Which is not a ground state electron configuration?
A. 1s2
B. 1s2 2p1
C. 1s2 2s2
D. 1s2 2s2 2p1
Neon has a configuration of:
1s2 2s2 2p6
So do you find one of the choices have electrons that are out of place?
Yes 1s2 2s2 2p1,I am right?
Electrons are filled in order of the orbitals such that there is least energy, or the ground state.
The first to be filled are:
1s2 2s2 2p6 (configuration for neon).
If they are filled out of order, it will be in the excited state (not ground state).
So for
H 1s1
He 1s2
Li 1s2 2s1
Be 1s2 2s2
B 1s2 2s2 2p1
...
Ne 1s2 2s2 2p6
So can you now find one of the choices where the orbitals are filled "out of turn", or not in the ground state?
To help you understand, and as a reference, you can look at:
http://www.mikeblaber.org/oldwine/chm1045/notes/Struct/EPeriod/Struct09.htm
1s2 2p1 is that right? Thank you so much!
I know that 1s2 2s2 2p1 is the excited state of 1s2 2s2 but then 1s2 2p1 its orbital are filled out of turn. So I am kinda confused about it because you said that if its excited state then that means its not ground state and if the orbitals are filled out of turn then that's not in the ground state too. So does it mean that b and d are both not in ground state?
To determine which is not a ground state electron configuration, we need to understand the concept of electron configurations and what a ground state electron configuration represents.
Electron configuration refers to the arrangement of electrons in the energy levels or orbitals around an atomic nucleus. The ground state electron configuration represents the lowest energy arrangement of electrons in an atom.
Let's examine the given options and determine which one is not a ground state electron configuration:
A. 1s2
In this electron configuration, the 1s orbital is filled with 2 electrons, which is the lowest energy level. This is a valid ground state electron configuration since it represents the lowest energy arrangement.
B. 1s2 2p1
This electron configuration represents one electron in the 2p orbital in addition to the 2 electrons in the 1s orbital. However, the ground state electron configuration of carbon (the only atom with this configuration) is 1s2 2s2 2p2, not 1s2 2p1. This means option B is not a ground state electron configuration.
C. 1s2 2s2
This electron configuration represents two electrons in the 2s orbital in addition to the 2 electrons in the 1s orbital. This is a valid ground state electron configuration as it represents the lowest energy arrangement.
D. 1s2 2s2 2p1
This electron configuration represents one electron in the 2p orbital in addition to the 4 electrons in the 1s and 2s orbitals. However, the ground state electron configuration of nitrogen (the only atom with this configuration) is 1s2 2s2 2p3, not 1s2 2s2 2p1. Therefore, option D is not a ground state electron configuration.
In conclusion, the answer is option B. The electron configuration 1s2 2p1 is not a ground state electron configuration.