Hybridized Orbitals

myminifactory

This is a set of hybridized orbitals based on BlendLab's orbital shape, combining basic sp hybridized orbitals, sp2, and sp3 models. Unhybridized p orbitals are included for connection to the sp and sp2 models, demonstrating pi-bond orbital overlaps. ***This work in progress still has slightly off bond angles for the sp3 model. For best results, use hot glue to attach unhybridized orbitals to the models. Molecules have three-dimensional shapes that play a crucial role in their function, especially in biological systems. This model helps students visualize these shapes and understand the reasons they form based on hybridization and VSEPR theory. Students will gain insight into how orbitals combine when covalent bonds are formed. Students will be able to describe how orbital shapes relate to VSEPR theory. Students will understand the difference between pi and sigma bonds based on orbital overlap. Students will be able to relate orbital arrangement to molecular shape. Preparation: Students should already be familiar with atomic orbitals, valence shell electron repulsions (VSEPR) theory, single, double, and triple covalent bonds. Describe how s and p orbitals combine to form covalent bonds that repel each other, resulting in hybrid orbitals. This set can be combined with the atomic orbital set. Draw a tetrahedral molecule and discuss how it requires orbitals pointing in the correct directions to form. Show the relative positions of s and p orbitals using the atomic orbital set first, then demonstrate how these four orbitals combine into four hybrid orbitals in this set. Note that the farthest these four orbitals can get from each other is 109.5° as shown in the sp3 model. Next, draw a trigonal planar carbon molecule with one double bond on the board and discuss how only three orbitals are needed, resulting in the combination of one s orbital and two p orbitals to form three hybrid orbitals and the sp2 shape. Point out that there is a leftover p orbital. Use provided unhybridized p orbitals to show how these stick out from the shape. Use a second sp2 model with attached p orbitals to discuss how the double bond forms, which can then be used to differentiate sigma and pi bonds. More advanced classes can use these models to discuss bond rotation. Draw a linear carbon molecule with a triple bond and a single bond, repeating the procedure above and noting that two p orbitals are left over. Use the sp model and unhybridized p orbitals to demonstrate the formation of two pi bonds with this geometry.