Number of visible lines in Balmer's series

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(B) The Balmer series corresponds to transitions of electrons in a hydrogen atom to the $n = 2$ energy level from higher energy levels $(n = 3, 4, 5,

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$4$

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(B) The Balmer series corresponds to transitions of electrons in a hydrogen atom to the $n = 2$ energy level from higher energy levels $(n = 3, 4, 5, 6, \dots)$.Among these,the transitions from $n = 3, 4, 5,$ and $6$ to $n = 2$ result in wavelengths that fall within the visible spectrum.Specifically,the transitions are:$1$. $n = 3 	o n = 2$ ($H_{\alpha}$ line,red)$2$. $n = 4 	o n = 2$ ($H_{\beta}$ line,blue-green)$3$. $n = 5 	o n = 2$ ($H_{\gamma}$ line,blue-violet)$4$. $n = 6 	o n = 2$ ($H_{\delta}$ line,violet)Transitions from $n > 6$ to $n = 2$ result in wavelengths shorter than $364.6 \ nm$,which lie in the ultraviolet region.Therefore,there are exactly $4$ visible lines in the Balmer series.

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