Question

Chemist Hydrogen Spectrum Drac 8 m/s = 4.487 X 10' Lab A10 W est 2010 (2) 1. For each of the obse of the observed wavelengths in the hydrogen spectrum, calculate the energy of each photon emited. 110nm - E-hc 6.626 xE-345s 3.00xE8 m/s - 4.8483 x 1015 j 7 41xE-7AM 104 nm -> E he= 6.626x E-3935 <0.00 xE8 ms - 4.481 -19 4.34E-7m. 186 nm - E= he = 6.626 xE-34 35 X 3.00 xE8B/s, 4.090 x 10 j 4.86 xE-7m -19 56 m2L họ 602 3435 4 100 Eglº - 50 50 x 40 3 71 - 6.56 xE-7m. 2. The visible lines in the hydrogen emission spectrum arise from electrons relaxing from an excited state to the n=2 energy level. For each line that you observed in the hydrogen spectrum, determine the initial energy level (n). (Hint: you need to consider the sign of energy change for the hydrogen atom above) 3. Although we observe four electronic transitions in the hydrogen discharge lamp, these are not the only transitions that occur. For each of the following transition, determine the wavelength of the photon that will be emitted and note the region of the electromagnetic spectrum that corresponds to that wavelength. n2n=1 n. 43

Answer 1

4 12) E= -13.00 mt manger T E =4.85 X10-19T 4.85x10-19x6242x1018 ev = -13-6 hair -0.223+5 inay? .. (no)35.7 na = 6 (2) E = 4.487 X10-195 4.487x 10-19 x 6.242 X10'' = -13.6( -) ne = 5 (3) E=4.09081079 J ng = 4 (4) E = 3.0 3x10-19 J in 2 - 3

3. Ş= Ro ove strat) . Ra Rujd besorg's constant § 5 1096 X10'm-' ( ) x=1-216 x 10-7 X100 nm 1=1.44610% nm = 121.6 mm uu-c (Dangerous says ) = 1.096X1071 to 6) = 18 16.9 nm Near Infrared Region.