7.1 Application of the Schrödinger Equation to the Hydrogen Atom

7.2 Solution of the Schrödinger Equation for Hydrogen

7.3 Quantum Numbers

7.4 Magnetic Effects on Atomic Spectra – Normal Zeeman Effect

7.5 Intrinsic Spin

7.6 Energy Levels and Electron Probabilities

CHAPTER 7The Hydrogen Atom

By recognizing that the chemical atom is composed of single separable electric quanta, humanity has taken a great step forward in the investigation of the natural world.

- Johannes Stark

7.1: Application of the Schrödinger Equation to the Hydrogen Atom

The approximation of the potential energy of the electron-proton system is electrostatic:

The three-dimensional time-independent Schrödinger Equation is

For Hydrogen-like atoms (He+ or Li++) Replace e2 with Ze2 (Z is the atomic number) Use appropriate reduced mass μ

Application of the Schrödinger Equation The potential (central force) V(r) depends on

the distance r between the proton and electron.

Transform to spherical polar coordinates because of the radial symmetry.

Insert the Coulomb potential into the transformed Schrödinger equation.

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Application of the Schrödinger Equation

The wave function ψ is a function of r, θ, . Equation is separable. Solution may be

We can separate the equation into three separate differential equations, each depending on one coordinate: r, θ, or .

Separation of Variables The derivatives are

Substitute them into the equation:

7.2: Solution of the Schrödinger Equation for Hydrogen

Multiply both sides by r2 sin2 θ / Rfg

r and θ appear on the left side and only appears on the right side The left side of the equation cannot change as changes. The right side cannot change with either r or θ.

Each side needs to be equal to a constant Set the constant −mℓ2

It is convenient to choose a solution to be:

azimuthal equation

Solution of the Schrödinger Equation

The solution be single valued in order to have a valid solution for any ,

mℓ to be zero or an integer (positive or negative).

Now set the left side of Eq (7.7) equal to −mℓ2

and rearrange it

Everything depends on r on the left side and θ on the right side of the equation.

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0( 0) ( 2 ) img g e e

Solution of the Schrödinger Equation

Set each side equal to constant ℓ(ℓ + 1).

Schrödinger equation has been separated into three ordinary second-order differential equations, each containing only one variable.

Radial equation

Angular equation

azimuthal equation

Solution of the Radial Equation

The radial equation is called the associated Laguerre equation and the solutions R that satisfy the appropriate boundary conditions are called associated Laguerre functions.

Assume the ground state has ℓ = 0 (this will require mℓ = 0)

The derivative of yields two terms. Inserting the potential,

Radial Equation:

Try a solution , where A is a normalization constant.

For any r, each of the two expressions in parentheses must be zero. Set the second parentheses equal to zero and solve for a0.

Set the first parentheses equal to zero and solve for E.

(Note) Both are identical to the Bohr radius and ground state E0.

(ℓ = 0)

Quantum Numbers:

The appropriate boundary conditions to the equations leads to the following restrictions on the quantum numbers ℓ and mℓ: ℓ = 0, 1, 2, 3, . . . orbital quantum number mℓ = −ℓ, −ℓ + 1, . . . , −2, −1, 0, 1, 2, . ℓ . , ℓ − 1, ℓ

(|mℓ| ≤ ℓ ) magnetic quantum number Full solution of the radial equation requires a third quantum number

n = 1, 2, 3,... principal quantum number also restricts ℓ to values less than n n defines the energy level (Identical to Bohr result)

, ,n m

20 /nE E n

Hydrogen Atom Radial Wave Functions Rnℓ

Solution of the Angular and Azimuthal Equations

Solutions to the angular and azimuthal equations are linkedbecause both have mℓ

Group these solutions together into functions

---- spherical harmonics

The solutions are

Normalized Spherical Harmonics

Full wave function for electron in hydrogen atom

The radial wave function R and the spherical harmonics Ydetermine the probability density for the various quantum states.

The total wave function depends on n, ℓ, and mℓ.

Example 7.2Show that the hydrogen wave function ψ211 is properly normalized.

We need to prove

In spherical polar coordinates: