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per photon!

per photon!. Energy of a single photon: 4.67 x 10 -18 J / 10 = 4.67 x 10 -19 J. = 426 nm. Assuming the Bohr model of the atom; calculate the wavelength of the band in the spectrum of atomic hydrogen for the transition involving orbits n = 2 and n = 3. 410 nm b. 656 nm

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per photon!

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  1. per photon! Energy of a single photon: 4.67 x 10-18 J / 10 = 4.67 x 10-19 J =426 nm

  2. Assuming the Bohr model of the atom; calculate the wavelength of the band in the spectrum of atomic hydrogen for the transition involving orbits n = 2 and n = 3. • 410 nm b. 656 nm • c. 486 nm d. 434 nm

  3. In a multielectron atom, which quantum number combination (n,l,ml, ms) is associated with the electron with the same energy as one with n=3, l=1, ml = 0, ms= +1/2 ? a. 3, 1, 0, -1/2 b. 2, 1, 0, +1/2 c. 3, 0, 1, +1/2 d. 3, 1, 1/2, -1/2

  4. Calculate the change in energy of a hydrogen atom that emits a photon with a frequency of 2.5x1015 s-1. a. 1.6 × 10-18 J b. -1.6 × 10-18 J c. 6.1x1017 J d. - 6.1x1017 J

  5. Carbon has the electron configuration 1s22s22p2. The following diagrams show the arrangements of two electrons in the 2p orbital of carbon. . i ii . iii iv Select all the electron configurations that are NOT allowed for carbon. a. i only b. i, iii c. iii only d. iii, iv Which electron configuration(s) lead(s) to the most stable carbon atom? a. i only b. i, ii c. iv only d. iii, iv

  6. The ground state electron configuration of Fe is [Ar]4s23d6. What is the electron configuration of iron in FeCl3 ? a. [Ar]4s23d3 b. [Ar]3d6 c. [Ar]4s23d4 d. [Ar]3d5

  7. ( i ) ( ii ) ( iii ) ( iv ) What is the maximum number of electrons that a subshell that contains orbital (iv) can have? a. 2 b. 4 c. 5 d. 10 Which of the following statements is NOT correct • Orbital ( i) always has smaller energy than orbital (iv). • b. Orbital (ii) and orbital (iii) can have different principal quantum number n. • c. Orbital (i) can be associated with any principal quantum number n. • d. ml = +2, ms = -1/2 is a possible combination of quantum numbers for orbital (iv).

  8. What is the valence electron configuration of elements in group 3A of the periodic table? a. ns1np2 b. ns2np1c. ns2np2 d. ns2np3

  9. Which of the following pairs of ions and atoms are isoelectronic? [He]2s22p6or [Ne] [Ar]4s23d104p6or [Kr] [He]2s22p6or [Ne] I. O2- and Na+ II. Sr2+ and Kr III. F- and Ne a. I. only b. I. and II.c. none d. all

  10. DHorxn = [DHof [H2SO4 (l)] – [DHof [H2O](g)+ DHof [SO3](g)] DHof [H2SO4 (l) = DHorxn + [DHof [H2O](g)+ DHof [SO3](g)] =-177.0 kJ + [-241.8kJ- 395.2kJ] = -814 kJ

  11. DG = DH - TDS

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