I don't even know how to start this...The valence electron configurations of several atoms are shown below. How many bonds can each atom make without hybridization?
1. Si 3S2 3P2
2. P 3S2 3P3
3. F 2S2 2P5
Hey! So remember electron orbitals will fill up one by one. If you have Si notated by 3s2 3p2, you have 2 electrons that are unpaired, right? That means you can have 2 bonds.
With P (3s2 3p3), you have 3 electrons that are each unpaired in the 3 p orbitals, so P can make 3 bonds without hybridization.
With F (2s2 2p5), you'll have 1 unpaired electron. Since p has 3 orbitals, and you have 5 electrons, you'll start with one in each orbital (3 electrons) then the 2 left over will each join an orbital, so 2 of your 3 p orbitals are full. That means you have 1 unpaired electron, so you can have 1 bond without hybridization.
I realize I'm answering this question 4 years later, but hopefullly others can benefit from the explanation. :)
Emma, it did benefit someone! thanks for the awesome and easy explanation.
Shout out to Emma for making this so simple.
Help, exam on monday!!
Emma you're my hero :)
It's a question in Mastering Chemistry, I don't know how else to reword it? That's their words =( I did plug in those #'s and it came back wrong, but it doesnt show me the right anwsers....so I dunno??
Emma, you saved my life. Thank you.
I wish you could @ people. Emma you saved my life. Thanks
Thanks Emma, Stacy may have failed but me in 2020 I’ll learn from her mistakes.
Thank you for the help Emma.
1)2
2)2
3)1
I'm a little confused about the question; however, my best guess is that we determine the electron loss/gain. Do you have a way of verifying the answer?
For Si, 3s2 2p2 means valence of +4 (4 bonds or 4 more electrons to make 8).
P of 3s2 2p3 = 3 (5 electrons 3 more to make 8).
F of 2s2 2p5 = 1 (7 electons + 1 mor to make 8).