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ch 5 part 1

# Thus to move to a higher energy orbit a greater value

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Unformatted text preview: e orbit to another by either emitting or absorbing photons with specific frequencies. Thus: • To move to a higher energy orbit (a greater value of n) an electron must _absorb _____________________energy. • To move to a lower energy orbit (a lower value of n) an electron must emit energy. • The frequency of the absorbed or emitted energy corresponds exactly to the energy difference between the orbits. those two 20 10 05-Sep-13 Ground state Excited states Absorption and emission energy (cont) Clip 21 Absorption and emission energy (cont) 1 λ =R 1 m2 - 1 n2 m: shell the transition is to (inner-shell) higher We use the Rydberg equation to identify spectral lines n: shell the transition is from (outer-shell) higher where n > m R: Rydberg constant 1.097x10-2 nm-1 or 3.29x1015 Hz Aside: c = λ · v 1 1 = R 2 − 2 λ n m 1 1 1 ν = Rc 2 − 2 n m 22 11 05-Sep-13 n=1 to n=2-->more distance and need more energy. as it is close to the nucleus,it requires more force bcoz of the attraction. Which requires greater energy, an electron promoted from n=1 to n=2, or an electron promoted from n=3 to n = 4? n=1 to n=2 Which releases a photon with greater frequency, an n = 5 to n = 4 transition or an n = 3 to n = 2 transition? Α) Α) ν=R(1/42 – 1/52)= 7.4x1013 Hz vs Β) Β) ν=R(1/22 – 1/32)= 4.6x1014 Hz Which releases a photon with greater wavelength, an n = 5 to n = 4 transition or an n = 3 to n = 2 transition? Α) Α) λ=c/ν= (3 x 108 m/s)/(7.4 x 1013 Hz) •λ= 4.05x10-6 m or 4052 nm near infrared Β) Β) λ=c/ν= (3 x 108 m/s)/(4.6 x1014 Hz) •λ= 6.56x10-7 m or 656 nm red light 23 12...
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