The following is a diagram of energy states and transitions in the hydrogen atom. Match each arrow with the correct response below. The emission line with the longest wavelength. The absorption line with the longest wavelength. The emission line with the highest energy. The absorption line with the highest energy. The emission line with the lowest frequency. The line corresponding to the ionization energy of hydrogen.

wave length is inversely proportional to frequency of radiation
the relation between frequency f and wavelength lamda
f= hc/lamda
Also energy and frequency are directly proportional
E= h x frequency
Thus from above to formulas it is clear that
1.Longest wavelength will have lowest frequency[thus lowest energy]
2.Shortest wavelength will have highest frequency[thus highest energy]
also
**Emission takes place when electron move from higher level to
lower level
**Absorption takes place when electron move from lower to higher
Using above points let us answer this

a) emission with longest wavelength means it emit light with least energy
Answer 5. from n=2 to n=1

b) The absorption line with longest wavelength-it needs least energy
Answer.1 -- from n=1 to n=2

c) emission line with highest energy- Transfer of electron from
highest to the lowest level happens
Answer 4-- from n=4 to n=1

d)
The absorption line with highest energy
Answer 3--- from n=1 to n=infinity

e) emission with lowest frequency-means longest wavelength

Answer. 5--from n=2 to n=1

f) the lie corresponds to ionization energy- It is the energy
needed to take electron from n=1 to infinity

Answer.3 -- from n=1 to n=infinity