I\'m learning about hybrid orbitals and both my book andprofesor can\'t seem to

Question

I'm learning about hybrid orbitals and both my book andprofesor can't seem to explain the concept of hybrid orbitals in anunderstandable way. I don't grasp what exactly is a hybrid orbital,or how to tell which type of hybrid orbital is formed. I don't evenget when one can make a hybrid orbital. Basically, if someone couldexplain things simply and clearly, that would be good. As to a specific question (which may help explaination0, whatis the hybrid orbital of BeH2? Its sp orbital, but Idon't get why. Thanks ahead of time, as I know this question is loaded. I'm learning about hybrid orbitals and both my book andprofesor can't seem to explain the concept of hybrid orbitals in anunderstandable way. I don't grasp what exactly is a hybrid orbital,or how to tell which type of hybrid orbital is formed. I don't evenget when one can make a hybrid orbital. Basically, if someone couldexplain things simply and clearly, that would be good. As to a specific question (which may help explaination0, whatis the hybrid orbital of BeH2? Its sp orbital, but Idon't get why. Thanks ahead of time, as I know this question is loaded.

Explanation / Answer

Hybridization accounts for the bond-angles with each geometricshape. This is because an atom will hybridize as many orbitals asneeded in order to form -bonds with other atoms. Lone pairscomplicate matters but also are taken into account when assigninghybridization. So the key to determinehybridization is to count how many atoms the central atom will bonddirectly to (including lone pairs as a region of electron density,but not counting -bonds). Let's use carbon to explain how hybridization works. Carbon is inthe 2nd period, whose valence electrons are in the 2nd energylevel. This energy level contains 1 s-orbital, and 3p-orbitals. Draw the -bond skeleton of the following structures, withoutincluding -bonds if any. For example, take CH4. The carbon isbonding to four atoms ofhydrogen, therefore it will hybridize all four ofits orbitals to form -bonds. Thus is uses 1 s orbital and 3 porbitals (hence sp3) With Ethene, CH2CH2, each carbon isbonding to three atomsthrough -bonds, therefore will hybridize three of itsorbitals - 1 s orbital, and 2 p orbitals (hencesp2). The oneunhybridized p orbital is used to form a -bond. Finally with Ethyne, CHCH, each carbon is bonding to two atoms through -bonds, therefore will hybridize twoof its orbitals - 1 s orbital and 1 p orbital (hencesp). The two unhybridizedp orbitals are used to form two -bonds. Thus in BeH2, the Be atomis bonding directly to two atoms through -bonds. Thereforeits hybridization is sp just like the carbons in Ethyne. We can also use that rule for Hydrogen. It is bonding to one atomthrough a -bond, therefore will be an s configuration(hydrogen also only has an s-orbital since it is in period1) Note: The actual process of hybridization involves promotion of anelectron from the s-orbital to give half-filled orbitals. To"hybridize" means to combine, and in this case, the s and porbitals combine to form a new orbital shape with a differentquantum value.

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