drawn with 2, so the rule violated is the Aufbau Principle (filling the correct subshell orbitals) or the orbital filling (number of orbitals in a subshell).

Wait, let's list the rules:

1. Aufbau Principle: Electrons fill the lowest - energy orbitals first.
2. Pauli Exclusion Principle: No two electrons in the same atom can have the same set of four quantum numbers (max 2 per orbital, opposite spins).
3. Hund's Rule: Electrons in degenerate (same energy) orbitals fill singly first, with parallel spins, before pairing.

For (1):

• The 2p subshell has 3 degenerate orbitals. In (1), the 2p is shown with two orbitals (lines) with paired electrons. So electrons are paired in orbitals before all orbitals have one electron (violates Hund's Rule). Also, the number of orbitals in 2p is 3, but the diagram shows 2, which is[SSE Completed, Client Connection Error][SSE onError error]