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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.

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Semester 1 Review

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  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

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

  6. 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

  7. NET IONIC EQUATIONS

  8. 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

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

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

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

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

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

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

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

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

  17. Aromatics

  18. alcohols R – OH amines R – NH2

  19. aldehyde

  20. ketone

  21. carboxylic acid

  22. ester

  23. amide

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

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

  26. condensation polymers

  27. Chapter 12 Gases and Their Properties

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

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

  30. van der Waal’s Equation

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

  32. Graham’s Law

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