A) \[{{(C{{H}_{3}})}_{3}}B\]
B) \[{{(C{{H}_{3}})}_{2}}O\]
C) \[{{(C{{H}_{3}})}_{2}}P\]
D) \[{{(C{{H}_{3}})}_{3}}N\]
Correct Answer: A
Solution :
| Key Idea According to Lewis concept, "Acids are electron acceptor and bases are electron donor". |
| Since, electron deficient compounds also have an ability to accept electrons, these are regarded as acids. |
| \[\frac{{{\varepsilon }^{2}}R}{\left[ {{R}^{2}}+{{\left( L\omega -\frac{1}{C\omega } \right)}^{2}} \right]}\] \[\frac{{{\varepsilon }^{2}}\sqrt{{{R}^{2}}+{{\left( L\omega -\frac{1}{C\omega } \right)}^{2}}}}{R}\] |
| \[\frac{{{\varepsilon }^{2}}\left[ {{R}^{2}}+{{\left( L\omega -\frac{1}{C\omega } \right)}^{2}} \right]}{R}\] \[\frac{{{\varepsilon }^{2}}R}{\sqrt{{{R}^{2}}+{{\left( L\omega -\frac{1}{C\omega } \right)}^{2}}}}\] |
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