[GregoryC4]

I have been trying to determine whether a hybrid orbital affects the geometric structure of a molecule. A question I have been stuck with asks to use the hybridization theory (which I understand reasonably) to account for the shape and bonding of an ethyne molecule. Any ideas on how to answer this question? This is what I have so far:

"A Carbon atom can make 4 bonds in a molecule; however, Carbon only contains 2 half-filled orbitals and therefore must hybridize its orbitals into a sp3 hybrid orbital to attain 4 bonds. The linear geometry of Ethyne molecule is not affected by the hybrid orbital but now contains a stronger and more stabilized bond."

I would just like clarification on

1. what the question is asking for.
2. do hybrid orbitals affect the geometric structure?
3. What can I add to my answer to answer the question more fully?

Thank you so much everyone, you guys are great.      

[Xenonman]

Most molecules follow the VSEPR theory: http://en.wikipedia.org/wiki/VSEPR_theory.

The theory only accounts lone electron pairs and number of bonds.

[orgopete]

I agree this question is not well written. This is what it is telling you. Carbon has 2s2 2px1 2px1 electrons, therefore can only form two bonds. If it hybridizes to sp3, it can form four bonds. "The linear geometry of ethane is not affected by the hybrid orbital..." I think this is saying carbon forms sp3 orbitals to form four bonds, but they must not be used to form ethyne. It seems as though they could have asked, "What is the hybridization of the carbon in ethyne?"

[kriggy]

I dont see any question except those Gregory asked. I think it is missing something IMO.

[kekie]

Sp3 has a tetrahedral structure - like a D4 die - Sp2 has Trigonal planar structure, and Sp has a linear structure. Is this what you're asking for?

http://en.wikipedia.org/wiki/Orbital_hybridisation#sp3_hybrids
http://en.wikipedia.org/wiki/Trigonal_planar_molecular_geometry
http://en.wikipedia.org/wiki/Orbital_hybridisation#sp_hybrids

[Irlanur]

Hybridization is NOT a physical process. It's just a theoretical concept to account for the local symmetry of the carbon atom.

[GregoryC4]

Sorry for not making the question more clear. The question is: Explain the bonding and shape of ethyne, C2H2(g), using the hybridization theory. The bonding would be stronger as well as more stable after hybridization, but how does hybridization affect the shape of ethyne?

[kekie]

It would make it linear/have a bond angle of 180 degrees. See my previous posts third link.

[kekie]

Oh, and I would recommend;
https://www.khanacademy.org/science/organic-chemistry/gen-chem-review/hybrid-orbitals-jay/v/sp3-hybrid-orbitals-jay
For a full explanation.