Semester 1 Review

Chapters

1 - 12

Ch 1: Matter & Measurementselement - molecule

extensive – intensivemicroscopic- macroscopic

pure substances – mixtureshomogeneous – heterogeneous

metric prefixesdimensional analysisprecision – accuracy

significant figures

Ch 2: Atoms & Elementsatomic theory / historyisotopes / abundance

Avogadro’s # / molar massperiodic tablefamily names

periods

Ch 3: Molecules & Ionselements ions

monatomic/polyatomic ions [CEH2,3]molar mass – atomic mass

mole concept% composition

empirical formula water of hydration

mass spectophotometryCoulomb’s Law

2

2

d

ennkF

Law s'Coulomb

Ch 4: Chemical Equations & Stoichiometry

Law of Conservation of Massmass-mass problems

limiting reactantspercent yield

Ch 5: Reactions in Aqueous Solution

electrolytes/non-electrolytessolubility rules

common acids/bases [CEH4]strong/weak acids/bases

metathesis reactions [CEH9]oxidation numbers

redox reactions [CEH8,11]preparation of solutionssolution stoichiometry

Reaction Type Driving Force

precipitation insoluble cmpd

acid-base molecular water

gas forming molecular gas

redox transfer of e-

NET IONIC EQUATIONSNET IONIC EQUATIONS

Ch 6: Energy & Chemical Changes temperatue - heat

joulesystem - surroundings

exothermic - endothermicspecific heat capacity

heat of fusionheat of vaporization

state & path functionsenthalpy of formation

heat of reaction

TmCq p VPw

wqE

tstanreacHproductsHH 0f

0f

0rxn

Ch 7: Atomic Structure c =

electromagnetic radiation & E = h

line emissionenergy level

sub-levelorbital shapeselectron spin

Quantum NumbersPrincipal QN (n = 1,2, ..)

Angular Momentum QN (l = 0,1,, n-1)Magnetic QN (ml = ±l)

Spin QN (ms = ±½)

2i

2f

18

n

1

n

1J10179.2E

Ch 8: Electron Configuration& Chemical Periodicity electron configurationenergy level diagramelectron dot structure

paramagnetic/diamagneticPauli exclusion principal

Hund’s Rule

Chemical Periodicity atomic size

ionization energyelectron affinity

chemistry of elements

Ch 9: Bonding &Molecular Structure

ionic & covalent bondinglattice energy

Lewis structuresresonance structures

formal charge

BE#NBE#VE#FC 21

electronegativityTrends in

bond orderbond length

bond dissociation energyVSEPR theory

Electron pair geometrymolecular geometrymolecular polarity

ALL tables & figures

Ch 10: Orbital Hybridization& Molecular Orbitalsvalence bond theory

molecular orbital theory and bonds

hybrids & structure

2

e bonding anti # e bonding # order bond MO

--

Ch 11: Carbon ChemistryNomenclature [CEH6]

isomers and bonds

AlkanesC – C

AlkenesC = C

AlkynesC ≡ C

Aromatics

alcohols

R – OH

amines

R – NH2

aldehyde

CO

H

R

CO

R

Rketone

CO

OH

R

carboxylic acid

ester

O

O

R

R

amide

N

O

R

R

H

addition reactionsH2C = CH2

+HX↓

H2C - CH2

| |H X

where X = F, Cl, Br, I, OH, H

addition polymersHC = CH

| |H X

↓H H H H H H| | | | | |

.C – C - C – C – C – C.

| | | | | |H X H X H X

condensation polymers

C

O

OH R

R OH

O

O

R

R

Chapter 12

Gases and Their Properties

Combined Gas Law – Fixed Amount of Gas

Covers Charles’s and Boyle’s LawsCovers Charles’s and Boyle’s Laws

2

22

1

11

T

VP

T

VP

Ideal Gas Law: PV = nRT

n = m/MDerive Density of a GasDerive molar mass of a gas

van der Waal’s Equation

nRTbnVV

anP

2

2

Dalton’s Law of Partial Pressures

PT = P1 + P2 + P3 + ….

Gas collected over waterPA = A P(Total)

Graham’s Law

1 gas of mass molar

2 gas of mass molar

2 gas of )(diffusion effusion of Rate

1 gas of )(diffusion effusion of Rate