chemistry final exam: practice problems name per. · 2014-06-13 · chemistry final exam: practice...

Chemistry Final Exam: Practice Problems Name __________________________ Per. __________

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1. Key Vocabulary/Terms: x atomic number x element x compound x kinetic theory x acid x base salt x vaporization x condensation x evaporation x boiling x sublimation x energy level x valence electron x metal x nonmetal x metalloid x Charles’ law x Boyle’s Law x Gay-Lussac’s law

x atm x torr x Combined Gas law x Ideal Gas Law x kPa x ion x ionic bond x covalent bond x Kelvin x Celsius x mole x Avogadro’s number x endothermic x exothermic x octet rule x solid x liquid x gas x molar mass

x empirical formula x balanced equation x heat x temperature x specific heat x heat capacity x Joule x Calorie x calorie x Conservation of mass x Conservation of energy x diffusion x effusion x isotope(s) x representative elements x transition elements (metals) x (Lewis) electron dot diagrams x catalyst

Problems/Concepts: Know (memorize) and be able to apply the following equivalents, relationships, formulas, etc.:

P1 × V1 = P2 × V2 (Boyle’s)

V V 1 2 --- = ---- (Charles’)

T1 T2

Moles = mass (g) / molar mass

P P 1 2 ----- = ----- (Gay-Lussac)

T1 T2

P x V P x V 1 1 2 2 ---------- = ----------- (Combined)

T1 T2

PV = nRT or… n = PV/RT (remember R = 8.31) (Ideal)

Ptotal = P1 + P2 + P3 + … (partial pressure)

4.184 J = 1 cal

1 J = 0.2390 cal

q (heat in joules or calories) C = --------------

m · ǻT

q = C · m · ǻT q = s · m · ǻT

moles of solute Molarity = -------------------------

liters of solvent

Moles of solute = Molarity (M) x Liters of solution

Dilution: M1V1 = M2V2 or N1V1 = N2V2

D = m/v 1. Find the following temperatures in Kevin: a. 0 °C = _______ b. 23 °C = _______ c. 100 °C = _______ d. -273°C = _______ 2. Find the following temperatures in °C: a. 0 K = _______ b. 100 K = _______ c. 373 K = _______ d. 273 K = ________ 3. Define STP in…

K and mmHg _______________________ K and kPa _______________________

K and atm _______________________ K and torr _______________________

°C and kPa _______________________ °C and mmHg _______________________

°C and torr _______________________ °C and atm _______________________

4. Which of the above is the SI unit for pressure? ________________________

5. How many atoms are in a mole of any element? ________________________

6. Which of the above have the same numerical value? ________________________

7. Fill in the blanks: 1 atm = _____ mmHg = ______ torr = ______ kPa

8. What kinds of atoms form covalent bonds? _________________________________________________

9. What kinds of atoms form ionic bonds? _________________________________________________


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10. Which of the following would form covalent (C), which would form ionic (I) bonds and which would not bond (N)?

a. Ca & Cl ______ b. S & O ______ c. Mg & Fe ______ d. C & H _____

11. What is meant by an atom’s the ground state and atoms that have ‘excited electrons?

_______________________________________________________________________________ 12. How can you identify atoms that have the same number of electrons in their highest occupied energy (valence )

levels? _______________________________________________________________________________

13. How can you identify atoms that have similar chemical properties?

_______________________________________________________________________________ 14. Where are the metals located in the periodic table? _____________________________________________

15. Where are the nonmetals located in the periodic table? _____________________________________________

16. Where are the metalloids located in the periodic table? _____________________________________________

Describe each of the following types of chemical reactions:

17. Combination/Synthesis: ________________________________________________________________________

18. Decomposition: ________________________________________________________________________

19. Single replacement: ________________________________________________________________________

20. Double replacement: ________________________________________________________________________

21. Combustion: ________________________________________________________________________

22. In any period of the periodic table, what kind of changes occur as you go from left to right?

a. ______________________________ (atomic radius)

b. ______________________________ (ionization energy)

c. ______________________________ (electronegativity)

d. ______________________________ (metallic character) 23. What happens to atomic size (radius) as you go down a column (group) and why?

________________ / _______________________________________________________________________

24. What happens to atomic size (radius) as you go across a period and why?

________________ / _______________________________________________________________________

25. Which of the following elements would have the greatest atomic radius?

a. P b. F c. Cl 26. Which of the following elements would have the greatest ionization energy?

a. P b. F c. Cl 27. What do all acids contain? ______________________________________________

28. What do all bases contain? ______________________________________________

29. What is a salt? ______________________________________________________________

30. Neutralization reaction result in what kinds of products? _______________ & _______________

31. What term is used when a substance like CO2 turns directly from a solid to a gas? ____________________

32. __________________________ A 47.7-g piece of copper increases from 25.0°C to 48.0°C when it absorbs 425 J

of heat. What is the specific heat of copper? (show your work) 33. Circle which units can be used to measure heat flow: Joules moles degrees calories(c) kilocalories (C) 34. What is the octet rule? ______________________________________________________________________

35. If a compound’s name ends with “-ate” or “-ite” it must contain ____________________.


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AB

C

DE

In a graph below … 36. Where is the substance only a solid? ___________

37. Where is the substance only a liquid? ___________

38. Where is the substance only a gas? ___________

39. Where is the substance turning from liquid to gas? ___________

40. Where is the substance solid to liquid? ___________

41. How do cations form and what type of element(s) form(s) them? _______________________________________

42. How do anions form and what type of element(s) form(s) them? _______________________________________

43. At STP what is the volume of 1 mole of any gas? _____________________

44. What is the relationship between the size of a gas molecule and diffusion and effusion? _________________

_______________________________________________________________________________________

45. At the same temperature and pressure, which gas will move fastest (and therefore diffuse or effuse faster)?

a. H2 b. O2 c. N2 d. Ar

0___1___2___4___5___6___7___8___9__10__11__12__13__14 46. On a pH scale like the one above…

a. … where would bases fall? __________ b. … where would neutral substances fall? __________ c. … where would bases fall? __________

47. If you decrease the volume of a container holding a gas without changing temperature of the gas what happens to its

pressure. ___________________________________________________

48. At what temperature will water boil when the external pressure is 115.5 mmHg? (Initial conditions are at STP)

_______________________________ 49. If you triple the temperature of a gas in a rigid inflexible container, what happens to its pressure?

___________________________________________________ 50. In terms of arrangement and movement of particles what is the difference between a solid, a liquid and a gas?

__________________________________________________________________________________________________

__________________________________________________________________________________________________

__________________________________________________________________________________________________ 51. In terms of volume and shape what is the difference between a solid, a liquid and a gas?

__________________________________________________________________________________________________

__________________________________________________________________________________________________

__________________________________________________________________________________________________ 52. The formation of aluminum oxide is expressed in the following reaction:

Balance the equation: ______ Al + ______ O2 Æ ______ Al2O3

How many moles of aluminum are needed to form 3.7 moles of Al2O3? ______________________


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53. Acetylene gas (C2H2) is produced by adding water to calcium carbide (CaC2). CaC2 + 2H2O Æ C2H2 + Ca(OH)2

54. How many grams of acetylene are produced by adding water to 5.00 g CaC2? ______________________

55. What is molar mass? __________________________________________________________________

56. What is and how do you calculate the molar mass of CuSO4? ______________________

_____________________________________________________________________________________________

57. How can molar mass of a compound be determined? ______________________________________________

_______________________________________________________________________________________ 58. What is the molar mass of C6H12O6 (glucose)? _______________________________ 59. What is the empirical formula for glucose in then above question? _______________________________ 60. Balance the following chemical equations:

a. ____ Mg (s) + ____ HCI (aq) Æ ____ MgCl2 (aq) + ____ H2 (g)

b. ____ Al + ____ H2SO

4 o ____ Al

2(SO

4)

3 + ____ H

2

c. ____ Fe + ____ O2 o ____ Fe2O3

61. How many moles are present in 34 g of Cu(OH)2? _________________________________

62. How many moles of hydrogen molecules (H2) are there in 2.45 x 1023 molecules of CH4? ___________

63. How many moles of aluminum are needed to react completely with 1.2 mol of FeO below? __________ (Show your work) 2Al + 3FeO Æ 3Fe + Al2 O3

64. How much heat is required to raise the temperature of 68.0 g of iron from 30.0 °C to 55.0 °C? (Show your work) (Specific heat of iron = 0.44 J/g °C)

65. Given the reaction at STP: 2KClO3 (s) Æ 2KCl (s) + 3O2 (g)

What is the total number of liters of O2 (g) produced from the complete decomposition of 0.500 mole of KClO3(s)? (Show your work)


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Given the reaction: 2Al2O3 Æ 4Al + 3O2

66. What is the total volume of oxygen released when 1.00 mole of Al2O3 decomposes? (Show your work)

67. What is the electron configuration for a phosphorus atom? ______________________________

68. What is the correct e- configuration for an argon atom? ______________________________

69. How many covalent bonds formed in the compound CO2? ______________________________

70. A gas has a volume of 50 L at a temperature of 200 °C. What will the new volume of the gas be if the temperature is reduced to 100 °C? ______________________________

71. Draw Lewis Dot Structure for the following atoms:

a. Ca b. Xe c. Ga d. Al

72. How many milliliters of 0.50 M HCI are needed to exactly neutralize 20 milliliters of 1.0 M KOH?

73. How many moles of a gas will a 1000 ml flask hold at 65.0 °C and a pressure of 56 kPa?

74. What is the correct formula for the following acids? a. sulfuric acid _______ b. nitric acid ______

75. Given the reaction: 4Al + 3O2 Æ 2Al2O3 How many moles of aluminum are needed to form 3.7 mol Al2O3? (Show your work) 76. The energy absorbed when a substance dissolves in water and the surroundings cool down may be expressed as?

a. Degrees b. Kilocalories c. Moles d. Grams per mole 77. If 148 grams of calcium hydroxide [Ca(OH)2] are used to prepare a 4.00 M solution, what volume in mL of solution

can be made? ______________________


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The reaction of fluorine with ammonia produces dinitrogen tetrafluoride and hydrogen fluoride.

5F2 (g) + 2NH3 (g) ĺ N2F4 (g) + 6HF(g)

78. If you have 66.6 g NH3, how many grams of F2 are required for complete reaction? (Show your work)

79. A solution with a pH between 7 and 14 would be a(n) _______________.

80. A solution with a pH between 0 and 7 would be a(n) _______________.

81. A solution with a pH of exactly 7.0 would be _______________.

82. What is the molarity of a 500 ml solution that contains 150.0 grams of NaCl?

83. A 2.4 g sample of a metal requires 6 J of energy to change its temperature from 18 °C to 30 °C. What is the specific heat of the sample?

84. Define a base: __________________________________________________________________________________

85. Define an acid: __________________________________________________________________________________

86. Define a salt: __________________________________________________________________________________

87. What are the names for the following groups?

IA _______________ IIA _______________ 1B - 7B _______________

VIIA _______________ VIIIA _______________

88. What is the pH of a solution with a hydrogen ion concentration of 0.1 moles per liter? _________________

89. What is the pH of a solution with a hydrogen ion concentration of 0.05 moles per liter? _________________

---

90. ______________ Given the structural formula for ethyne: H–C C–H, What is the total number of electrons shared between the two carbon atoms?

91. List at least 5 properties of acids and 5 properties of bases.

Acid Base

a. ________________________________________ _________________________________________

b. ________________________________________ _________________________________________

c. ________________________________________ _________________________________________

d. ________________________________________ _________________________________________

e. ________________________________________ _________________________________________

92. Make a sketch below of the following orbitals (see chapter 5.1)

s p d 93. Aluminum and hydrochloric acid are mixed resulting in the formation of aluminum chloride and hydrogen gas.

Write the balanced equation for this reaction below:


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At STP, what is the total number of liters of hydrogen gas produced when 6.00 moles of hydrochloric acid solution is completely consumed?

94. The temperature of a piece of lead with a mass of 110 g changes from 28.0°C to 48.0°C when the metal absorbs

283J of heat. What is the specific heat of the lead? 95. How many milliliters of 2 M HCI are needed to exactly neutralize 40 milliliters of 6 M Ca(OH)2?

96. What is the pOH of a solution if the [H+] = 1 x 10-6 moles /L?

97. Hydrogen peroxide (H2O2) decomposes into water and oxygen gas. Write a balanced equation of this reaction

below:

If 3.0 moles of hydrogen peroxide decomposes, what volume of oxygen gas is produced? 98. Balance the following equation: ___ C2H6 (g) + ____ O2 (g) Æ ___ CO2 (g) + ___ H2O (g)

How many grams of O2 (g) are needed to react completely with 2 moles of C2H6 (g)? 99. What are the principle contributions of each of the following scientists to the creation of the modern model of the

atom? (You may use pictures in as well as words in your answer.)

JJ Thomson Ernest Rutherford Niels Bohr Modern Quantum (wave) Model

chemistry final exam: practice problems name per. · 2014-06-13 · chemistry final exam: practice...

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