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∙ 10y agoms=-1/2
Anand Krishnan
ms -1/2
ms -1/2
The next highest energy atomic sublevel after 4p is the 5s sublevel. In the electron configuration of an atom, energy levels increase with increasing principal quantum number (n), so the 5s sublevel is higher in energy than the 4p sublevel.
The s sublevel in the third main energy level indicates that the electrons are in the third energy level (n=3) and have a spherical shape. The s sublevel can hold a maximum of 2 electrons.
The second energy level can hold a maximum of 8 electrons when it is full. This level can accommodate two electrons in the first sublevel (s) and six electrons in the second sublevel (p).
The second quantum number (l) for the electrons in the 4 p energy sublevel of bromine would be 1.
ms -1/2
M1 = -1
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l = 1
ms -1/2
M1 = -1
The unabbreviated electron configuration for bromine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5. It indicates the distribution of electrons in each energy level and sublevel of the bromine atom.
The sixth energy level can hold up to 72 electrons, with each sublevel accommodating a specific number of electrons: s sublevel = 2 electrons, p sublevel = 6 electrons, d sublevel = 10 electrons, and f sublevel = 14 electrons.
The next highest energy atomic sublevel after 4p is the 5s sublevel. In the electron configuration of an atom, energy levels increase with increasing principal quantum number (n), so the 5s sublevel is higher in energy than the 4p sublevel.
There are two sublevels in the second principal energy level: the s sublevel and the p sublevel. The s sublevel can hold a maximum of 2 electrons, while the p sublevel can hold a maximum of 6 electrons.
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