Spring Final study guide PDF

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Spring final exam study guide. Lecture notes and examples...

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Name: ________________________ Class: ___________________ Date: __________

ID: A

1 Multiple Choice Identify the choice that best completes the statement or answers the question. ____

1. 1.8 kilograms contain this many grams. 3 a. 1.8 u 10 2 b. 1.8 u 10 1 c. 1.8 u 10 2 d. 1.8 u 10 3 e. 1.8 u 10

____

2. 485.5 K equals a. 212.5°F b. 873.9°C c. 758.5°F d. 212.5°C e. 758.5°C

____

3. Aluminum has a density of 2.70 g/cm3. What is the mass of a rectangular block of aluminum

measuring 11.1 cm by 22.2 cm by 34.5 cm? a. 183 kg 3 b. 3.15 u 10 kg c. 0.318 kg d. 23.0 kg e. none of these ____

4. The symbol N stands for the element a. nitrogen b. nickel c. neon d. nobelium e. niobium

____

5. Which of the following contains the largest number of oxygen atoms? a. 4H2O b. 3CO2 c. O3 d. H2SO4 e. Al(NO3)3

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Name: ________________________

____

6. The number of neutrons in one atom of a. b. c. d. e.

ID: A 204 80

Hg is

124 80 204 284 none of these

____

7. An atom with 15 protons and 16 neutrons is an atom of a. P b. Ga c. S d. Pd e. Rh

____

8. Which of the following is a nonmetal? a. cerium b. cesium c. carbon d. calcium e. copper

____

9. Which of the following formulas is incorrect? a. AlO3 b. c. d. e.

KBr KNO3 Li2O CaSO4

____ 10. When the following equation is balanced using the smallest possible integers, what is the number in

front of the substance in bold type? Pb(NO3)2 + K2CO3 o PbCO3 + KNO3 a. b. c. d. e.

5 4 3 2 1

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Name: ________________________

ID: A

____ 11. When the following equation is balanced using the smallest possible integers, what is the number in

front of the substance in bold type? Al + Fe3O4 o Al2O3 + Fe a. b. c. d. e.

1 3 6 9 12

____ 12. A substance that, when dissolved in water, produces a solution that conducts electric current very

efficiently is called a. a strong electrolyte b. a weak electrolyte c. a strong ion d. an electrical solute e. none of these ____ 13. 1.2 moles of oxygen atoms represent a. 0.7 u 1024 atoms b. 0.4 g c. 1.0 u 102 g d. 1.9 u 101 atoms e. none of these ____ 14. How many atoms of calcium are present in 58.2 g of calcium? a. b. c. d. e.

8.74 u 1023 2.41 u 10– 24 3.50 u 1025 6.02 u 1023 none of these

____ 15. Calculate the mass of 23.7 moles of He in grams. a. 94.9 b. 27.7 c. d. e.

1.43 u 1025 5.92 6.02 u 1023

____ 16. The molar mass of blood sugar, C6H12O6, also known as glucose and dextrose, is a. b. c. d. e.

180.16 g/mol 6.02 u 1023 g/mol 108.10 g/mol 168.06 g/mol none of these 3

Name: ________________________

ID: A

____ 17. Convert: 44.4 g NO2 = ___________ mol NO2 a. 0.965 b. c. d. e.

2.04 u 103 2.67 u 1025 44.4 1.04

____ 18. What is the mass percentage of carbon in the compound C6H6O2? a. b. c. d. e.

5.5 % 70.9 % 65.5 % 29.1 % 14.3 %

____ 19. Analysis of a compound showed that it contained 76.0 % fluorine atoms and 24.0 % carbon atoms

by mass. What is its empirical formula? a. CF2 b. C2F3 c. CF3 d. C2F5 e. CF ____ 20. Pure copper may be produced by the reaction of copper(I) sulfide with oxygen gas as follows:

Cu2S(s) + O2(g) o 2Cu(s) + SO2(g) If 0.680 kg of copper(I) sulfide reacts with excess oxygen, what mass of copper metal may be produced? a. 0.680 kg b. 0.136 kg c. 0.271 kg d. 0.543 kg e. 1.36 kg ____ 21. 2Al(s) + 6HCl(aq) o 2AlCl3(aq) + 3H2(g)

According to the equation above, how many grams of aluminum are needed to completely react with 3.83 mol of hydrochloric acid? a. 310 g b. 46.6 g c. 34.4 g d. 3.83 g e. 103.3 g

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Name: ________________________

ID: A

____ 22. The oxidation number of barium in BaO is a. +1. b. +4. c. –1/2. d. +2. e. –2. ____ 23. Identify the spectator ions in the following reaction.

Ca2+(aq) + 2NO3–(aq) + 2Na+(aq) + CO32–(aq) o CaCO3(s) + 2Na+(aq) +2NO3–(aq) a. b. c. d. e.

NO3– and CO32– Ca2+ and Na+ Ca2+ and CO32– Ca2+ and NO3– Na+ and NO3–

____ 24. Choose the correct ground-state electron configuration for chlorine.

d.

[Ne] 3s23p5 [Ne] 3s23p7 [Ar] 3s23p5 [Ne] 4s24p5

e.

[Ne] 2s23p7

a. b. c.

____ 25. How many d electrons are in an atom of cobalt? a. 7 b. 9 c. 10 d. 27 e. 59 ____ 26. Which of the following has the electron configuration [Ar] 4s23d5 ? a. Mn b. Ca c. Br d. V e. none of these ____ 27. Which of the following atoms has the highest ionization energy? a. F b. Be c. N d. C e. Li

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Name: ________________________

ID: A

____ 28. Rank the following from smallest to largest atomic radius. a. O, Zn, Ca, Ba b. O, Ca, Zn, Ba c. Ba, Ca, Zn, O d. O, Zn, Ba, Ca e. Ca, Ba, Zn, O ____ 29. Which of the following has primarily ionic bonding? a. N2O3 b. Na2O c. CO2 d. CCl4 e. none of these ____ 30. Perform the following conversion of pressure units:

193 torr = ____________ atm a. b. c. d. e.

1.91 13.1 0.254 3.94 953

____ 31. A gas originally occupying 10.1 L at 0.925 atm and 25°C is changed to 13.3 L at 625 torr. What is

the new temperature? a. 349 °C b. 76 °C c. –244 °C d. 622 °C e. 50 °C ____ 32. What volume will 55.6 g of N2 occupy at STP? a. 48.5 L 2 b. 5.85 u 10 L c. 44.5 L d. 4.07 L e. none of these ____ 33. Which of the following species exhibit hydrogen bonding? a. HBr b. NO3– c. H2O d. SF4 e. KrCl4 f. I3–

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Name: ________________________

ID: A

____ 34. What is the major attractive force in CO? a. dipole-dipole b. London dispersion c. ionic d. hydrogen bonding e. none of these ____ 35. A solution is prepared by dissolving 8.29 g of Na2SO4 in enough water to make 225 mL of solution.

Calculate the solution molarity. a. 0.0584 M b. 1.87 M c. 0.603 M d. 0.259 M e. 0.484 M ____ 36. Which of the following is not a conjugate acid-base pair? a. H2SO4, SO42– b. HNO3, NO3– c. HC2H3O2, C2H3O2– d. H2PO4–, HPO42– e. HBr, Br– ____ 37. Calculate the [H+] in a solution that has a pH of 8.82. 8 a. 6.6 u 10 M 5 b. 1.5 u 10 M c. d. e.

7

1.0 u 10 M 1.5 u 10 9 M none of these

____ 38. A solution has [H+] = 5.0 u 10–8 M. The pH of this solution is a. 6.70 b. 5.98 c. 7.30 d. 9.77 e. none of these ____ 39. Alpha particles are a. electrons b. protons c. neutrons d. helium nuclei e. X rays

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Name: ________________________

ID: A

____ 40. The cesium-137 nuclide has a half-life of 30 years. After 90 years, about 10 g remains. The original

mass of the cesium-137 is closest to a. 80 g b. 60 g c. 100 g d. 90 g e. 70 g ____ 41. Which of the following formulas represents butane? a. CH3CH3 b. CH3CH2CH3 c. d. e.

CH3CH2CH2CH2CH3 CH3CH2CH2CH3 CH4

____ 42. Which of the following class of compounds does not contain an oxygen atom? a. aldehyde b. alkyne c. alcohol d. ester e. ketone ____ 43. Express the number 0.00395 in scientific notation. a. 3.95 u 10–3 b. 3.95 u 103 c. 0.395 u 10–3 d. 395 u 10–5 e. none of these ____ 44. A person has a mass of 9.82 u 104 g. What is this person's mass in pounds?

(1 kg = 2.2046 lb) a. 2.16 u 105 lb b. 4.45 u 104 lb c. 216. lb d. 98.2 lb e. 982. lb ____ 45. Which of the following is not the correct chemical formula for the compound named? a. hydrocyanic acid HCN b. calcium sulfate CaSO4 c. beryllium oxide BeO d. nickel(II) peroxide Ni2O e. ammonium chromate (NH4)2CrO4

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Name: ________________________

ID: A

____ 46. The molecular geometry of the CH3– ion is a. tetrahedral. b. square planar. c. square pyramidal. d. trigonal planar. e. trigonal pyramidal. ____ 47. What is the electron geometry (or electron arrangement) around an atom in a molecule or ion which

is surrounded by one lone pair of electrons and four single bonds. a. trigonal bipyramidal b. see-saw or distorted tetrahedron c. T-shaped d. linear e. trigonal planar ____ 48. What is the IUPAC name for the following compound?

a. b. c. d. e.

4-ethyl-3-methylheptane 2,3-diethylhexane 3-propyl-4-methylhexane 4,5-diethyldecane 4-ethyl-5-methylheptane

____ 49. Consider the following compounds:

CO

NH3

CO2

CH4

H2

How many of the compounds above exhibit London dispersion forces? a. 1 b. 2 c. 3 d. 4 e. 5 ____ 50. What is the best answer to the following expression?

(55.78 cm + 0.829 cm + 4.6666 cm – 52.4 cm) a. b. c. d. e.

9 cm 8.8756 cm 8.876 cm 8.88 cm 8.9 cm

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ID: A

1 Answer Section MULTIPLE CHOICE 1. ANS: KEY: 2. ANS: KEY: 3. ANS: KEY: 4. ANS: KEY: 5. ANS: TOP: MSC: 6. ANS: TOP: MSC: 7. ANS: TOP: MSC: 8. ANS: KEY: 9. ANS: TOP: MSC: 10. ANS: TOP: MSC: 11. ANS: TOP: MSC: 12. ANS: TOP: MSC: 13. ANS: TOP: MSC: 14. ANS: TOP: MSC: 15. ANS: TOP: MSC: 16. ANS: TOP: MSC:

A PTS: 1 DIF: easy TOP: general concepts | measurement factor label method | conversion factor MSC: general chemistry D PTS: 1 DIF: easy TOP: general concepts | measurement Celsius scale | Kelvin MSC: general chemistry D PTS: 1 DIF: moderate TOP: general concepts | measurement factor label method | dimensional analysis MSC: general chemistry A PTS: 1 DIF: easy TOP: general concepts | matter element MSC: general chemistry E PTS: 1 DIF: easy early atomic theory | chemical substance KEY: chemical formula general chemistry A PTS: 1 DIF: easy early atomic theory | atomic theory of matter KEY: nuclear structure | isotope general chemistry A PTS: 1 DIF: easy early atomic theory | atomic theory of matter KEY: nuclear structure | isotope general chemistry C PTS: 1 DIF: easy TOP: early atomic theory | periodic table nonmetal MSC: general chemistry A PTS: 1 DIF: easy early atomic theory | chemical substance KEY: chemical formula | ionic substance general chemistry D PTS: 1 DIF: easy early atomic theory | chemical equation KEY: balancing chemical equation general chemistry D PTS: 1 DIF: easy early atomic theory | chemical equation KEY: balancing chemical equation general chemistry A PTS: 1 DIF: easy chemical reactions | ions in aqueous solution KEY: electrolyte | strong electrolyte general chemistry A PTS: 1 DIF: easy stoichiometry | mass and moles of substance KEY: mole | mole calculations general chemistry A PTS: 1 DIF: moderate stoichiometry | mass and moles of substance KEY: mole | mole calculations general chemistry A PTS: 1 DIF: easy stoichiometry | mass and moles of substance KEY: mole | mole calculations general chemistry A PTS: 1 DIF: easy stoichiometry | mass and moles of substance KEY: mole | mole calculations general chemistry 1

ID: A 17. ANS: TOP: MSC: 18. ANS: OBJ: TOP: MSC: 19. ANS: OBJ: 3.10) KEY: 20. ANS: OBJ: TOP: MSC: 21. ANS: OBJ: TOP: MSC: 22. ANS: OBJ: TOP: KEY: 23. ANS: OBJ: TOP: MSC: 24. ANS: TOP: KEY: 25. ANS: TOP: KEY: 26. ANS: TOP: KEY: 27. ANS: TOP: KEY: 28. ANS: TOP: MSC: 29. ANS: KEY: 30. ANS: KEY: 31. ANS: KEY:

A PTS: 1 DIF: moderate stoichiometry | mass and moles of substance KEY: mole | mole calculations general chemistry C PTS: 1 DIF: easy REF: 3.3 Calculate the percentage composition of the elements in a compound. (Example 3.7) stoichiometry | determining chemical formulas KEY: mass percentage general chemistry A PTS: 1 DIF: moderate REF: 3.5 Determine the empirical formula of a binary compound from the masses of its elements. (Example TOP: stoichiometry | determining chemical formulas empirical formula MSC: general chemistry D PTS: 1 DIF: easy REF: 3.7 Relate the quantities of two reactants or two products. (Example 3.14) stoichiometry | stoichiometry calculation KEY: amounts of substances general chemistry C PTS: 1 DIF: moderate REF: 3.7 Relate the quantities of two reactants or two products. (Example 3.14) stoichiometry | stoichiometry calculation KEY: amounts of substances general chemistry D PTS: 1 DIF: difficult REF: 4.5 Assign oxidation numbers. (Example 4.7) chemical reactions | types of chemical reactions oxidation-reduction reaction | oxidation number MSC: general chemistry E PTS: 1 DIF: easy REF: 4.2 From the complete ionic equation, write the net ionic equation. chemical reactions | ions in aqueous solution KEY: ionic equation | net ionic equation general chemistry A PTS: 1 DIF: easy atomic theory | electronic structure of atoms electron configuration | aufbau principle MSC: general chemistry A PTS: 1 DIF: easy atomic theory | electronic structure of atoms electron configuration | aufbau principle MSC: general chemistry A PTS: 1 DIF: easy atomic theory | electronic structure of atoms electron configuration | aufbau principle MSC: general chemistry A PTS: 1 DIF: easy atomic theory | periodicity of the elements periodic properties | ionization energy MSC: general chemistry A PTS: 1 DIF: moderate atomic theory | periodicity of the elements KEY: periodic properties | atomic radius general chemistry B PTS: 1 DIF: easy TOP: bonding | ionic bonding Lewis electron-dot symbol MSC: general chemistry C PTS: 1 DIF: easy TOP: phases | gas gas pressure | pressure MSC: general chemistry B PTS: 1 DIF: moderate TOP: phases | gas empirical gas laws | combined gas law MSC: general chemistry

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ID: A 32. ANS: KEY: 33. ANS: KEY: 34. ANS: KEY: 35. ANS: KEY: 36. ANS: KEY: 37. ANS: KEY: 38. ANS: KEY: 39. ANS: TOP: KEY: 40. ANS: TOP: KEY: 41. ANS: OBJ: TOP: MSC: 42. ANS: OBJ: MSC: 43. ANS: KEY: 44. ANS: KEY: 45. ANS: TOP: KEY: 46. ANS: OBJ: TOP: KEY: MSC: 47. ANS: OBJ: 48. ANS: OBJ: TOP: MSC: 49. ANS: KEY:

C PTS: 1 DIF: moderate TOP: phases | gas ideal gas law | calculations with the ideal gas law MSC: general chemistry C PTS: 1 DIF: easy TOP: phases | liquid intermolecular forces | hydrogen bonding MSC: general chemistry A PTS: 1 DIF: easy TOP: phases | liquid intermolecular forces | dipole-dipole forces MSC: general chemistry D PTS: 1 DIF: moderate TOP: solutions | colligative properties expressing concentration | molarity MSC: general chemistry A PTS: 1 DIF: easy TOP: acids and bases | acid-base concepts Brønsted-Lowry concept of acids and bases MSC: general chemistry D PTS: 1 DIF: moderate TOP: acids and bases | acid-base concepts pH of a solution MSC: general chemistry C PTS: 1 DIF: moderate TOP: acids and bases | acid-base concepts pH of a solution MSC: general chemistry D PTS: 1 DIF: easy nuclear chemistry | radioactivity and nuclear bombardment reactions radioactive decay | alpha emission MSC: general chemistry A PTS: 1 DIF: moderate nuclear chemistry | radioactivity and nuclear bombardment reactions rate of radioactive decay | half-life MSC: general chemistry D PTS: 1 DIF: easy REF: 23.5 Write the structural formula of an alkane given the IUPAC name. (Example 23.5) alkane | nomenclature KEY: IUPAC nomenclature organic chemistry B PTS: 1 DIF: easy REF: 23.6 Define functional group. TOP: alkyne | structural characteristic organic chemistry A PTS: 1 DIF: easy TOP: general concepts | measurement significant figures | scientific notation MSC: general chemistry C PTS: 1 DIF: moderate TOP: general concepts | measurement si unit | mass MSC: general chemistry D PTS: 1 DIF: easy early atomic theory | chemical substance nomenclature of simple compound | ionic compound MSC: general chemistry E PTS: 1 DIF: easy REF: 10.1 Predict the molecular geometry (two, three, or four electron pairs). (Example 10.1) bonding | molecular geometry the valence-shell electron-pair repulsion model | tetrahedral arrangement general chemistry A PTS: 1 DIF: easy REF: 10.1 Electron Geometry-5 electron pairs TOP: bonding | molecular geometry A PTS: 1 DIF: moderate REF: 23.5 Write the IUPAC name of an alkane given the structural formula. (Example 23.4) alkane | nomenclature KEY: IUPAC nomenclature organic chemistry E PTS: 1 DIF: easy TOP: phases | liquid intermolecular forces | London forces MSC: general chemistry

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ID: A 50. ANS: OBJ: TOP: MSC:

E PTS: 1 DIF: easy REF: 1.5 Apply the rules of significant figures to reporting calculated values. general concepts | measurement KEY: significant figures general chemistry

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