Choose the correct match
A)Gama line in Lyman series in H--UV
B)Beta line in Balmer series in He+---UV
C)Delta line in Balmer series in H---visisble
D)Delta line in Paschen series in H--- Infrared
Answer is all the options are correct but I don't understand how B is correct. Also explain the others. How can a beta line in Balmer series in He+ is UV. How do I know if it will be UV. It must be visible?
Lyman series is transition from n=1 to higher orbits.
Alpha line is the first transition, i.e from n=2 to n=1, beta is from n=3 to n=1. gamma is from n=4 to n=1 and so on.....
Balmer series is transition from n=2 to higher orbits.
Alpha line is the first transition, i.e from n=3 to n=2, beta is from n=4 to n=2, gamma is from n=5 to n=2 and so on......
Paschen series is transition from n=3 to higher orbits.
Alpha line is the first transition, i.e from n=4 to n=3, beta is from n=5 to n=3, gamma is from n=6 to n=3 and so on......
We can find the wavelength corresponding to these transitions by applying the formula:
a) Lyman-alpha is wavelength corresponding to n=2 to n=1
See that this Lyman series lines is in UV region (less tan 400 nm).
b) Beta line in Balmer series in He+ is line corresponding to n=4 to n=2.
Rydberg constant, R for He is 4 times (Z2 and Z=2 for He) the Rydberg constant of Hydrogen.
Beta line in Balmer series in H is in visible region but for He+ the value of Z2 is 4, so the wavelength is four times shorter than the Balmer series of H atom and hence it lies in UV region.
c) Delta line in Balmer series in H can be calculated similarly:
d) Delta line in Paschen series in H
Hope that's clear now.
series is transition from n=1 to higher orbits.
Balmer series is transition from n=2 to higher orbits.
Paschen series is transition from n=3 to higher orbits.
We can find the wavelength corresponding to these transitions by applying the fomula:
After applying the fomula and finding the wavelengths you will find that all the Lyman series lines are in UV region.
Beta line in Balmer series in H is in visible region but for He+ the value of Z2 is 4, so the wavelength is four times shorter than the Balmer series of H atom and hence it lies in UV region.
Alpha line is the first transition, i.e from n=2 to n=1, beta is from n=3 to n=1. gamma is from n=4 to n=1 and so on.....
Balmer series is transition from n=2 to higher orbits.
Alpha line is the first transition, i.e from n=3 to n=2, beta is from n=4 to n=2, gamma is from n=5 to n=2 and so on......
Paschen series is transition from n=3 to higher orbits.
Alpha line is the first transition, i.e from n=4 to n=3, beta is from n=5 to n=3, gamma is from n=6 to n=3 and so on......
We can find the wavelength corresponding to these transitions by applying the formula:
a) Lyman-alpha is wavelength corresponding to n=2 to n=1
See that this Lyman series lines is in UV region (less tan 400 nm).
b) Beta line in Balmer series in He+ is line corresponding to n=4 to n=2.
Rydberg constant, R for He is 4 times (Z2 and Z=2 for He) the Rydberg constant of Hydrogen.
Beta line in Balmer series in H is in visible region but for He+ the value of Z2 is 4, so the wavelength is four times shorter than the Balmer series of H atom and hence it lies in UV region.
c) Delta line in Balmer series in H can be calculated similarly:
d) Delta line in Paschen series in H
Hope that's clear now.
series is transition from n=1 to higher orbits.
Balmer series is transition from n=2 to higher orbits.
Paschen series is transition from n=3 to higher orbits.
We can find the wavelength corresponding to these transitions by applying the fomula:
After applying the fomula and finding the wavelengths you will find that all the Lyman series lines are in UV region.
Beta line in Balmer series in H is in visible region but for He+ the value of Z2 is 4, so the wavelength is four times shorter than the Balmer series of H atom and hence it lies in UV region.