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Silver Shell

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Frequently Asked Questions...

what is the electronic structure of silver?

im looking at how the electrons of more complex elements orbit the nucleus, so how many electrons and shells would there be?


Answer:

Ag has 47 electrons.

Here is the order of filling out the electron configuration for an element:

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6p^6 7s^2 5f^14 6d^10 7p^6

You can look at the electron configuration and find the valence electrons so first you need the electron configuration for each element.

First, I'll write out the entire electron configuration which you need to know how to do in order to know how to write each element's electron configuration;

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6p^6 7s^2 5f^14 6d^10 7p^6

You can memorize this order or use a mnemonic diagram that helps in writing the electron configuration:

1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p

First draw an arrow through the 1s going down diagonaly from right to left and then write 1s down.

Second go to the next row and draw an arrow through 2s the same way and write 2s after the 1s.

Third go over to 2p and draw an arrow through this and the 3s in the next row and write down 2p 3s after the 1s 2s.

Fourth go to the third row and since you've already drawn an arrow through 3s go to 3p and draw an arrow through this and the 4s in the next row and write down 3p 4s after the 1s 2s 2p 3s.

Continue doing this until you have draw an arrow through every sublevel and have the entire electron configuration written out.

A few things to remember: s sublevel holds a maximum of 2 electrons, p sublevel holds a maximum of 6 electrons, d sublevel holds a maximum of 10 electrons, and f sublevel holds a maximum of 14 electrons.

Here are a couple of websites that show a picture of what I was explaining with the diagram:

https://chemistry.twu.edu/tutorial/AufbauSum.html

http://chemistry.about.com/od/electronicstructure/ss/aufbau_2.htm

so to do Ag, keep filling orbitals until you've depleted all 47 electrons:

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^9

There are exceptions to the Aufbau principal, Ag is one of them.

1.) Completely filled sublevels (in particular more complex ones such as d and f sublevels), are more stable than partially filled sublevels

2.) Half filled sublevels, (in particular more complex more complex ones such as d and f sublevels), are more stable than partially filled sublevels but are less stable than completely filled ones.

3.) Partially filled sublevels are the least stable.

With these 3 exceptions in mind, look at the electron configuration of Ag again:

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^9 notice that the end is 5s^2 4d^9 d is a more complex sublevel than s so it will be more stable if it has a completely filled sublevel; therefore, one of the electrons from 5s goes to 4d to make 4d completely filled and more stable and 5s will be half filled. Having 4d filled and 5s only half filled is more stable than 5s completely filled and 4d partially filled so the electron configuration for Ag is actually:

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^1 4d^10

Hope this helped.

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