1. Welcome to Chemistry I – Day IX
Portland Evening Scholars
Mr. Treothe Bullock - Instructor
 Unit 3 - Work which should be
completed – ready for questions
and review
 Chapter 3 Review
 We will sign off on and
go over
 Math Take Home Test - 1st
problem set done – we will
continue 1st
problem sign
offs
 Minimum of 1 Radioactivity or
Half Life labs –
 Recovery contract work -
turn in as done
 Unit 3 - Chapter 4 – Arrangement
of the electrons in the atom
 Emission Spectrum Lab –
how have models changed?
 Equations of Light &
Electromagnetic Energy
 Quantum numbers & Electron
Configurations
 Forgotten Genius Project –
Science & Society
 Homework for next week
 Complete Chapter 4 review
 Complete Orbital Diagrams
 Recovery Completions

2. Mathematical Philosophy in
Chemistry’s Quantum Model
 The Heisenberg Uncertainty
Principle
 Werner Heisenberg
 “It is impossible to determine
simultaneously both the position
and velocity of an electron or
particle.”
 Schrödinger Wave Equation
 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
probability clouds or orbitals centered
around the nucleus.
 Erwin
 Schrödinger

4. Old atomic model
Quantum atomic
model

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

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