what is the name of the hybrid orbitals used by phosphorus in pcl3? This is a topic that many people are looking for. secret-life.org is a channel providing useful information about learning, life, digital marketing and online courses …. it will help you have an overview and solid multi-faceted knowledge . Today, secret-life.org would like to introduce to you Orbital Hybridization of Phosphorus. Following along are instructions in the video below:
Do yall. Mr. Cozzi.
Come to you from beautiful atascocita in texas with another another homework. Helper and today. Were gonna talk about orbital hybridization of phosphorus.
So out your periodic table and get ready to be amazed. Im gonna make a few assumptions. Im going to assume that you understand valence electrons that you know how to write lewis symbols you know electron configuration and you are familiar with orbital hybridization.
If youre not familiar with any of these topics. Please go to my youtube channel and check out the movies. Remember that orbital hybridization is the combining of valence orbitals to create orbitals of equal energy.
Now heres the problem.
How is it that phosphorus can have five bonds such as phosphorus pentachloride. Its because of orbital hybridization and lets take a look and see how can that happen. What is the possible hybridization of phosphorus well first lets look at the electron configuration.
Then lets decide on the valence electrons third. Well draw the lewis dot symbol fourth. Well check the electron notation and finally we will determine the hybridization of phosphorus that allows it to make five bonds.
So the configuration bring up your periodic table. Find phosphorus note. What its electron configuration.
Is 1s2. 2s2 and 2p. Six.
Are the first two energy levels.
Then we have three s 2. And free p. 3.
Which are our valence electrons. So we have five valence electrons now back to the blackboard and right up. There well put the electron configuration and lets look at the decimal and youll notice.
There we have only three bonds not the five bonds that we need. But hybridization is the answer to our problems. So first lets go and look at the orbital to give an idea of how this happens and so ill ride up the orbital rotation on the board and note that what were going to do is take an electron from the 3s and were going to jump.
It over into the 3d. Now notice that gives us five available electrons for five covalent bonds. Three s1 and then we have free three piece and then we also have one 3d and 1s plus three ps plus 1 d is 5 sp.
Now if youre not sure how to name those be sure to look up on my channel for an atomic hybridization now. We see that we have 5 sp. 3 d.
Which will give us a shape as on the right and we have 5 bonds and then of course. If we had 5 chlorine atoms bonding that would give us a trigonal bi pyramidal shape. That is the answer to our question.
How can phosphorous have 5 bonds. Instead of 3. Lets recap.
You wrote. The electron configuration you determine the valence electrons. You drew the lewis dot symbol.
You determine the orbital hybridization and you found out how phosphorous can have 5 bonds well thanks for watching dont forget to give me a thumbs up if this was helpful and check out my videos and most of all dont forget to subscribe. Thank you so much now happy ions yall. .
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