line spectra - spectrum containing radiation of specific wavelengths
- monochromatic radiation - consists of a single wavelength
- spectrum - separation of radiation into different wavelengths
- continuous spectrum - contains light of all wavelengths
Rydberg equation - allowed calculation of wavelengths of all spectral lines
- 1/l = (Rh)(1/n12 - 1/n22) = [(2.18 x 10-18 J) / hc] (1/n12 - 1/n22)
- Rh = 1.096776 x 107 m-1
Bohr's Model - electrons moving in circular paths lose energy and spiral towards nucleus
- only orbits w/ certain radii, dependent on energies of electrons
- electron in allowed energy state has specific energy, doesn't radiate energy
- energy emitted/absorbed by electrons when it changes energy states
- E = (-2.18 x 10-18 J)(1/n2) = energy in hydrogen atom
- n = integer from 1 to ¥ = quantum number
- ground state - lowest energy state
- excited state - higher energy state
- E = (-2.18 x 10-18 J)(1/¥2) = 0
- DE = Efinal - Einitial = Ephoton = hn = hc/l = (-2.18 x 10-18 J)(1/nf2 - 1/ni2)
- ni = initial energy state
- nf = final energy state
- l = hc / DE
- n = = DE / h
- doesn't explain spectra of any atom besides hydrogen
- electrons actually show properties of waves
Find the de Broglie wavelength of an electron w/ velocity 5.97 x 106 m/s
- Given:
- l = h/(mv)
- m = 9.11 x 10-28 g = 9.11 x 10-31 kg
- h = 6.63 x 10-34
- v = 5.97 x 106
- l = (6.63 x 10-34) / (9.11 x 10-31 x 5.97 x 106)
- l = 1.22 x 10-10 m
Subject:
Subject X2:
