![]() ![]() The most straightforward hybridization is accomplished by mixing the single 2s orbital containing 2 electrons, with all three p orbitals, also containing a total of 2 electrons. Watch the video below for a quick overview of sp³ hybridization with examples. Today, I will focus heavily on sp³, sp² and sp hybridization, but do understand that you can take it even further to create orbitals like sp³ d and sp³ d², as well (brief mention at the end). The number of electrons that move and orbitals that combine, depends on the type of hybridization we’re looking to create. Instead, each electron will go into its own orbital. Now that we have a total of 4 degenerate orbitals and 4 electrons, why would we make them share a ‘room’ if they don’t have to? Why would we choose to share once we had the option to have our own rooms?Įlectrons are the same way. When we moved to an apartment with an extra bedroom, we each got our own space. We didn’t love it, but it made sense given that we’re both girls and close in age. Growing up, my sister and I shared a bedroom. This gives us 4 degenerate orbitals, meaning orbitals that have the same amount of energy. We take that s orbital containing 2 electrons and give it a partial energy boost.Īt the same time, we rob a bit of the p orbital energy. Here is how I like to think of hybridization. So what do we do, if we can’t follow the Aufbau Principle?Įnter hybridization! How does hybridization occur? This too is covered in my Electron Configuration videos. This can’t happen though, because the Aufbau Principle says that electrons must fill atomic orbitals from lowest to highest energy. If we can find a way to move ONE of the paired s electrons into the empty p orbital, we’d get something like this. Which isn’t very helpful if we’re trying to build complex macromolecules. With its current configuration, carbon can only form 2 bonds,
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