Transcript Semester 1 Review

Semester 1
Review
Chapters
1 - 12
Ch 1: Matter & Measurements
element - molecule
extensive – intensive
microscopic- macroscopic
pure substances – mixtures
homogeneous – heterogeneous
metric prefixes
dimensional analysis
precision – accuracy
significant figures
Ch 2: Atoms & Elements
atomic theory / history
isotopes / abundance
Avogadro’s # / molar mass
periodic table
family names
periods
Ch 3: Molecules & Ions
elements  ions
monatomic/polyatomic ions [CEH2,3]
molar mass – atomic mass
mole concept
% composition
empirical formula
water of hydration
mass spectophotometry
Coulomb’s Law
Coulomb' s Law

n n e
Fk


2
d
2
Ch 4: Chemical Equations
& Stoichiometry
Law of Conservation of Mass
mass-mass problems
limiting reactants
percent yield
Ch 5: Reactions in
Aqueous Solution
electrolytes/non-electrolytes
solubility rules
common acids/bases [CEH4]
strong/weak acids/bases
metathesis reactions [CEH9]
oxidation numbers
redox reactions [CEH8,11]
preparation of solutions
solution stoichiometry
Reaction Type
Driving Force
precipitation
insoluble cmpd
acid-base
molecular water
gas forming
molecular gas
redox
transfer of e-
NET IONIC EQUATIONS
Ch 6: Energy & Chemical Changes
temperatue - heat
joule
system - surroundings
exothermic - endothermic
specific heat capacity
heat of fusion
heat of vaporization
state & path functions
enthalpy of formation
heat of reaction
w  PV
q  mCp T
E  q  w
H
0
rxn




  H products   H reac tan ts
0
f
0
f
Ch 7: Atomic Structure
c = ln
electromagnetic radiation & l
E = hn
line emission
energy level
sub-level
orbital shapes
electron spin
E   2.179  10
18
 1 1
J 2  2 
 nf ni 
Quantum Numbers
Principal QN (n = 1,2, ..)
Angular Momentum QN (l = 0,1,, n-1)
Magnetic QN (ml = ±l)
Spin QN (ms = ±½)
Ch 8: Electron Configuration
& Chemical Periodicity
electron configuration
energy level diagram
electron dot structure
paramagnetic/diamagnetic
Pauli exclusion principal
Hund’s Rule
Chemical Periodicity
atomic size
ionization energy
electron affinity
chemistry of elements
Ch 9: Bonding &
Molecular Structure
ionic & covalent bonding
lattice energy
Lewis structures
resonance structures
formal charge
FC  # VE  # NBE 
1
2
# BE
electronegativity
Trends in
bond order
bond length
bond dissociation energy
VSEPR theory
Electron pair geometry
molecular geometry
molecular polarity
ALL tables & figures
Ch 10: Orbital Hybridization
& Molecular Orbitals
valence bond theory
molecular orbital theory
s and p bonds
hybrids & structure
# bonding e -  # anti bonding e MO bond order 
2
Ch 11: Carbon Chemistry
Nomenclature [CEH6]
isomers
s and p bonds
Alkanes
C–C
Alkenes
C=C
Alkynes
C≡C
Aromatics
alcohols
R – OH
amines
R – NH2
aldehyde
R
O
C
H
ketone
R
O
C
R
carboxylic acid
R
O
C
OH
ester
O
R
R
O
amide
O
R
R
N
H
addition reactions
H2C = CH2
+
HX
↓
H2C - CH2
|
|
H X
where X = F, Cl, Br, I, OH, H
addition polymers
HC = CH
| |
H X
↓
H H H H H H
| | |
| | |
.C – C - C – C – C – C.
| | |
| | |
H X H X H X
condensation polymers
O
R
OH
OH
C
R
O
R
R
O
Chapter 12
Gases and Their
Properties
Combined Gas Law – Fixed
Amount of Gas
P1V1 P2 V2

T1
T2
 Covers
Charles’s and Boyle’s Laws
Ideal Gas Law: PV = nRT
n
= m/M
 Derive Density of a Gas
 Derive molar mass of a gas
van der Waal’s Equation

an 
 P  2 V  bn  nRT
V


2
Dalton’s Law of Partial
Pressures
PT = P1 + P2 + P3 + ….
Gas collected over water
PA = A P(Total)
Graham’s Law
Rate of effusion (diffusion ) of gas 1

Rate of effusion (diffusion ) of gas 2
molar mass of gas 2
molar mass of gas 1