Chapter 6 in Review Some stuff you might have forgotten already Some practice A mercury atom is initially in its lowest possible or ground state energy level The atom absorbs a photon with a wavelength of 185nm and then emits a photon with a frequency of 688x10 ID: 747933
Download Presentation The PPT/PDF document "Chem 167 SI Sunday, September 30 at 4:1..." is the property of its rightful owner. Permission is granted to download and print the materials on this web site for personal, non-commercial use only, and to display it on your personal computer provided you do not modify the materials and that you retain all copyright notices contained in the materials. By downloading content from our website, you accept the terms of this agreement.
Slide1
Chem 167 SI
Sunday, September 30 at 4:10pmSlide2
Chapter 6 in Review
Some stuff you might have forgotten (already)Slide3
Some practice
A mercury atom is initially in its lowest possible (or ground state) energy level. The atom absorbs a photon with a wavelength of 185nm, and then emits a photon with a frequency of 6.88x10
14
Hz. At the end of this series of transitions, the atom will still be in an energy level above ground state.
Q: Draw an energy level diagram for this process, and find the energy of this resulting excited state, assuming we assign E = 0 to the ground state.Slide4
Photoelectric Practice
What is the kinetic energy of an electron removed from iron using light with a wavelength of 101 nm? The binding energy of an electron in iron is
7.5x10
–19
J
.
Bonus: what is the speed of this electron?Slide5
The Bohr Model
A brief look atSlide6
Bohr’s major contribution was the suggestion of stable orbits that electrons occupy. His model is the most common depiction of atoms, but sadly is also incorrect.Slide7
Quantum Numbers
Now to the real show!Slide8
What the heck are these things?
The principle quantum number indicates the shell
The second indexes energy differences between orbitals in the same shell (subshells)—also, gives letter designations
The magnetic quantum number gives insight to the orientation of the orbitalSlide9
Some ways to remember…
Principal quantum number—periods on the periodic table
Second quantum number—region of the periodic table (
s,p,d
, or f)
Each orbital actually has a 4
th
quantum number, the “spin” – we’ll learn this tomorrowSlide10
Practice
An orbital has quantum numbers of n = 4, l = 2, and m
l
= -1. Which type of orbital is this?
How many orbitals are there in an s sub-shell? p sub-shell, d, f?Slide11
More practice
Which of the following represent valid sets of quantum numbers? For a set that is invalid, explain briefly why it is not correct.
n = 3, l = 3, m
l
= 0
n = 2, l = 1, m
l
= 0
n = 6, l = 5, m
l
= -1
n = 4, l = 3, m
l
= -4Slide12
Owl homework due this Wednesday
Exam
next week
! Wednesday 10/10
Don’t forget!