sp hybridization results in a pair of directional sp hybrid orbitals pointed in opposite directions. We will get two sp hybrid orbitals since we started with two orbitals (s and p). An sp hybrid orbital results when an s orbital is combined with p orbital (Figure 2). This only happens when two atoms, such as two carbons, both have two p orbitals that each contain an electron. These p orbitals come into play in compounds such as ethyne where they form two addition? bonds, resulting in in a triple bond. These p orbitals are at right angles to one another and to the line formed by the two sp orbitals.įigure 1: Notice how the energy of the electrons lowers when hybridized. Because only one p orbital was used, we are left with two unaltered 2p orbitals that the atom can use. This formation minimizes electron repulsion. The front lobes face away from each other and form a straight line leaving a 180° angle between the two orbitals. In it, the 2s orbital and one of the 2p orbitals hybridize to form two sp orbitals, each consisting of 50% s and 50% p character. Sp Hybridization can explain the linear structure in molecules. However, the structure of each molecule in ethene, the two carbons, is still trigonal planar. Because a double bond was created, the overall structure of the ethene compound is linear. These orbitals form a ? bonds through p-p orbital overlap, creating a double bond between the two carbons. This leaves us with the two p orbitals on each carbon that have a single carbon in them. The remaining sp 2 orbitals on each carbon are bonded with each other, forming a bond between each carbon through sp 2-sp 2 orbital overlap. For each carbon, two of these sp orbitals bond with two 1s hydrogen orbitals through s-sp orbital overlap. These hybridized orbitals align themselves in the trigonal planar structure. For each carbon, one 2s orbital and two 2p orbitals hybridize to form three sp 2 orbitals. Similar hybridization occurs in each carbon of ethene. The three Al sp 2 orbitals bond with with 1s orbitals from the three hydrogens through sp 2-s orbital overlap. In aluminum trihydride, one 2s orbital and two 2p orbitals hybridize to form three sp 2 orbitals that align themselves in the trigonal planar structure. Sp 2 hybridization results in trigonal geometry.Įxample: sp 2 Hybridization in Aluminum Trihydride Hybridization of an s orbital with two p orbitals ( p x and p y ) results in three sp 2 hybrid orbitals that are oriented at 120 o angle to each other (Figure 3). The remaining p orbital remains unchanged and is perpendicular to the plane of the three sp 2 orbitals.Įnergy changes occurring in hybridization The frontal lobes align themselves in the trigonal planar structure, pointing to the corners of a triangle in order to minimize electron repulsion and to improve overlap. In it, the 2s orbitals and two of the 2p orbitals hybridize to form three sp orbitals, each consisting of 67% p and 33% s character. Sp 2 hybridization can explain the trigonal planar structure of molecules. The next section will explain the various types of hybridization and how each type helps explain the structure of certain molecules. This results in more stable compounds when hybridization occurs. The hybridization of orbitals is favored because hybridized orbitals are more directional which leads to greater overlap when forming bonds, therefore the bonds formed are stronger. Now that carbon has four unpaired electrons it can have four equal energy bonds. That would give us the following configuration: One way CH 4 can be explained is, the 2s and the 3 2p orbitals combine to make four, equal energy sp 3 hybrid orbitals. To form four bonds the configuration of carbon must have four unpaired electrons. Therefore, this does not explain how CH 4 can exist. Carbon's ground state configuration is:Īccording to Valence Bond Theory, carbon should form two covalent bonds, resulting in a CH 2, because it has two unpaired electrons in its electronic configuration.However, experiments have shown that \(CH_2\) is highly reactive and cannot exist outside of a reaction. \)Ĭarbon is a perfect example showing the value of hybrid orbitals.
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