1 IA 1 ydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 1.01 IIA IIIA IVA VA VIA VIIA 2 e 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00 10 Ne 20.18 11 Na 22.99 12 Mg 24.31 IIIB IVB VB VIB VIIB VIIIB IB IIB 13 Al 26.98 14 Si 28.09 15 P 30.97 16 S 32.07 17 Cl 35.45 18 Ar 39.95 19 K 39.10 20 Ca 40.08 21 Sc 44.96 22 Ti 47.88 23 V 50.94 24 Cr 52.00 25 Mn 54.94 26 Fe 55.85 27 Co 58.93 28 Ni 58.69 29 Cu 63.55 30 Zn 65.39 31 Ga 69.72 32 Ge 72.59 33 As 74.92 34 Se 78.96 35 Br 79.90 36 Kr 83.80 37 Rb 85.47 38 Sr 87.62 39 Y 88.91 40 Zr 91.22 41 Nb 92.91 42 Mo 95.94 43 Tc (99) 44 Ru 101.07 45 Rh 102.91 46 Pd 106.42 47 Ag 107.87 48 Cd 112.41 49 In 114.82 50 Sn 118.71 51 Sb 121.75 52 Te 127.60 53 I 126.90 54 Xe 131.29 55 Cs 132.91 56 Ba 137.33 57 La 138.91 72 f 178.49 73 Ta 180.95 74 W 183.85 75 Re 186.91 76 Os 190.23 77 Ir 192 78 Pt 195.08 79 Au 196.97 80 g 200.59 81 Tl 204.38 82 Pb 207.2 83 Bi 208.98 84 Po (209) 85 At (210) 86 Rn (222) 87 Fr (223) 88 Ra (226) 89 Ac (227) 104 Rf (261) 105 Db (262) 106 Sg (263) 107 Bh (262) 108 s (265) 109 Mt (266) Lanthanide series 58 Ce 140.12 59 Pr 140.91 60 Nd 144.24 61 Pm (147) 62 Sm 150.36 63 Eu 157 64 Gd 157.25 65 Tb 158.93 66 Dy 162.50 67 o 164.93 68 Er 167.26 69 Tm 168.93 70 Yb 173.04 71 Lu 174.97 Actinide series 90 Th (232) 91 Pa (231) 92 U (238) 93 Np (237) 94 Pu (244) 95 Am (243) 96 Cm (243) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (260)
Please RETURN this sheet to the instructor after the test Keep it up & Enjoy at IntroChem! Dr. Edward Wen 1A Electronegativity of Elements 8A 2.1 2A 3A 4A 5A 6A 7A Li 1.0 Be B 2.1 C 2.5 N 3.2 O 3.5 F 4.0 Na 0.9 Mg 1.2 3B 4B 5B 6B 7B 8B 8B 8B 1B 2B Al Si P 2.1 S 2.5 Cl 3.0 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 0.8 Rb 0.8 Cs 0.7 Fr 0.7 1.0 Sr 1.0 Ba 0.9 Ra 0.9 1.3 Y 1.2 La-Lu 1.0-1.2 Zr 1.4 f 1.3 Nb Ta Mo W 1.7 Metal ions w/ fixed charge Tc Re Ru Os Rh Ir Pd Pt Ag Au 2.4 Cd 1.7 g In 1.7 Tl Sn Pb 2.0 Sb Bi 2.4 Te 2.1 Po 2.0 2.8 I 2.5 At 3.0 Xe 2.6 Constants 1 kg = 0 lb 3.78 L = 1 gal 2.54 cm = 1 inch Common molecular geometries: Linear, Bent (or Angular, Trigonal planar, Tetrahedral, Trigonal pyramidal F 32 = C C + 273.15 = K Isotonic solutions: 5%(m/v) glucose; 0.9%(m/v) NaCl 1 mole = 6.022 10 23 unit Gas constant R atm L = 0. 0821 mol K p = -log[ + ] At 25 C, [ + ] [O - ] = 1.0 10-14
Chem 2A Test 3 Name Score: /150 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. 2 pts for each question. 1) If the pressure of a gas is doubled, the volume is doubled provided that the temperature and the number of particles remains constant. 1) MATCING. Choose the item in column 2 that best matches each item in column 1. 3 pts for each question. 2) ydrogen bonding 3) London dispersion force 4) Dipole-dipole interaction A) The intermolecular force between X- bonds (X = N, O, F) and high electronegative atoms (N, O, F) B) The intermolecular force between X- bonds (X = any atom) and high electronegative atoms (N, O, F) 2) 3) 4) C) The intermolecular force caused by instantaneous induced dipoles among molecules D) The intermolecular force caused by permanent dipoles among molecules MULTIPLE COICE. 3 pt for each question. 5) Which of the following is NOT part of the kinetic theory of gases? A) Gas particles move faster when the temperature increases. B) There is very little empty space in a gas. C) A gas is composed of very small particles. D) Gas particles move rapidly. E) Gas particles do not attract or repel one another. 5) 6) According to the diagram below, which one of the listed phase changes is endothermic? 6) A) IV B) I C) V D) III 7) Weak intermolecular force is responsible for A) weaker covalent bonding B) higher vapor pressure C) more viscous D) higher boiling point 7) A-1
8) Under which of the following conditions does the solute has the lowest solubility? A) Oxygen gas in water with P = 1 atm and T = 100 C B) Oxygen gas in water with P = 2 atm and T = 0 C C) Oxygen gas in water with P = 2 atm and T = 25 C D) Oxygen gas in water with P = 1 atm and T = 25 C 8) 9) Under which of the following conditions does table salt has the greatest solubility in water? A) P = 2 atm and T = 0 C B) P = 1 atm and T = 25 C C) P = 1 atm and T = 100 C D) P = 2 atm and T = 25 C 9) 10) Which of the following is an intermolecular force that occurs between C3F molecules? I. London dispersion forces II. Dipole-dipole interaction III. ydrogen bonding A) II only B) I and II C) I only D) I, II, and III 10) 11) In which of the following substances, in the pure liquid state, would hydrogen bonding occur? A) Cl B) F N C) C O 12) Predict which one of the following compounds is most soluble in water A) SO2 B) CO2 C) Li3SO4 D) N2 D) Si O Si 11) 12) 13) An osmosis device is illustrated below, where two chambers A (pure water) and B (tap water) are separated by semipermeable membrane that allows only water molecules to pass through: 13) Which one of the following statement is true? A) water will transfer from B to A. B) the concentration of ions in A will increase. C) the concentration of ions in B will increase D) water will transfer from A to B. 14) For every 10.0 g of sea water, there is 0.35 g of salt. What is the mass percent concentration of salt in sea water? A) 100% B) 0.35% C) 3.5% D) 10.0% 14) 15) There is 7.5 g of acetic acid in 160. ml white vinegar sample. What is the weight/volume percent concentration of acetic acid in this vinegar? A) 4.7% B) 7.5% C) 0.75% D) 16% 15) 16) At 25 C, the concentration of + of an aqueous solution is found to be 10-4 M. The p of this solution is A) 8.3 B) 3.8 C) 2.10 D) -2.1 16) A-2
17) At 25 C, the concentration of + of an aqueous solution is found to be 8.0 10-3 M. The concentgration of hydroxide ion is A) 1.3 10-12 M B) 1.0 10-7 M C) 1.0 10-14 M D) 8.0 10-12 M 17) 18) At 25 C, the concentration of + of an aqueous solution is found to be 8.0 10-10 M. The solution is A) not enough information B) basic C) neutral D) acidic 18) 19) Which of the following p represents a solution where the concentration of hydrogen ion is lower than the concentration of hydroxide ion? A) 10 B) 7 C) 1 D) 4 19) 20) What is the p of a 0.20 M nitric acid solution? A) 0.020 B) 1.7 C) 2.0 D) 0.7 20) 21) Which p is most alkaline (basic)? A) 10 B) 1 C) 7 D) 4 21) 22) Which one of the following reactions is an acid-base neutralization reaction? A) 2SO4 + 2 KO K2SO4 + 2 2O 22) B) 4 NaO + ZnCl2 2 NaCl + Na2Zn(O) 4 C) 2Al + 6 Cl 2AlCl3 + 32 D) AgNO3 + Br NO3 + AgBr 23) Which of the following conjugate pairs would form a good buffer? A) KO / 2O B) 2SO4/KSO4 C) NO3 / NaNO3 D) C23O2 / NaC23O2 23) 24) Which of the following combinations of compounds would produce a buffer? A) A weak base and a salt of the weak base B) A salt of a strong acid and a salt of a weak acid C) A strong acid and a salt of the strong acid D) A strong base and a salt of the strong base 24) PROBLEMS. Show work with proper Significant Figures and Units to receive credit. 5 pts for each question unless otherwise noted. 25) (10 pts) If the volume of a gas container at 32.0 C changes from 5 L to 755 ml, what will the final temperature be? A-3
26) (10 pts) Calculate the pressure, in atmosphere, of 0.100 mole of 2 gas in a 3.78-L container at a temperature of 25 C. 27) A vinegar solution contains 5.0% (w/v) acetic acid. ow many grams of acetic acid are contained in 160. ml of this vinegar solution? 28) (10 pts) ow many milliliters of 0.500 M solution can be prepared by dissolving 2.00 g NaCl in water? 29) A 25.0 ml solution contains 0.500 g NaO. Find the molarity of NaO in the sample. 30) Determine the final concentration of the solution after 15.0 ml of water is added to 25.0 ml 0.450 M NaCl solution. A-4
31) Find the p of 8.0 10-3 M NaO solution. 32) (13 pts) One tablet of anti-acid pill contains 1.00 g calcium carbonate. The chemical reaction to neutralize the gastric acid is 2 Cl + CaCO3 CaCl2 + 2O + CO2 ow many milliliters of gastric acid (0.130 M Cl) can be neutralized by two tablets of this pill? 33) (5 + 10 pts) During a titration experiment, 20.0 ml 2SO4 solution of unknown concentration is neutralized by 45.0 ml 0.200 M NaO solution. A. Write balanced equation for this reaction. B. Determine the molar concentration of this 2SO4 solution. A-5