Free Printable Electron Configuration Worksheets - Free Printable

Problem Analysis:

The worksheet focuses on electronic configurations of elements, using noble gas abbreviations and identifying elements based on their electron configurations. Let's solve each section step by step.

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Section 1: Abbreviated Electron Configurations Using Noble Gases

#### i. Li (Lithium)
- Full configuration: \(1s^2 2s^1\)
- Abbreviated using noble gas: \([He] 2s^1\)

#### ii. B (Boron)
- Full configuration: \(1s^2 2s^2 2p^1\)
- Abbreviated using noble gas: \([He] 2s^2 2p^1\)

#### iii. O (Oxygen)
- Full configuration: \(1s^2 2s^2 2p^4\)
- Abbreviated using noble gas: \([He] 2s^2 2p^4\)

#### iv. Mg (Magnesium)
- Full configuration: \(1s^2 2s^2 2p^6 3s^2\)
- Abbreviated using noble gas: \([Ne] 3s^2\)

#### v. Cl (Chlorine)
- Full configuration: \(1s^2 2s^2 2p^6 3s^2 3p^5\)
- Abbreviated using noble gas: \([Ne] 3s^2 3p^5\)

#### vi. V (Vanadium)
- Full configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3\)
- Abbreviated using noble gas: \([Ar] 4s^2 3d^3\)

#### vii. Se²⁻ (Selenium Ion with 2 extra electrons)
- Selenium (Se) full configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^4\)
- With 2 extra electrons: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6\)
- Abbreviated using noble gas: \([Kr]\)

#### viii. Cr²⁺ (Chromium Ion with 2 fewer electrons)
- Chromium (Cr) full configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^5\)
- With 2 fewer electrons: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^4\)
- Abbreviated using noble gas: \([Ar] 3d^4\)

#### ix. I⁻ (Iodide Ion with 1 extra electron)
- Iodine (I) full configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^5\)
- With 1 extra electron: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6\)
- Abbreviated using noble gas: \([Xe] 6s^2 4f^{14} 5d^{10} 6p^6\)

#### x. Ag (Silver)
- Full configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^1 4d^{10}\)
- Abbreviated using noble gas: \([Kr] 5s^1 4d^{10}\)

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Section 2: Identify the Element with the Following Electron Configuration

#### i. \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4p^4\)
- This is the configuration for Germanium (Ge).

#### ii. \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2\)
- This is the configuration for Strontium (Sr).

#### iii. \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^7\)
- This is the configuration for Promethium (Pm).

#### iv. \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10}\)
- This is the configuration for Gold (Au).

#### v. \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^6 7s^1\)
- This is the configuration for Francium (Fr).

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Section 3: Determine if the Following Electron Configurations Are Correct

#### i. \(1s^2 2s^2 2p^6 3s^2 4d^{10} 4p^6 5s^1\)
- Incorrect: The \(4d\) orbitals should be filled after \(3d\) and before \(4p\). The correct order is \(3d^{10}\) before \(4p^6\).

#### ii. \(1s^2 2s^2 2p^6 3s^3\)
- Incorrect: The \(3s\) orbital can hold a maximum of 2 electrons. The correct configuration would involve filling the \(3p\) orbitals next.

#### iii. \([Rn] 7s^2 5f^3 6d^2\)
- Correct: This configuration follows the Aufbau principle correctly, as \(5f\) fills before \(6d\).

#### iv. \([Ar] 5s^2 4d^{10} 5p^5\)
- Incorrect: The \(4d\) orbitals should be filled after \(4s\) and before \(5p\). The correct configuration would involve filling \(4d\) before \(5p\).

#### v. \([Xe] 6s^2 4f^{10}\)
- Incorrect: The \(4f\) orbitals should be filled after \(5s\) and before \(5p\). The correct configuration would involve filling \(5p\) before \(4f\).

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Section 4: Identify the Following Elements

#### i. \(1s^2 2s^2 2p^2\)
- This is the configuration for Carbon (C).

#### ii. \(1s^2 2s^2 2p^6\)
- This is the configuration for Neon (Ne).

#### iii. \([Ar] 4s^2 3d^{10} 4p^5\)
- This is the configuration for Chlorine (Cl).

#### iv. \([Kr] 5s^2 4d^1\)
- This is the configuration for Rubidium (Rb).

#### v. \([Ne] 3s^2 3p^3\)
- This is the configuration for Phosphorus (P).

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Final Answers:

1. Abbreviated Electron Configurations:
- i. \([He] 2s^1\)
- ii. \([He] 2s^2 2p^1\)
- iii. \([He] 2s^2 2p^4\)
- iv. \([Ne] 3s^2\)
- v. \([Ne] 3s^2 3p^5\)
- vi. \([Ar] 4s^2 3d^3\)
- vii. \([Kr]\)
- viii. \([Ar] 3d^4\)
- ix. \([Xe] 6s^2 4f^{14} 5d^{10} 6p^6\)
- x. \([Kr] 5s^1 4d^{10}\)

2. Identify the Element:
- i. Germanium (Ge)
- ii. Strontium (Sr)
- iii. Promethium (Pm)
- iv. Gold (Au)
- v. Francium (Fr)

3. Determine if Correct:
- i. Incorrect
- ii. Incorrect
- iii. Correct
- iv. Incorrect
- v. Incorrect

4. Identify the Following Elements:
- i. Carbon (C)
- ii. Neon (Ne)
- iii. Chlorine (Cl)
- iv. Rubidium (Rb)
- v. Phosphorus (P)

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Boxed Final Answer:

\[
\boxed{
\begin{array}{l}
\text{1. Abbreviated Configurations:} \\
\text{i. [He] 2s^1} \\
\text{ii. [He] 2s^2 2p^1} \\
\text{iii. [He] 2s^2 2p^4} \\
\text{iv. [Ne] 3s^2} \\
\text{v. [Ne] 3s^2 3p^5} \\
\text{vi. [Ar] 4s^2 3d^3} \\
\text{vii. [Kr]} \\
\text{viii. [Ar] 3d^4} \\
\text{ix. [Xe] 6s^2 4f^{14} 5d^{10} 6p^6} \\
\text{x. [Kr] 5s^1 4d^{10}} \\
\\
\text{2. Identified Elements:} \\
\text{i. Germanium (Ge)} \\
\text{ii. Strontium (Sr)} \\
\text{iii. Promethium (Pm)} \\
\text{iv. Gold (Au)} \\
\text{v. Francium (Fr)} \\
\\
\text{3. Correctness of Configurations:} \\
\text{i. Incorrect} \\
\text{ii. Incorrect} \\
\text{iii. Correct} \\
\text{iv. Incorrect} \\
\text{v. Incorrect} \\
\\
\text{4. Identified Elements:} \\
\text{i. Carbon (C)} \\
\text{ii. Neon (Ne)} \\
\text{iii. Chlorine (Cl)} \\
\text{iv. Rubidium (Rb)} \\
\text{v. Phosphorus (P)}
\end{array}
}
\]