(a) 7.27 m (b) m (c) 5.38 m (d) 5380 m (e) m

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Joleen Copeland
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1 1. The density of liquid cesium at 30 C is 1.87 g/ml. Because of its wide liquid range (28 to 678 C), cesium could be used as a barometer fluid at high temperatures. What height of cesium will be supported on a day when the temperature is 30 C and a mercury barometer reads 740 torr? (The density of mercury is 13.6 g/ml.) (a) 7.27 m (b) m (c) 5.38 m (d) 5380 m (e) m 2. A cylinder with a moveable piston contains 26.4 cm 3 of a gas at 21 C. If the maximum capacity of the cylinder is 56.8 cm 3, what is the temperature to which the cylinder must be heated to extend the piston to its maximum position? (a) 360 C (b) 462 C (c) 633 C (d) 532 C (e) 280 C 3. A weather balloon is filled with helium to a volume of 31.5 L at 20 C and 1.3 atm. In the stratosphere the temperature and pressure are 23 C and atm respectively. What will be the volume of the balloon in the stratosphere? (a) L (b) L (c) L (d) L (e) L

2 4. A 4.40 g piece of solid CO 2 (dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 300 K. What is the pressure of the gas? (a) 246 atm (b) 2.46 atm (c) atm (d) 122 atm (e) 24.6 atm 5. Four identical 1.0- L flasks contain the following gases each at 0 C and 1 atm pressure. Which gas has the lowest density? (a) HCl (b) Cl 2 (c) CH 4 (d) SO 2 (e) C 2 H 4 6. Which of the following samples contains molecules with the greatest average kinetic energy? (a) 1.0 mol N 2 at 580 K (b) 0.3 mol CO 2 at 440 K (c) 2.0 mol CO at 298 K (d) 0.5 mol O 2 at 480 K (e) 2.5 mol N 2 O at 140 K 7. A mixture of neon and argon is 25.0% neon by mass. What is the partial pressure of neon in the mixture at standard temperature and pressure (0 C and 1 atm)? The atomic masses of Ne and Ar are and g/mol, respectively. (a) 460 torr (b) 301 torr (c) 520 torr (d) 250 torr (e) 380 torr

3 8. Which gases, N 2 O, C 2 H 2, NO, diffuse more slowly than O 2 under identical experimental conditions? (a) N 2 O only (b) C 2 H 2 only (c) NO only (d) NO and C 2 H 2 (e) N 2 O and C 2 H 2 9. Which of the following gases will exhibit the least ideal behavior? (a) N 2 (b)n 2 H 4 (c) CH 4 (d) Ne (e) F Which of the following effects will make PV/RT less than 1 for a 1.0 mole sample of a real gas? (a) The gas molecules are large enough to occupy a substantial amount of space (b) A large number of molecules have speeds greater than the average speed. (c) The gas molecules have very low molecular weights. (d) The gas molecules attract one another (e) The gas molecules are placed in a larger container 11. Which of the following substances has the lowest normal boiling point? (a) H 2 O (b) H 2 S (c) H 2 Se (d) H 2 Te 12. For each of the following pairs determine the substance with the higher normal boiling point: (1) Cl 2 or Br 2, (2) acetic acid CH 3 COOH or 1-propanol CH 3 CH 2 CH 2 OH, (3) SO 2 or CO 2. (a) Higher normal boiling point = Cl 2, CH 3 COOH and SO 2 (b) Higher normal boiling point = Br 2, CH 3 CH 2 CH 2 OH and SO 2 (c) Higher normal boiling point = Cl 2, CH 3 COOH and SO 2 (d) Higher normal boiling point = Br 2, CH 3 COOH and SO 2 (e) Higher normal boiling point = Br 2, CH 3 COOH and CO 2

4 13. Three organic molecules are shown below: acetone, 2-methyl propane and isopropanol. acetone 2-methyl propane isopropanol CH 3 COCH 3 CH 3 CHCH 3 CH 3 CH 3 CHOHCH 3 molar mass = 58 g/mol molar mass = 57 g/mol molar mass = 60 g/mol Which of the following answers correctly arranges these three substances in order of increasing normal boiling point? (a) Lowest b.p. CH 3 COCH 3 < CH 3 CHCH 3 CH 3 < CH 3 CHOHCH 3 (b) Lowest b.p. CH 3 CHCH 3 CH 3 < CH 3 COCH 3 < CH 3 CHOHCH 3 (c) Lowest b.p. CH 3 CHOHCH 3 < CH 3 COCH 3 < CH 3 CHCH 3 CH 3 (d) Lowest b.p. CH 3 CHCH 3 CH 3 < CH 3 CHOHCH 3 < CH 3 COCH 3 (e) Lowest b.p. CH 3 CHOHCH 3 < CH 3 CHCH 3 CH 3 < CH 3 COCH 3 highest b.p. highest b.p. highest b.p. highest b.p. highest b.p. 14. Given below are the temperatures at which two different liquid compounds with the same empirical formula have a vapor pressure of 400 torr. Compound Temperature ( C) Dimethyl ether, H 3 COCH Ethanol, CH 3 CH 2 OH 63.5 Which of the following statements is FALSE? (a) Increasing the temperature will increase the vapor pressure of both liquids. (b) Intermolecular attractive forces are stronger in (liquid) ethanol than in (liquid) dimethyl ether. (c) The normal boiling point of dimethyl ether will be higher than the normal boiling point of ethanol. (d) The reason that ethanol reaches a vapor pressure of 400 torr at a higher temperature than dimethylether is that there is strong hydrogen bonding in ethanol, but not in dimethyl ether. 15. Which of the following phase transitions is exothermic? (a) Vaporization (b) Melting (c) Sublimation (d) Freezing (e) None of the above processes are exothermic

5 16. Which of the following statements regarding viscosity is FALSE? (a) Viscosity increases as the strength of the intermolecular forces increases (b) Viscosity increases as the temperature decreases (c) Viscosity is generally higher for a liquid with large nonpolar molecules than it is for a liquid with small nonpolar molecules (d) All other things being equal viscosity is higher for a liquid with rigid molecules than it is for a liquid with flexible molecules (e) As the number of hydrogen bonds a molecule can form increases the viscosity increases 17. If 40.0 kj is added to 36.0 g of solid H 2 O (ice) initially at a temperature of 25.0 C what is the final temperature of the H 2 O? The specific heat of solid H 2 O is 2.03 J/g K, liquid H 2 O is 4.18 J/g K, and gaseous H 2 O is 1.84 J/g K. The heat of fusion is 6.01 kj/mol and the heat of vaporization is kj mol. The melting and boiling points of water are 0 and 100 C respectively. (a) 273 K (b) 312 K (c) 405 K (d) 373 K (e) 380 K 18. Which of the following descriptions best describes the characteristics of molecules that are prone to form liquid crystalline phases? (a) Nonpolar, rigid molecules with a rodlike shape (b) Polar, rigid molecules with a rodlike shape (c) Nonpolar, flexible molecules with a spherical shape (d) Polar, rigid molecules with a spherical shape (e) Polar, flexible molecules with a rodlike shape

6 19. The table below gives the temperature and pressure of the triple point for five different substances. Substance Temperature (K) Pressure (atm) Xe UF I CO Zn On heating from low temperature at 1 atm of pressure which substance is most likely to sublime rather than melt? (a) Xe (b) UF 6 (c) I 2 (d) CO (e) Zn 20. Consider the properties of ruthenium (IV) oxide and ruthenium (VIII) oxide given in the table below Compound Appearance Melting point Electrical Properties Solubility in H 2 O RuO 2 Black crystalline solid 1300 C Conducting Insoluble RuO 4 Yellow crystalline solid 25 C Insulating Slightly soluble How would you classify these two solids? a. Both RuO 2 and RuO 4 are ionic solids b. Both RuO 2 and RuO 4 are metallic solids c. Both RuO 2 and RuO 4 are molecular solids d. RuO 2 is a covalent- network solid and RuO 4 is a molecular solid e. RuO 2 is a ionic solid and GeBr 4 is an molecular solid

per unit cell = 1 A + 1 B (e) Lattice = square, Atoms per unit cell = 1 A + 2 B 22. For the 2D crystal structure shown below what is the lattice type and how many atoms are there per unit cell?

7 21. For the 2D crystal structure shown below what is the lattice type and how many atoms are there per unit cell? (a) Lattice = rectangular, Atoms per unit cell = 1 A + 2 B (b) Lattice = rectangular, Atoms per unit cell = 1 A + 3 B (c) Lattice = square, Atoms per unit cell = 1 A + 3 B (d) Lattice = square, Atoms per unit cell = 1 A + 1 B (e) Lattice = square, Atoms per unit cell = 1 A + 2 B 22. For the 2D crystal structure shown below what is the lattice type and how many atoms are there per unit cell? (a) Lattice = hexagonal, Atoms per unit cell = 1 A + 1 B (b) Lattice = oblique, Atoms per unit cell = 1 A + 2 B (c) Lattice = centered rectangular, Atoms per unit cell = 2 A + 4 B (d) Lattice = rectangular, Atoms per unit cell = 1 A + 1 B (e) Lattice = hexagonal, Atoms per unit cell = 1 A + 2 B

8 23. Which of the following properties of metals cannot be adequately explained by the electron sea model? (a) The high electrical conductivity of metals (b) The high thermal conductivity of metals (c) The close packed structures of most metals (d) The high melting points of metals in the middle of the transition series, like rhenium (Re) and tungsten (W) (e) The low melting points of metals at the very end of the transition series, like cadmium (Cd) and mercury (Hg) 24. Tantalum crystallizes with a body centered cubic structure. Given the molar mass ( g/mol) and the density of tantalum, ρ = g/cm 3 at 20 C, what value would you calculate for the radius of a tantalum atom? (a) 1.16 Å (0.116 nm) (b) 1.25 Å (0.125 nm) (c) 1.35 Å (0.135 nm) (d) 1.42 Å (0.142 nm) (e) 1.54 Å (0.154 nm) 25. Which of the following metals will have the highest melting point: Rb, Re, Sr, Cd or Au? a. Rb b. Re c. Sr d. Cd e. Au 26. One unit cell of the crystal structure of a cubic compound that forms between copper and oxygen is shown below (the black spheres are copper and the gray spheres are oxygen). If the density of this compound is 4.95 g/cm 3, and the ionic radius of the oxide ion is 1.26 Å, what is the radius of the copper ion? Assume the atoms touch along the bonds shown in the figure. a Å b Å c Å d Å e Å

9 27. If you were to take the zinc blende crystal structure and make all of the atoms the same, what structure type would result? (a) Hexagonal close packed metal (e.g. Zn) (b) Face centered cubic metal (e.g. Al) (c) Body centered cubic metal (e.g. Na) (d) Primitive cubic metal (e.g. Po) (e) Diamond structure (e.g. Si) 28. Which of the following statements is false? a. In a semiconductor the molecular orbitals in the valence band are filled and those in the conduction band are empty b. In a semiconductor the molecular orbitals in the conduction band are bonding molecular orbitals and those in the valence band are antibonding molecular orbitals c. Replacing a tiny fraction of silicon atoms with aluminum atoms would produce a p- type semiconductor d. As the bond distance in a semiconductor increases the band gap decreases e. Many compound semiconductors have the zinc blende structure 29. Arrange the following compound semiconductors from lowest to highest band gap: GaP, GaN, InSb, InAs (a) Smallest band gap InAs < InSb < GaN < GaP Largest band gap (b) Smallest band gap GaN < GaP < InAs < InSb Largest band gap (c) Smallest band gap InSb < InAs < GaP < GaN Largest band gap (d) Smallest band gap InSb < InAs < GaN < GaP Largest band gap (e) Smallest band gap GaN < GaP < InAs < InSb Largest band gap 30. The first light emitting diodes (LEDs) were made from GaAs which has a band gap of 1.43 ev. What wavelength of light would be emitted from an LED built from GaAs? (a) 565 nm (green light) (b) 868 nm (infrared light) (c) 477 nm (blue light) (d) 680 nm (red light) (e) None of the above

10 Equations Pressure P = F a Ideal gas law PV = nrt Dalton s Law of Partial Pressures P Tot RT RT RT = P1 + P2 + P = n1 + n2 + n V V V Kinetic energy Root mean square speed of a gas mu E kinetic = 2 2 3RT u rms = M 2 n a V van der Waals Equation P ( V nb) = nrt + 2 Physical Constants and Conversion Factors Avogadro s Number N = Planck s Constant h = J- s Speed of Light c = m/s Charge of an Electron e = C Ideal Gas Constant R = L- atm/mol- K = J/mol- K = L- torr/mol- K Atmospheric Pressure 1 atm = 760 torr = 760 mm Hg = 101,325 Pa = bar Temperature Conversions K = C STP 273 K and 1 atm 1 ml = 1 cm 3 1 Å = cm = m

11 IA 1 H IIA IIIA IVA VA VIA VIIA 3 Li Na K Rb Cs Fr (223) 4 Be Mg IIIB VIB VB VIB VIIB IB IIB 20 Ca Sr Ba Ra (226) 21 Sc Y La * Ac (227) 22 Ti Zr Hf Unq (261) 23 V Nb Ta Unp (262) 24 Cr Mo W Unh (263) 25 Mn Tc (98) 75 Re Uns (262) 26 Fe Ru Os Uno 27 Co Rh Ir Une 28 Ni Pd Pt Cu Ag Au Zn Cd Hg B Al Ga In Tl C Si Ge Sn Pb N P As Sb Bi O S Se Te Po (209) 9 F Cl Br I At (210) VIIIA 2 He Ne Ar Kr Xe Rn (222) * Lanthanide Series 58 Ce Pr Nd Pm (145) 62 Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Actinide Series 90 Th Pa U Np (237) 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (260)

Part 1. Preparation and Color of Solutions. Experiment 1 (2 session lab) Electrons and Solution Color. Pre-lab Report, page 29

Experiment 1 (2 session lab) Electrons and Solution Color Pre-lab Report, page 29 Session 1 One hour discussion (E2) Two hour lab (E1) Aim to complete Parts 1, 2, and 3 of E1. Part 1. Preparation and Color