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June 29, 2016
Posted by **Hannah** on Tuesday, November 1, 2011 at 10:28pm.

34

2) Write the full electron configuration for selenium following the (n+l) rule?

I am not sure what is meant by n+l

3) write the electron configuration, grouping electrons by their "n" values.

[Ar]3d10 4s2 4p4

Are these correct?

4) What is the number of valence electrons for selenium?

6

what is the number of core electrons?

I do not understand what core electrons are.

5) what is the number of unpaired electrons? Show how you determined this.

i think the answer is two but im not sure why.

6) What is the number of filled shells?

3

7) What is the number of filled orbitals?

4

Are these correct?

Please ignore the first two posts with these questions. My computer was acting up and submitted the question more than once. Sorry.

- Chemistry -
**DrBob222**, Wednesday, November 2, 2011 at 12:53am1) What is the atomic # for selenium?

34**The atomic number is 34, what else?**

2) Write the full electron configuration for selenium following the (n+l) rule?**I must admit I don't know what the n+one rule is (although that could be n + ell rule). However the electron configuration is**

[Ar]3d10 4s2 4p4

I am not sure what is meant by n+l

3) write the electron configuration, grouping electrons by their "n" values.

[Ar]3d10 4s2 4p4**I would write 2,8,18,6 for n = 1,2,3,and 4.**

4) What is the number of valence electrons for selenium?**6. Those are the 4s2 4p4 and you are correct.**

6

what is the number of core electrons?

I do not understand what core electrons are.**The core electrons are those inside the valence shell; i.e., that will be 34-6 = 28. Another way to look at it is to look at the n shells of 2,8,18,6 and take off the last 6 which leaves 2,8,and 18 = 28.**

5) what is the number of unpaired electrons? Show how you determined this.**You have 4s2 4p4 in the valence shell (all of the others are paired; i.e., the 2, 8, and 18). The two in 4s2 are paired. That leaves just the 4p4 electrons to worry about. Since there are three p orbitals (the Px, Py, Pz) and Hund's rule says we fill all orbitals BEFORE we start pairing which means we have 1 in Px, 1 in Py, and 1 in Pz. The fourth one must pair up with the 1 already there in Px and there are no more electrons. Therefore, that leaves the last two electrons, 1 in Py and 1 in Pz, unpaired. So the answer is 2 unpaired electrons. So you are right!**

i think the answer is two but im not sure why.

6) What is the number of filled shells?

3**right.**

7) What is the number of filled orbitals?

4**I'm not sure what the question means by filled orbitals. Is that completely filled or partially filled. Either way it is a filled orbital. I would count 1s2 as 1 orbital + 2s2 as 1, + 2p6 as 3, + 3s2 as 1, 3p6 as 3 + 3d10 as 5 + 4s2 as 1 + 4p2 as 1 and I'm not counting the last two unpaired since those orbitals are only partially filled. You can add those numbers but I think that is 16. If you interpret the question differently you can adjust the answer.** - Chemistry -
**Hannah**, Wednesday, November 2, 2011 at 10:53amThank you for your help!!!