answer the following questions:
1. identify the element with the given electron configuration:
a. $1s^2 2s^2 2p^6$
b. $1s^2 2s^1$
c. $1s^2 2s^2 2p^6 3s^2 3p^4$
d. $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6$
2. list the maximum number of total electrons each sublevel can hold:
3. list the 4 sublevels in order of increasing energy
4. which of the following orbital diagrams disobey hunds rule:
a. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑, ↑, ↑)
b. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑↓, ↑, empty)
c. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑, ↓, ↑)
5. which of the following orbital diagrams obey the aufbau principle:
a. orbital diagram with 1s (↑↓), 2s (↑↑), 2p (↑, empty, empty)
b. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑, empty, ↑)
c. orbital diagram with 1s (↑↓), 2s (↑, empty), 2p (↑, empty, empty)
d. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑↓, empty, empty)
6. which orbital diagram obeys the pauli exclusion principle:
a. orbital diagram with 1s (↓)
b. orbital diagram with 1s (↑↑)
c. orbital diagram with 1s (↓↑)

Question

answer the following questions:
1. identify the element with the given electron configuration:
   a. $1s^2 2s^2 2p^6$
   b. $1s^2 2s^1$
   c. $1s^2 2s^2 2p^6 3s^2 3p^4$
   d. $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6$
2. list the maximum number of total electrons each sublevel can hold:
3. list the 4 sublevels in order of increasing energy
4. which of the following orbital diagrams disobey hunds rule:
   a. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑, ↑, ↑)
   b. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑↓, ↑, empty)
   c. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑, ↓, ↑)
5. which of the following orbital diagrams obey the aufbau principle:
   a. orbital diagram with 1s (↑↓), 2s (↑↑), 2p (↑, empty, empty)
   b. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑, empty, ↑)
   c. orbital diagram with 1s (↑↓), 2s (↑, empty), 2p (↑, empty, empty)
   d. orbital diagram with 1s (↑↓), 2s (↑↓), 2p (↑↓, empty, empty)
6. which orbital diagram obeys the pauli exclusion principle:
   a. orbital diagram with 1s (↓)
   b. orbital diagram with 1s (↑↑)
   c. orbital diagram with 1s (↓↑)

Accepted Answer

### Question 1a
# Explanation:
## Step1: Calculate total electrons
Sum the exponents: $2 + 2 + 6 = 10$.
## Step2: Identify element
Atomic number = 10, which is Neon (Ne).
# Answer: Neon (Ne)

### Question 1b
# Explanation:
## Step1: Calculate total electrons
Sum exponents: $2 + 1 = 3$.
## Step2: Identify element
Atomic number = 3, which is Lithium (Li).
# Answer: Lithium (Li)

### Question 1c
# Explanation:
## Step1: Calculate total electrons
Sum exponents: $2 + 2 + 6 + 2 + 4 = 16$.
## Step2: Identify element
Atomic number = 16, which is Sulfur (S).
# Answer: Sulfur (S)

### Question 1d
# Explanation:
## Step1: Calculate total electrons
Sum exponents: $2 + 2 + 6 + 2 + 6 + 2 + 6 = 26$ (wait, $1s^2(2) + 2s^2(2) + 2p^6(6) + 3s^2(2) + 3p^6(6) + 4s^2(2) + 3d^6(6)$: $2+2+6+2+6+2+6 = 26$? Wait, no: $2+2=4; +6=10; +2=12; +6=18; +2=20; +6=26$. Atomic number 26 is Iron (Fe). Wait, electron configuration for Fe is $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6$, yes.
## Step2: Identify element
Atomic number 26, Iron (Fe).
# Answer: Iron (Fe)

### Question 2
# Explanation:
## Step1: Recall sublevel electron capacities
- $s$-sublevel: 1 orbital, max $2 \times 1 = 2$ electrons.
- $p$-sublevel: 3 orbitals, max $2 \times 3 = 6$ electrons.
- $d$-sublevel: 5 orbitals, max $2 \times 5 = 10$ electrons.
- $f$-sublevel: 7 orbitals, max $2 \times 7 = 14$ electrons.
# Answer: $s$: 2, $p$: 6, $d$: 10, $f$: 14

### Question 3
# Explanation:
## Step1: Recall energy order
The order of sublevels by increasing energy is $1s < 2s < 2p < 3s$ (wait, the 4 main sublevels? Wait, the first four sublevels in order of increasing energy are $1s$, $2s$, $2p$, $3s$? No, wait, the order is $1s$, $2s$, $2p$, $3s$, $3p$, $4s$, $3d$... But the question says "List the 4 sublevels in order of increasing energy". Typically, the first four sublevels are $1s$, $2s$, $2p$, $3s$ (or $1s$, $2s$, $2p$, $3s$)? Wait, no, the correct order of filling (Aufbau) for the first few sublevels is $1s$, $2s$, $2p$, $3s$, $3p$, $4s$, $3d$... So the first four sublevels in order of increasing energy are $1s$, $2s$, $2p$, $3s$.
# Answer: $1s$, $2s$, $2p$, $3s$

### Question 4
# Explanation:
## Step1: Recall Hund's Rule
Hund's rule: electrons fill degenerate orbitals (same energy) singly first, with parallel spins.
- Option a: $1s^2$, $2s^2$, $2p^3$ (three unpaired electrons in $2p$) – follows Hund's.
- Option b: $2p$ has one orbital with two electrons and one with one, and one empty – violates (should fill singly first).
- Option c: $2p$ electrons have parallel spins (one up, one down, one up – no, wait, spins: first $2p$ is up, second down, third up – no, Hund's requires parallel spins when singly occupied. Wait, no: Hund's rule is that in degenerate orbitals, electrons are placed singly with same spin before pairing. So in option b, $2p$ orbitals: first orbital has two electrons (paired), second has one, third empty. But $2p$ has three orbitals, so electrons should fill each orbital once (singly) before pairing. So for $2p^3$, three electrons, each in a separate $2p$ orbital (singly). For $2p^2$, two electrons in separate orbitals (singly). For $2p^4$, two orbitals with one electron (singly) and one orbital with two (paired). Wait, the electron count here: $1s^2 2s^2$ (4 electrons) + $2p$ electrons: option b has $2p$ with $2 + 1 + 0 = 3$? Wait, no, the diagram: $1s$ (2), $2s$ (2), $2p$: first orbital (paired), second (one), third (empty). So total $2+2+2+1+0=7$ electrons? Wait, no, the diagram: $1s$ (two arrows), $2s$ (two arrows), $2p$: first box (two arrows), second (one), third (empty). So total electrons: $2+2+2+1=7$? Wait, no, each box is an orbital. $1s$ (1 orbital, 2 e⁻), $2s$ (1 orbital, 2 e⁻), $2p$ (3 orbitals). So in option b, $2p$ orbitals: first has 2, second has 1, third has 0. But for $2p^3$, three electrons, each in a $2p$ orbital (singly). For $2p^2$, two electrons in separate $2p$ orbitals (singly). So option b: if the electron count is $1s^2 2s^2 2p^3$? No, $1s^2(2) + 2s^2(2) + 2p^3(3)$ = 7 electrons. But $2p^3$ should have three unpaired electrons (each $2p$ orbital has one). But option b has $2p$ with one orbital paired, one with one, one empty – violates Hund's. Option c: $2p$ orbitals: first (up), second (down), third (up) – spins are not parallel (first up, second down) – violates? Wait, no, the spins: in option c, $2p$ electrons: first is up, second down, third up. So spins are not parallel for the singly occupied orbitals. Wait, no, Hund's rule requires that when electrons are singly occupied in degenerate orbitals, they have the same spin. So in option c, the first $2p$ is up, second down, third up – different spins for the first and second, which are singly occupied? No, first $2p$ has one electron (up), second $2p$ has one (down), third $2p$ has one (up). So two singly occupied orbitals with opposite spins – violates Hund's. Wait, I think I made a mistake. Let's re-express:

Hund's rule: electrons in degenerate orbitals (same energy) are placed in separate orbitals with parallel spins before pairing.

- Option a: $2p$ orbitals: three orbitals, each with one electron (up spin) – follows (parallel spins, singly occupied).
- Option b: $2p$ orbitals: first orbital with two electrons (paired), second with one (up), third empty – violates (should fill each orbital singly first; for $2p^3$, three electrons, each in a separate $2p$ orbital).
- Option c: $2p$ orbitals: first (up), second (down), third (up) – spins are not parallel (first and second are singly occupied with opposite spins) – violates.

Wait, but the question is which DISOBEY Hund's rule. So option b: because it pairs electrons in a $2p$ orbital before filling all $2p$ orbitals singly. For example, if the electron configuration is $1s^2 2s^2 2p^3$, the $2p$ electrons should be in three separate orbitals (singly). If it's $1s^2 2s^2 2p^2$, two separate orbitals (singly). If it's $1s^2 2s^2 2p^4$, two orbitals with one electron (singly) and one with two (paired). But in option b, the $2p$ has one orbital with two, one with one, one with zero – which is incorrect for $2p^3$ (should be three singly occupied) or $2p^2$ (two singly occupied) or $2p^4$ (two singly, one paired). So option b violates Hund's rule.
# Answer: b

### Question 5
# Explanation:
## Step1: Recall Aufbau Principle
Electrons fill orbitals in order of increasing energy: $1s$ → $2s$ → $2p$ → $3s$ → ..., and each orbital holds a maximum of 2 electrons (Pauli), with spins paired after singly filling (Hund, but Aufbau is about order).
- Option A: $2s$ has two up spins – violates Pauli (max 2 electrons, opposite spins).
- Option B: $1s^2$, $2s^2$, $2p^2$ (two electrons in $2p$, each in separate orbitals) – follows Aufbau (fills $1s$, $2s$, then $2p$).
- Option C: Fills $2p$ before $2s$ is full – violates ( $2s$ has one electron, then $2p$ is filled).
- Option D: $2p$ has two electrons in the same orbital (paired) before filling other $2p$ orbitals – violates Hund, but also, $2p$ orbitals should be filled after $2s$ is full. Wait, $1s^2$, $2s^2$, $2p^2$ – no, option D has $2p$ with two electrons in the first $2p$ orbital (paired), but $2p$ has three orbitals. So for $2p^2$, electrons should be in separate $2p$ orbitals (singly). But the Aufbau principle is about the order of filling orbitals (energy order). So $1s$ (lowest energy) is filled first, then $2s$ (next), then $2p$ (next). So:
- Option A: $2s$ has two up spins – invalid (Pauli), so violates Aufbau (since it's an invalid configuration).
- Option B: $1s^2$ (filled), $2s^2$ (filled), $2p^2$ (two electrons in $2p$, each in separate orbitals) – valid, follows Aufbau (fills in order, and within $2p$, follows Hund for $2p^2$).
- Option C: $2s$ has one electron, then $2p$ is filled – violates (should fill $2s$ completely before $2p$).
- Option D: $2p$ has two electrons in the same orbital (paired) for $2p^2$ – violates Hund, but also, the order: $1s$, $2s$, $2p$ – but the $2p$ filling is incorrect. Wait, the electron count: $1s^2$ (2), $2s^2$ (2), $2p^2$ (2) – total 6? No, $2+2+2=6$? Wait, $1s^2$ (2), $2s^2$ (2), $2p^2$ (2) – but $2p$ has three orbitals, so two electrons in $2p$ should be in separate orbitals. Option B has $2p$ with two electrons in separate orbitals (correct for $2p^2$), and $1s$ and $2s$ are filled (each with two electrons, opposite spins). So option B follows Aufbau principle.
# Answer: B

### Question 6
# Explanation:
## Step1: Recall Pauli Exclusion Principle
No two electrons in the same orbital can have the same spin (must be opposite, or max 2 electrons with opposite spins).
- Option a: $1s$ has one electron (spin down) – valid (Pauli allows 1 or 2 electrons, with opposite spins for 2).
- Option b: $1s$ has two electrons with the same spin (both up) – violates Pauli (same orbital, same spin).
- Option c: $1s$ has three electrons – violates Pauli (max 2 electrons per orbital).
So option a obeys Pauli Exclusion principle (has one electron, which is allowed; or if it's a single electron, spin is either up or down – valid).
# Answer: a

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Question

Explanation:

Question 1a

Step1: Calculate total electrons

Step2: Identify element

Step1: Calculate total electrons

Step2: Identify element

Step1: Calculate total electrons

Step2: Identify element

Answer:

Question 1b