Which of the following electronic transitions in a hydrogen atom will require the largest amount of energy?

Question

Which of the following electronic transitions in a hydrogen atom will require the largest amount of energy? (A) From n = ∞ to n = 1 (B) From n = 1 to n = 2 (C) From n = 2 to n = 5 (D) From n = 5 to n = 1

Tardigrade Admin · Accepted Answer

As ‘n’ increases the difference in energy between successive orbits decreases
From

n = 1

to

n = 2

, difference in energy,

Δ E = E_{2} - E_{1} = 10.2 e V

From

n = 1

to

n = \infty

,

Δ E = E_{\infty} - E_{1} = 0 - (13.6) = 13.6 e V

∴

From

n = 2

to any higher stationary state,

Δ E \leq

(13.6 - 10.2 = 3.4 e V)

In option

(1)

and

(4)

, energy is released

Q. Which of the following electronic transitions in a hydrogen atom will require the largest amount of energy?

From $n = \infty$ to $n = 1$

From $n = 1$ to $n = 2$

From $n = 2$ to $n = 5$

From $n = 5$ to $n = 1$

Q. Which of the following electronic transitions in a hydrogen atom will require the largest amount of energy?

From n=∞ to n=1

From n=1 to n=2

From n=2 to n=5

From n=5 to n=1

From $n = \infty$ to $n = 1$

From $n = 1$ to $n = 2$

From $n = 2$ to $n = 5$

From $n = 5$ to $n = 1$