This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: energy Use this diagram to complete the table below. Which is the ground state? (pick one) How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the emission line at the shortest wavelength? Which transition causes the emission line at the longest wavelength?

This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: energy Use this diagram to complete the table below. Which is the ground state? (pick one) How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the emission line at the shortest wavelength? Which transition causes the emission line at the longest wavelength?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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This energy diagram shows the allowed energy levels of an electron in a certain atom or molecule: energy C Which is the ground state? B A Use this diagram to complete the table below. How many excited states are there? How many lines are in the absorption line spectrum? Which transition causes the absorption line at the shortest wavelength? Which transition causes the absorption line at the longest wavelength? (pick one) 0 0 0-0 0-0 ? 000 18 Ar
The dazzling colors produced by fireworks result from excited gaseous atoms or molecules emitting light. The normal electron configuration of an atom is known as the "ground state." In ground state, all electrons are in the lowest energy levels available. When atoms or ions are heated, some electrons may absorb enough energy to allow them to "jump" to higher energy levels. The atom or ion is then said to be in the "excited state." The electrons cannot remain in this excited state for long and will emit energy in the form of light when they return to ground state. It is this light we see when an atom is heated in a flame. The frequency or color of light emitted depends on the energy difference between the excited state and the ground state. Chose the correct ground state configuration for Sr O 1:2322p 3s23p 43² 3d104p65s2 O 1:22p 3323p°4=?3410 4p7 O 1:?2,2p 3s23p 4s24p 441052 p75st
When an electron moves to a lower state, a photon will be (emitted/absorbed) .
2. Calculate the theoretical energy value of each wavelength of light in the helium spectrum to complete the following chart. Table view D List view Helium gas emission spectrum Theoretical energy (J) Wavelength (nm) Color 447 violet 471 blue 501 green 587 yellow 668 red
ot ot ot at Consider the transition from the energy levels n-3 to n-7. What is the wavelength associated with this transition, in nm? nm In what spectral region does this transition occur? this wavelength is in the ultraviolet this wavelength is in the visible Othis wavelength is in the infrared Is energy absorbed or released for this transition? O energy is absorbed O energy is released
Electrons in potassium ions (excited by heating in a flame) emit visible light whose wavelength is 409nm. What is the frequency of this light? What is the energy of one quantum of this light? What color light is it?
Which happens when an atom in an excited state returns to the ground state
This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10-21. You can find the meaning of any SI prefix in the ALEKS Data tab.) energy (zJ) 1400 1200 1000 800 600 400 200 0 I B -A Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from A to C, will a photon be absorbed or emitted? Calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. 250 ZJ 400 ZJ absorbed emitted nm x10 X S
This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI prefix 'zepto' means 10-21. You can find the meaning of any SI prefix in the ALEKS Data tab.) energy (z)) 1400. 1200- 1000 800- 600- 400 200 0 C B A Use this diagram to complete the table below. What is the energy of the electron in the ground state? What is the energy of the electron in the first excited state? If the electron makes the transition shown by the red arrow, from A to C, will a photon be absorbed or emitted? Calculate the wavelength of the photon that would be absorbed or emitted. Round your answer to 3 significant digits. 100 ZJ 550 ZJ absorbed O emitted nm x10 X S
3. List the following forms of electromagnetic spectra from lowest to highest energy. Yellow light, Microwaves, Ultra Violet, Blue light, Radio waves
What is a photon? How is the energy of a photon related to its wavelength? Its frequency?