CHEM101/3; E2 & G1
Quiz Checklist
2006 09 22
HT
Note: This list is not necessarily exhaustive; ultimately, you are responsible for whatever came up in class!
Up to Rutherford
Schroedinger Model of H Atom
Dalton’s ideas about matter, elements & cmpds
evidence for subatomic particles
Thomson & Millikan experiment
“Plum Pudding” model
radioactivity & X-rays, experimental description
Rutherford experiment
Rutherford model: dense nucleus, empty space …
subatomic particles: e –, p +, n o
atomic number, mass number & atomic mass
isotopic notation
atomic mass of elements (= isotopic mixtures)
ions: charge as a result of loss/gain of e’s
names of first 36 elements
review SI units & SI prefixes
de Broglie equation
Heisenberg Uncertainty Principle
properties of standing waves
general description of Schroedinger equation &
wavefunction
quantum numbers n, l, ml and their relationships
visualization of orbitals:
Ψ , Ψ2 , 4πr2Ψ2 , electron density chart,
containing envelope (surface boundary) graph
recognize orbital identity from various imagery
description of nodes & phases
penetration phenomenon
Bohr Model
behavior of waves (diffraction, refraction)
regions of EMR
photoelectric effect: functional diagram,
workfunction (= binding energy)
minimumfrequency, KE of emitted electrons
EMR as particle phenomenon, photons
Planck equation
continuous & line spectra
gas discharge tubes, functional diagram
empirical analysis of H spectrum
modern analysis of H spectrum
emission & absorption of EMR
Bohr atom
quantum number, radius, energy level
extension to “hydrogenic” atoms
Multielectron Atoms & Periodic Table
penetration effect on energy level degeneracy
ms, e – spin quantum number
rules for building e – configurations
various notation methods for e – configurations
Periodic Table as a reflection of e – configurations
effective nuclear charge, Zeff
periodic trends in PT
size of atoms and ions
ionization energy
electron affinity
chemical properties
CHEM101/3, E2 &G1
Checklist for MidTerm Exam
2006 10 20
HT
The midterm exam will include all materials starting from the beginning of the course.
Consequently, the Checklist for the Quiz, provided earlier, is also applicable and
all items should be reviewed.
Note: This list is not necessarily exhaustive; ultimately, you are responsible for whatever came up in class!
Formula and Data sheets will be the same as for the Quiz.
Review
Nomenclature,
see lecture notes 7 – 5 a-d
Stoichiometry
formulas, mole concept,
balancing equations,
mass relationships in chem. rxns,
limiting reactant, yield calc.,
determination of empirical & molecular
formulas,
concentration & dilution
Lewis Theory
differentiate between ionic and covalent
Lewis structures
use concept of electronegativity to assess
covalent and ionic bonds
apply “extended octet rule”
determine formal charge
systematic derivation of Lewis structures:
skeletal structure and e– distribution
describe concept of resonance
derive resonance structures, incl.
assessment of major/ minor contributors
based on “preference rules”
Shapes of Molecules
foundation of VSEPR theory
concept of e – groups
distinguish between e – and atom
arrangement
derive shapes for AX2 ........AX4E2 type
molecules from Lewis structures
using VSEPR theory
use geometry to assess molecular polarity
based on bond polarity
Valence Bond Theory
foundation of VB
( bonds a result of overlapping AO’s
occupied by 2 paired e – )
σ and π bonds
concept of hybridization of AO’s
multiple bonds
correlation between hybridization type and
molecular shape
MO Theory
foundation: combination of AO’s
bonding & antibonding MO’s
MO’s and energy diagrams for row 1 & 2
homonuclear diatomics
tentative: MO’s for heteronuclear diatomics
CHEM101/3, E2 & G1
Checklist for Final Exam
2006 11 24
HT
The final exam will include all materials starting from the beginning of the course.
Consequently, the Checklists for the Quiz and the MidTerm Exam, provided earlier, are applicable
and all items should be reviewed.
The Data Sheet (CDS) will be the same as for the midterm exam;
the formula tables the same as for the the Sample Final Exam.
Note: This list is not necessarily exhaustive; ultimately, you are responsible for whatever came up in class!
Properties and Behavior of Gases
explain T and P on the molecular basis
differentiate between various expressions
for pressure: atmospheric,
gage(differential), absolute, barometric
know the avg. atmospheric pressure in Edm.
Ideal Gas Law & derivation of individual
gas laws
applications of IGL: determination of
D↔MM; gas stoichiometry
vapor pressure of liquids & VP curves
def. of mole fraction & partial pressure
Dalton’s Law of partial pressures
application of Dalton’s Law: collection of
gases over liquids; use of partial pressures
in stoichiometry
Kinetic Molecular Theory
basic assumptions
overall results
dependence of molecular speeds & KE on
temperature and MM
distribution of molecular speeds (Maxwell Boltzmann)
definition & application of effusion &
diffusion phenomena
deviation of real gases from ideal behavior
correction factors in the vdW equation
comparison between real & ideal gases
Intermolecular Forces
describe the forces that cause deviation from
ideal gas behavior; illustrate & give
examples
intramolecular forces: covalent, ionic,
metallic
intermolecular forces: ion-dipole, ioninduced dipole, dipole-dipole, H-bonding,
dipole-induced dipole, momentary dipoleinduced dipole
predict major IMF’s based on molecular
structure
assess H-bonding between identical & different
molecules
describe the nature of LDF’s
effect of polarizability on LDF’s
effect of IMF’s on solubility, vapor pressure,
b.p., m.p.
Liquids
liquid properties: dense, but mobile
know definition of viscosity, surface tension,
cohesive & adhesive forces
Solids
distinguish between amorphous & crystalline
solids
for molecular, network covalent, ionic &
metallic solids:
describe nature of IMF’s,
indicate resulting macroscopic properties
provide examples, incl. structures
rudimentary knowledge of band theory
basic crystallography:
unit cells, close packing, coordination
numbers, density
Phase Diagrams (PD)
provide definition for pure substances
draw generic PD & identify/describe various
points/regions: triple point, critical point,
phase transitions, single phases (S, L, G)
assess effect of P & T changes on the
existence of various phases
Acid/Base (A/B) Chemistry
3 different definitions of A/B
A/B behavior of hydrides & oxides
periodic trends of acid strength of
hydrides/oxides and of oxoacids
conjugate A/B concept