1. Welcome Chemistry I – Day VI
Portland Evening Scholars
Mr. Treothe Bullock - Instructor
 Element Reports ?
 Unit 2 Exam – Measurements &
 Anyone would like to go?
Calculations
 Last Questions
 Pair Share
 Exam
 Unit Packets turned in with Exam
 Questions on Unit 2 Review Work
 Unit 3 – Atomic Structures &
 Chemistry Math Check in Accounting
 Dimensional Analysis Check in
 Pre Assessment & Overview
 % Error Calculations from Labs
 Science & Society – Critical Thinking
 Work time to:  Forgotten Genius Project Intro
 Complete & Review all Packet
 Film Viewing
Work
 Self Score all work
 Get a peer review of your initial
inquiry write up

2. Homework for Day 7
 Unit I & II Packet should be completed if
anything was not completed Day 6
 Unit I test recoveries should be completed
 Complete Unit 3 Pre Assessment
 Preread Chapter 3
 Complete Chapter 3 Review Section 1

3. Test Recovery
If you scored under 90% and would like to improve your grade
follow the steps below. 89% is the highest grade allowed on
recovered tests. ½ Credit is given for all questions corrected as
instructed.
 I. State what your  III. State the correct
mistaken question and answer.
answer were.  IV. Justify your answer
 II. Explain the thinking with a reference in the
error that caused you to text. Show any work
miss the question. necessary to solve the
problem.

4. Mathematical Philosophy in
Chemistry’s Quantum Model
 The Heisenberg Uncertainty  Schrödinger Wave Equation
Principle
 Solutions to this equation are known
as wave functions. Based on the
Heisenberg uncertainty principle
quantum theory determined that wave
functions give only the probability of
finding an electron at a given place
around the nucleus
 Electron are located in 3 dimensional
 Werner Heisenberg probability clouds or orbitals centered
around the nucleus.
 “It is impossible to determine  Erwin
simultaneously both the position  Schrödinger
and velocity of an electron or
particle.”

6. Old atomic model
Quantum atomic
model

8. Quantum numbers – specify the properties of
atomic orbitals and the properties of electrons
in the orbitals
 Quantum theory describes  Angular Momentum Quantum
mathematically the wave Number – At all but the first
properties of electrons and other sublevel multiple orbital shapes
very small particles. exist. Angular momentum
quantum number symbolized by l
indicates the shape of the orbital
 Principal Quantum Number –
symbolized by n, indicates the  s, spherical
main energy level occupied by the  p, dumbbell
electron  d, four are double dumbbell one is
 Total number of orbitals at a level a donut around a dumbbell shape
is n2  f etc.
 correspond to l levels 0,1,2,3

9. Quantum numbers
 Magnetic Quantum  Spin Quantum Number –
Number – symbolized by has only two possible
m, indicates the values +1/2 , -1/2 which
orientation of an orbital indicate the two
around the nucleus fundamental spin states of
 s m=0 an electron in an orbital
 p m=-1,0 or +1
 d m= -2,-1,0,+1,+2
 Etc.

10. Quantum numbers
 Magnetic Quantum  Spin Quantum Number –
Number – symbolized by has only two possible
m, indicates the values +1/2 , -1/2 which
orientation of an orbital indicate the two
around the nucleus fundamental spin states of
 s m=0 an electron in an orbital
 p m=-1,0 or +1
 d m= -2,-1,0,+1,+2
 Etc.