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Andreyy89
3 years ago
13

N2 molecules absorb ultraviolet light but not visible light. I2 molecules absorb both visible and ultraviolet light. Which of th

e following statements explains the observations?
More energy is required to make N2 molecules vibrate than is required to make I2 molecules vibrate.
A

More energy is required to remove an electron from an I2 molecule than is required to remove an electron from a N2 molecule.
B

Visible light does not produce transitions between electronic energy levels in the N2 molecule but does produce transitions in the I2 molecule.
C

The molecular mass of I2 is greater than the molecular mass of N2.
Chemistry
1 answer:
Umnica [9.8K]3 years ago
4 0

C. Visible light does not produce transitions between electronic energy levels in the N₂ molecule but does produce transitions in the I₂ molecule.

Explanation:

Abortion of light by molecules will produce electronic transitions from a ground level to a higher level equal to the energy of absorbed light.

In the case of nitrogen (N₂) the allowed electronic transitions are between electronic energy levels with a energy difference equal to the energy of photons of the ultraviolet light. Nitrogen will not absorb from the visible range so it is colorless.

Now iodine (I₂) have the allowed electronic transitions between electronic energy levels with a energy difference equal to the energy of photons of the visible light. As a consequence Iodine vapors have a violet color.

Learn more about:

electronic transitions

brainly.com/question/11328705

#learnwithBrainly

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Explanation:

  • We can calculate the molarity of a solution using the relation:

<em>M = (mass x 1000) / (molar mass x V)</em>

  • M is the molarity "number of moles of solute per 1.0 L of the solution.
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∴ M = (mass x 1000) / (molar mass x V) = (87.75 g x 1000) / (58.44 g/mol x 500.0 ml) = 3.0 mol/L.

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