1. Welcome to Chemistry I – Day VIII
Portland Evening Scholars
Mr. Treothe Bullock - Instructor
 Radioactive Chemistry
 Discussion of Labs
 Half Life Problems
 Isotopes
 Chapter 3 Review – Section 2 & 3
 Have out work to be signed
 Review
 Unit 3 Math – Converting from Mass
to Moles to # of Particles
 Practice Problems
 Guided Sign off Problems
 Take Home Quiz Problems
 Mid Term Grades
 Interpreting marks
 Individual check-ins during
Emission Spectrum Lab
 Contracting repair of any below C
work
 Introduction to Quantum Numbers
 Wave vs. particle
 Heisenberg’s Uncertainty
Paradox
 The modern atom & Emission
Spectrum’s
 Lab – Models of the Hydrogen Atom -
Emission Spectrum Lab

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