1 • If there is a magnetic field in direction z, it will act on the magnetic moment, this brings in an extra potential energy term When there is no magnetic field to align them, doesn’t have a effect on total energy. In a magnetic field a dipole has a potential energy The “Normal” Zeeman Effect We ignore space quantization for the sake of the (essentially wrong) argument μ B = eħ / 2m is called a Bohr magneton. We get quantized contribution to the potential energy, combined with space quantization, m l being a positive, zero or negative integer As │L│ magnitude and z-component of L vector are quantized in hydrogen
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• If there is a magnetic field in direction z, it will act on the magnetic moment, this brings in an extra potential energy term
When there is no magnetic field to align them, doesn’t have a effect on total energy. In a magnetic field a dipole has a potential energy
The “Normal” Zeeman EffectWe ignore space quantization for the sake of the (essentially wrong) argument
μB = eħ / 2m is called a Bohr magneton.
We get quantized contribution to the potential energy, combined with space quantization, ml being a positive, zero or negative integer
As │L│ magnitude and z-component of L vector are quantized in hydrogen
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The “Normal” Zeeman Effect• The potential energy is quantized due to the magnetic
quantum number mℓ.
• When a magnetic field is applied, the 2p level of atomic hydrogen is split into three different energy states with energy difference of ΔE = μBB Δmℓ.
mℓ Energy1 E0 + μBB
0 E0
−1 E0 − μBB
μB = eħ / 2m is called a Bohr magneton, 9.27 10-24 Ws T-1.
Don’t confuse with the reduced mass of the electron, μ
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The “Normal” Zeeman Effect• A transition from 2p to 1s. E = 2 μB BThe larger B, the larger the splitting, if B is switched off suddenly, the three lines combine as if nothing ever happened, total intensity of line remains constant in the splitting
What is really observed with good spectrometers: there is a lot more lines in atomic spectra when they are in a magnetic field !!! So called Anomalous Zeeman effect, which is the only one observed with good spectrometers.
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Probability Distribution Functions• from wave functions one calculates the probability
density distributions of the electron.
• The “position” of the electron is spread over space and is not well defined.
• We use the radial wave function R(r) to calculate radial probability distributions of the electron.
• The probability of finding the electron in a differential volume element dτ is .
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Radial part of Probability Distribution Functions• The differential volume element in spherical polar
coordinates is
Therefore,
• We are only interested in the radial dependence.
• The radial probability density is P(r) = r2|R(r)|2 and it depends only on n and l.
Are both 1 due to normalization !!
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R(r) and P(r) for the lowest-lying states of the hydrogen atom.
Probability Distribution Functions
It is always the states with the highest l for each n that “correspond” to the Bohr radii.
Actually a0 is just a length scale as nothing is moving in the ground state – no angular momentum
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Is the expectation value of the smallest radius in the hydrogen atom also the Bohr radius??
dP1s / dr = 0
For all hydrogen like atoms, i.e. He+, Li++Why the extra r2 factor? Kind of two extra dimensions, accounts for surface of sphere
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