![Student Solutions Manual For Silberberg Chemistry: The Molecular Nature Of Matter And Change With Advanced Topics](https://www.bartleby.com/isbn_cover_images/9781259982927/9781259982927_largeCoverImage.gif)
Concept explainers
(a)
Interpretation:
The energy level to which a ground state electron in a hydrogen atom jumps to after it absorbs a photon of wavelength
Concept introduction:
An atom of hydrogen contains one electron. But the spectrum of hydrogen consists of a large number of lines. This is so because a sample of hydrogen contains a very large number of atoms. When energy is supplied to a sample of gaseous atoms of hydrogen, different atoms absorb different amounts of energy. Therefore, the electrons in different atoms jump to different energy levels. Upon losing the energies gained initially, the electrons jump back to lower energy levels and release radiations of different wavelengths.
The equation used to predict the position and wavelength of any line in a given series is called the Rydberg’s equation.
Rydberg’s equation is as follows:
Here,
The conversion factor to convert wavelength from
(a)
![Check Mark](/static/check-mark.png)
Answer to Problem 7.73P
An electron in a hydrogen atom moves to energy level 5 from the ground state upon absorption of a photon of wavelength
Explanation of Solution
In the ground state of a hydrogen atom,
The value of the Rydberg’s constant is
Substitute 1 for
Rearrange the above equation and calculate the value of
An electron in a hydrogen atom moves to energy level 5 from the ground state upon absorption of a photon of wavelength
(b)
Interpretation:
The intermediate energy level to which the electron jumps after emission of a photon of wavelength
Concept introduction:
An atom of hydrogen contains one electron. But the spectrum of hydrogen consists of a large number of lines. This is so because a sample of hydrogen contains a very large number of atoms. When energy is supplied to a sample of gaseous atoms of hydrogen, different atoms absorb different amounts of energy. Therefore, the electrons in different atoms jump to different energy levels. Upon losing the energies gained initially, the electrons jump back to lower energy levels and release radiations of different wavelengths.
The equation used to predict the position and wavelength of any line in a given series is called the Rydberg’s equation.
Rydberg’s equation is as follows:
Here,
The conversion factor to convert wavelength from
(b)
![Check Mark](/static/check-mark.png)
Answer to Problem 7.73P
The intermediate energy level to which the electron jumps after emission of a photon of wavelength
Explanation of Solution
The emission of a photon leads to the transition of an electron from a higher energy level to a lower energy level. Initially, the electron was in energy level 5. Since in the Rydberg’s equation,
The value of the Rydberg’s constant is
Substitute 5 for
Rearrange the above equation and calculate the value of
The intermediate energy level to which the electron jumps after emission of a photon of wavelength
(c)
Interpretation:
The wavelength of the photon emitted after the electron jumps from
Concept introduction:
An atom of hydrogen contains one electron. But the spectrum of hydrogen consists of a large number of lines. This is so because a sample of hydrogen contains a very large number of atoms. When energy is supplied to a sample of gaseous atoms of hydrogen, different atoms absorb different amounts of energy. Therefore, the electrons in different atoms jump to different energy levels. Upon losing the energies gained initially, the electrons jump back to lower energy levels and release radiations of different wavelengths.
The equation used to predict the position and wavelength of any line in a given series is called the Rydberg’s equation.
Rydberg’s equation is as follows:
Here,
The conversion factor to convert wavelength from
(c)
![Check Mark](/static/check-mark.png)
Answer to Problem 7.73P
The wavelength of the photon emitted after the electron jumps from
Explanation of Solution
The emission of a photon leads to the transition of an electron from a higher energy level to a lower energy level. Initially, the electron was in energy level 3 and later jumps to energy level 1. Since in the Rydberg’s equation,
The value of the Rydberg’s constant is
Substitute 3 for
The wavelength of the photon emitted after the electron jumps from
Want to see more full solutions like this?
Chapter 7 Solutions
Student Solutions Manual For Silberberg Chemistry: The Molecular Nature Of Matter And Change With Advanced Topics
- Rel. Intensity Q 1. Which one of the following is true of the compound whose mass spectrum is shown here? Explain how you decided. 100 a) It contains chlorine. b) It contains bromine. c) It contains neither chlorine nor bromine. 80- 60- 40- 20- 0.0 0.0 TT 40 80 120 160 m/z 2. Using the Table of IR Absorptions how could you distinguish between these two compounds in the IR? What absorbance would one compound have that the other compound does not? HO CIarrow_forwardIllustrate reaction mechanisms of alkenes with water in the presence of H2SO4, detailing each step of the process. Please show steps of processing. Please do both, I will thumb up for sure #1 #3arrow_forwardDraw the following molecule: (Z)-1-chloro-1-butenearrow_forward
- Identify the molecule as having a(n) E, Z, cis, or trans configuration. CH3 H₁₂C ○ E ○ z ○ cis transarrow_forwardIdentify the molecule as having a(n) E, Z, cis, or trans configuration. H₂C- CH3 О Е ○ cis ○ transarrow_forwardThe decomposition of dinitrogen pentoxide according to the equation: 50°C 2 N2O5(g) 4 NO2(g) + O2(g) follows first-order kinetics with a rate constant of 0.0065 s-1. If the initial concentration of N2O5 is 0.275 M, determine: the final concentration of N2O5 after 180 seconds. ...arrow_forward
- Don't used hand raitingarrow_forwardCS2(g) →CS(g) + S(g) The rate law is Rate = k[CS2] where k = 1.6 × 10−6 s−¹. S What is the concentration of CS2 after 5 hours if the initial concentration is 0.25 M?arrow_forwardCS2(g) → CS(g) + S(g) The rate law is Rate = k [CS2] where k = 1.6 × 10-6 s−1. S Calculate the half-life.arrow_forward
- The following is a first order reaction where the rate constant, k, is 6.29 x 10-3 min-*** What is the half-life? C2H4 C2H2 + H2arrow_forwardControl Chart Drawing Assignment The table below provides the number of alignment errors observed during the final inspection of a certain model of airplane. Calculate the central, upper, and lower control limits for the c-chart and draw the chart precisely on the graph sheet provided (based on 3-sigma limits). Your chart should include a line for each of the control limits (UCL, CL, and LCL) and the points for each observation. Number the x-axis 1 through 25 and evenly space the numbering for the y-axis. Connect the points by drawing a line as well. Label each line drawn. Airplane Number Number of alignment errors 201 7 202 6 203 6 204 7 205 4 206 7 207 8 208 12 209 9 210 9 211 8 212 5 213 5 214 9 215 8 216 15 217 6 218 4 219 13 220 7 221 8 222 15 223 6 224 6 225 10arrow_forwardCollagen is used to date artifacts. It has a rate constant = 1.20 x 10-4 /years. What is the half life of collagen?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)