For the hydrogen atom, the relative probability of finding an electron at any single point in an orbital Ψn,ℓ(θ, φ, r) is Ψ2(θ,φ,r). If the graph below plots Ψ2 versus the distance r for an electron in an s-orbital. What is its principal quantum number n? n = The wave function Ψ can be factored into the product of three independent functions Ψ(θ,φ,r) = Θ(θ)Φ(φ)R(r). The square of the so-called radial function, R2(r), gives the relative probability of finding the electron at a single point at distance r from the nucleus.
For the hydrogen atom, the relative probability of finding an electron at any single point in an orbital Ψn,ℓ(θ, φ, r) is Ψ2(θ,φ,r).
If the graph below plots Ψ2 versus the distance r for an electron in an s-orbital. What is its principal quantum number n?
n =
The wave function Ψ can be factored into the product of three independent functions Ψ(θ,φ,r) = Θ(θ)Φ(φ)R(r). The square of the so-called radial function, R2(r), gives the relative probability of finding the electron at a single point at distance r from the nucleus.
That should be distinguished from the so-called radial probability distribution 4πr2R2, which gives the total probability of finding the electron anywhere at distance r from the nucleus -- i.e. in a spherical shell at distance r.
This probability is precisely zero at only (n - ℓ) finite values of r.
If the graph below represents the radial probability distribution for an electron in an s-orbital, what is its principal quantum number (n)?
n =
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