write the unabbreviated electron configurations of the following elements:
1) copper_______________________________
2) iodine _______________________________
3) potassium _______________________________
4) bismuth _______________________________
5) zirconium _______________________________
write the abbreviated electron configurations of the following elements:
6) iridium _______________________________
7) chlorine _______________________________
8) nobelium _______________________________
9) caesium _______________________________
10) magnesium _______________________________

Question

write the unabbreviated electron configurations of the following elements:
1)  copper_______________________________
2)  iodine _______________________________
3)  potassium _______________________________
4)  bismuth _______________________________
5)  zirconium _______________________________
write the abbreviated electron configurations of the following elements:
6)  iridium _______________________________
7)  chlorine _______________________________
8)  nobelium _______________________________
9)  caesium _______________________________
10) magnesium _______________________________

Accepted Answer

### 1) Copper (Cu, atomic number 29)
# Explanation:
## Step1: Recall electron filling rules (Aufbau, Pauli, Hund's).
Electrons fill orbitals in order: $1s$, $2s$, $2p$, $3s$, $3p$, $4s$, $3d$, etc. Copper has an exception: one electron from $4s$ moves to $3d$ for stability (full $d$-subshell is more stable, $3d^{10}$ instead of $3d^9$).
## Step2: Fill orbitals with 29 electrons.
$1s^2$ (2 e⁻), $2s^2$ (4 e⁻), $2p^6$ (10 e⁻), $3s^2$ (12 e⁻), $3p^6$ (18 e⁻), $4s^1$ (19 e⁻), $3d^{10}$ (29 e⁻).
# Answer: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^{10}$

### 2) Iodine (I, atomic number 53)
# Explanation:
## Step1: Follow Aufbau order: $1s$, $2s$, $2p$, $3s$, $3p$, $4s$, $3d$, $4p$, $5s$, $4d$, $5p$.
## Step2: Fill 53 electrons.
$1s^2$ (2), $2s^2$ (4), $2p^6$ (10), $3s^2$ (12), $3p^6$ (18), $4s^2$ (20), $3d^{10}$ (30), $4p^6$ (36), $5s^2$ (38), $4d^{10}$ (48), $5p^5$ (53).
# Answer: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^5$

### 3) Potassium (K, atomic number 19)
# Explanation:
## Step1: Aufbau order: $1s$, $2s$, $2p$, $3s$, $3p$, $4s$.
## Step2: Fill 19 electrons.
$1s^2$ (2), $2s^2$ (4), $2p^6$ (10), $3s^2$ (12), $3p^6$ (18), $4s^1$ (19).
# Answer: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^1$

### 4) Bismuth (Bi, atomic number 83)
# Explanation:
## Step1: Aufbau order: $1s$, $2s$, $2p$, $3s$, $3p$, $4s$, $3d$, $4p$, $5s$, $4d$, $5p$, $6s$, $4f$, $5d$, $6p$.
## Step2: Fill 83 electrons.
$1s^2$ (2), $2s^2$ (4), $2p^6$ (10), $3s^2$ (12), $3p^6$ (18), $4s^2$ (20), $3d^{10}$ (30), $4p^6$ (36), $5s^2$ (38), $4d^{10}$ (48), $5p^6$ (54), $6s^2$ (56), $4f^{14}$ (70), $5d^{10}$ (80), $6p^3$ (83).
# Answer: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^3$

### 5) Zirconium (Zr, atomic number 40)
# Explanation:
## Step1: Aufbau order: $1s$, $2s$, $2p$, $3s$, $3p$, $4s$, $3d$, $4p$, $5s$, $4d$.
## Step2: Fill 40 electrons.
$1s^2$ (2), $2s^2$ (4), $2p^6$ (10), $3s^2$ (12), $3p^6$ (18), $4s^2$ (20), $3d^{10}$ (30), $4p^6$ (36), $5s^2$ (38), $4d^2$ (40).
# Answer: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^2$

### 6) Iridium (Ir, atomic number 77) - Abbreviated (use [Xe] for noble gas core, Xe is atomic number 54)
# Explanation:
## Step1: Find noble gas before Ir: Xenon (Xe, 54 electrons).
## Step2: Fill remaining electrons (77 - 54 = 23) in orbitals after Xe: $6s$, $4f$, $5d$.
Order: $6s^2$, $4f^{14}$, $5d^7$ (2 + 14 + 7 = 23).
# Answer: $[Xe] 6s^2 4f^{14} 5d^7$

### 7) Chlorine (Cl, atomic number 17) - Abbreviated (use [Ne] for noble gas core, Ne is atomic number 10)
# Explanation:
## Step1: Noble gas before Cl: Neon (Ne, 10 electrons).
## Step2: Remaining electrons: 17 - 10 = 7, fill $3s$ and $3p$: $3s^2 3p^5$.
# Answer: $[Ne] 3s^2 3p^5$

### 8) Nobelium (No, atomic number 102) - Abbreviated (use [Rn] for noble gas core, Rn is atomic number 86)
# Explanation:
## Step1: Noble gas before No: Radon (Rn, 86 electrons).
## Step2: Remaining electrons: 102 - 86 = 16, fill $7s$, $5f$: $7s^2 5f^{14}$ (2 + 14 = 16).
# Answer: $[Rn] 7s^2 5f^{14}$

### 9) Caesium (Cs, atomic number 55) - Abbreviated (use [Xe] for noble gas core, Xe is atomic number 54)
# Explanation:
## Step1: Noble gas before Cs: Xenon (Xe, 54 electrons).
## Step2: Remaining electrons: 55 - 54 = 1, fill $6s$: $6s^1$.
# Answer: $[Xe] 6s^1$

### 10) Magnesium (Mg, atomic number 12) - Abbreviated (use [Ne] for noble gas core, Ne is atomic number 10)
# Explanation:
## Step1: Noble gas before Mg: Neon (Ne, 10 electrons).
## Step2: Remaining electrons: 12 - 10 = 2, fill $3s$: $3s^2$.
# Answer: $[Ne] 3s^2$

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QUESTION IMAGE

Question

Explanation:

1) Copper (Cu, atomic number 29)

Step1: Recall electron filling rules (Aufbau, Pauli, Hund's).

Step2: Fill orbitals with 29 electrons.

Step1: Follow Aufbau order: \(1s\), \(2s\), \(2p\), \(3s\), \(3p\), \(4s\), \(3d\), \(4p\), \(5s\), \(4d\), \(5p\).

Step2: Fill 53 electrons.

Step1: Aufbau order: \(1s\), \(2s\), \(2p\), \(3s\), \(3p\), \(4s\).

Step2: Fill 19 electrons.

Answer:

2) Iodine (I, atomic number 53)