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quantummech - n l ml used to describe orbitals o n =...

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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 o represented by y, but has no physical meaning by itself o probability density = y2 o electron density - areas w/ high probability of finding electrons orbital - describes distribution of electron density in space o not the same as the orbits mentioned in Bohr's model o path of electron can't be precisely tracked (due to uncertainty principle) quantum numbers
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Unformatted text preview: - n, l, ml used to describe orbitals o n = positive integer, principle quantum number ; increases as electron gets farther away from nucleus o En = (-2.18 x 10-18 J)(1/n2) o l = integer from 0 to n-1, azimuthal quantum number ; describes orbital shape o 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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