Final Exam ReviewExam 1 Concepts You Should Know:Exam 1 Concepts You Should Know:Exam 1 Practice ProblemExam 1 Practice ProblemExam 1 Practice ProblemExam 2 Concepts You Should Know:Exam 2 Practice ProblemExam 2 Practice ProblemExam 3 Concepts You Should Know:Exam 3 Practice ProblemExam 3 Practice ProblemExam 3 Practice ProblemFinal Concepts You Should Know:Final Practice ProblemFinal Practice ProblemFinal Practice ProblemFinal Practice ProblemFinal Practice ProblemFinal Exam ReviewCH110 FA11 SAS 1FINAL EXAMMonday, Dec. 12th, 2:30 PM• The usual rules apply: Bring an approved calculator, you will get a clean periodic table and equation sheet, no cheating.• The final is CUMULATIVE. Expect about half of the questions to be Exams 1-3 and half the new material.• The final is longer than the three previous exams. There are 40 questions and you have more time.• If you are still here, you have probably done well on the other three exams. I am confident you will do well again.Exam 1 Concepts You Should Know:CH110 FA11 SAS 2• What do the numbers on the periodic table mean?• How do we name common ions, acids, etc.?Chapter 2: NomenclatureChapter 3: Chemical FormulasChapter 6: Energy, Atoms, Orbitals, and the Origins of the Periodic Table• What is mass percent?• What is a mole? What is molecular weight?• What are the empirical formula and the molecular formula of a compound?• What is the relationship between photons, their wavelength, their frequency, and their energy?• How does all that stuff about photons help chemists to understand the nature of atoms?• What is an orbital? How is it defined?• What is the electron configuration of an atom? How do I represent it?• How do the shape, size, and number of orbitalshelp me to understand the periodic table?Exam 1 Concepts You Should Know:CH110 FA11 SAS 3Chapter 7: Periodic TrendsChapter 8: Bonding and Lewis Structures• What are ionization energy, electron affinity, and electronegativity?• What are the trends in atomic size?• How are the sizes of atoms and ions related?• How do these show up in the periodic table?• What are the three types of bonding?• How do we describe bonding in ionic solids?• How is covalent bonding described in terms of enthalpy, strength, bond order, etc.?• What is a Lewis structure?• What do we learn about a molecule when we see that it has more than one Lewis structure?• How do you use the octet rule and its violations to help predict Lewis structures?Exam 1 Practice ProblemCH110 FA11 SAS 4The following substances are fertilizers that contribute nitrogen to the soil: urea [(NH2)2CO] ammonium nitrate ammonium sulfateExam 1 Practice ProblemCH110 FA11 SAS 5Which one of the following could not be an electron configuration for vanadium, V?Exam 1 Practice ProblemCH110 FA11 SAS 6Which of the following compounds would have the largest lattice energy?Exam 2 Concepts You Should Know:CH110 FA11 SAS 7• How do we determine the composition of a compound from the various chemical formulas?• What is combustion analysis?Chapter 3: Chemical Formulas AgainChapter 25: Organic MoleculesChapter 9: Bonding and Geometry• What are the properties of hydrocarbons?• What do the functional groups we learned about look like and how do they affect properties?• What are the shapes of the electron domain and molecular geometries we have studied?• What is molecular polarity and how is it determined by shape?• What are sigma and pi bonds?• How do hybrid orbitals relate to molecular shape and bond angles?• What are the IMFs we have learned about?• How do IMFs impact boiling and melting points?Chapter 11: Intermolecular ForcesExam 2 Practice ProblemCH110 FA11 SAS 8The labeled carbon in the molecule below has what type of hybrid orbitals?Exam 2 Practice ProblemCH110 FA11 SAS 9Which one of the following has the strongest intermolecular forces?Exam 3 Concepts You Should Know:CH110 FA11 SAS 10• What are the properties of ideal gases?• What is the partial pressure of a gas in a mixture?• How does kinetic molecular theory connect the microscopic properties of gases with observables?• How are real gases different from ideal gases?Chapter 10: GasesChapter 18: Atmospheric ChemistryChapter 13: (Aqueous) Solutions• What reactions occur in the atmosphere?• How do Chem 110 concepts show up in the atmosphere and environment?• What are electrolytes and how do we calculate the concentration of chemicals in solution?• What is meant by solubility and saturation?• What are colligative properties?• What is heat capacity?• What are the properties of liquids?• How do you use phase diagrams?Chapter 11: Intermolecular ForcesExam 3 Practice ProblemCH110 FA11 SAS 11An unlabelled 2 L canister is found in a laboratory. The gas inside is expanded to a total volume of 10 L where its final temperature is 21oC, pressure 2.1 atm, and its density is measured to be 3.48 g/L.Exam 3 Practice ProblemCH110 FA11 SAS 12Exam 3 Practice ProblemCH110 FA11 SAS 13Rank these aqueous solutions in order of increasing freezing point.Final Concepts You Should Know:CH110 FA11 SAS 14• How do I balance a chemical equation?• What is the percent yield of a reaction?Chapter 3: Chemical EquationsChapter 4: Chemical ReactionsChapter 5: Thermochemistry• What are precipitation reactions?• What are metathesis reactions? • What are redox reactions in particular and what are oxidation numbers?• What are net ionic equations and spectator ions?• What is enthalpy and the enthalpy of a reaction?• What is heat of formation?• How do bond enthalpies relate to both of these?• What is Hess’s Law?• What is an equilibrium constant?• How do you use an “ICE” table to calculate equilibrium constants or concentrations?• What is LeChâtlier’s principle?Chapter 15: Chemical EquilibriumFinal Practice ProblemCH110 FA11 SAS 15A solution of silver nitrate and sodium chloride are mixed.Final Practice ProblemCH110 FA11 SAS 16What is ∆H° for the combustion of 11.42 g of methanol?.Final Practice ProblemCH110 FA11 SAS 17When an Alka-Seltzer tablet dissolves in water, the following reaction between sodium bicarbonate and citric acid occurs:3 NaHCO3(aq) + H3C6H5O7(aq) →3 CO2(g) + 3 H2O(l) + Na3C6H5O7(aq)Final Practice ProblemCH110 FA11 SAS 18Consider the following reaction at equilibrium:2 NH3(g) N2(g) + 3H2 (g) ΔHo= + 92.4 kJFinal Practice ProblemCH110 FA11 SAS 19The following reaction is allowed to reach
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