Ch 7 - Quantum Theory and Atomic Structure Flashcards
energy of a photon equation (change to an adjacent state)
E = hv = hc/λ
v = frequency
h = Planck’s constant
c = speed of light
λ = wavelength
absorbtion
AKA excitation
positive ΔH
electron moves to outer orbit
absorbtion
AKA excitation
positive ΔH
electron moves to outer orbit
emission
AKA relaxation
negative ΔE
electron returns to lower orbit
ΔE association with absorbtion/emission (energy difference between two levels)
ΔE = -2.18^-18(z^2/n^2final - z^2/n^2inital)
per atom/ photon
ionization energy
energy to completely remove an electron
nfinal = infinity
deBroglie wavelength
λ = h/mu
m = kg
u = m/s
object’s wavelength is inversely proportional to its mass
principal quantum number (n)
positive integer that specifies the energy and relative size of an atomic orbital
approximate distance of electron from nucleus
angular momentum quantum number (l)
integer from 0 to n-1 that is related to the shape of the orbital
0 = s
1 = p
2 = d
3 = f
magnetic quantum number (ml)
integer from -l to l that specifies the orientation of atomic orbital
number of possible values = number of orbitals of that type in a subshell
spin quantum number (ms)
spin of electron in orbital
-1/2 or 1/2
energy is directly proportional to ___ and inversely proportional to ___
energy is directly proportional to frequency and inversely proportional to wavelength
rydberg equation
wavelength of a line in H atom
1/λ = R(1/n1^2 - 1-/n2^2)
R = rydberg constant
n2 > n1
what happens to the energy gap at higher n values
smaller energy gap at higher n values