Download Chapter 30: EQUATION SHEET

Name__________________________________
Reference Sheet
Physics 212
Mr. Dristle
Chapter 30: EQUATION SHEET
BOHR MODEL OF THE ATOM
Ei − E f = h f
Ln = n
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h
2π
Energies of emitted photons
n = 1, 2, 3,L
Orbital angular momentum of the electron is quantized
n2
rn = ( 5.29× 10−11 m )
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Z
n = 1, 2, 3,L
Radii of the Bohr orbits are quantized.
Z2
En = −(13.6 eV) 2
n €
n = 1, 2, 3,L
Energies of the Bohr atom are quantized.
1
1
1
= RZ 2  2 − 2  €
λ
 n f ni 
ni , n f = 1, 2, 3, L and ni > n f
Wavelengths comprising the line spectra of the Bohr atom.
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In the hydrogen atom (Z = 1)
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the Lyman series results when n f = 1.
the Balmer series results when n f = 2 .
the Paschen series results when n f = 3.
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The principal quantum number n, can have the integer values n = 1, 2, 3,L €
The orbital quantum number l , can have the integer values l = 0, 1, 2,L (n −1)
The magnetic quantum number ml can have the positive and negative values in the range of
−l,L, −2, −1, 0, +1, + 2,L,+l
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The spin quantum number ms , which for an electron,
s
2
s
2
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The Pauli Excluion Principle
states that no two electrons in an atom can have the same set of values
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for the four quantum numbers n, l, ml , and ms .
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X-RAYS
QUANTUM MECHANICAL PICTURE OF THE ATOM
λo =
hc
eV
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Cutoff wavelength of the Bremsstrahlung
CONSTANTS
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R = 1.097× 10 7 m -1
Rydberg constant