This document provides an overview of topics to be covered in Chemistry I class, including radioactive chemistry, half-life problems, isotopes, quantum numbers, the Heisenberg uncertainty principle, Schrodinger's wave equation, atomic orbitals, and an emission spectrum lab. It discusses converting between mass, moles, and number of particles. The class will review previous chapters, work on practice problems, and receive midterm grades.

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