Question

DOES ANYBODY TAKE CHEMISTRY AT CONNECTIONS....





I was wondering if you could possibly help me with understanding the periodic trends lab and possibly tutoring.....PLEASE LET ME KNOW ASAP!!!!!!!!!!!!!!!!!!!! I'M DESPERATE

Answer 1

What is your question?

Answer 2

What is electron configuration?

Answer 3

describes the number of electronic energy sublevels of an atom.

Answer 4

How do you solve for it for each element on the periodic table... Like for period 2 Li to Ne

Answer 5

My teacher has had us research periodic trends and now wants us to do this complex lab.... So I'm a little confused

Answer 6

Well, you know that everytime that you start a new row, you go back to s-orbital.
For instance, you know that helium, He has a electron configuration of 1s\(^2\). The 1 meaning row 1 I believe, and the s\(^2\) means it has TWO electrons. Since you know that s-orbitals can hold a max of 2 electrons.

Now, if we look at carbon, C, we can see that it is in row 2. So, in terms of electron configuration, you can look at the number above. It not only has the 2 electrons from the
1s\(^2\) and 2s\(^2\) orbital, but it also has 2p\(^2\) since it is on the p-orbital level.

Answer 7

anything that is on the number above where it says 13-18 is in the p-orbital range!
And the p-orbital can hold a maximum of 6 electrons! Giving it a maximum of 2 + 2 + 6 = 10 electrons!

That means that you have, for carbon: \(\uparrow \downarrow\), \(\uparrow \downarrow\), and \(\uparrow \downarrow\)

Now, what if I asked for electron configuration for, Nitrogen, N?
Well, just ADD one more electron! The electron configuration for nitrogen would be:
1s\(^2\)2s\(^2\)2p\(\sf \color{red}{^3}\)

Answer 8

And electron wise, that means that you have: \(\uparrow \downarrow\), \(\uparrow \downarrow\), and \(\uparrow \downarrow~\uparrow \)

Answer 9

I hope this is making sense, if you have questions, feel free to ask.

Answer 10

Kinda lol...I'm still a little lost but your description has definitely helped me out sooooo much!!! Thanks

Answer 11

One question @abb0t what ionization energy levels to the transition elements have...or do they have any?

Answer 12

Transition metals are a bit tricky, they occupy a lower sub-level than others, and they occupy electrons in the d-orbital. Which can hold a total of 10 electrons.
Also, they can occupy various charges, meaning they can occupy different number of electrons

Answer 13

Also, where are you still "lost" so I can try and clarify a bit more. I realize this is a lot to take in, but you also need to try and study this on your own. I'm trying to give you a very basic general overview to a complex topic thats studied in both inorganic and quantum chemistry.