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

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  1. Help, exam on monday!!

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  2. 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).

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  3. 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 I dunno??

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  4. 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. :)

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  5. Emma, it did benefit someone! thanks for the awesome and easy explanation.

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  6. 1)2

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  7. Emma, you saved my life. Thank you.

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  8. I wish you could @ people. Emma you saved my life. Thanks

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