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Spectrum of Li^(2+) is similar to that ...

Spectrum of `Li^(2+)` is similar to that of

A

H

B

Be

C

He

D

Ne .

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The correct Answer is:
To determine which atom or ion has a spectrum similar to that of \( \text{Li}^{2+} \), we can follow these steps: ### Step 1: Understand the Electronic Configuration of Lithium - Lithium (Li) has an atomic number of 3, which means it has 3 electrons. Its electronic configuration is \( 1s^2 \, 2s^1 \). ### Step 2: Determine the Configuration of \( \text{Li}^{2+} \) - The ion \( \text{Li}^{2+} \) means that 2 electrons have been removed from lithium. Therefore, the electronic configuration of \( \text{Li}^{2+} \) will be \( 1s^1 \). ### Step 3: Compare with Other Elements - Now, we need to compare the electronic configuration of \( \text{Li}^{2+} \) with the other options provided: - **Hydrogen (H)**: \( 1s^1 \) - **Helium (He)**: \( 1s^2 \) - **Beryllium (Be)**: \( 1s^2 \, 2s^2 \) - **Neon (Ne)**: \( 1s^2 \, 2s^2 \, 2p^6 \) ### Step 4: Identify the Similarity - The electronic configuration of \( \text{Li}^{2+} \) is \( 1s^1 \), which is identical to that of hydrogen. Both have one electron in their outermost shell. ### Step 5: Conclusion - Since both \( \text{Li}^{2+} \) and hydrogen have the same electronic configuration of \( 1s^1 \), they will exhibit similar spectral lines due to their one-electron systems. ### Final Answer - The spectrum of \( \text{Li}^{2+} \) is similar to that of **Hydrogen**. ---
To determine which atom or ion has a spectrum similar to that of \( \text{Li}^{2+} \), we can follow these steps: ### Step 1: Understand the Electronic Configuration of Lithium - Lithium (Li) has an atomic number of 3, which means it has 3 electrons. Its electronic configuration is \( 1s^2 \, 2s^1 \). ### Step 2: Determine the Configuration of \( \text{Li}^{2+} \) - The ion \( \text{Li}^{2+} \) means that 2 electrons have been removed from lithium. Therefore, the electronic configuration of \( \text{Li}^{2+} \) will be \( 1s^1 \). ...
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