Consider Valence Bond Theory. a. In valence bond theory, how are bonds formed b.

Question

Consider Valence Bond Theory.

a. In valence bond theory, how are bonds formed

b. What are hybrid orbitals?

c. What hybridization (or what "hybrid orbital set") corresponds to the carbon in CH4?

P.s. If taking a photo of your explanations, please make sure the photo can be read, the same questions to these couldn't be read because of the poor photo quality, thanks in advance!

2. Consider valence bond theory a. In valence bond theory, how are bonds formed? b. What are hybrid orbitals? c. What hybridization (or what "hybrid orbital set") corresponds to the carbon in CH4? 3. Fill in the table below using your knowledge of molecular geometry, bond angles, and electron electron repulsion for the molecule represented. (bp bonding pair, lp lone pair)

Explanation / Answer

Ans

a) When two half filled atomic orbitals of the atoms containing one unpaired electron overlap each other , a covalent bond is formed in between them . The inner electrons or the core electrons do not participate in the bond formation.

b) When the atomic orbitals of the atoms combine with each other , they form a new set of orbitals. These orbitals are called as hybrid orbitals.

c) In methane molecule, one 2s and three 2p atomic orbitals of carbon hybridise into four equivalent sp3 hybrid orbitals. So the hybridisation of C in CH4 is SP3.

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