<Li> The final column gives the historical origin of the labels s, p, d, and f . They come from early studies of atomic spectral lines . The other labels, namely g, h and i, are an alphabetic continuation following the last historically originated label of f . </Li> <P> Although it is commonly stated that all the electrons in a shell have the same energy, this is an approximation . However, the electrons in one subshell do have exactly the same level of energy, with later subshells having more energy per electron than earlier ones . This effect is great enough that the energy ranges associated with shells can overlap (see valence shells and Aufbau principle). </P> <Table> <Tr> <Th> Shell name </Th> <Th> Subshell name </Th> <Th> Subshell max electrons </Th> <Th> Shell max electrons </Th> </Tr> <Tr> <Td> </Td> <Td> 1s </Td> <Td> </Td> <Td> </Td> </Tr> <Tr> <Td> </Td> <Td> 2s </Td> <Td> </Td> <Td> 2 + 6 = 8 </Td> </Tr> <Tr> <Td> 2p </Td> <Td> 6 </Td> </Tr> <Tr> <Td> </Td> <Td> 3s </Td> <Td> </Td> <Td> 2 + 6 + 10 = 18 </Td> </Tr> <Tr> <Td> 3p </Td> <Td> 6 </Td> </Tr> <Tr> <Td> 3d </Td> <Td> 10 </Td> </Tr> <Tr> <Td> </Td> <Td> 4s </Td> <Td> </Td> <Td> 2 + 6 + 10 + 14 = 32 </Td> </Tr> <Tr> <Td> 4p </Td> <Td> 6 </Td> </Tr> <Tr> <Td> 4d </Td> <Td> 10 </Td> </Tr> <Tr> <Td> 4f </Td> <Td> 14 </Td> </Tr> <Tr> <Td> </Td> <Td> 5s </Td> <Td> </Td> <Td> 2 + 6 + 10 + 14 + 18 = 50 </Td> </Tr> <Tr> <Td> 5p </Td> <Td> 6 </Td> </Tr> <Tr> <Td> 5d </Td> <Td> 10 </Td> </Tr> <Tr> <Td> 5f </Td> <Td> 14 </Td> </Tr> <Tr> <Td> 5g </Td> <Td> 18 </Td> </Tr> </Table> <Tr> <Th> Shell name </Th> <Th> Subshell name </Th> <Th> Subshell max electrons </Th> <Th> Shell max electrons </Th> </Tr>

Max number of electrons in the third energy level
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