Consider only transitions involving the n = 1 through n = 4 energy levels for the hydrogen atom (see Figures 6.7 and 6.10).

(a) How many emission lines are possible, considering only the four quantum levels?

(b) Photons of the lowest energy are emitted in a transition from the level with n =__________ to a level with n =__________ . 

(c) The emission line having the shortest wavelength corresponds to a transition from the level with n =__________ to the level with n =__________ .

Data given in figure 6.7

Data given in figure 6.10

Transcribed Image Text:

The difference between successive energy levels becomes smaller as n becomes larger. States with n > 1 are excited states. 10 ---7/²2 (Rhc) O 1619 1/4 5555 ||||||||| n = E₁ = -2.18 x 10-18 8654 4 n = 3 19 = -2.42 × 10-1⁹ J/atom The energy of the electron in the H atom depends on n. The larger the value of n, the larger the E₂=-5.45 x 10-19 J/atom radius and the less negative the value of the energy. -n2.... n = 1 Ground state. 18 J/atom Figure 6.7 Energy levels for the H atom in the Bohr model.