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- For the Li atom, the energy difference between the ground state and the first excited state, in which the outermost electron is in a 2p orbital, is 2.961019J . In the Li2+ ion, the energy difference between the 2s and 2p levels is less than 0.00002 of this value. Explain this observation.Suppose that the spin quantum number did not exist, and therefore only one electron could occupy each orbital of a many-electron atom. Give the atomic numbers of the first three noble-gas atoms in this case.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.
- Is the spin orbital 1s for the H atom still spherically symmetric? Explain your answer.Photoelectron spectroscopy studies have determined the orbital energies for fluorine atoms to be 1s689eV2s34eV2p12eV Estimate the value of Zeff for F in each of these orbitals.3. A helium atom is in the state 'D2. Write the values of its total spin, total orbital angular momentum and the total angular momentum. .
- An experiment called the Stern–Gerlach experiment helpedestablish the existence of electron spin. In this experiment,a beam of silver atoms is passed through a magnetic field,which deflects half of the silver atoms in one direction andhalf in the opposite direction. The separation between thetwo beams increases as the strength of the magnetic fieldincreases. (a) What is the electron configuration for a silveratom? (b) Would this experiment work for a beam of cadmium(Cd) atoms? (c) Would this experiment work for abeam of fluorine (F) atoms?What is the number of possible orientation for a nucleus with spin quantum number 1 ?IV. There is one more policy that helps the hotel run smoothly and keep customers happy. Hund's Rule states that if electrons are being placed in the same section of a floor (rooms that cost the same) then each one gets their own room and has the same spin until the floor is half-filled. If any more electrons want to stay in that same section, then they must pair up with another electron and assume the opposite spin. This does not necessarily apply to electrons that have purchased more expensive rooms. In the diagrams below identify the areas in which Hund's Rule was broken. Describe how the rule is being broken in each case. D1111 |1|1||1| 1 1 1 1 1 November 26, 1995 February 12, 1997 July 10, 1983 A В V. OBSERVATIONS: A. How many "rooms" are there in an "s" suite of a floor? B. How many "rooms" are there in a "p" suite of a floor? C. How many "rooms" are there in a "d" suite of a floor? D. How many electrons can stay on the first floor? second floor? third floor? E. Describe how the…
- predict ground state spin of nitrogenIV. There is one more policy that helps the hotel run smoothly and keep customers happy. Hund's Rule states that if electrons are being placed in the same section of a floor (rooms that cost the same) then each one gets their own room and has the same spin until the floor is half-filled. If any more electrons want to stay in that same section, then they must pair up with another electron and assume the opposite spin. This does not necessarily apply to electrons that have purchased more expensive rooms. In the diagrams below identify the areas in which Hund's Rule was broken. Describe how the rule is being broken in each case. 14 February 12, A 1L 1L 1L 12 12 [16] 14 November 26, B 1 14 14 14 14 14 14 July 10, 1983 CConsider the four electron configurations for atoms: 1s22s22p63s33p64s23d104p5 1s22s22p63s23p64s23d104p1 1s22s22p63s23p64s13d104p1 1s22s22p63s23p63d104p5 Which of the following statements is correct. There are: 1 ground state, 1 excited state, and 2 impossible states There are: 1 ground state, 2 excited states, and 1 impossible state There are: 1 ground state, no excited states, and 3 impossible states There are: 2 ground states, 1 excited state, and 1 impossible state
