Homework #6Name ________________ Student ID ______________ Date ______________6.10Calculate the wavelengths, in meters, of radiation of the following frequencies.(a) 5.00 1015 s1, (b) 2.11 1014 s1, (c) 5.44 1012 s1a) Frequency () = Speed(c) * wavelength()=c= c/ = 2.998*108 /5.00 1015= 5.996*10-8mb) = 2.998*108 / 2.11 1014=1.4209 *10-6mc) 2.998*108 / 5.44 1012= 5.511*10-5m6.28According to the Bohr model of the atom, what happens when an atomabsorbs energy?The electrons in the atom absorbs the energy and thus become exited and in turn jump tothe next energy level i.e. the exited state condition. When in this excited state condition,the atom is unstable and for it to regain stability i.e. the lowest energy state the electronloses the excess energy by emitting light energy.6.32A neon atom emits light at many wavelengths, two of which are at 616.4 nm and 638.3nm. Both of these transitions are to the same final state. (a) What is the energy differencebetween the two states for each transition? (b) If a transition between the two higherenergy states could be observed, what would the frequency of the light be?E= h =h c/ Where h= 6.63*10-34J.SC=2.998*108ms-1E =E1-E2E1= h c/ =(6.63*10-34 *2.998*108)(616.4*10-9)=3.225*10-19 JE2= h c/ =(6.63*10-34 *2.998*108)(638.3*10-9)=3.114*10-19 JE =E1-E2=3.225*10-19 J -3.114*10-19 J=1.11*10-20 JE=1.11*10-20 J = hFrequency ()= E/h =1.11*10-20 J/ 6.63 ...

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