QuestionMay 4, 2025

What is the correct ground state electron configuration of titanium, Ti? A [Ar]3d^2 B 1s^22s^22p^63s^23p^64d^2 C [Ne]3d^2 D 1s^22s^22p^63s^23p^63d^2 E 1s^22s^22p^63s^23p^64s^23d^2

What is the correct ground state electron configuration of titanium, Ti? A [Ar]3d^2 B 1s^22s^22p^63s^23p^64d^2 C [Ne]3d^2 D 1s^22s^22p^63s^23p^63d^2 E 1s^22s^22p^63s^23p^64s^23d^2
What is the correct ground state electron configuration of titanium, Ti? A [Ar]3d^2 B 1s^22s^22p^63s^23p^64d^2 C [Ne]3d^2 D 1s^22s^22p^63s^23p^63d^2 E 1s^22s^22p^63s^23p^64s^23d^2

Solution
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Answer

The correct ground-state electron configuration of titanium is **E**: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2. Explanation 1. Understand the question The problem asks for the correct ground-state electron configuration of titanium (Ti). Titanium has an atomic number of 22, meaning it has 22 electrons in its neutral state. We need to distribute these electrons into orbitals following the Aufbau principle, Hund's rule, and the Pauli exclusion principle. --- 2. Apply the Aufbau principle According to the Aufbau principle, electrons fill orbitals in order of increasing energy levels. The general filling order is: \[ 1s \rightarrow 2s \rightarrow 2p \rightarrow 3s \rightarrow 3p \rightarrow 4s \rightarrow 3d \rightarrow 4p \dots \] For titanium, we distribute 22 electrons as follows: - **1s**: 2 electrons → 1s^2 - **2s**: 2 electrons → 2s^2 - **2p**: 6 electrons → 2p^6 - **3s**: 2 electrons → 3s^2 - **3p**: 6 electrons → 3p^6 - **4s**: 2 electrons → 4s^2 - **3d**: 2 electrons → 3d^2 Thus, the electron configuration is: \[ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2 \] --- 3. Identify the shorthand notation Using the noble gas shorthand notation, the core electrons (up to 3p^6) are represented by [Ar], the electron configuration of argon. Therefore, the shorthand configuration becomes: \[ [Ar] 4s^2 3d^2 \] --- 4. Eliminate incorrect options Analyze each option: - **A**: [Ar]3d^2 → Incorrect because it omits the 4s^2 electrons. - **B**: 1s^2 2s^2 2p^6 3s^2 3p^6 4d^2 → Incorrect because it incorrectly places electrons in the 4d orbital instead of 3d. - **C**: [Ne]3d^2 → Incorrect because it uses [Ne] instead of [Ar] and omits 4s^2. - **D**: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 → Incorrect because it omits 4s^2. - **E**: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2 → Correct, as it matches the full configuration derived above. ---

Explanation

1. Understand the question<br /> The problem asks for the correct ground-state electron configuration of titanium (Ti). Titanium has an atomic number of 22, meaning it has 22 electrons in its neutral state. We need to distribute these electrons into orbitals following the Aufbau principle, Hund's rule, and the Pauli exclusion principle.<br /><br />---<br /><br />2. Apply the Aufbau principle<br /> According to the Aufbau principle, electrons fill orbitals in order of increasing energy levels. The general filling order is:<br />\[<br />1s \rightarrow 2s \rightarrow 2p \rightarrow 3s \rightarrow 3p \rightarrow 4s \rightarrow 3d \rightarrow 4p \dots<br />\]<br />For titanium, we distribute 22 electrons as follows:<br />- **1s**: 2 electrons → $1s^2$<br />- **2s**: 2 electrons → $2s^2$<br />- **2p**: 6 electrons → $2p^6$<br />- **3s**: 2 electrons → $3s^2$<br />- **3p**: 6 electrons → $3p^6$<br />- **4s**: 2 electrons → $4s^2$<br />- **3d**: 2 electrons → $3d^2$<br /><br />Thus, the electron configuration is:<br />\[<br />1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2<br />\]<br /><br />---<br /><br />3. Identify the shorthand notation<br /> Using the noble gas shorthand notation, the core electrons (up to $3p^6$) are represented by $[Ar]$, the electron configuration of argon. Therefore, the shorthand configuration becomes:<br />\[<br />[Ar] 4s^2 3d^2<br />\]<br /><br />---<br /><br />4. Eliminate incorrect options<br /> Analyze each option:<br />- **A**: $[Ar]3d^2$ → Incorrect because it omits the $4s^2$ electrons.<br />- **B**: $1s^2 2s^2 2p^6 3s^2 3p^6 4d^2$ → Incorrect because it incorrectly places electrons in the $4d$ orbital instead of $3d$.<br />- **C**: $[Ne]3d^2$ → Incorrect because it uses $[Ne]$ instead of $[Ar]$ and omits $4s^2$.<br />- **D**: $1s^2 2s^2 2p^6 3s^2 3p^6 3d^2$ → Incorrect because it omits $4s^2$.<br />- **E**: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2$ → Correct, as it matches the full configuration derived above.<br /><br />---
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