Ground State e- Configuration

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Emilee Hosking 1D
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Joined: Fri Sep 28, 2018 12:17 am

Ground State e- Configuration

Postby Emilee Hosking 1D » Sun Oct 28, 2018 2:34 pm

In problem 2A21, the ground state electron configuration of Ag+ is 4d^10. Why is this the case rather than it being 4d^9 5s^1?

Posts: 64
Joined: Fri Sep 28, 2018 12:15 am

Re: Ground State e- Configuration

Postby 005115864 » Sun Oct 28, 2018 3:02 pm

Hi, to answer your question simply, an element has the tendency to seek stable energy levels. So, in this case stability would be filling the 4d energy level completely before starting to fill the 5s energy level. It typically is easier to fulfill an energy level completely before jumping to a higher energy level. I would refer to the building-up particle AUFBAU Principle.

Rhea Churi 4K
Posts: 62
Joined: Fri Sep 28, 2018 12:28 am

Re: Ground State e- Configuration

Postby Rhea Churi 4K » Sun Oct 28, 2018 4:41 pm

Atoms typically seek to fill each energy level before moving onto the next one as it helps with stability. Thus, Ag would fill up the 4d energy level before moving up.

Luc Lorain 1L
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

Re: Ground State e- Configuration

Postby Luc Lorain 1L » Sun Oct 28, 2018 6:06 pm

You should be able to answer your question after memorizing the number of electrons that each subshell can hold. These numbers are fixed no matter how many shells there are in an atom, and (except for in certain special cases that Dr. Lavelle has singled out) tend to be filled completely before electrons enter the next subshell. Remember that each subshell has a certain number of orbitals (connected to the quantum number ml), which can each hold 2 electrons (one of each type of spin).

To recap, the s subshell has 1 orbital and can hold 2 electrons, the p subshell has 3 orbitals and can hold 6 electrons, the d subshell has 5 orbitals and can hold 10 electrons, and the f subshell has 7 orbitals and can hold 14 electrons.

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