the following electron configurations belong to which elements:
11) 1s²2s²2p⁶3s¹ ______
12) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁶ ______
13) kr 5s²4d¹⁰ ______
14) xe 6s²4f¹⁴5d¹⁰6p² ______
15) rn 7s²5f¹⁴6d⁴ ______

determine if the following electron configurations are correct:
16) 1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p⁶5s¹ ______
17) 1s²2s²2p⁶3s³ ______
18) rn 7s²5f⁹6d² ______
19) ar 5s²4d¹⁰5p⁵ ______
20) xe 6s²4f¹⁰ ______

Question

the following electron configurations belong to which elements:
11)  1s²2s²2p⁶3s¹ ______
12)  1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁶ ______
13)  kr 5s²4d¹⁰ ______
14)  xe 6s²4f¹⁴5d¹⁰6p² ______
15)  rn 7s²5f¹⁴6d⁴ ______

determine if the following electron configurations are correct:
16)  1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p⁶5s¹ ______
17)  1s²2s²2p⁶3s³ ______
18)  rn 7s²5f⁹6d² ______
19)  ar 5s²4d¹⁰5p⁵ ______
20)  xe 6s²4f¹⁰ ______

Accepted Answer

### Question 11
# Explanation:
## Step1: Calculate total electrons
Sum the exponents: $2 + 2 + 6 + 1 = 11$.
## Step2: Identify element
Atomic number 11 is Sodium (Na).
# Answer: Sodium (Na)

### Question 12
# Explanation:
## Step1: Calculate total electrons
Sum exponents: $2+2+6+2+6+2+10+6+2+6 = 46$? Wait, no: $1s^2(2)+2s^2(2)+2p^6(6)+3s^2(2)+3p^6(6)+4s^2(2)+3d^{10}(10)+4p^6(6)+5s^2(2)+4d^6(6)$. Sum: $2+2=4; +6=10; +2=12; +6=18; +2=20; +10=30; +6=36; +2=38; +6=44$. Wait, maybe I miscounted. Wait, $1s^2 2s^2 2p^6$ (10) $3s^2 3p^6$ (8, total 18) $4s^2 3d^{10} 4p^6$ (18, total 36) $5s^2 4d^6$ (8, total 44). Wait, atomic number 44 is Ruthenium (Ru)? Wait, no, maybe the electron config has a typo? Wait, correct for Ru: $[Kr] 4d^7 5s^1$ or $[Kr] 4d^6 5s^2$. Wait, $Kr$ is 36, so $36 + 2 + 6 = 44$. So element with atomic number 44 is Ruthenium (Ru).
## Step2: Confirm
Atomic number 44: Ru.
# Answer: Ruthenium (Ru)

### Question 13
# Explanation:
## Step1: Find Kr's atomic number
Krypton (Kr) has atomic number 36.
## Step2: Add electrons from configuration
$5s^2 4d^{10}$ has $2 + 10 = 12$ electrons. Total: $36 + 12 = 48$.
## Step3: Identify element
Atomic number 48 is Cadmium (Cd).
# Answer: Cadmium (Cd)

### Question 14
# Explanation:
## Step1: Find Xe's atomic number
Xenon (Xe) has atomic number 54.
## Step2: Add electrons from configuration
$6s^2 4f^{14} 5d^{10} 6p^2$: $2 + 14 + 10 + 2 = 28$. Total: $54 + 28 = 82$.
## Step3: Identify element
Atomic number 82 is Lead (Pb).
# Answer: Lead (Pb)

### Question 15
# Explanation:
## Step1: Find Rn's atomic number
Radon (Rn) has atomic number 86.
## Step2: Add electrons from configuration
$7s^2 5f^{14} 6d^4$: $2 + 14 + 4 = 20$. Total: $86 + 20 = 106$.
## Step3: Identify element
Atomic number 106 is Seaborgium (Sg).
# Answer: Seaborgium (Sg)

### Question 16
# Explanation:
## Step1: Analyze electron filling order
Electrons fill $4s$ before $3d$, but after $4s$ and $3d$, $4p$ fills before $5s$? Wait, the configuration is $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4d^{10} 4p^6 5s^1$. Wait, $3d$ should fill before $4p$. The correct order after $4s$ is $3d$, then $4p$. So $4d$ should not fill before $4p$ is complete. Wait, $4s^2 3d^{10} 4p^6$ is correct for Kr (36). Then $5s^1$ would be Rb (37). But the given config has $4d^{10}$ after $4s^2$ and before $4p^6$, which is incorrect because $3d$ (n=3) is lower than $4d$ (n=4). So the filling order is wrong: $4s$ → $3d$ → $4p$ → $5s$ → $4d$ → etc. So the config has $4d^{10}$ before $4p^6$, which is incorrect.
## Step2: Conclusion
Incorrect, because $3d$ (not $4d$) should fill after $4s$ and before $4p$. The $4d$ orbital is higher in energy than $4p$, so $4p$ should fill before $4d$.
# Answer: Incorrect

### Question 17
# Explanation:
## Step1: Analyze s - orbital capacity
s - orbitals can hold a maximum of 2 electrons (Pauli exclusion principle). The $3s$ orbital has $3s^3$, which is more than 2.
## Step2: Conclusion
Incorrect, because $s$ - orbitals (like $3s$) can only hold 2 electrons, not 3.
# Answer: Incorrect

### Question 18
# Explanation:
## Step1: Recall f - orbital filling
f - orbitals (like $5f$) follow the Aufbau principle. The $5f$ orbital can hold up to 14 electrons, but when filling, after $7s^2$, the $5f$ fills. However, for elements after Rn, the $5f$ (actinides) fill. The configuration $[Rn] 7s^2 5f^9 6d^2$: let's check the atomic number. Rn is 86, $7s^2$ (2) $5f^9$ (9) $6d^2$ (2). Total: $86 + 2 + 9 + 2 = 99$ (Einsteinium? No, Es is 99, but Es has $[Rn] 7s^2 5f^11$? Wait, no, the filling of $5f$ and $6d$: actually, the correct configuration for element 99 (Einsteinium) is $[Rn] 7s^2 5f^{11}$, but maybe the given config is for a different element? Wait, no, the problem is to check if the configuration is correct. Wait, the $5f$ orbital: when filling, after $7s^2$, the $5f$ starts filling. The $6d$ orbitals fill after $5f$ is more filled? Wait, actually, the Aufbau principle for actinides: $7s$ → $5f$ → $6d$. So having $5f^9$ and $6d^2$ is possible? Wait, no, the correct order is that $5f$ fills before $6d$ for actinides. Wait, maybe the configuration is correct? Wait, no, let's check the electron count. Rn is 86, $7s^2$ (2) $5f^9$ (9) $6d^2$ (2): total 99. Element 99 is Einsteinium (Es). But the actual electron configuration of Es is $[Rn] 7s^2 5f^{11}$? Wait, no, I think I made a mistake. Wait, the atomic number of Es is 99. $7s^2$ (2) + $5f^{11}$ (11) = 13, 86 + 13 = 99. So the given config has $5f^9 6d^2$ (total 11 electrons: 9 + 2 = 11), which is the same as $5f^{11}$ (since $6d^2$ electrons might have moved from $5f$? No, that's not the case. Wait, maybe the configuration is using the excited state? But the question is about the correct electron configuration (ground state). The ground state of Es is $[Rn] 7s^2 5f^{11}$, so the given config $[Rn] 7s^2 5f^9 6d^2$ is an excited state, but the question is about correct (ground state) configuration. So it's incorrect? Wait, no, maybe I'm wrong. Wait, let's check the Aufbau principle again. The energy levels: $7s$ < $5f$ < $6d$ for actinides. So electrons fill $7s$ first, then $5f$, then $6d$. So in ground state, electrons should fill $5f$ before $6d$. So having $6d^2$ while $5f$ is only $9$ is incorrect because $5f$ is lower in energy than $6d$ for actinides. So the configuration is incorrect? Wait, maybe the element is different. Wait, element 101 (Mendelevium) has $[Rn] 7s^2 5f^{13}$, no. Wait, maybe the question is about the format. Wait, the configuration is written as $[Rn] 7s^2 5f^9 6d^2$. Is this a valid ground - state configuration? Actually, some actinides have electrons in $6d$ while filling $5f$. For example, Thorium (Th) has $[Rn] 7s^2 6d^2$ (no $5f$ electrons), Protactinium (Pa) has $[Rn] 7s^2 5f^2 6d^1$, Uranium (U) has $[Rn] 7s^2 5f^3 6d^1$, Neptunium (Np) has $[Rn] 7s^2 5f^4 6d^1$, Plutonium (Pu) has $[Rn] 7s^2 5f^6$ (no $6d$ electrons), Americium (Am) has $[Rn] 7s^2 5f^7$, Curium (Cm) has $[Rn] 7s^2 5f^7 6d^1$? Wait, no, maybe my memory is off. Anyway, the key point: the $5f$ and $6d$ orbitals are close in energy for actinides, so some elements have electrons in $6d$ while $5f$ is being filled. But the given configuration $[Rn] 7s^2 5f^9 6d^2$: let's calculate the atomic number. Rn (86) + $7s^2$ (2) + $5f^9$ (9) + $6d^2$ (2) = 99. Element 99 is Einsteinium. The actual ground - state configuration of Es is $[Rn] 7s^2 5f^{11}$, so the given configuration is incorrect because it has electrons in $6d$ instead of $5f$ (since $5f$ can hold more electrons before $6d$ starts filling significantly). So the answer is incorrect.
## Step2: Conclusion
Incorrect, because for actinides, $5f$ orbitals should fill before $6d$ orbitals to a greater extent in the ground state (the given configuration misallocates electrons between $5f$ and $6d$).
# Answer: Incorrect

### Question 19
# Explanation:
## Step1: Find Ar's atomic number
Argon (Ar) has atomic number 18.
## Step2: Analyze the configuration
The configuration is $[Ar] 5s^2 4d^{10} 5p^5$. The correct filling order after Ar ($1s^2 2s^2 2p^6 3s^2 3p^6$) is $4s$ → $3d$ → $4p$ → $5s$ → $4d$ → $5p$. So after Ar, we should fill $4s$, $3d$, $4p$ (to reach Kr, atomic number 36), then $5s$, $4d$, $5p$. But the given configuration skips the $4s$, $3d$, and $4p$ orbitals after Ar. The correct configuration for the element with this electron count ($18+2 + 10+5=35$) should be $[Ar] 4s^2 3d^{10} 4p^5$ (Bromine, Br), not $[Ar] 5s^2 4d^{10} 5p^5$ (which would be atomic number $18 + 2+10 + 5=35$? No, $18+2+10 + 5 = 35$, but $5s^2 4d^{10} 5p^5$ is actually $18+2+10 + 5=35$? Wait, no, $5s^2$ is $n = 5$, $4d^{10}$ is $n = 4$, $5p^5$ is $n = 5$. The correct order for atomic number 35 (Br) is $[Ar] 4s^2 3d^{10} 4p^5$, not $[Ar] 5s^2 4d^{10} 5p^5$ (which would be a different element, but the electron count here is wrong because $5s^2 4d^{10} 5p^5$ has $2 + 10+5 = 17$ electrons after Ar, so total $18 + 17=35$, but the filling order is wrong. The $4s$, $3d$, and $4p$ orbitals (n = 4 and n = 3) should be filled before $5s$ and $4d$ (n = 5 and n = 4) for atomic number 35.
## Step3: Conclusion
Incorrect, because the filling order is wrong (skips $4s$, $3d$, and $4p$ orbitals that should be filled before $5s$ and $4d$ for this electron count).
# Answer: Incorrect

### Question 20
# Explanation:
## Step1: Recall f - orbital filling
The $4f$ orbitals are part of the lanthanide series. The correct filling order after $Xe$ ($[Xe] 6s^2 4f^{14} 5d^{10} 6p^6$): for lanthanides, the filling order is $6s$ → $4f$ → $5d$. But the $4f$ orbital starts filling after $6s$. However, the $4f$ orbital can hold up to 14 electrons. But the configuration $[Xe] 6s^2 4f^{10}$: let's check the atomic number. Xe is 54, $6s^2$ (2) $4f^{10}$ (10). Total: $54+2 + 10=66$. Element 66 is Dysprosium (Dy). Wait, but the correct configuration of Dy is $[Xe] 4f^{10} 6s^2$ (same as given, just order? Wait, the order of writing electron configurations: usually, orbitals are written in order of increasing principal quantum number, but for f - orbitals, sometimes they are written after the valence s - orbital. Wait, the standard notation for Dy is $[Xe] 4f^{10} 6s^2$, which is the same as $[Xe] 6s^2 4f^{10}$ (just order of writing, since $6s$ is filled before $4f$). Wait, but is the configuration correct? Wait, the $4f$ orbital: when filling, after $6s^2$, the $4f$ starts filling. So the configuration $[Xe] 6s^2 4f^{10}$ is correct for Dy (atomic number 66). Wait, but earlier I thought maybe the order, but actually, the order of writing can have the s - orbital first or the f - orbital first, as long as the electron count is correct. Wait, no, the Aufbau principle says that $6s$ fills before $4f$, so the configuration should have $6s^2$ before $4f$ (or after, but the electron count is what matters). Wait, the electron count: $Xe$ (54) + $6s^2$ (

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Question

Explanation:

Question 11

Step1: Calculate total electrons

Step2: Identify element

Step1: Calculate total electrons

Step2: Confirm

Step1: Find Kr's atomic number

Step2: Add electrons from configuration

Step3: Identify element

Answer:

Question 12