Use the emission spectra below to answer the following questions.D2D,s89,6 |589G|637|656,3527|518,3|| 517,2|486,1|430,8700SUN600500400|656,3|436,1|434ол700600500400Hydrogen H|667,8|587,5501,5| |492,1 1471,3 147,1| 402,6700600500400Helium He623,4| |615,2 579||S77|548,1|502,5435,8|407,8||404,7||700600500400200Mercury Hg700Uranium600500400 From the spectra above, which element does not emit red light?MercuryUraniumHeliumHydrogenQuestion 52 pUse the visible spectra above to complete the table for helium. Report your answerusing the appropriate wavelengths and including correct units.HeliumLongest WavelengthWavelength with Highest FrequencyWavelength with Lowest Energy

According to question, In question,we have given spectra which shows the region of lower to higher…

Answered: Use the emission spectra below to…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter7: Electronic Structure

Section: Chapter Questions

Problem 7.3QE

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Similar questions

The speed of sound in dry air at 20°C is 343.5ms1 , and the frequency of the sound from the middle C note on a piano is 261.6s1 (according to the American standard pitch scale). Calculate the wavelength of this sound and the time it will take to travel 30.0 m across a concert hall.
Chapter 3 introduced the concept of a double bond between carbon atoms, represented by C=C , with a length near 1.34 Å. The motion of an electron in such a bond can be treated crudely as motion in a one-dimensional box. Calculate the energy of an electron in each of its three lowest allowed states if it is confined to move in a one-dimensional box of length 1.34 Å. Calculate the wavelength of light necessary to excite the electron from its ground state to the first excited state.
Consider the following transitions 1. n=3 to n=1 2. n=2 to n=33. n=4 to n=34. n=3 to n=5(a) For which of the transitions is energy absorbed? (b) For which of the transitions is energy emitted? (c) Which transitions involve the ground state? (d) Which transition absorbs the most energy? (e) Which transition emits the most energy?
Consider Figure 11.4 and choose the correct phrase: As the vibrational quantum number increases, the extension of the vibration increases/decreases/stays the same while the average length of the oscillator itself increases/decreases/stays the same. Explain your choices.
In a FranckHertz experiment on sodium atoms, the first excitation threshold occurs at 2.103 eV. Calculate the wavelength of emitted light expected just above this threshold. (Note: Sodium vapor lamps used in street lighting emit spectral lines with wavelengths 5891.8 and 5889.9 Å.)
Ultrasonic waves have frequencies too high to be detected by the human ear, but they can be produced and detected by vibrating crystals. Calculate the wavelength of an ultrasonic wave of frequency 5.0104s1 that is propagating through a sample of water at a speed of 1.5103ms1 . Explain why ultrasound can be used to probe the size and position of the fetus inside the mother’s abdomen. Could audible sound with a frequency of 8000s1 be used for this purpose?
Using a simple particle-in-a-box model for the multiple bonding in 1,2-butadiene (see Example 4.7) and the n=2 wave function for the weakest bound electron, calculate the probability of finding the electron in an 0.1 interval centered midway between the two inner carbon atoms (that is, the center is at x=2.11 , so this interval is from x1=2.06 to x2=2.16 ). Then calculate the probability of finding the electron in an 0.1 interval centered midway between an end carbon atom and the carbon atom that is double-bonded to it in the Lewis dot structure. (You may calculate the appropriate integrals or estimate the relevant areas under the curve graphically.) Then recalculate the probabilities by approximating the integral as |( x 0)|2x , where x0 is evaluated in the middle of the range from x1 to x2 . Finally, explain why you can’t approximate the integral needed for Problem 37(a) in this way.
When a helium atim is bombarded, the atom rose into a higher energy state and then fell back to the lower energy level. What are the three lower frequency spectra lines emitted by the helium atom as it returns to ground state? Give your answer to three significant figures.
Atomic Emission and Atomic Absorption Explain the diagrams below
Give typed full explanation not a single word hand written otherwise leave it Which of the following statements are 'correct' regarding the fluorescence and phosphorescence emission processes commonly used in spectroscopy? I- Fluorescence and phosphorescence events are important emission processes that occur after the excitation of atoms or molecules with a thermal or chemical energy. II. In the photoluminescence processes called fluorescence and phosphorescence, a ray-excited species returns to its ground state by releasing its extra energy in the form of photons. III-If gaseous atoms are excited with any energy, the atom emits a beam with the wavelength that characterizes it, and makes fluorescent radiation. IV. It is possible for a light-excited atom or molecule to return to a lower energy level or ground state by heat transfer by collisions without emitting any rays. A. IandIII B. IandII C. II and IV D. Il and III
For which one of the following reasons are spectra unique to each element and molecule?
Why do some line spectra have only a few visible lines while others have so many lines that you almost can’t count them?

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