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The IE(1) of C atom is greater than that...

The `IE_(1)` of `C` atom is greater than that of boron `(B)` atom, whereas the reverse is true for `IE_(2)`. Explain?

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To explain why the first ionization energy (IE1) of carbon (C) is greater than that of boron (B), while the second ionization energy (IE2) of boron is greater than that of carbon, we can break down the explanation into several steps: ### Step 1: Understand the Electronic Configurations - **Carbon (C)** has an atomic number of 6, and its electronic configuration is \(1s^2 2s^2 2p^2\). - **Boron (B)** has an atomic number of 5, and its electronic configuration is \(1s^2 2s^2 2p^1\). ### Step 2: Analyze the First Ionization Energy (IE1) - **IE1 of Boron**: When we remove one electron from boron, we take it from the \(2p^1\) subshell, resulting in a stable configuration of \(1s^2 2s^2\). This configuration is stable because both the \(1s\) and \(2s\) subshells are completely filled. ...
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