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Which of the following do not exist ?...

Which of the following do not exist ?

A

`NCl_(5)`

B

`PH_(5)`

C

`[BCl_(6)]^(3-)`

D

All of these

Text Solution

AI Generated Solution

The correct Answer is:
To determine which of the given compounds do not exist, we will analyze each option one by one. ### Step 1: Analyze NCl5 - **NCl5**: - Nitrogen (N) has an atomic number of 7, with an electronic configuration of 1s² 2s² 2p³. - Nitrogen can accommodate a maximum of 8 electrons in its valence shell (octet rule). - To form NCl5, nitrogen would need to accommodate 5 pairs of electrons (10 electrons), which exceeds its capacity. - Therefore, **NCl5 does not exist**. ### Step 2: Analyze PH5 - **PH5**: - Phosphorus (P) has an atomic number of 15, with an electronic configuration of [Ne] 3s² 3p³. - Phosphorus can expand its octet and can accommodate more than 8 electrons due to the presence of vacant d-orbitals. - However, the bond between phosphorus and hydrogen is not stable because the interaction between the p-orbital of phosphorus and the s-orbital of hydrogen is not energetically favorable. - Thus, **PH5 does not exist**. ### Step 3: Analyze BCl6³⁻ - **BCl6³⁻**: - Boron (B) has an atomic number of 5, with an electronic configuration of 1s² 2s² 2p¹. - Boron can only accommodate a maximum of 6 electrons in its valence shell due to its small size and lack of vacant d-orbitals. - To form BCl6³⁻, boron would need to accommodate 6 pairs of electrons (12 electrons), which exceeds its capacity. - Therefore, **BCl6³⁻ does not exist**. ### Step 4: Conclusion - Since all three compounds (NCl5, PH5, and BCl6³⁻) do not exist, the correct answer is **"all of these"**. ### Final Answer All of the compounds listed (NCl5, PH5, BCl6³⁻) do not exist. ---
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