Hybrid orbitals problem

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I'm seeing conflicting answers among various textbooks. I would predict that it forms SP3 hybrid orbitals, and yet its bond angles are far from 109.5.

Edit: H2S, rather.
 
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  • #2
Borek
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No hybridization at all and pure sp3 are just two ends of a continuum.

For some highly symmetrical molecules (say, CH4) hybridization of the central atom is a pure sp3. But for some other molecules, like H2S, what we observe is just some partial hybridization, in which bonds are not equivalent.
 
  • #3
DrDu
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Note also that hybridization is not a property of the molecule but entirely your personal choice of a convenient expression for the molecules wavefunction.
E.g. molecules like ethylene can equally well be described in terms of sp2+p or sp3 hybrids and water in terms of s+p or sp3 or even something intermediate.
In the case of H2S a description in terms of pure s and p orbitals makes probably more sense than the assumption of sp3 hybrid orbitals as the s and p orbitals in second row atoms differ considerably in size and energy.
 
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  • #4
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No hybridization at all and pure sp3 are just two ends of a continuum.

For some highly symmetrical molecules (say, CH4) hybridization of the central atom is a pure sp3. But for some other molecules, like H2S, what we observe is just some partial hybridization, in which bonds are not equivalent.
I see. How does one determine whether pure hybridization is a more appropriate model to describe orbital shape?
 
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What about HCl, are orbitals of chlorine hybridized in that case?
 
  • #6
Borek
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No need for that.
 

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