[References]liation and the Electronic Structure of the AtomUse the References to access important values if needed for this question.X-ray radiation has frequencies from 3.0x10° to 3.0x10" Hz, whereas the frequency region for ultraviolet radiationis 3.0x1015 to 3.0x1016 Hz.We can say that:1. The speed of X-ray radiation isv ultraviolet radiation.2. The wavelength of X-ray radiation isv ultraviolet radiation.Submit AnswerTry Another Version1 item attempt remaining

X-ray and Ultraviolet radiation, both are electromagnetic waves. If we carefully observe the…

X-ray radiation has frequencies from 3.0x100 to 3.0x10 Hz, whereas the frequency region for ultraviolet radiation is 3.0×1015 to 3.0x1016 Hz. We can say that: 1. The speed of X-ray radiation is v ultraviolet radiation. 2. The wavelength of X-ray radiation is ultraviolet radiation. Submit Answer Try Another Version 1 item attempt remaining

X-ray radiation has frequencies from 3.0x100 to 3.0x10 Hz, whereas the frequency region for ultraviolet radiation is 3.0×1015 to 3.0x1016 Hz. We can say that: 1. The speed of X-ray radiation is v ultraviolet radiation. 2. The wavelength of X-ray radiation is ultraviolet radiation. Submit Answer Try Another Version 1 item attempt remaining

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 45AP: Suppose an atom in an excited state can return to the ground state in two steps. It first falls to...

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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.
Schrodinger and de Broglie suggested a ‘Wave—particle duality" for small particles—that is, if electromagnetic radiation showed some particle-like properties, then perhaps small punicles might exhibit same wave-like properties. Explain. How does the wave mechanical picture of the atom fundamentally differ from the Bohr model? How do wave mechanical arbitals differ from Bohr’s orbits? What does it mean to say that an orbital represents a probability map for an electron?
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.
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.
Select the INCORRECT statement about the theories of electronic structure from the followings?
The stratospheric ozone 1O32 layer helps to protect usfrom harmful ultraviolet radiation. It does so by absorbingultraviolet light and falling apart into an O2 molecule and anoxygen atom, a process known as photodissociation.O31g2¡O21g2 + O1g2Use the data in Appendix C to calculate the enthalpy changefor this reaction. What is the maximum wavelength a photoncan have if it is to possess sufficient energy to cause thisdissociation? In what portion of the spectrum does thiswavelength occur?
16.The frequency of vibration of a bond is a function of which two (2) factors?
In the experiment shown schematically below, a beam ofneutral atoms is passed through a magnetic field. Atoms thathave unpaired electrons are deflected in different directionsin the magnetic field depending on the value of the electronspin quantum number. In the experiment illustrated,we envision that a beam of hydrogen atoms splits into twobeams. (a) What is the significance of the observation that the single beam splits into two beams? (b) What do you thinkwould happen if the strength of the magnet were increased?(c) What do you think would happen if the beam of hydrogenatoms were replaced with a beam of helium atoms? Why?(d) The relevant experiment was first performed by OttoStern and Walter Gerlach in 1921. They used a beam of Agatoms in the experiment. By considering the electron configurationof a silver atom, explain why the single beam splitsinto two beams.
Consider the three electronic transitions in a hydrogen atomshown here, labeled A, B, and C.(a) Three electromagnetic waves, all drawn on the samescale, are also shown. Each corresponds to one of thetransitions. Which electromagnetic wave (i), (ii), or (iii),is associated with electronic transition C? (b) Calculate the energy of the photon emitted for eachtransition.(c) Calculate the wavelength of the photon emitted for eachtransition. Do any of these transitions lead to the emissionof visible light? If so which one(s)?
Microwave ovens use microwave radiation to heat food. Theenergy of the microwaves is absorbed by water molecules infood and then transferred to other components of the food.(a) Suppose that the microwave radiation has a wavelengthof 11.2 cm. How many photons are required to heat 200 mL ofcoffee from 23 to 60 °C? (b) Suppose the microwave’s power is900 W 11 watt = 1 joule@second2. How long would you haveto heat the coffee in part (a)?
Assuming the wavelength for fluorescence is observed at 475 nm and the wavelength of the phosphorescence process occurs at 523 nm, find the energy released from 12.35 g of Calcium atoms. (Assume that there is 1 excited electron per calcium atom and every one of them relaxes via the processes above.) (Fluorescence occurs 2.45 times more frequently than phosphorescence)
The stratospheric ozone (O3) layer helps to protect usfrom harmful ultraviolet radiation. It does so by absorbingultraviolet light and falling apart into an O2 molecule and anoxygen atom, a process known as photodissociation.O3(g)----->O2(g) + O(g) Use the data in Appendix C to calculate the enthalpy changefor this reaction. What is the maximum wavelength a photoncan have if it is to possess sufficient energy to cause thisdissociation? In what portion of the spectrum does thiswavelength occur?