Which of the following hybrides electron deficient?
- \(\text{CH}_4\)
- NaH
- \(\text{B}_2\text{H}_4\)
- \(\text{CaH}_2\)
The Correct Option is C
Solution and Explanation
The term "electron-deficient" refers to a compound that lacks sufficient valence electrons to form conventional covalent bonds. Based on this definition, the electron-deficient compound among the options provided is:
(C) B2H4: Diborane (B2H4) is an example of an electron-deficient compound. It exhibits a bridged structure with boron atoms sharing electrons but not forming enough conventional covalent bonds to satisfy the octet rule. Diborane is known for its electron-deficient nature and its ability to undergo unique reactions due to the presence of vacant bonding orbitals.
The other options,
(A) CH4 (methane),
(B) NaH (sodium hydride), and
(D) CaH2 (calcium hydride), do not exhibit electron-deficient characteristics as they follow conventional covalent bonding patterns and possess sufficient valence electrons to satisfy the octet rule.
Therefore, the correct answer is (C) B2H4.
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