5. The element Chromium has a KB X-ray wavelength of 0.209nm. The K-shell binding energy is 5989eV. a. Sketch a level scheme to show the relationship between the X-ray transitions of the K, L, and M series. b. What is the energy of the Ka X-ray transition in Chromium? α c. What is the energy of the La X-ray transition? d. What is the L-shell binding energy?

5. The element Chromium has a KB X-ray wavelength of 0.209nm. The K-shell binding energy is 5989eV. a. Sketch a level scheme to show the relationship between the X-ray transitions of the K, L, and M series. b. What is the energy of the Ka X-ray transition in Chromium? α c. What is the energy of the La X-ray transition? d. What is the L-shell binding energy?

Chemistry

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Chapter7: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 151AE: One of the visible lines in the hydrogen emission spectrum corresponds to the n = 6 to n = 2...

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Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
Most retinal tears and detachments are treated by photocoagulation with a laser. A commonly used laser is one with a wavelength of 514 nm. Calculate (a) the frequency. (b) the energy in joules/photon. (c) the energy in kJ/mol.
Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff, using the spectroscope they invented in 1859. The name came from the Latin caesius ("sky blue") because of the prominent blue line observed for this element at 455.5 nm. Calculate the frequency and energy of a photon of this light.
The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
The Doppler effect is one of the sources of the line broadening in atomic absorption spectroscopy. Atoms moving toward the light source encounter higher-frequency radiation than atoms moving away from the source. The difference in wavelength experienced by an atom moving at speed v (compared to one atrest) is / = v/c , where c is the velocity of light. Estimate the line width (in nanometers) of the lithiumline at 670.776(6707.76 Å) when the absorbing atoms are at a temperature of (a) 2000 K and (b) 3120 K.The average speed of an atom is given by v=8kT/m , where k is Boltzmann’s constant, Tis the absolute temperature, and m is its mass.
A line in the Lyman series (nlo=1) occurs at 97.23 nm. Calculate nhi for the transition associated with this line.
6.86 An excited He+ ion returns to the ground state by emitting a series of three photons, with wavelengths of 26 nm, 469 nm, and 1014 nm. The process is represented in the energy level diagram below. Which arrow (A, B, or C) in the diagram represents the 1014-nm light?
6.72 LED bulbs offer a fairly new lighting alternative, and are becoming increasingly popular in home lighting. These bulbs combine excellent energy efficiency with the “warm” light and dimming ability of incandescent lights. Although LED bulbs are expensive, manufacturers claim that subsequent savings will more than offset the initial costs. Analyze the relative cost of incandescent versus LED lighting, assuming that the information in the table below is accurate. Are industry claims of cost savings justified? LED Incandescent Initial cost $4.00 $0.75 Electricity usage 8 watts 60 watts Electricity cost $0.04/kwh $0.04/kwh Lifetime 25,000 hours 1,500 hours
The first-row transition metals from chromium through zinc all have some biologic function in the human body. How many unpaired electrons are present in each of these first-row transition metals in the ground state?
6.28 A neon atom cmi light at many wavelengths, two of which are at 616.4 and 638.3 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) If a transition between the two higher energy states could be observed, what would be the frequency of the light?
The retina of the eye contains two types of light-sensitive cells rods (responsible for night vision) and cones (responsible for color vision). Rod cells are about a hundred times more sensitive to light than cone cells and are able to detect a single photon. Suppose a group of rod cells are radiated with a pulse of light having an energy equal to 1.60 1016 J. If the wavelength of this light was 498 nm (the wavelength at which rod cells are most sensitive), how many photons are in this light pulse?
what is the multiplicity for a state that has 1 unpaired electron? a. 0 b. 1 c. 2 d. 3

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