matter waves - describes wave characteristics of material particles
- all matter have wavelengths
- wavelength inversely proportional to mass/velocity
- l = Planck's constant / (mass x velocity) = h / mv
- microscopes use wave properties of electrons to map out surfaces
quantum (wave) mechanics - studies w/ subatomic particles
- wave functions - mathematical functions describing electron's matter wave
- represented by y, but has no physical meaning by itself
- probability density = y2
- electron density - areas w/ high probability of finding electrons
- orbital - describes distribution of electron density in space
- not the same as the orbits mentioned in Bohr's model
- path of electron can't be precisely tracked (due to uncertainty principle)
- quantum numbers - n, l, ml used to describe orbitals
- n = positive integer, principle quantum number; increases as electron gets farther away from nucleus
- En = (-2.18 x 10-18 J)(1/n2)
- l = integer from 0 to n-1, azimuthal quantum number; describes orbital shape
- ml = integers between l and -l, magnetic quantum number; describes orientation of orbital
- electron shell - collection of orbitals w/ same n value
- subshell - orbitals w/ same n and l values
- n subshells in the shell w/ principle quantum number n
- each subshell has 2(l)+1 number of orbitals
- n2 = total number of orbitals in a shell
- ground state - electron in lowest energy orbital
- excited state - electron in any other orbital, reaches this level by absorbing photons
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