11 - General Chemistry I March 12, 2008 Lecture Alexander...

Info iconThis preview shows pages 1–11. Sign up to view the full content.

View Full Document Right Arrow Icon
General Chemistry I March 12, 2008 Lecture Alexander Shekhtman
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
The Third Hour Examination is Monday March 17 th . The overflow for students with last names P – Z is LC 23
Background image of page 2
Quantum Mechanics and Atomic Orbitals Schrödinger proposed an equation that contains both wave and particle aspects. Solving the equation leads to wave functions . The wave functions for a hydrogen atom are called atomic orbitals . The square of the wave function, gives the probability of finding the electron at some position. that is, it gives the electron density for the atom.
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Wave Function for the Hydrogen Atom Ground State 2200 Ψ 1s (r) = N e -r/ao where r is the distance of the electron from the proton (nucleus) • and a o is the Bohr radius a o = 0.529 x 10 -10 m a o = 0.529 Angstroms
Background image of page 4
The Probability Distribution for Finding an Electron in the Hydrogen Atom Ground State
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Atomic Orbitals and Quantum Numbers Atomic Orbitals and Quantum Numbers Solution of Schrödinger’s equation for a one-electron atom produces wave functions with 3 quantum numbers : Principal Quantum Number, n . This is the same as Bohr’s n . As n becomes larger, the atom becomes larger and the electron is further from the nucleus. Azimuthal Quantum Number , l . This quantum number depends on the value of n. The values of l begin at 0 and increase to (n - 1). We usually use letters for l (s, p, d and f for l = 0, 1, 2, and 3). Usually we refer to the s, p, d and f- orbitals. l specifies the angular momentum of the orbital.
Background image of page 6
Atomic Orbitals and Quantum Numbers Atomic Orbitals and Quantum Numbers Magnetic Quantum Number , m l . This quantum number depends on l . The magnetic quantum number has integral values between - l and + l . Magnetic quantum numbers give the angular orientation of each orbital.
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Atomic Orbitals with Allowed Combinations of Quantum Numbers
Background image of page 8
Hydrogen Atomic Orbital Hydrogen Atomic Orbital Energies and Quantum Numbers Energies and Quantum Numbers
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
The Shape of s Atomic Orbitals The The s s orbitals have l = 0
Background image of page 10
Image of page 11
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 35

11 - General Chemistry I March 12, 2008 Lecture Alexander...

This preview shows document pages 1 - 11. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online