Chemistry-2 Final Exam Objectives

Format of the Final: 90 minutes, 100 multiple choice questions – equations will not be given. NO CHEAT SHEATS!Ch Topics Practice Prob.

Lab Know lab equipment and what it is used for

2 Be able to tell the difference between chemical and physical changes and properties

(definition, examples)

Be able to tell the difference between solids, liquids and gases (properties, diagrams)

Be able to identify heterogeneous and homogeneous mixtures

Be able to identify elements, compounds and mixtures

Pg.51 (18-19)

Pg. 58 (45, 47, 49,

69)

3 Know the metric prefixes – sizes and metric units (mass, temp, energy etc.)

Understand scientific notation and relative sizes

Understand the law of conservation of matter (mass)

Be able to calculate density and understand the concept of a constant density value

Be able to convert metric units

Be able to calculate percent error

Pg. 84 (32, 33)

Pg. 91 (46, 47)

4 Know the subatomic particles (relative sizes and charges, location)

Be able to write atomic symbols and determine number of p, n, e, mass number, atomic

number, or charge in atoms and ions

Know how to differentiate between isotopes

Pg. 112 (17-18)

Pg. 117 (23-24)

Pg. 122 (41, 49)

5 Be able to write electron configurations of atoms and ions Pg. 135 (8)

Pg. 167 (8-9)

6 Know the trends on the periodic table (type ion, ion size, electronegativity, metal/NM)

Know the organization of periods and families (names and locations) on Periodic Table

Know how Mendeleev organized the periodic table and the periodic law

Know properties of metals and nonmetals and their location of the Periodic Table

Pg. 181 (28, 36,

39, 43)

7 Be able to write electron configurations of ions

Be able to determine the number of valence electrons using the Periodic Table

Be able to identify formulas as ionic or metallic and know their properties

Be able to identify how ionic bonds form

Pg. 207 (31, 41,

63, 67, 79)

8 Be able to draw lewis dot structures (lone pairs/bonding pairs)

De able to identify how covalent bonds form

Be able to identify types of intermolecular forces and bond types and affect on properties

Know how strength of attraction affects properties (melting, boiling etc.)

Pg. 220 (8)

Pg. 239 (30)

Pg. 247 (40, 43,

54, 61)

9 Be able to determine if elements will form ionic or covalent compounds

Be able to write names/formulas of ionic compounds (transition metal,8 polyatomic ions)

Know charges of ions by family location

Be able to write names/formulas of molecular compounds (prefixes)

Pg. 265 (13)

Pg. 281 (43, 57,

61, 65, 67, 69)

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10 Be able to calculate mole conversions (gmolL, at/molecmolg, atmolL), molar

mass, atoms or ions in a compound

Be able to calculate percent composition (by mass)

Be able to determine molecular formulas from empirical formulas

Pg. 292-312 (5-8,

16-21, 34-39)

Pg. 315 (49, 53,

59, 63, 75)

317 (84)

11 Be able to balance equations

Be able to identify reactants and products in a chemical equation

Be able to determine types of reactions

Be able to predict products for single and double replacement reactions

Pg. 327-8 (3, 5)

Pg. 347 (43, 52)

Ch Topics Practice Prob.

12 Stoichiometry

Be able to calculate amount of one substance in a reaction from another (g, mol, L)

Pg. 361-6 (13-20)

Pg. 379 (41, 45, 49)

13 Know the phase changes and related energy changes

Know kinetic theory for gases

Understand how a barometer works

Be able to convert pressure units (atm, kPa, mmHg, torr)

How are temperature and kinetic energy related

Interpret a phase diagram and heating curve.

Pg. 387 (1-2)

Pg. 407 (29, 41, 43,

59)

Pg 386

14 How does temperature affect volume or pressure of gases

Calculate with Ideal Gas Law, Charles Law, Boyles Law, Gay-Lussac’s Law

Know what the graphs of the laws look like

Know how the number of particles, volume and temperature affect pressure of a gas

Pg. 419-27 (7-14,

23-24)

Pg. 439 (47, 51, 55,

57, 61)

15 Be able to determine which compounds will dissolve (like dissolves like)

Be able to identify solutes and solvents in a solution

Be able to identify which solutions conduct electricity and why

Pg. 465 (33, 36)

16 Be able to calculate molarity (mol, mL, M)

Know what factors affect the rate of solution and why

Know how to read a solubility curve and identify saturated, unsaturated and

supersaturated solutions

Explain the effect of temperature on solubility of gases and solids

Pg. 481-2 (8-11)

Pg. 492 (29-30)

Pg 473 (vocab)

Pg 474 (graph)

17 Know endothermic/exothermic phase changes

Understand the concept of calorimetry and energy transfer

Be able to interpret how specific heat affects changes in temperature

Be able to read a heating/cooling curve (phase changes, phases present) - page 523

Pg. 536 (62)

18 Be able to read a potential energy diagram (activation energy, catalyst, forward/reverse,

heat reaction)

Pg. 547 (2)

Pg. 581 (45, 79)

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Know what factors affect the rate of a reaction (how/collision theory)

19 Know the properties and definitions of acids and bases

Be able to identify formulas of acids and bases

Be able to write neutralization reactions

Know why water is neutral

Be able to describe the relationship between concentration of H+ and OH-

Be able to calculate pH/pOH/concentration H+ /concentration OH-

Pg. 599-601 (11-16)

Pg. 625 (45, 55, 57,

63, 81)

Equations you will need to knowPercent error = exp-act x 100 D = M mass number = #p+ + #n0

act V charge = #p - #eMM = mass 6.02 x 1023 22.4 L % = part x 100 mole mole mole total

Mole ratio = mole wanted Percent Yield = actual x 100 PV = nRT P1V1 = P2V2 P1 = P2

mole given theroetical T1 T2

V1 = V2 P1V1 = P2V2 Molarity = moles of soluteT1 T2 T1 T2 Liters of solution

q = mCΔT pH + pOH = 14 pH = -log(H3O+)

MatterObjective 1: Students will be able to define matter, differentiate between its different states, and understand how it remains constant within a system.101. I can define what matter is.102. I can differentiate between a solid, liquid, and gas.103. I can explain that matter cannot be created or destroyed in a chemical reaction or physical change.104. I can classify matter as an element, compound, or mixture.

Objective 2: Students will be able to identify physical and chemical properties. 201. I can explain what physical and chemical properties are, and list examples.202. I can describe how density relates to mass and volume for matter.203. I can calculate density given the mass and volume, or calculate relationships between density, mass and volume.204. I can differentiate between mass and density.

Objective 3: Students will be able to differentiate between physical and chemical changes 301. I can explain what happens to matter during a physical or chemical change.

Nomenclature Objective 4: Students will be able to name and write formulas for compounds.401. I can use naming rules to name or write the formula for ionic compounds.402. I can use naming rules to name or write the formula for molecular compounds.

ReactionsObjective 6: Students will be able to identify types of reactions.

601. I can identify reactants and products in a chemical reaction.602. I can identify a given chemical reaction as single replacement (displacement), double replacement

(displacement/metathesis), decomposition, synthesis (combination/formation) and combustion.603. I can predict products of reactions: single-replacement, double-replacement, and combustion.

Objective 7: Students will be able to apply the Law of Conservation of Matter to balance equations.701. I can balance equations.

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Objective 8: Students will be able to describe how various factors affect the rate of a reaction.801. I can determine if the rate of reaction will increase or decrease with changes in temperature, concentration, surface area

and addition of a catalyst.

Moles and StoichiometryObjective 9: Students will be able to use the mole concept to quantify matter. 901. I can apply the mole concept to convert between volume, mass, and particles.902. I can define the mole in terms of 6.02 x 1023 (Avogadro’s number) particles903. I can calculate molar mass.

Objective 10: Students will calculate percent composition of an element in a compound.1001. I can calculate the percent composition given the masses of elements in a compound.

Objective 11: Students will be able to use stoichiometry to interpret quantities in reactions.1101. I can predict the quantity of product (mass, volume, particles and moles) from given reactants or vice versa.

Acids and BasesObjective 12: Students will be able to identify and define acids and bases.1201. I can identify a compound as an acid or a base based on formula.1202. I can describe physical properties of acids and bases.

(Operational definition- sour, bitter, slippery, litmus paper change)1203. I can identify an acid as producing hydrogen ions in solution and a base as producing hydroxide ions in solution.

Objective 13: Students will be able to relate hydrogen ion concentration to the hydroxide ion concentration and the pH scale. 1301. I can show that there is an inverse relationship between [H+] and [OH-] 1302. I can qualitatively describe the relationship between pH and hydrogen ion concentration.1303. I can correctly interpret whether a solution is acidic, basic or neutral depending upon the pH value.

Objective 14: Students will be able to explain acid-base neutralization reactions.1401. I can predict the products of an acid-base neutralization reaction.

MeasurementObjective 15: Students will be able to gather, interpret and analyze data to draw conclusions.1501. I can recognize the uncertainty of measurements.1502. I can choose and use appropriate lab equipment to measure properly.1503. I can choose appropriate metric units and convert between them.1504. I can use scientific notation and interpret the meaning of the power of ten. (For example, knowing that 10 -6 is smaller than 10-2)

SolutionsObjective 16: Students will be able to recognize and describe the characteristics and formation of solutions.1601. I can differentiate between solute & solvent.1602. I can explain why a compound, when dissolved in water, will or will not conduct electricity. 1603. I can determine if a given solution is unsaturated, saturated, or supersaturated using a solubility curve.1604. I can determine if a given solute will be soluble in a given solvent (like dissolves like). 1605. I can predict how factors (such as stirring, temperature, surface area) affect the dissolution rate.

Objective 17: Students will be able to quantitatively describe characteristics and formation of a solution.1701. I can calculate the molarity of a solution given moles and liters.

ATOMIC STRUCTUREObjective 18: Students will be able to describe the basic structure of the atom.1801. I can identify the location, charge, and relative mass of each subatomic particle (electron, neutron, proton).

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1802. I can identify the element based on the number of protons.

Objective 19: Students will be able to differentiate between ions and neutral atoms.1901. I can explain how ions are formed and predict their charge.1902. I can explain how the number of protons and electrons relates to the charge of the atom or ion.

Objective 20: Students will be able to describe isotopes.2001. I can explain how the number of protons and neutrons relates to the mass number.2002. I can define isotope by explaining that atoms of an element can contain different numbers of neutrons.

BondingObjective 21: Students will be able to describe characteristics of an ionic compound and how an ionic bond forms at an atomic level. 2101. I can identify a compound as ionic from the types of elements in the compound. 2102. I can apply octet rule and rules of electrostatic attraction to explain ionic bond formation. 2103. I can describe the general characteristics of an ionic compound (solubility, melting point, alternating ions create a simple crystalline structure, electrical conductivity).

Objective 22: Students will be able to describe characteristics of a molecular compound and howa covalent bond forms at an atomic level.2201. I can identify a compound as covalently bonded by the types of elements in the compound.2202. I can describe how a covalent bond forms at an atomic level. (sharing electrons, multiple bonds, octet rule)2203. I can describe the general characteristics of a molecular compound (melting and boiling points as they relate to intermolecular forces)2204. I can draw electron dot diagram (Lewis dot diagrams).

Periodic TableObjective 23: Students should be able to explain the organization of the periodic table and how that relates to physical and

chemical properties. 2301. I can differentiate between groups and periods on the periodic table and what is common about elements within a group.2302. I can locate metals, non-metals and metalloids on the periodic table.2303. I can list properties of metals, non metals and metalloids.2304. I can identify and recall the key properties of the Noble Gases.2305. I can determine the charge of a main block (representative) ion.2306. I can determine the number of valence electrons for a main block (representative) element.

Gas LawsObjective 24: Students will be able to apply the kinetic molecular theory to describe the motion of atoms and molecules and explain the properties of gases.2401. I can explain how the interaction between gas molecules and the sides of a closed container creates gas pressure.2402. I can relate the Kelvin temperature to molecular motion.2403. I can explain how when one condition (P, T, V, n) changes in a gas, the others change in response.

Objective 25: Students will be able to solve problems using the gas laws to explain the relationships between pressure, temperature, and volume of any amount of an ideal gas or mixtures of gases.2501. I can use the values of STP to solve gas law problems.2502. I can interpret graphical data that illustrate the relationship between P, T, V, and n.2503. Given a set of conditions, I can use the most appropriate mathematical equation to calculate a change in P, T, V, or n.

EnergyObjective 26: Students will be able to distinguish between temperature and heat..2601. I can differentiate between units of temperature (Celsius and Kelvin) and units of energy. (Joules and calories).2602. I can use specific heat capacity to explain changes in temperature of a substance.

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Objective 27: Students will be able to recognize that in all processes, energy will be conserved. (Law of Conservation of Energy)2701. I can explain that energy transfers conserve energy.

Objective 28: Students will be able to describe energy transfer in a physical change. 2801. I can identify that energy changes occur during phase changes.

Objective 29: Students will be able to describe energy transfer in a reaction.2901. I can differentiate between an endothermic and exothermic reaction given heat as a reactant or a product.

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Chemistry 1-2 FINAL EXAM REVIEWMatter

1. What are the properties of matter?

2. Which state of matter does each of the following diagrams represent?

3. According to the law of conservation of mass, when is mass conserved?

4. How can you differentiate an element from a compound?

5. What is the main difference between chemical changes and physical changes?

6. What is the density of a solid with a mass of 34.00g and a volume of 76.2 cm3?

7. Describe a homogenous mixture and give an example.

8. Describe a heterogeneous mixture and give an example.

Nomenclature

9. What is the proper name of Fe2SO4?

10. What is the proper name for AlCl3 ?

11. What is the proper name for the following molecular substances: N2O5, P5O10, CO, CO2

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12. Which of the following pairs has an error?

a. Sodium chloride, NaCl

b. Hydrofluoric acid, HF

c. Iron (II) carbonate, FeCO3

d. Calcium hydroxide, CaOH2

13. What is the proper formula for diphosphorous pentoxide?

14. What is the proper chemical formula for calcium nitrite?

Reactions

15. What is the meaning for each of the symbols that are used in equation writing: , +, (s), (l), (aq), (g)?

16. Write generic formulas for the following reactions: single replacement, double replacement , synthesis, decomposition, and combustion.

17. Write a balanced combustion reaction between methane and oxygen gas.

18. Balance and identify the following equation:_____ C3H8 + _____O2 _____CO2 + _____H2O

19. Balance and identify the following equation: _____Al2(SO4)3 + _____Ca(OH)2 → _____Al(OH)3 + _____CaSO4

20. Identify the reactants and products from #23.

21. Predict the products of this double replacement reaction?

AgNO3(aq) + NaCl(aq) → _________ + _________

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22. Why does a reaction happen faster if the concentration of the reactants is increased?

23. How can the rate of a chemical reaction be increased?

Moles and Stoichiometry

24. How many molecules are in 1 mole of methane gas, CH4?

25. What is the molar mass for Ca3(PO4)2?

26. What is the volume of 175g of oxygen, O2?

27. What is the mass of 2.33 x 1023 atoms of sulfur?

28. If you have 22.4 L of a gas, how many molecules do you have?

29. How many grams is the equivalent of 3.5L of carbon dioxide gas?

30. What is the volume, at STP, of 200.grams of H2S gas?

31. What is the mass in grams of 2.00 x 1024 atoms of neon?

32. What is the percent by mass of sodium in sodium acetate (NaC2H3O2)? Hint: Figure out the molar mass first!

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33. Find the molecular formula of ethylene glycol (antifreeze), which has a molar mass of 62.0g/mol and has an empirical formula of CH3O.

34. How many moles of ethane, C2H6, are needed to react with 13.0g of oxygen gas, O2? The chemical equation is 2C2H6 + 7O2 6H2O + 4CO2

35. Write the chemical equation for the following word equation and then use stoichiometry to solve the problem. Hydrogen and Oxygen gas combine to create water. If 5.3moles of hydrogen gas is used, how much water can be created? (Assume that there is an adequate supply of oxygen to complete the reaction.)

36. If 4.25 g of nitrogen, N2, react with Lithium, Li, according to the reaction shown in this equation, 6Li + N2 2Li3N, what would be the steps you would do to determine the mass of lithium nitride, Li3N, produced? Complete the steps and solve the problem.

Acids and Bases

37. Define and list the properties of bases.

38. Define and list the properties of acids.

39. On the pH scale: What is considered acidic? basic? neutral?

40. How can you differentiate between an acid and a base by only looking at the chemical formula?

41. Why does water have a neutral pH?

42. If the concentration of H+ ions is 1.0 x 10-5M, what is the pH of the solution?

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43. What is the relationship between pH and H+ concentration?

44. What is the relationship between H+ ion concentration and OH- concentration in an aqueous solution?

45. What are the products of this neutralization reaction? Ca(OH)2 + H2CO3 _________ + _________

Measurement

46. What do the following tools measure: barometer, balance, thermometer, graduated cylinder?

47. What would be the units of the tools mentioned in question #1?

48. Know your metric units and their values as they relate to other metric units (ex. 1kg = 1000g). Answer the following: ____cg= 6 g 5mL = ____cm3 3 L = _____mL 5mg = _____g

49. Put the following numbers in order from smallest to largest:a. 5.3 x 10-5

b. 5.3 x 105

c. 5.3 x 102

d. 5.3 x 10-2

50. If your experimental value is measured to be 6.45 g and the accepted (theoretical) value is 8.54 g, what is the percent error?

51. Which unit is the smallest: nanograms, centigrams, dekagrams, or kilograms?

Solutions

52. Give an example of a solution. Name the solute and the solvent for the solution.

53. Define solubility.

54. What are the factors that affect solubility?

55. How is solubility different from the rate of dissolving?

56. How can one increase the rate of dissolving?

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57. Define the term electrolyte and tell what types of compounds act as electrolytes.

58. How can you tell if a solution is saturated?

59. What is the molarity of 4.2 moles of HCl dissolved in 8.2 L of solution?

60. What is the molarity of a methanol solution that contains 25 g of methanol in 3.5 L of a solution? The molar mass of methanol is 32 g/mol.

61. How much glucose (molar mass = 180.0 g/mol) must be added to 800.0g of water in order to make a 0.300M solution?

62. Label the points A,B & C on the graph above as unsaturated, saturated, or supersaturated.

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ATOMIC STRUCTURE

63. What are the charges, relative masses, and locations of each of the subatomic particles in an atom?

64. What is an ion?

65. Which elements form ions with a charge of -2?

66. What distinguishes the atoms of one element from the atoms of another?

67. How do isotopes of a given element differ from one another?

68. What is the difference between the mass number and the atomic number of an atom?

69. What is the average atomic mass of an element?

70. In a sample of an element, 23.4% of the atoms have a mass of 11.0030amu and 76.6% of the atoms have a mass of 5.342 amu, what is the average atomic mass?

71. Why is an atom electrically neutral?

72. How many neutrons are present in

Bonding

73. What kinds of elements combine to form ionic compounds?

74. What kinds of elements combine to form molecular compounds?

75. What are the properties of ionic compounds?

76. What are the properties of molecular compounds?

77. How are cations formed?

78. How are anions formed?

79. How are intermolecular forces related to the melting point and boiling point of a compound?

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80. Draw the Lewis dot structure for SiS2.

81. What is the electron configuration of neutral Lithium?

82. What is the electron configuration of a chlorine ion?

83. If one element has the electron configuration of 2s22p3 and another element has two more protons than the first element, what would the electron configuration of the second element be?

84. Write the electron configuration of a fluoride ion.

85. What is the shape of a water molecule? Draw the Lewis Dot diagram of water.

Periodic Table

86. Where are the following found on the periodic table? alkali metals, alkaline earth metals, halogens, transition elements, noble gases, inner transition elements

87. How are elements arranged on the modern periodic table?

88. Name two elements that are in the same period as Carbon.

89. Name two elements that are in the same group as Carbon.

90. What are the properties of metals, nonmetals, and metalloids?

91. How do you determine the number of valence electrons in an element?

Gas Laws

92. What does a barometer measure?

93. On a graph of any pressure—volume readings on a contained gas at constant temperature, what would the line would look like?

94. Convert 2.45 atm to mmHg.

95. What happens to the average kinetic energy of molecules when a sample of gas is heated?

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96. How could you double the pressure on a contained gas at constant temperature?

97. The volume and amount of gas are constant in a tire. The initial pressure and temperature are 1.82 atm and 293 K. At what temperature will the gas in the tire have a pressure of 2.35 atm?

98. A sample of 0.34 moles of helium gas has a pressure of 2.4 atm at 30.0oC. What volume does this gas occupy? R = 0.0821 L · atm/K · mol

99. How many grams of oxygen gas have a pressure of 105.0kPa and occupy a volume of 2.0L at 50.0oC? R = 8.31 L x kPa/K x mol

Energy

100. Consider the following phase changes: vaporization, melting, freezing, sublimation, deposition, condensation. Make a list of the phase changes that are endothermic and those that are exothermic.

101. Why is it important for the bottom of a frying pan to have a low specific heat and the handle have a high specific heat?

102. Draw an endothermic potential energy graph and label the activation energy and the heat of reaction.

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103. Place an X on the above heating curve to mark where the melting point is found.

104. Place an O on the above heating curve to mark where the substance would begin to boil.

105. Which letters on the above heating curve represent phase changes?

106. Which letters on the above heating curve represent an increase in kinetic energy?

107. What letter on the above heating curve represents where solid and liquid exist at the same time?

Use the potential energy diagram for the next 4 questions.

108. Place an X on the diagram above to show where the activated complex would be located.109. Use the diagram above to calculate the Δ H of the reaction.

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110. What is the activation energy of the FORWARD CATALYZED reaction?

111. What is the activation energy of the REVERSE UNCATALYZED reaction?

112. Label the components of the phase diagram below.

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III

III

IV

V

VI

VII

VIII