Semester 1 Review Chapters

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

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 TypeDriving Force precipitationinsoluble cmpd acid-basemolecular water gas formingmolecular gas redoxtransfer 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

Ch 7: Atomic Structure c = electromagnetic radiation & E = h line emission energy level sub-level orbital shapes electron spin

Quantum Numbers Principal QN (n = 1,2,..) Angular Momentum QN (l = 0,1,, n-1) Magnetic QN (m l = ±l) Spin QN (m s = ±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

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  and  bonds hybrids & structure

Ch 11: Carbon Chemistry Nomenclature [CEH6] isomers  and  bonds Alkanes C – C Alkenes C = C Alkynes C ≡ C

Aromatics

alcohols R – OH amines R – NH 2

aldehyde

ketone

carboxylic acid

ester

amide

addition reactions H 2 C = CH 2 + HX ↓ H 2 C - CH 2 | H X where X = F, Cl, Br, I, OH, H

addition polymers HC = CH | H X ↓ H H H | | |. C – C - C – C – C – C. | | | H X H X H X

condensation polymers

Chapter 12 Gases and Their Properties

Combined Gas Law – Fixed Amount of Gas  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

Dalton’s Law of Partial Pressures   P T = P 1 + P 2 + P 3 + ….   Gas collected over water   P A =  A P (Total)

Graham’s Law