1 Answers
The sharp series is a series of spectral lines in the atomic emission spectrum caused when electrons descend from higher-energy s orbitals of an atom to the lowest available p orbital. The spectral lines include some in the visible light, and they extend into the ultraviolet. The lines get closer and closer together as the frequency increases never exceeding the series limit. The sharp series was important in the development of the understanding of electron shells and subshells in atoms. The sharp series has given the letter s to the s atomic orbital or subshell.
The sharp series has a limit given by
v = R 2 − R 2 with m = 2 , 3 , 4 , 5 , 6 , . . . {\displaystyle v={\frac {R}{\left^{2}}}-{\frac {R}{\left^{2}}}{\text{ with }}m=2,3,4,5,6,...}
The series is caused by transitions to the lowest P state from higher energy S orbitals.One terminology to identify the lines is: 1P-mS But note that 1P just means the lowest P state in an atom and that the modern designation would start at 2P, and is larger for higher atomic numbered atoms.