1. Calculate the wavelength and frequency of light emitted when an electron changes from N=6 to N=3 in the H atom.

Wavelength: m

Frequency: s^-1

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2. In what region of the spectrum is this radiation found?

a) visible light region

b) x-ray region

c) infrared region

d) ultraviolet region

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69. Calculate the wavelength of the light emitted when an electron in a hydrogen atom makes each transition and indicate the region of the electromagnetic spectrum (infrared, visible, ultraviolet, etc.) where the light is found. a. n = 2 n =1 b. n = 32n =1 C. M = 4 + n = 2 d. n = 5 — = 2

1. Radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. It is this radiation that causes dyes to fade and your skin to develop a sunburn. If you are bombarded with 1.00 mol of photons with a wavelength of 355 nm, what amount of energy, in kilojoules per mole of photons, are you being subjected to?

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2. Calculate the wavelength and frequency of light emitted when an electron changes from N=6 to N=3 in the H atom.

Wavelength = ___ m

Frequency = ___ s^-1

Calculate the wavelength of the light emitted when an electron in ahydrogen atom makes each of the following transitions as well asstate the region of the electromagnetic spectrum (infrared,visible, ultraviolet, etc.) where the light in part a,b,c, and dare found.

A. n = 2 -----> n = 1
_________________m

B. n = 3 ------> n =1
_________________m

C. n = 4 ------> n = 2
________________m

D. n = 5 -------> n = 2
________________m