Final Exam Chem 101, Section A0A, Spring 2000
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1 Final Exam Chem 101, Section A0A, Spring 2000 Name Attached is the periodic table you should use. The ideal gas law constant is l atm/(k mol) 1 atm = 760 Torr, 0 C = 273 K. 1 g = 6.85 x 10-5 slug 1. Classify each of the following as either a physical (P) or chemical (C) property: a. Silver tarnishes. b. Sodium chloride dissolves in water. c. Sodium chloride does not dissolve in olive oil. d. When mixed with a solution of silver nitrate, a solution of sodium chloride produces a white precipitate. e. When heated, sodium chloride (table salt) melts at 801 C. f. When heated, solid calcium carbonate (lime) gives off a gas and leaves a solid. g. Sulfur is yellow. 2. Write the chemical formulas for the following molecules: a. A diatomic molecule containing hydrogen b. A diatomic molecule of hydrogen bromide c. A molecule of methane, which contains 1 carbon and 4 hydrogens 3. The smallest piece of a pure substance, which displays all of the chemical and physical properties of that substance, is called a. 4. Identify each of the elements described in problem 4 and write its chemical symbol in the form which indicates which isotope it is: a. 3 protons and 1 neutron b. 14 protons and 14 neutrons c. 30 protons and 35 neutrons d. 78 protons and 117 neutrons name chemical symbol of isotope 1
2 5. Write the complete electronic configuration for the neutral species of each of the elements describe in problem 4: Electronic configuration a. b. c. d. 6. Antimony has two naturally occurring isotopes, Sb and Sb. The percent natural abundance and isotope mass for each isotope is shown in the table below. Calculate the atomic weight of antimony % natural abundance isotope mass (u) 121 Sb 59.25% Sb 40.75% Identify the noble gas that is isoelectronic with each of the following ions: a. Rb +1 b. Al +3 c. O Air is 20%(w/w) oxygen and 80%(w/w) nitrogen. If you breath in 4 L of air and the barometric pressure is 752 Torr, and the temperature is 25 C, how many molecules of air (oxygen plus nitrogen) are in your lungs? 9. How many grams NH 4 Cl are needed to prepare 750 ml of a M solution NH 4 Cl? 2
3 10. Draw Lewis dot structures for each of the following molecules, use the VSEPR theory to predict the geometry of the molecule, and use the electronegativity index along with the VSEPR theory to predict which are polar and which are non-polar moleculess: Chemical Formula Lewis dot structure Polar or Nonpolar? a. CH 4 (with carbon in the center) Geometry b. SO 2 (with sulfur in the center c. H 2 O (with oxygen in the center) Geometry Geometry 11. Identify the oxidizing and reducing agents in the Haber proces for producing ammonia from elemental nitrogen and hydrogen: N 2 (g) + 3 H (g) 2 2 NH 3 (g) Oxidizing agent _ Reducing agent 12. Balance the following equations: a. B 2 O 3 + Mg B + MgO b. P 4 O 10 + H 2 O H 4 P 2 O 7 3
4 c. N 2 O N 2 + O 2 d. KClO 3 KClO 4 + KCl 13. Is the freezing point of 2.00 M solution of CsCl less than, equal to, or greater than the freezing point of a 1.00 M solution of AlCl 3? _ Explain. 14. Complete the following table: Solution [H 3 O + ] [OH - ] ph poh A 3.25 x 10-2 M B 4.35 C 4.32 x 10-9 M 15. The K a value for acetic acid is 1.8 x10-5 M. What is the ph of a solution made by mixing 25.0 ml of M acetic acid with 50 ml of M sodium acetate. 16. Equal molar solutions are made of three monoprotic acids: HA, HB, and HC. The ph values of solutions are respectively 1.32, 6.35, and a. Rank the acids in order of increasing acid strength: < < b. If 100 ml of each are titrated with M NaOH, which will require the greatest amount of NaOH to be completely neutralized? _Explain 4
5 17. A sample of 10.0 g of methane (CH 4 ) is reacted with 30 g of chlorine (Cl 2 ) to produce carbon tetrachloride (CCl 4 ) and hydrogen chloride (HCl). a. Write a balance chemical equation for this reaction: b. Which reactant is limiting? c. What is the maximum mass of carbon tetrachloride (CCl 4 ) that can be produced, i.e., what is its theoretical yield? 18. Give the IUPAC name for the following molecules: CH C CH 19. For each of the following types of hybrid orbitals, indicate the kind and number of atomic orbitals that combine to form each, the number of hybrid orbitals that are formed, and the geometrical arrangement of the hybrid orbitals: Hybrid orbital Atomic orbtials combined to form Number Geometry sp 1 s + 1 p 2 linear sp 2 sp 3 5
6 H Chem 101 Spring 2000 Final Exam 20. Circle the molecules below that are structural isomers of this molecule: CH : C a. b. c. CH d. 3 e. CH CH f. 3 CH 21. Draw a condensed structural formula for each of the following compounds: a. 2-methylpentane: b. sec-butylcyclohexane: c. hexane d. 4-ethyl-2-heptene 22. Complete and balance the following reactions. If no reaction occurs,write "no reaction": a. + O 2 b. + Br 2 c. CH CH + H 2 Pt d. + H 2 O H 2 SO 4 H 2 C CH C 3 6 Score
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