The 2p sub-level can hold a maximum of 6 electrons. The 2p sub-level is divided into 2px, 2py and 2pz. Each of those orbitals can hold a maximum of 2 electrons. There are 3 of them and thus 6 total for the 2p sub-level.
The maximum number of electrons in the s orbital is 2.
The 2s orbital has only 2 electrons. There are 8 total electrons in the 2 level set of orbitals - 2s2 2px2 2py2 2pz2
There are maximally two electrons in any s subshell.
In a 2p orbital, a maximum of 6 electrons are allowed.
Every s-orbital can carry two electrons at most.
A maximum of two electrons can be accommodated in each s orbital.
Each orbital can accommodate two electrons. There is one s orbital per principal quantum number, so for any Ns orbital level there are a maximum of two electrons.
It has the maximum capacity of holding only 2 electrons
It can accommodate 2 electrons.
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The 2s orbital and 3s orbital both have the same spherical shape and can hold a maximum of two electrons of opposite spin. They only differ because the 3s orbital is further out from the nucleus than the 2s orbital, thus the 3s orbital has a higher energy value.
First orbital can be occupied by a total of 2 electrons and the second orbital can be occupied by a total of 8 electrons. 1s^2 2s^2 2p^6 ( what element is this ? )
2
2s: 2 electrons 5p: 6 4f: 14 3d: 10 4d: 10
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When n=2, you have an s orbital with 2 electrons, and you have 3 p orbitals each with 2 electrons (total of 6). So, total number of electrons for n=2 is 8 electrons.
The 2s orbital and 3s orbital both have the same spherical shape and can hold a maximum of two electrons of opposite spin. They only differ because the 3s orbital is further out from the nucleus than the 2s orbital, thus the 3s orbital has a higher energy value.
First orbital can be occupied by a total of 2 electrons and the second orbital can be occupied by a total of 8 electrons. 1s^2 2s^2 2p^6 ( what element is this ? )
A total number of 8 electrons. Two in the 2s orbital and six in the 2p orbital
2
The maximum number of electrons in any s sublevel is 2, irrespective of what the principal quantum number, i.e., the number before the s in an electron configuration, may be.
2s: 2 electrons 5p: 6 4f: 14 3d: 10 4d: 10
4 electrons. First orbital is the 1s which has 2 electrons. Second orbital is the 2s which has 2 electrons.
There can be 10 electrons in the n=2 shell. Two can fit in the 1s orbital, two can fit in the 2s orbital, and six can fit in the 2p orbital.
Nitrogen has 5 valence electrons. Valence electrons are the electrons that are found in the outer most shell of an atom, and are consequently the electrons that move from atom to atom in the formation of compounds. The reason for this is a result of the electron configuration. A nitrogen atom has 3 orbitals; the 1s orbital, the 2s orbital, and the 2p orbital. In this case, the 2s and 2p orbitals are the valence orbitals, as they have the electrons with the most energy. With 7 protons, a neutral nitrogen atom has 7 electrons. The s orbitals can only hold 2 electrons, and the p orbitals can hold up to 6 electrons. The 1s orbital is filled first, leaving five electrons, then the 2s orbital is filled, leaving 3 electrons, and then these remaining electrons fill the 2p orbital halfway. There are a total of 5 electrons in the 2s and 2p orbitals, and since these orbitals have the most energy, there are 5 valence electrons.
In the excited state of Beryllium the electron configuration is Be = 1s2 2s1 2p1 this is caused by one electron from 2s orbital jumping to 2p orbital to create a new orbital to allow maximum bond capacity. Maximum bond capacity is mostly used in hybridization in organic chemistry. The two new orbitals that have 1 electrons need to get a pair so each can pair with 1 electron thus making Beryllium bond with 2 electrons.