Chem 101, Spring 2000 Exam I
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1 Chem 101, Spring 2000 Exam I Name_ Attached is a periodic table you may use. Scratch paper is available at the front of the room. 1. Classify each of the following as either a physical (P or chemical (C property: a. Gold does not rust b. Gold is ductile (can be drawn out into a wire c. Sugar dissolves in water d. When mixed with copper(ii nitrate, potassium chromate produces brown precipitate. e. When heated, sodium chloride (table salt melts at 801 C. f. When heated, sodium bicarbonate (baking soda gives off two different gases. g. When lead shot is placed in water it sinks. h. Sulfur is yellow. 2. For each of the following molecules indicate whether they are homoatomic or heteroatomic; mono-, di-, tri-, or polyatomic; and element or compound: homoatomic or heteroatomic monoatomic, diatomic, triatomic, or polyatomic element or compound a. CO 2 b. H 2 O c. O 3 d. Ne e. SO 3 f. NO g. N 2 h. CH 4 1
2 3. Write the chemical formulas for the following molecules: a. A diatomic molecule containing chlorine b. A diatomic molecule of hydrogen bromide c. A molecule of ammonia, which contains 1 nitrogen and 3 hydrogens 4. The smallest piece of a pure substance, which displays all of the chemical and physical properties of that substance, is called. 5. Indicate the charge and approximate mass in atomic mass units (u of nuclei made up of the following subatomic particles: charge mass a. 3 protons and 1 neutron b. 15 protons and 17 neutrons c. 16 protons and 16 neutrons d. 82 protons and 126 neutrons 6. 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. 15 protons and 17 neutrons c. 16 protons and 16 neutrons d. 82 protons and 126 neutrons name chemical symbol of isotope 7. Write the complete electronic configuration for each of the elements describe in problem 6: Electronic configuration a. b. c. d. 2
3 8. Determine the molecular weights of the following compounds in atomic mass units (u: a. Carbon dioxide (CO 2 b. Fructose (C 6 H 12 O 6 c. Bromine (Br 2 d. Urea (CH 4 NO 9. An older surveying unit that is not used much anymore is the rod. If 1 rod is equal to 16.5 feet, and 1 inch is defined as 2.54 cm (exactly, express the length of 2.50 rods in units of meters and in unites of micrometers. Be sure to round your answer to the correct number of significant figures. 10. The molecular weight is determined for a gas that is known to be an oxide of nitrogen. The value obtained experimentally was u. Which of the following is most likely to be the formula of the gas? NO, N 2 O or NO Platinum (Pt has four naturally occurring isotopes. The following table reports the abundance of each along with their masses in atomic mass units (u. What is the atomic weight of platinum? _ % natural abundance isotope mass (u Pt 32.9% Pt 33.8% Pt 26.1% Pt 7.21%
4 12. Name the elements that have the following electronic configurations: a. 1s 2 2s 2 2p 6 3s 2 3p 3 b. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 14 6p Detemine the number of valence electrons for each of the elements described problem 12: a. b. c. d. 14. Use the trends in the periodic table to predict with member of the each of the following pairs is more metallic: a. Na or Al b. Ca or As c. C or Sn 15. Identify the noble gas that is isoelectronic with each of the following ions: a. Mg 2+ b. Pb 4+ c. Se Write equations to represent positive and negative ion formation for the following pairs of elements. Then write a formula for the ionic compound that results when the ions combine: a. Barium and Chlorine Formula b. Aluminum and Selenium Formula c. Potassium and Bromine Formula 4
5 17. Write chemical formulas for the following binary compounds: a. Dinitrogen oxide b. Platinum(IV iodide c. Calcium chloride d. Magnesium nitride 18. Draw Lewis dot structures for each of the following molecules, use the VSEPR theore 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. OI 2 (with oxygen in the center Geometry b. SO 2 (with sulfur in the center Geometry c. CCl 4 (with carbon in the center d. NO Geometry Geometry 5 Score
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