Read Microsoft Word - Fall Final Review NMUSD Worksheet I, II, III.DOC text version

Final Exam Worksheet I

Editted and Combined from Several Previous Documents. Read all the way to the end. Pay attention to the questions that are not crossed out. This document contains stuff from about 4 review documents. Pay attention to the concepts more than the math...the math counts, but the concepts count more. Some of the questions may be duplicates. If you have any questions about an answer, send me an email at [email protected] Final exam will cover chapters 2-7, 10, 12-14 and possibly 15-17.

1. 2. Titanium, which has the symbol Ti, is as a member of which of the following groups a. nonmetal b. transition metal c. metalloid d. inner transition metal e. noble gas Select the single best answer that completes this sentence. The nucleus of an atom may contain a. proton(s). b. proton (s) and neutron(s). c. neutron(s). d. electron(s). e. proton(s) and electron(s). An atom of Chlorine-36 contains a. 17 protons, 17 neutrons & 19 electrons b. 19 protons, 17 neutrons & 19 electrons c. 36 protons, 17 neutrons & 17 electrons d. 19 protons, 19 neutrons & 17 electrons e. 17 protons, 19 neutrons & 17 electrons Which term most correctly refers to the number of protons in an atom? a. mass number b. atomic mass c. atomic number d. isotope number e. none of the above Determine the density of a material with a mass of 58.216 grams and a volume of 29.2 milliters. Determine if this material will sink or float in a beaker of water. Determine the volume of an object with a density of 0.983 g/cm3 and a mass of 15.02 grams. Determine the mass of an object with a density of 1.26 g/ml and a volume of 35.4 ml. Food coloring is added to water and the mixture is stirred in a beaker. Select the term that best describes the mixture: a. solution. b. heterogneous material. c. pure substance. d. element. e. The question does not supply enough information. Find the ion in the following list that is not likely to form: a. Na+ b. S2c. I2d. Ca2+ e. Al3+ Complete the sentence: A liquid has a. definite volume and definite shape. b. indefinite volume and indefinite shape. c. indefinite volume and definite shape. d. definite volume and indefinite shape. Select the statement that is true. a. Metals tend to lose electrons to form negatively charged ions called cations. b. Metals tend to gain electrons to form negatively charged ions called cations. c. Metals tend to lose electrons to form negatively charged ions called anions. d. Metals tend to lose electrons to form positively charged ions called cations. e. Metals tend to lose electrons to form positively charged ions called anions. Which of the following statements is incorrect? a. The nucleus of an atom is negatively charged and contains all the mass of the atom. b The protons travel outside the nucleus in orbits like planets around the sun. c. Protons and neutrons attract each other because they have opposite charges. d. Electrons behave as waves because they are positively charged. e. More than one statement is incorrect. ab. None of the statements are incorrect. (Mark both a & b if you select this answer). A student measures the volume of water in a beaker three times and records the following measurements: 32.41 ml, 35.16 ml and 33.95 ml. Using other techniques the student determines that the true volume of the water is 31.04 ml. Select the letter of the statement that most completely describes this situation. a. The student's measurements were accurate, but not precise. b. The student's measurements were precise, but not accurate. c. The student's measurements were both accurate and precise. d. The student's measurements were neither accurate nor precise. e. The sentences provide insufficent information to answer this question. Determine the number of significant figures in 754.3 millimeters a. 1 b. 2 c. 3 d. 4 e. 5 Determine the number of significant figures in 0.023 grams a. 1 b. 2 c. 3 d. 4 e. 5 Helium is in the ____________ (family/group)on the periodic table.

a.

alkali metals

b.

alkaline earth metals

c.

halogens

d.

noble gases

3.

4. 5. 6. 7. 8. 9. 10. 11. 12.

13.

14.

18. Convert to exponential notation: 25032.56 19. Convert to exponential notation: 0.09862 20. Convert to exponential notation: 1.02 21. For 88Sr2+Determine the number of protons. For 88Sr2+Determine the number of neutrons. 22. 23. For 88Sr2+Determine the number of electrons. Classify the following as element, molecule, ion and/or compound. 24. hydroxide 25. H2 26. LiCl 27. N2O5 Write the formula of the ion formed by each of the following: 28. Sr 29. K 30. Al 31. N 32. P 33. O 34. I 35. Se 36. S 37. Locate the alkali metals, alkine earth metals, transition metals, inner transition metals, halogens and noble gases. 38. Which of the following best describes the contribution of the proton to an atom? a. mass b. mass and charge c. mass, charge and reactivity d. mass, charge and identity e. charge 39. Salad oil is added to vinegar and the mixture is shaken. Select the term that best describes the mixture: a. solution. b. heterogneous material. c. pure substance. d. element. e. compound. 40-47. Convert units as indicated: 40. 89.34 meters to kilometers 41. 56.1 millileters to liters 42. 16.2 kilograms to grams 43. 14.2 ml to cm3 44. 6.4 kg to ng 45. 21.2 pm to Mm 46. 13.1 hrs to seconds 47. 10 years to seconds 48-49. Convert to regular notation: 48. 4.0236 x 104 49. 23.6 x 10-6 50-52. Determine the number of significant figures in the following 50. 6.89 meters 51. .003250 mg 52. 25010. mL Perform the following calculations following sig fig rules: 53. 2.3 grams/ 4.50 mL 54. 204.3 + 19.57 + 3.0089

15. 16. 17.

© Russell Cramm 2001

© Russell Cramm 2001

Answers: 1. b 2. b. 3. e. 4. c. 5. 1.99 g/mL 6. sink 7. 15.3 mL 8. 44.6 g 9. a. 10. c. 11. d. 12. d. 13. e., (a-d incorrect) 14. d. 15. d. 16. b. 17. d. 18. 2.503256 x 104 19. 9.862 x 10-2 20. 1.02 x 100 21. 38 22. 50 23. 36 24. ion 25. molecule & element 26. molecule & compound 27. molecule & compound 28. Sr2+ 29. K+ 30. Al3+ 31. N332. P333. O234. I35. Se236. S237. See attached. 38. d. 39. b. 40. .08934 km 41. .0561 L 42. 16,200 g 43. 14.2 cm3 44. 6,400,000,000,000 ng or 6.4 x 1012 ng 45. 2.12 x 10-17 Mm 46. 47160 seconds 47. 3.15 x 108 seonds 48. 40236 49. .0000236 50. 3 51. 4 52. 5 53. .51 g/mL 54. 226.9

(A) 2. (A) 3. (A) 4. (A) 5. (A) 6.

FeSO4 (B)

Fe(SO4)2

(C)

Fe2SO4 (D)

Fe2(SO4)3

(E)

Fe3(SO4)2

The one correct formula among these is Na2OH (B) Cu(SO4)2 (C) ZnCl2 (D) Zn(NO3)3 (E) BaNO3

What is the formula for aluminum sulfate? AlSO4 (B) Al2SO4 (C) Al3SO4 (D) Al3(SO4)2 (E) Al2(SO4)3

In which pair of anions do both names end in `­ate'? (C) ClO3­, NO3­ Cl­, ClO3­ (B) NO2­, NO3­

(D)

HS­, HSO4­

The number of atoms of oxygen indicated by the formula Ca3(PO4)2 is 12 (B) 8 (C) 7 (D) 4 (E) 3 Cu + 4HNO3 Cu(NO3)2 + 2H2O + ? would be completed and balanced by using (A) NO2 (B) 2NO2 (C) 3NO2 (D) 4NO2 When the equation ? Sb + ? Cl2 ? SbCl3 is correctly balanced, the sum of the coefficients is (A) 2 (B) 3 (C) 6 (D) 7 The equation

(E)

2NO

7.

(E)

9

8.

Which expression is correctly balanced? (A) Na2O2 + 2H2O 2NaOH + O2 (B) 2Na2O2 + 2H2O 4NaOH + 2O2 (C) 4Na2O2 + 3H2O 4NaOH + 2O2 (D) 2Na2O2 + 2H2O 4NaOH + O2 (E) 3Na2O2 + 2H2O 6NaOH + O2 Which set of coefficients balances this equation? ? CH4(g) ? C3H8(g) + ? H2(g) (A) 3, 1, 1 (B) 3, 2, 1 (C) 3, 1, 2 (D) 6, 2, 2 (E) What is the coefficient of P when the expression is balanced? ? H2SO4 + ? P ? H3PO4 + ? H2O + ? SO2 (A) 1 (B) 2 (C) 4 (D) 5 Upon analysis a compound is found to contain 22.8% sodium, 21.8% boron, and 55.4% oxygen. Its simplest formula is Atomic Molar Masses 11 g·mol­1 B 23 g·mol­1 Na O 16 g·mol­1 Na2B4O7 (B) Na3B4O (C) NaBO (D) Na3BO4 (E) NaB2O5

9.

6, 2, 6

10.

11.

(A)

College Prep Chemistry Fall Semester Final Review Worksheet II

1. The correct formula for iron(III) sulfate is © Russell W. Cramm 2001

Decomposition of 12 g of a compound containing only carbon and hydrogen yields 9 g of carbon and 3 g of hydrogen. 12. What is the simplest formula of the compound? Atomic Molar Masses 12.0 g·mol­1 C 1.0 g·mol­1 H (A) CH2 (B) CH4 (C) C2H5 (D) C3H7 (E) C3H9

© Russell W. Cramm 2001

14. A certain gaseous compound contains 46.2% carbon and 53.8% nitrogen by mass. At STP, 5.6 L of the gas has a mass of 13. 13 g. The molecular formula is Atomic Molar Masses 12.0 g·mol­1 C 14.0 g·mol­1 N (A) 14. CN (B) CN2 (C) C2N (D) C2N2 (E) C4N4 15. 16. 17.

Fe(s) + O2(g) --> Fe2O3(s) FeO(s) + O2(g) --> Fe2O3(s) Au2S3(s) + H2(g) --> Au(s) + H2S(g) Ca(s) + H2O(l) --> Ca(OH)2(aq) + H2(g)

Determine the number of atoms in each of the following: 23.5 grams of Co 18. 216 grams of Ag 19. Determine the number of grams in each of the following: 5.94 x 1023 atoms of Na 20. 21. 8.099 x 1023 atoms of Cu Determine the number of moles, molecules and atoms in each of the following: 45.23 grams of water 22. .8923 grams of potassium chloride, KClO3 23. 24. 1.00 kg of aluminium nitrate, Al(NO3)3.

The percentage by mass of oxygen in calcium carbonate (CaCO3) is Atomic Molar Masses 40. g·mol­1 Ca 12.0 g·mol­1 C O 16.0 g·mol­1 (A) 12% (B) 16% (C) 32% (D) 48% (E) 60%

15.

The percent of water of crystallization in MgSO4·7H2O is Molar Mass 120. g·mol­1 MgSO4 H2O 18. g·mol­1 51.2%

(A) 16.

4.8%

(B)

6.6%

(C)

25.6% (D)

48.8% (E)

Approximately how many molecules are in 11 g of carbon dioxide, CO2, gas? Atomic Molar Masses 12.0 g·mol­1 C 16.0 g·mol­1 O (A) (B) 1.5 x 1023 3.0 x 1023 (C) (D) 6.0 x 1023 2.4 x 1023

17.

The net ionic equation for the formation of barium phosphate, Ba3(PO4)2, is (A) Ba3+(aq) + (PO4)2­(aq) Ba3(PO4)2(s) (B) Ba3 2+(aq) + (PO4)23­(aq) Ba3(PO4)2(s) (C) 3Ba+(aq) + 2PO4­(aq) Ba3(PO4)2(s) (D) 3Ba2+(aq) + 2PO43­(aq) Ba3(PO4)2(s)

Balance and classify these equations: Zn + HCl ----> ZnCl2 + H2 1. 2. H2O ----> H2 + O2 3. NaOH + Pb(NO3)2 ----> NaNO3 + Pb(OH)2 4. H2O + CO2 ----> H2CO3 5. C4H10 + O2 ----> CO2 + H2O 6. CuSO4 + Mg ----> MgSO4 + Cu 7. C6H6(l) + O2(g) ----> CO2(g) + H2O(l) 8. H2O(l) + SO2(g) ----> H2SO3(aq) 9. Na2CO3(aq) + NH4OH(aq) ---> (NH4)2CO3(aq)+ NaOH(aq) 10. (NH4)2CO3(aq) ----> NH3(g)+ H2O(l)+ CO2(g) 11. HNO3(aq)+ Cu(s)---> Cu(NO3)2(aq)+ NO2(g)+ H2O(l) 12. Pb(NO3)2(aq)+ NaCl(aq)--> PbCl2(s)+ NaNO3(aq) 13. Fe(s) + O2(g) --> FeO(s) © Russell W. Cramm 2001

© Russell W. Cramm 2001

Answers to Multiple Choice 1. D 2. C 3. E 4. C 5. B 6. B 7. D 8. B 9. C 10. B 11. A 12. B 13. D 14. D 15. E 16. C 17. C Answers to Balancing Equations and Open Answer Questions: Balance and classify these equations: 1. Zn + 2HCl ----> ZnCl2 + H2 2. 2H2O ----> 2H2 + O2 3. 2NaOH + Pb(NO3)2 ----> 2NaNO3 + Pb(OH)2 4. H2O + CO2 ----> H2CO3 5. 2C4H10 + 13O2 ----> 8CO2 + 10H2O 6. CuSO4 + Mg ----> MgSO4 + Cu 7. 2C6H6(l) + 15O2(g) ----> 12CO2(g) + 6H2O(l) 8. H2O(l) + SO2(g) ----> H2SO3(aq) 9. Na2CO3(aq) + 2NH4OH(aq) ---> (NH4)2CO3(aq)+ 2NaOH(aq) 10. (NH4)2CO3(aq) ----> 2NH3(g)+ H2O(l)+ CO2(g) 11. 4HNO3(aq)+ Cu(s)---> Cu(NO3)2(aq)+ 2 NO2(g)+ 2H2O(l) 12. Pb(NO3)2(aq)+ 2NaCl(aq)--> PbCl2(s)+ 2NaNO3(aq) 13. 2Fe(s) + O2(g) --> 2FeO(s) 14. 4Fe(s) + 3O2(g) --> 2Fe2O3(s) 15. 4FeO(s) + O2(g) --> 2Fe2O3(s) 16. Au2S3(s) + 3H2(g) --> 2Au(s) + 3H2S(g) 17. Ca(s) + 2H2O(l) --> Ca(OH)2(aq) + H2(g) Combination: 4,813-15,17 Decomposition: 2,10 Combustion: 5,7 Single Replacement: 1,6,16 Double Replacement: 3,9,12 #17 could be combination or single replacement Determine the number of atoms in each of the following: 18. 23.5 grams of Co 19. 216 grams of Ag Determine the number of grams in each of the following: 20. 5.94 x 1023 atoms of Na 21. 8.099 x 1023 atoms of Cu Determine the number of moles, molecules and atoms in each of the following: 22. 45.23 grams of water 23. .8923 grams of potassium chloride, KClO3 24. 1.00 kg of aluminium nitrate, Al(NO3)3.

College Prep Chemistry Fall Semester

Final Review Worksheet III

1. An example of a chemical change is (A) freezing of water. (B) burning a match. (C) boiling carbon tetrachloride. (D) dissolving alcohol in water. (E) stretching a rubber band. A method of obtaining oxygen that illustrates a physical change and does not involve a chemical change is (A) heating mercuric oxide. (B) heating potassium chlorate. (C) decomposition of hydrogen peroxide. (D) distillation of liquid air. (E) electrolysis of water.

2.

3. When the components of the air at the same temperature are mixed in the proportions in which they are found in the air, no energy change is noticed. This fact indicates that air (A) is a compound. (B) has a negative heat of formation. (C) is a mixture. (D) contains free elements. (E) contains inert gases. 4. The formulas of a pair of compounds that could be used to illustrate the law of multiple proportions are (A) H2O and HBr (D) AgNO3 and Ag2S (B) NaCl and CaCl2 (E) MnO2 and H2O (C) NO2 and NO As far as can be detected by analytical balances, in any chemical reaction, the sum of the masses of all the reactants (A) always equals the sum of the masses of all the products. (B) is less than that of the products if a precipitate is formed. (C) is greater than that of the products if a gas is formed. (D) usually equals that of the products. (E) never equals that of the products. Which set consists only of compounds? (A) Na, Ca, He (C) (B) H3O+, Cl­, I3­ (D) NaCl, CH4, Br2 H2S, CuCl2, KI

5.

6.

7.

A solid, pure, orange substance was heated yielding a colorless gas and a green solid. What kind of material was heated? (A) an element (C) a mixture (B) a compound (D) a solution Which measurement is the most uncertain? (A) 1.00 ± 0.01 cm (C) 10 ± 1 g (B) 2.00 ± 0.05 L (D) 200 ± 1 mL Which temperature on the Celsius scale corresponds to 247 K on the Kelvin scale? ­16 °C (B) ­26 °C (C) 273 °C (D) 347 °C The volume of one milliliter most nearly equals 454 g (B) 1000 L (C) 1 mg (D) 1 in3 1 cm3 (E) 520 °C

8.

9. (A) 10. (A) 11. (A)

(E)

An insoluble solid has a mass of 20.0 g. It is placed in a graduated cylinder containing 40.0 mL of water. The final volume is read as 46.0 mL. What is the density of the solid? (B) 0.500 g·cm­3 (C) 2.30 g·cm­3 (D) 3.33 g·cm­3 0.300 g·cm­3 © Russell W. Cramm 2001

© Russell W. Cramm 2001

12. (A) 13.

Which is a unit for expressing volume? mm (B) g (C) cm3

(D)

g·cm­3 (A)

The mass of manganous chloride produced at the same time is most nearly Atomic Molar Mass 55 g·mol­1 Mn 12 g (B) 24 g (C) 32 g (D) 42 g (E) 84 g

The graph was obtained by plotting the volume of a material vs. the mass of that same material. 23. 20 mL of chlorine gas and 50 mL of hydrogen gas were mixed at STP and reacted. When the products were returned to STP, the volume of unreacted gas was Cl2 + H2 2Cl Atomic Molar Masses 35.5 g·mol­1 Cl 1.0 g·mol­1 H (A) 10 mL (B) 20 mL (C) 25 mL (D) 30 mL (E) 50 mL

1 3 5 7 mass (g) 9

volume (cm3)

5 3 1

(A) 14. (A) 15. (A) 16. (A) 17.

What is the density of the material? (B) 2.0 g·cm­3 1.5 g·cm­3 Which unit represents l x 10­3 gram? decigram (B) kilogram

(C)

0.67 g·cm­3

(D)

0.50 g·cm­3

How many grams of calcium carbonate, CaCO3, would be needed to produce 44.8 L of carbon dioxide gas, CO2, 24. measured at STP? Atomic Molar Masses 40.1 g·mol­1 Ca 12.0 g·mol­1 C O 16.0 g·mol­1 CaCO3 + 2HCl CaCl2 + H2O + CO2 111 (D) 200

(C)

milligram

(D)

microgram (A) 383 K 25-39. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 50.0 (B) 100 (C)

The value on the absolute (kelvin) temperature scale that corresponds to ­80 °C is ­383 K (B) ­193 K (C) 193 K (D) 273 K (E) The metric prefix for mega­ (B) kilo­ 10­6 is (C)

micro­

(D)

milli­

The number of grams of oxygen in 1.5 mol of atmospheric oxygen is Atomic Molar Mass 16.0 g·mol­1 O (A) 12 g (B) 16 g (C) 24 g (D) 32 g

(E)

48 g

18.

(A) 19.

What is the approximate mass of a mole of carbon tetrachloride, CCl4? Atomic Molar Masses 12.0 g·mol­1 C 35.5 g·mol­1 Cl 1.00 g (B) 22.4 g (C) 47.5 g (D) 83.5 g (E) 154. g How many mole(s) of calcium carbonate, CaCO3, is represented by 50 g of the compound? Atomic Molar Masses 40.1 g·mol­1 Ca 12.0 g·mol­1 C O 16.0 g·mol­1 1.0 (B) 2.0 (C) 0.20 (D) 4.0 (E) 0.50 How many sugar molecules are there in 1.00 mL of 0.100 M sugar solution? (A) 1. 20 · 1024 (D) 6. 02 · 1019 (B) 6.02 · 1023 (E) 3.01 · 1018 (C) 3.01 · 1019 The volume of hydrogen gas that can be liberated at STP by the decomposition of 18 g of water is Atomic Molar Masses 1.0 g·mol­1 H 16.0 g·mol­1 O 2.0 L (B) 11.2 L (C) 22.4 L (D) 36.0 L (E) 44.8 L In an experiment, 5.6 L of chlorine at STP was released according to this equation: 4HCl + MnO2 MnCl2 + 2H2O + Cl2 © Russell W. Cramm 2001

Write, complete and balance the following chemical equations: Magnesium reacts oxygen gas Iron metal reacts with sulfur powder. Charcoal, C, burns in the presence of oxygen gas. Nitrogen gas reacts with aluminum metal. Calcium carbonate is heated. Potassium chlorate is heated. Hydrogen peroxide decomposes. Sodium hydrogen carbonate is heated. Calcium hydroxided is heated. Zinc metal is dropped into hydrochloric acid. Chlorine gas reacts with sodium bromide. Magnesium metal reacts with silver nitrate. Sodium iodide reacts with lead (II) acetate. Benzene, C6H6, burns in oxygen gas. Butane burns in oxygen gas. How many grams of water will be formed when 32 g of hydrogen and 32 g of oxygen are mixed and allowed to react? 2H2 + O2 2H2O Atomic Molar Masses 1.0 g·mol­1 H 16.0 g·mol­1 O 18 (B) 2.0 (C) 36 (D) 64 Diborane, B2H6, has been used as a rocket fuel. It reacts with liquid oxygen according to the equation B2H6 + 3O2 B2O3 + 3H2O What mass of oxygen is required to react with 1.00 g of diborane? Atomic Molar Masses 10.8 g·mol­1 B 1.0 g·mol­1 H O 16.0 g·mol­1 (A) 1.16 g (B) 1.74 g (C) 3.48 g (D) 10.4 g

(A) 20.

(A) 41.

21.

(A) 22.

42. How many grams of water, H2O, can be prepared when 2.00 mol of hydrogen, H2, and 2.00 mol of oxygen, O2, are mixed and reacted in this process? 2H2 + O2 2H2O Atomic Molar Masses © Russell W. Cramm 2001

(A)

H O 18.0 g

1.0 g·mol­1 16.0 g·mol­1 (B) 36.0 g (C)

68.0 g

(D)

72.0 g

How many moles of FeS2 are required to produce 64 g of SO2 according to the equation: 43. 4FeS2(s) + 11O2(g) 2Fe2O3(s) + 8SO2(g) O (A) 44. 16. g·mol­1 0.40 (B) 0.50 S (C) 32. g·mol­1 3.2 (D) 6.0

What mass of water is produced by complete combustion of 126 g of propene, C3H6? 2C3H6 + 9O2 6H2O + 6CO2 Atomic Molar Masses 12.0 g·mol­1 C 1.0 g·mol­1 H O 16.0 g·mol­1 (A) 18.0 g (B) 54.0 g (C) 126 g (D) 162 g

Answers:

1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44.

B D. C. C. A. D. B. C. B. C. D. C. B. C. C. C. E E. E. D. C. C. D. D. Magnesium reacts oxygen gas: Mg + 2HCl H2 + MgCl2 Iron metal reacts with sulfur powder. 8Fe + S8 8FeS Charcoal, C, burns in the presence of oxygen gas. C+O2CO2 Nitrogen gas reacts with aluminum metal. 2Al + N22AlN Calcium carbonate is heated. CaCO3CaO + CO2 Potassium chlorate is heated. 2KClO32KCl+3O2 Hydrogen peroxide decomposes. 2H2O2 2H2O + O2 Sodium hydrogen carbonate is heated. 2NaHCO3 Na2O + H2O + 2CO2 Calcium hydroxided is heated. Ca(OH)2CaO + H2O Zinc metal is dropped into hydrochloric acid.Zn+2HClZnCl2 + H2 Chlorine gas reacts with sodium bromide. Cl2 + NaBrNaCl + Br2 Magnesium metal reacts with silver nitrate. Mg + 2AgNO3 Mg(NO3)2+ Ag Sodium iodide reacts with lead (II) acetate. NaI + Pb(C2H3O2)2 NaC2H3O2 + PbI2 2C6H6 + 15O2 12CO2 + 6H2O Benzene, C6H6, burns in oxygen gas. Butane burns in oxygen gas. 2C4H10 + 13O2 8CO2 + 10H2O C. C. B. B. D.

CHEMISTRY PRACTICE FOR STAR AND FINAL EXAM

1. 2. Titanium, which has the symbol Ti, is as a member of which of the following groups a. nonmetal b. transition metal c. metalloid d. inner transition metal e. noble gas Select the single best answer that completes this sentence. The nucleus of an atom may contain a. proton(s). b. proton (s) and neutron(s). c. neutron(s). d. electron(s). e. proton(s) and electron(s). An atom of Chlorine-36 contains a. 17 protons, 17 neutrons &19 electrons b. 19 protons, 17 neutrons & 19 electrons c. 36 protons, 17 neutrons &17 electrons d. 19 protons, 19 neutrons & 17 electrons © Russell W. Cramm 2001

3.

© Russell W. Cramm 2001

Pressure in lb/in2

e. 17 protons, 19 neutrons &17 electrons Which term most correctly refers to the number of protons in an atom? a. mass number b. atomic mass c. atomic number d. isotope number e. none of the above 5. Which of the following statements is incorrect? a. Metal atoms tend to gain electrons to have 8 electrons in their outer shell. b. Electrons tend to repel each other because they have similar charges. c. Photons demonstrate behavior like particles at times and like waves at other times. d. Electrons in the lowest energy state are in the ground state. e. More than one statement is incorrect. ab. None of the statements are incorrect. (Mark both a & b if you select this answer). 6. Which of the following statements is incorrect? a. The nucleus of an atom is negatively charged and contains all the mass of the atom. b The protons travel outside the nucleus in orbits like planets around the sun. c. Protons and neutrons attract each other because they have opposite charges. d. Electrons behave as waves because they are positively charged. e. More than one statement is incorrect. ab. None of the statements are incorrect. (Mark both a & b if you select this answer). 7. Complete the sentence: A liquid has a. definite volume and definite shape. b. indefinite volume and indefinite shape. c. indefinite volume and definite shape. d. definite volume and indefinite shape. 8. Food coloring is added to water and the mixture is stirred in a beaker. Select the term that best describes the mixture: a. solution. b. heterogneous material. c. pure substance. d. element. e. The question does not supply enough information. 9. A weather balloon contains 12 L of hydrogen at 740 mmHg pressure. At what pressure in mmHg will the volume become 20 L (temperature constant) (A) 370 (B) 444 (C) 760 (D) 1230 (E) 1480 10. A single molecule of calcium nitrate contains ___ oxygen atoms. a. 0 b. 3 c. 4 d. 5 e. 6 11. Find the ion in the following list that is not likely to form: a. Na+ b. S2c. I2d. Ca2+ e. Al3+ 12. Select the formula of the compound formed by magnesium and iodine a. MgI b. Mg2I c. MgI2 d. Mg2I2 e. Mg2I3 13. Which is STP? (A) 0 °C and 76 mmHg (D) 100 °C and 76 cmHg (B) 0 K and 76 mmHg (E) 273 K and 760 mmHg (C) 0 K and 760 mmHg 14. Select the statement that is true. a. Metals tend to lose electrons to form negatively charged ions called cations. b. Metals tend to gain electrons to form negatively charged ions called cations. c. Metals tend to lose electrons to form negatively charged ions called anions. d. Metals tend to lose electrons to form positively charged ions called cations. e. Metals tend to lose electrons to form positively charged ions called anions. 4.

15. (A) (B) (C) (D) (E) 16. (A) (B) (C) (D) (E) 17. (A) (B) (C) (D) (E) 18. 19. (A) (B) (C) 20. 21.

A sample of gas occupies 950 mL at 0 °C and 720 mmHg. Which expression gives the volume of this sample at standard pressure? Assume the temperature is constant. 720 mmHg 950 mL · 760 mmHg 760 mmHg 950 mL · 720 mmHg 1 720 mmHg 950 mL · 760 mmHg 1 760 mmHg 950 mL · 720 mmHg 720 mmHg 950 mL · 273 K · 760 mmHg The density of a gas at 27 °C and standard pressure is greater than at STP. the same as at STP. less than at STP. greater than at standard pressure and 273 K. less than at 310 K and standard pressure. Which statement best accounts for the fact that gases can be greatly compressed? Molecules occupy space. The collisions of molecules are elastic. Molecules of gases are in constant motion. The molecules of a given gas are identical. Molecules of gases are relatively far from each other. The gaseous molecules that have the greatest average velocity at 150 °C are represented by (A) O2 (B) F2 (C) H2 (D) N2 (E) H2O Equal volumes of oxygen, carbon dioxide, and methane under the same conditions of temperature and pressure contain the same number of atoms. (D) electrons. molecules. (E) neutrons. protons. The arrangement of atoms in a water molecule, H2O, is best described as (A) ring. (B) bent. (C) linear. (D) spherical In the experimental graph, the extrapolated line intersects the horizontal axis at about ­280 °C. Which term is applied to this value ?

25 20 15 10 5 0 ­300 ­200 ­100 0 Temperature in °C 100

(A) (B) 22.

23.

triple point (C) freezing point absolute zero (D) critical temperature The correct formula of copper(I) sulfate is a. Cu(SO4)2. b. Cu2SO4. c. CuS. d. Cu2(SO4)3. e. The question does not provide enough information. Determine the number of significant figures in 754.3 millimeters a. 1 b. 2 c. 3 d. 4 e. 5

© Russell W. Cramm 2001

© Russell W. Cramm 2001

24.

Determine the number of significant figures in 0.023 grams a. 1 b. 2 c. 3 d. 4 e. 5 25-30. Match the statements with the single corresponding term from the list below. A term may be used not at all. Each question has only one best answer. Mark both a & b for ab, and a & c for ac. a. Law of Multiple Proportions b. Pauli Exclusion Principle c. Law of Conservation of Mass d. Heisenberg Uncertainty Principle e. Hund's Rule ab. Aufbau Process ac. Law of Definite Composition

once, twice or

40.

41. 42. 43.

Pressure, mmHg

25. 26. 27. 28. 29. 30. 31.

The mass of the product formed in a reaction is always the same as the mass of the reactants. In a given compound the atoms always exist in a specific fixed ratio. No more than two electrons can occupy a single orbital in an atom. There is a limit to how much can be known simultaneously about the position and momentum of an electron. Two elements such as hydrogen and oxygen can combine to form more that one compound or formula. Electrons fill the lowest energy orbital that is available. What is the charge on Vanadium in V2(SO4)3? a. 2+ b. 3+ c. 4+ d. 2e. 3ab. 432. Helium is in the ____________ (family/group)on the periodic table. a. alkali metals b. alkaline earth metals c. halogens d. noble gases

(A) gaseous hydrogen, H2 (C) xenon tetrafluoride, XeF4 (B) lithium fluoride, LiF (D) gaseous fluorine, F2 The type of bond formed when two atoms share a pair of electrons is called (A) ionic. (D) bivalent. (B) double. (E) electrovalent. covalent. (C) Which molecule is essentially nonpolar? (A) CH4 (B) HCl (C) HBr (D) H2O (E) NH3 What type of intermolecular bonding accounts for the fact that water is a liquid at room temperature? (A) ionic bonding (C) hydrogen bonding (B) covalent bonding (D) van der Waal forces On the phase diagram, in what state or states of matter does the substance exist at 5 mmHg and 10° Celsius?

40

30

.

solid

liquid

20

33. Which of the following represents a mix of nitrogen gas, N2, and hydrogen gas, H2, that will completely react to form ammonia, NH3? N2 + H2 NH3

10 0 ­10

vapor

0

10 20 Temperature, °C

30

44.

(A) solid (B) liquid Consider this diagram:

(C) (D)

vapor liquid and vapor

34.

35.

36.

37.

38. 39.

When an atom is changed to a negatively charged ion, A. oxidation occurs. B. protons are lost. C. electrons are lost. D. there is an increase in radius. E. the ion becomes a better electron acceptor. Neon atoms produce characteristic spectral lines when their electrons (A) return to lower energy levels. (B) orbit the nucleus in a single energy level. (C) remain in their normal energy levels and move faster. (D) remain in their normal energy levels and move slower. In which pair do both compounds exhibit ionic bonding? (A) SO2, HCl (D) KCl, CO2 (B) KNO3, CH4 (E) NaCl, H2O (C) NaF, KBr Which of these is a characteristic of a highly ionic salt? (A) melts at a low temperature (B) has a non­crystalline structure (C) conducts electricity when melted (D) forms long chain­like molecules (E) is a liquid or gas at room temperature Which bond has the least ionic character? (A) P--Cl (B) H--Cl (C) Br--Cl (D) S--Cl Which substance has bonds of greatest ionic character? © Russell W. Cramm 2001

40° Temperature, °C 20° 0° ­20° ­40° Time of heating

45. 46.

47. (E) Cl--Cl 48.

A solid at ­40 °C was heated uniformly until it changed into a gas. What is the melting point of the solid? (A) ­20 °C (B) 0 °C (C) 20 °C (D) 40 °C Which is the weakest type of attractive force between particles? (A) ionic bond (C) covalent bond (B) hydrogen bond (D) van der Waals forces What gas is released when a piece of zinc, Zn, is dropped into hydrochloric acid, HCl(aq)? (A) chlorine, Cl2 (C) hydrogen chloride, HCl (B) hydrogen, H2 (D) zinc chloride, ZnCl2 Which two formulas represents a nonpolar molecules? (A) HCl (B) CF4 (C) NH3 (D) H2S The shape of a chloroform molecule, CHCl3, is © Russell W. Cramm 2001

49. (A) (B) (C) (D) (E) 50. 51. (A)

H Li Na

(A) linear. (D) tetrahedral. (B) cubical. (E) planar triangular. octahedral. (D) A gas is compressed and then cooled to its original temperature. Compared to the original conditions the particles move faster. move slower. are farther apart. are closer together. have contracted in proportion to the pressure applied. The outermost shell of element X has 3 electrons while that of element Y has 6. The probable formula of a compound of these elements is (A) X3Y2 (B) X2Y3 (C) XY (D) X2Y (E) XY2 M represents a metallic element, the oxide of which has the formula M2O. The formula of the chloride of M is MCl (B) MCl2 (C) MCl3 (D) MCl4 (E) M2Cl

He Ne Ar

Q R T

(C) (B)

TR

Q

QR

T

Be Mg

B Al

C Si

N P

O S

F Cl

59.

(D) This potential energy diagram shows that the reaction A + B C is

Energy

52. (A) 53. (A) 54.

The number of valence electrons in the outermost shell of O is 8 (B) 2 (C) 3 (D) 6 (E) 5 What element in the fourth period has 5 valence electrons? calcium, Ca (B) iron, Fe (C) arsenic, As (D) selenium, Se The element with the greatest tendency to lose electrons is Main Groups 1 2 3 4 5 6 7 (O) First Period Second Period Third Period D Mg Al E P S L G J Fourth Period M D (B) E (C) G (D) J (E) L (A) 55. Which picture best represents the arrangement of gas molecules in a sealed container?

A+B

x

C

(A) 60.

Reaction Coordinate slow. (B) rapid. (C)

exothermic.

(D)

endothermic.

(E)

at equilibrium.

For the reaction, A + B C + D, the figure is the potential­energy diagram

Potential energy

1

3 C+D 2 4

Energy

Energy

Energy

Q R T

(A)

Reaction (C)

Reaction (B)

Reaction (D)

Energy

56. A. 57. a. b. c. d. e. f. 58.

How many electrons can be in the third energy level? 1 B. 2 C. 6 D. 10 E. 14 F. 18 The statement represents a chemical reaction at equilibrium. A + B C + D + heat. The yield of substance D is increased by removing substance A. removing substance B. removing substance C. raising the temperature. adding a catalyst to the mixture. The letters Q, R, and T stand for three elements whose fluorides have the formulas QF, RF2, and TF3. Where could Q, R, and T be located in the periodic table?

A+B

Reaction coordinate (B) What interval represents the net energy change for this reaction? (A) 1 61. Which energy diagram represents an exothermic reaction?

..

2

(C)

3

(D)

4

Reaction

(A) © Russell W. Cramm 2001 © Russell W. Cramm 2001

62. (A) 63. (A) 64.

If 0.100 mol of iron reacts in the equation below, how much heat is liberated? 2Fe(s) + 3/2O2(g) Fe2O3(s) H = ­840 kJ·mol­1 Fe2O3 42.0 kJ (B) 84.0 kJ (C) 210 kJ (D) 420 kJ (E) 840 kJ lThe burning of 0.500 mol of carbon to form carbon dioxide releases 197 kJ of heat. How much heat is released when 1.00 mol of CO2 is produced in a similar reaction? 98.4 kJ (B) 197 kJ (C) 394 kJ (D) 590 kJ What is the heat (enthalpy) of reaction, H, for this equation? 2H2S(g) + 3O2(g) 2H2O(l) + 2SO2(g) Compound Hf (kJ·mol­1) H2S(g) O2(g) H2O(l) SO2(g) ­21 0 ­285 ­297 74. (B) ­603 kJ (C) +561 kJ (D) +1122 kJ 75.

(A) (B) (C) 73.

[Ag+] [Cl­] [Ag+] [Cl­]

(D) (E)

[Ag+] [Cl­] [AgCl] [AgCl] [Ag+] [Cl­]

(A) 65.

­1122 kJ

66.

67. 68.

69.

Which pair of changes insures that a chemical system undergoes a spontaneous reaction? (A) a decrease in enthalpy and entropy (B) an increase in enthalpy and entropy (C) an increase in enthalpy with entropy constant (D) an increase in enthalpy and a decrease in entropy (E) a decrease in enthalpy and an increase in entropy In which system does randomness decrease? (A) ice melting (B) solid iodine subliming (C) methane gas crystallizing (D) salt dissolving in water (E) liquid alcohol evaporating The heat of vaporization of water is 44.0 kJ·mol­1. How much energy is released when 36.0 g of steam condenses into liquid water? (A) 22.0 kJ (B) 88.0 kJ (C) 195 kJ (D) 1580 kJ The equilibrium equation for the Haber process at 500 °C is N2 + 3H2 2NH3 + heat If heat is added in the above equilibrium mixture at constant pressure, then the concentration of (A) nitrogen decreases. (B) hydrogen decreases. (C) ammonia increases. (D) ammonia decreases. (E) ammonia remains constant. The statement represents a chemical reaction at equilibrium. A+ B + D + heat. The yield of substance D is increased by (A) removing substance A. (B) removing substance B. (C) removing substance C. (D) raising the temperature. (E) adding a catalyst to the mixture. What is the expression for the dissociation constant for acetic acid, CH3COOH? (A) K = [H+] [CH3COO­] [CH3COOH] (B) K = [H4+] [C2O2­] [CH3COOH] [H+] [CH3COO­] (C) K = [CH COOH] 3 [CH3COOH] (D) K= + [H ] [CH3COO­] Which expression represents the equilibrium constant, Keq for this equation? 2NO(g) + O2(g) 2NO2(g) [NO] [O2] [NO2]2 (A) Keq = [NO ] (C) Keq = [NO]2 [O2] 2 [NO]2 + [O2] [NO2] (B) Keq = (D) Keq = [NO] [O ] [NO2]2 2 Consider the equation: AgCl(s) Ag+(aq) + Cl­(aq) Which is the expression for the solubility product constant, Ksp, of silver chloride? © Russell W. Cramm 2001

(A) 76. 77.

[AgCl] [Ag+] [Cl­] What is the net ionic equation for the reaction between potassium iodide solution, KI(aq), and silver nitrate solution, AgNO3(aq)? (A) K+(aq) + I­(aq) KI(s) (B) K+(aq) + NO3­(aq) KNO3(s) (C) Ag+(aq) + NO3­(aq) AgNO3(s) (D) Ag+(aq) + I­(aq) AgI(s) In the reaction 4Al + 3O2 2Al2O3, how many moles of aluminum oxide, Al2O3, are produced from one mole of aluminum, Al? (A) 0.5 (B) 2 (C) 3 (D) 4 Consider the unbalanced expression: ? CH3CH2CHO(l) + ? O2(g) ? CO2(g) + ? H2O(g) Which set of coefficients balances the equation? 2, 8, 3, 6 (B) 3, 8, 6, 6 (C) 1, 4, 3, 2 (D) 1, 8, 3, 3 (E) 1, 4, 3, 3 How many moles of oxygen, O2, are produced from 3.0 mol of potassium chlorate, KClO3, in this equation? 2KClO3(s) 2KCl(s) + 3O2(g) (A) 6.0 (B) 9.0 (C) 3.0 (D) 4.5 Which is the net ionic equation for the reaction of lead(II) nitrate and sodium chromate? (A) Pb2+(aq) + CrO42­(aq) PbCrO4(s) (B) Pb(NO3)2(aq) + Na2CrO4(aq) PbCrO4(s) + 2NaNO3(aq) (C) 2Na+(aq) + CrO42­(aq) Na2CrO4(aq) (D) Pb2+(aq) + NO3­(aq) + Na+(aq) + CrO42­(aq) PbCrO4(s) + Na+(aq) + NO3­(aq) How many moles of magnesium, Mg, remain after 5.0 mol of Mg is ignited in a closed vessel containing 2.0 mol of oxygen, O2? 2Mg(s) + O2(g) 2MgO(s) (A) 1.0 (B) 2.0 (C) 3.0 (D) 2.5 A compound is composed of 80% C and 20% H. What is its simplest formula? (A) CH (B) CH2 (C) CH3 (D) C2H6 (E) C4H The simplest formula for a compound is CH. If the molar mass of the compound is 78 g·mol­1, what is the true formula? (A) CH (B) C2H2 (C) C5H18 (D) C6H6 (E) C6H14 The percentage by mass of oxygen in calcium carbonate (CaCO3) is (A) 12% (B) 16% (C) 32% (D) 48% (E) 60% The percent of water of crystallization in MgSO4·7H2O is (A) 4.8% (B) 6.6% (C) 25.6% (D) 48.8% (E) 51.2% Approximately how many molecules are in 11 g of carbon dioxide, CO2, gas? (A) 1.5 ·1023 (B) 3.0 · 1023 (C) 6.0 · 1023 (D) 2.4 · 1023 The molar mass of propanal (C2H5CHO) is (A) 10 g·mol­1 (D) 58 g·mol­1 (B) 29 g·mol­1 (E) 64 g·mol­1 (C) 42 g·mol­1 40 g of copper is heated with 4 g of sulfur. The reaction goes to completion without loss of sulfur, as represented by the equation: 2Cu + S Cu2S Approximately how many grams of copper remain uncombined? (A) 4g (B) 8g (C) 16 g (D) 24 g (E) 32 g d d d

78.

79. 80. 81. 82. 83. 84.

70.

85.

71.

86. 87. 88. 89.

72.

© Russell W. Cramm 2001

1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45. 46. 47. 48. 49.

Answers b b e c a e d a b (12·740/20) e Ca(NO3)2 c, I forms Ic e d a c d c b b b b d b c ac b d a ab b d c d a c c e b c a c c a d b b and d d d.

© Russell W. Cramm 2001

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