The electronic energy level in a hydrogen atom is J higher than the level.If an electron moves from the level to the level then a photon of wavelength
A) 1.3 nm,which is in the ultraviolet region,is emitted.
B) 1.3 nm,which is in the ultraviolet region,is absorbed.
C) 1,300 nm,which is in the infrared region,is absorbed.
D) 1,300 nm,which is in the infrared region,is emitted

Question

The  electronic energy level in a hydrogen atom is  J higher than the  level.If an electron moves from the  level to the  level then a photon of wavelength
A) 1.3 nm,which is in the ultraviolet region,is emitted. 
B) 1.3 nm,which is in the ultraviolet region,is absorbed. 
C) 1,300 nm,which is in the infrared region,is absorbed. 
D) 1,300 nm,which is in the infrared region,is emitted

Quizplus · Accepted Answer

When an electron moves from a higher energy level to a lower energy level in a hydrogen atom, a photon is emitted. The wavelength of the photon can be calculated using the Rydberg formula:

1/λ = R*(1/n1^2 - 1/n2^2)

where λ is the wavelength of the photon, R is the Rydberg constant, and n1 and n2 are the initial and final energy levels, respectively.

In this case, the electron is moving from the 11eaa3e3_41a2_98f6_a4ea_c9dc499a374b_TB4068_11 level to the 11eaa3e3_41a2_98f7_a4ea_0b0d408aa259_TB4068_00 level, so n1=2 and n2=1. Plugging these values into the Rydberg formula gives:

1/λ = R*(1/2^2 - 1/1^2)
1/λ = R*(3/4)
λ = 4/3R

The value of the Rydberg constant is 1.097 × 10^7 m^-1, so:

λ = (4/3)*(1.097 × 10^7 m^-1)
λ = 1.463 × 10^7 m^-1 = 1,463 nm

Therefore, the photon emitted when the electron moves from the 11eaa3e3_41a2_98f6_a4ea_c9dc499a374b_TB4068_11 level to the 11eaa3e3_41a2_98f7_a4ea_0b0d408aa259_TB4068_00 level has a wavelength of 1,463 nm, which is in the infrared region. So the correct answer is D) 1,300 nm, which is in the infrared region, is emitted.

The Electronic Energy Level in a Hydrogen Atom Is