Comprehensive Review of Chemistry Concepts for Semester 1

1. Semester 1 Review Chapters 1 - 12

2. Ch 1: Matter & Measurements element - molecule extensive – intensive microscopic- macroscopic pure substances – mixtures homogeneous – heterogeneous metric prefixes dimensional analysis precision – accuracy significant figures

3. Ch 2: Atoms & Elements atomic theory / history isotopes / abundance Avogadro’s # / molar mass periodic table family names periods

4. 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

6. Ch 4: Chemical Equations & Stoichiometry Law of Conservation of Mass mass-mass problems limiting reactants percent yield

7. 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

8. NET IONIC EQUATIONS

9. 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

11. Ch 7: Atomic Structure c = ln electromagnetic radiation & l E = hn line emission energy level sub-level orbital shapes electron spin

12. Quantum Numbers Principal QN (n = 1,2, ..) Angular Momentum QN (l = 0,1,, n-1) Magnetic QN (ml = ±l) Spin QN (ms = ±½)

13. Ch 8: Electron Configuration & Chemical Periodicity electron configuration energy level diagram electron dot structure paramagnetic/diamagnetic Pauli exclusion principal Hund’s Rule

14. Chemical Periodicity atomic size ionization energy electron affinity chemistry of elements

15. Ch 9: Bonding & Molecular Structure ionic & covalent bonding lattice energy Lewis structures resonance structures formal charge

16. electronegativity Trends in bond order bond length bond dissociation energy VSEPR theory Electron pair geometry molecular geometry molecular polarity ALL tables & figures

17. Ch 10: Orbital Hybridization & Molecular Orbitals valence bond theory molecular orbital theory s and p bonds hybrids & structure

18. Ch 11: Carbon Chemistry • Nomenclature [CEH6] • isomers • and p bonds Alkanes C – C Alkenes C = C Alkynes C ≡ C

19. Aromatics

20. alcohols R – OH amines R – NH2

21. aldehyde

22. ketone

23. carboxylic acid

24. ester

25. amide

26. addition reactions H2C = CH2 + HX ↓ H2C - CH2 | | H X where X = F, Cl, Br, I, OH, H

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

28. condensation polymers

29. Chapter 12 Gases and Their Properties

30. Combined Gas Law – Fixed Amount of Gas • Covers Charles’s and Boyle’s Laws

31. Ideal Gas Law: PV = nRT • n = m/M • Derive Density of a Gas • Derive molar mass of a gas

32. van der Waal’s Equation

33. Dalton’s Law of Partial Pressures • PT = P1 + P2 + P3 + …. • Gas collected over water • PA = A P(Total)

34. Graham’s Law