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1st Semester Final Review * DO THESE PROBLEMS WITHOUT A CALCULATOR! * p. 1 of 7 Name _________________________ KEY Per ____ Date _______ Chemistry 1st Semester Final Review Bring a pencil and eraser for the exam. There will be no calculators allowed. You will be given: PT (know names of #1-36, Au, Ag, Sn, Pb, Hg), activity series, solubility chart. There will be 80 M/C questions worth 2.5 points each for a total of 200 points % breakdown: o 6 questions each on Units 1 (ch 1 & 3), 2 (ch 2), 3 (ch 4 and 25), 4 (ch 5 & 6) o about 14 questions each on Units 5 (ch 7,8,9), 6 (ch 10), 7 (ch 11), part of 8 (ch 12.1-12.2 (up to mole-mole) Your lowest unit test score will be replaced if you score higher (in %) on the final [NOT the midterm] o Example: Final Exam Unit 1 Unit 2 Midterm Unit 5 Unit 6 previous % 80 74 60 97 70 83 adjusted % 80 74 60 97 83 83 o Note: if your final score is not higher than any past unit exams, your scores will remain as is. To review for Units 1-4, refer back to the 1st quarter midterm review WS Final Schedule: Jan 28 (Wednesday) Jan 29 (Thursday) Jan 30 (Friday) Per 5 (8:00-10:02) Per 4 (8:00-10:02) Per 3 (8:00-10:02) Break (10:02-10:07) Break (10:02-10:07) Break (10:02-10:07) Passing (10:07-10:14) Passing (10:07-10:14) Passing (10:07-10:14) Period 2 (10:14-12:16) Period 6 (10:14-12:16) Period 1 (10:14-12:16) 1st Quarter – a few questions to review (for the rest refer back to the 1st Quarter Midterm Review WS) 1. Complete the table: Species Name Atomic Mass (amu) # of Protons # of Electrons # of Neutrons Al3+ Aluminum ion 27 13 13 14 S2- Sulfide ion 32 16 16 16 2. Which pair of the following is correct to compare the size of radius? A) F >F- , Na >Na+ B) F >F- , Na <Na+ C) F <F- , Na >Na+ D) F <F- , Na <Na+ UNIT 5 (Chapters 7, 8, 9) REVIEW – Ionic & Covalent Compounds … Ionic Compounds 3. On the periodic table, label the charge with elements for groups 1, 2, and 13 – 18 when/if they form ions. Label the charge of silver _+1, cadmium_+2, zinc +2, aluminum +3, and gallium +3 when they form ions. 1+ 2+ 3+ 3- 2- 0 1- 4. Which of the followings correctly explained? A) Metals lose electrons to form anions and nonmetals gain electrons to form cations. B) Metals lose electrons to form cations and nonmetals gain electrons to form anions. C) Metals gain electrons to form anions and nonmetals lose electrons to form cations. D) Metals gain electrons to form cations and nonmetals lose electrons to form anions. 5. What types of elements compose an ionic compound? A) all nonmetals B) metals and nonmetals C) all metals D) none of the above 6. What are the characteristics/properties of an ionic compound (circle all that apply)? A) dull B) lustrous C) malleable D) ductile E) hard F) soft G) usually solids at room temperature H) are all soluble in water I) conducts electricity as a solid J) conducts electricity when dissolved in water 1st Semester Final Review 7. Which of the followings is correctly written in chemical formula if iron (III) ion and oxide ion. A) FeO B) Fe2O C) FeO2 D) Fe2O3 E) Fe3O2 8. Write the corresponding name or formula. Compound Compound Name Formula Sodium sulfide Na2S p. 2 of 7 Compound Name Compound Formula Ammonium Sulfate (NH4)2SO4 ZnCO3 Zinc carbonate Iron (III) Bromide FeBr3 Mg3N2 Magnesium nitride Copper (II) Chloride CuCl2 Ni(OH)2 Nickel(II) hydroxide Silver Acetate AgC2H3O2 AlCl3 Aluminum chloride Potassium Oxide K2O Ca3(PO4)2 Calcium phosphate Lithium Fluoride LiF … Covalent Compounds 9. Indicate the number represented by the prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca. 1-10, respectively 10. Complete the following chart bonds between (M+NM, NM) Transfer or shares electrons? IONIC M+ NM Transfer COVALENT NM Share Use charges to determine formula? (yes/no) Yes No Switch charges to balance out formula? (yes/no) Yes No Use prefixes? (yes/no) Simplify to lowest whole # ratio? (yes/no) Acids or ammonium compounds Conducts electricity High melting and boiling point No Yes Yes Yes In aqueous form, yes Yes magnesium phosphide Mg3P2 No No No No (have lower) disulfur monobromide S2Br Provide formula 11. What is the correct chemical name for NH3? a. nitrogen hydroxide b. nitrogen (III) hydride c. nitrogen (III) hydroxide 12. What is the correct name for P4O10? a. potassium oxide d. decphosphoroush tetraphosphide d. nitrogen trihydride b. potassium decoxide c. phosphorous decoxide e. tetraphosphorous decoxide 13. Write the corresponding formula and indicate if the substance is ionic or covalent. Name I/C Formula Name I/C Formula Sulfur hexafluoride C SF6 triphosphorus dioxide C P3O2 Nitrogen trihydride C NH3 tetracarbon monofluoride C C4F Pentaphosphorus monoxide C P5O lead (III) phosphide I PbP iron (II) hydroxide I Fe(OH)2 zinc nitrate I Zn(NO3)2 ammonium sulfide I (NH4)2S Aluminum carbonate I Al2(CO3)3 14. Describe the difference between an intramolecular bond and an intermolecular force. Use water as your example. Intramolecular – within a molecule (ex: for H-O-H, it is the bond between H-O and O-H). Intermolecular – between molecules (ex: for H2O, the attraction between many H2O molecules). 15. Rank the following forces in increasing intermolecular attraction: dipole-dipole, hydrogen-bond, electrostatic, dispersion force. Dispersion, dipole-dipole, hydrogen-bond, electrostatic attraction 1st Semester Final Review p. 3 of 7 16. What type of intermolecular forces does water, sodium chloride, oxygen, and carbon monoxide have? Hydrogen bonding, electrostatic attraction, dispersion, and dipole-dipole, respectively. 17. Which is stronger: intermolecular forces or ionic bonds? dipole-dipole or covalent bonds? Ionic bonds or covalent bonds? hydrogen bonds or covalent bonds? 18. Explain the octet rule. In forming compounds, atoms tend to achieve the electron configuration of a noble gas such as ns2np6. An octet is a set of eight. 19. Complete the following table. A reference chart is provided at the bottom. # valence Formula Lewis dot structure 3-D Lewis Dot electrons SO3 6 + 3(6) = 24 CSe2 4 + 2(6) = 16 NCl3 5 + 3(7) = 26 : Se = C = Se : .. .. Geometry/ Shape Trigonal planar (3 bonds, 0 lone) Linear (2 bonds, 0 lone) : Se = C = Se : .. .. Trigonal pyramidal (3 bonds, 1 lone) Reference chart: Geometry # atoms around central atom # lone pairs around central atom Linear 2 0 Trigonal planar 3 0 Bent 2 1 Tetrahedral 4 0 Trigonal pyramidal 3 1 Bent 2 2 4 20. Given the following Lewis Dot structure, how many electrons are shared between AX? 21. Given the following Lewis Dot structures, how many lone pairs are around the central atom? A. 2 0 B. 22. Which of the following structures is the correct VSEPR shape for carbon dioxide? A. B. C. 23. Which of the following is the correct Lewis Dot Representation for phosphorous trihydride? a. b. c. d. e. none of these 24. Which of the following is the correct Lewis Dot Representation for boron trifluoride a. b. c. d. e. none of these (should look like this: 25. Which of the following is an example of a non-polar covalent bond? a. water b. hydrofluoric acid c. sodium bromide d. chlorine (Cl – Cl) ) 1st Semester Final Review UNIT 6 (Chapter 10) REVIEW – The Mole p. 4 of 7 26. Avogadro's number of representative particles is equal to one ____. A) gram B) mole C) kilogram D) atom E) two of the above are true 27. All of the following are equal to Avogadro's number EXCEPT ____. A) the number of atoms of bromine in 1 mol Br2 (there are 2 (6.022x1023) atoms in Br2) B) the number of atoms of gold in 1 mol Au C) the number of molecules of nitrogen in 1 mol N2 D) the number of molecules of carbon monoxide in 1 mol CO E) the number of formula units of magnesium chloride in 1 mol MgCl2 28. How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O? A) 5 x (6.02 x 1023) B) 35 x (6.02 x 1023) C) 35 D) 5 5 molecules C3H 7 O E) 7 7 atoms H 35 atoms H 1 molecule C3H 7 O 29. How many moles of gold atoms are in 2.0 x 1023 atoms of gold? A) 6.022 x 1023 B) 1.0 C) 0.50 D) 0.33 2.0 x1023 atoms Au 1 mol Au 0.33 mol Au 6.022 x1023 atoms Au 30. How many formula units are in 0.50 mol of sodium chloride? A) 6.022 x 1023 B) 3.0 x 1023 C) 1.20 x 1024 0.50 mol NaCl E) 0.50 / 6.022x 1023 D) 3.0 6.022 x1023 formula units NaCl 3.0 x1023 mol Au 1 mol NaCl 31. The mass of a mole of NaCl is the ____ A) atomic mass B) molecular mass C) molar mass 32. How many carbon atoms are found in 2.0 mol of C6H12O6? A) 6.0 B) 12 C) 12 x (6.022 x 1023) 2.0 mol C6 H12O6 E) 2 (6.022 x 1023) D) average mass D) 1.2 x 1024 E) 12 / (6.022 x 1023) 6.022 x1023 molecules C6 H12O6 6 atoms C 12(6.022 x1023 ) atoms C 1 mol C6 H12O6 1 molec. C6 H12O6 33. What is the molar mass of carbon dioxide? A) 28.01 g/mol B) 40.02 g/mol C) 44.01 g/mol CO2 = 1 (12.01) + 2 (16.00) = 44.01 g/mol D) 76.01 g/mol 34. What is the molar mass of calcium hydroxide? A) 41 g/mol B) 57 g/mol C) 58 g/mol Ca(OH)2 = 1 (40) + 2 (16) + 2 (1.01) = 74.02 g/mol D) 74 g/mol 35. What is the number of moles of argon atoms in 120 g of argon? A) 0.50 mol B) 2.0 mol C) 3.0 mol D) 120 x (6.022 x 1023) mol 120 g Ar E) 6.022 x 1023 mol 1 mol Ar 3.0 mol Ar 40 g Ar 36. Pencil lead is composed of graphite, which is made of carbon. How many atoms of carbon can be found in 6.0 g of pencil lead? A) 1.0 B) 3.01 x 1023 C) 6.022 x 1023 D) 6 x 12 (6.022 x 1023) E) 6.0 6.0 g C 1 mol C 6.022 x1023 atoms C 3.01x1023 atoms C 12.01 g C 1 mol C 1st Semester Final Review p. 5 of 7 37. The lowest whole-number ratio of the elements in a compound is called the ____. A) empirical formula B) molecular formula C) mole ratio D) lowest common denominator formula 38. Which of the following is NOT an empirical formula? A) C2N2H7 B) C3H9O6 C) Na2SO4 D) Sb2S3 E) at least two of the above 39. Which of the following is NOT true about empirical and molecular formulas? A) The molecular formula of a compound can be the same as its empirical formula. B) The molecular formula of a compound can be some whole-number multiple of its empirical formula. C) Several compounds can have the same empirical formula, but have different molecular formulas. D) The empirical formula of a compound can be triple its molecular formula. E) at least two of the above are not true 40. If the molar mass of a compound is 266.7 g/mol and its empirical formula is B2H5, determine the molecular formula. A) 23 B) 10 C) B4H10 D) B6H15 E) B20H50 n MM MF 266.7 266.7 10 MF 10( EF ) 10(B2 H 5 )= B20 H 50 MM EF 2(11) 5(1) 26 UNIT 7 (Chapter 11) REVIEW – Balancing Equations, Reaction Types 41. When performing an experiment evidence of a chemical change includes A) a color change B) release of a gas C) release of energy in form of heat or light D) all of the above 42. The choice with the correct shorthand and meaning is: A) (s) = solid, (aq) = gas B) (g) = gas, (l) = liquid C) (aq) = aqueous, (l) = lethal D) all of these 43. Which of the following is true about this reaction: NaCl (aq) + AgNO3 (aq) NaNO3(aq) + AgCl (s) A) This is a single replacement reaction. B) The cations of both reactants will switch places. C) A white solid will form from two solutions. D) Two of the above are true (choices B and C are true) Balance each reaction and choose the answer that lists the correct coefficients 44. _____ (NH4)2Cr2O7 _____ N2 + _____ H2O a) 2, 4, 1, 2 b) 1, 1, 4, 1 c) 1, 1, 4, 2 d) 2, 2, 4,1 45. _____ C8H18 + _____ O2 _____ CO2 ___ Ag + ___ Cu(NO3)2 + _____ H2O a) 2, 4, 16, 18 b) 1, 1, 4,1 c) 1, 1, 4, 2 d) 2, 25, 16, 18 46. _____ Cu + ____ AgNO3 a) 2, 4, 1, 2 b) 1, 1, 4, 1 c) 1, 2, 2, 1 d) 2, 2, 4, 1 + ____ Cr2O3 1st Semester Final Review p. 6 of 7 47. Use the activity series to circle the more reactive element. A) Br2 or I2 B) Na or Mg C) H2 or Na 48. Circle the reaction that will take place: A) Cu + NaCl (Cu is less reactive than Na) C) I2 + KBr (I2 is less reactive than Br2) D) Li or Cu E) F2 or Cl2 B) Ca + HCl (Ca is more reactive than H2) D) they all take place 49. Circle all the following soluble salts. Refer to the solubility chart. A) PbI2 B) Fe(OH)3 C) AgCl D) (NH4)2SO4 E) PbNO3 H) (NH4)2SO4 I) Cu(C2H3O2)2 J) PbI2 K) Ca3(PO4)2 L) NaCl F) Fe(OH)3 M) CuCO3 G) AgNO3 N) (NH4)2SO4 50. Determine which combination will result in a precipitate. Give the formula of the precipitate. A) PbNO3 and AgNO3 solutions are mixed N/R B) AgNO3 and CuBr solutions are mixed AgNO3 (aq) + CuBr (aq) AgBr (s) + CuNO3 (aq) C) NaCl and (NH4)2SO4 solutions are mixed N/R D) Cu(C2H3O2)2 and NaCl solutions are mixed N/R 51. Determine the type of reaction (combination/synthesis (S), decomposition (D), combustion ( C ), single displacement (SR), and double displacement (DR) ). Give the lowest whole number coefficients (include a "1") that will balance the equation. __ DR ___ a) ___3__ CaCl2 + ___2__ Na3PO4 __ D ___ b) ___1__ (NH4 )2Cr2O7 __1___ N2 __ C ___ c) ___2__ C8H18 + __25___ O2 ___16__ CO2 + ___18__ H2 O __ S ___ d) ___2__ Na __ SR ___ e) ___1__ Cu + __2__ AgNO3 + ___1__ Cl2 __6___ NaCl + ___1__ Ca3(PO4)2 + __4___ H2O + __1__ Cr2O3 ___2__ NaCl __2_ Ag + __1_ Cu(NO3)2 UNIT 8 (Chapter 12.1 – 12.2) REVIEW – Stoichiometry In the reaction: 2 Al(OH)3 + 3 Ca(NO3)2 3 Ca(OH)2 + 2 Al(NO3)3. If 6 moles of aluminum nitrate were produced, how many moles of calcium nitrate were consumed? a. 2 moles b. 3 moles c. 5 moles d. 6 moles e. 9 moles f. 12 moles g. 15 moles 3 mol Ca(NO3 ) 2 6 mol Al(NO3 )3 9.0 mol Ca(NO3 ) 2 2 mol Al(NO3 )3 53. If 10 moles of methane combusts in an excess of oxygen, how many moles of water would be produced? a. 2. 5 moles b. 5 moles c. 10 moles d. 20 moles e. 40 moles 2 mol H 2 O 10 mol CH 4 20 mol H 2 O 1 CH4 + 2 O2 2 H2O + 1 CO2 1 mol CH 4 54. In the unbalanced equation: __3__CuSO4 + ___2_K3PO4 __3__K2SO4 + __1__Cu3(PO4)2 if 12 moles of copper (II) sulfate reacted with an excess of potassium phosphate, how many moles of potassium sulfate are produced? a. 4 moles b. 8 moles c. 12 moles d. 16 moles e. 24 moles 3 mol K 2SO 4 12 mol CuSO4 12 mol K 2SO4 3 mol CuSO 4 52. 1st Semester Final Review 55. p. 7 of 7 If 4 moles of potassium carbonate reacts with an excess of iron (III) hydroxide, how many moles of potassium hydroxide will be produced? a. 1 mole b. 2 moles c. 4 moles d. 8 moles e. 12 moles 6 mol KOH 8 mol KOH 3 mol K 2 CO3 56. Consider the unbalanced equation: __1___Cu + __2__AgNO3 __1__Cu(NO3)2 + __2__Ag . If 3 moles of silver are produced, how many moles of copper were used? a. 1 mole b. 1.5 moles c. 2 moles d. 2.5 moles e. 3 moles 3 K2CO3 + 2 Fe(OH)3 6 KOH + 1 Fe2(CO3)3 3 mol Ag 57. 58. 4 mol K 2 CO3 1 mol Cu 1.5 mol Ag 2 mol Ag What is the molar mass of propanol? (CH3CH2CH2OH) a. 48.09 g/mol b. 90.06 g/mol c. 48.09 amu d. 60.09 amu f. 48.09 mol/g g. 60.09 mo/g h. 90.06 amu i. 60.09 g/mol 3(12.01 g C) + 8(1.01 g H) + 16.00 g O = 60.09 g/mol e. 90.06 mol/g j. 90.06 atoms Which of the following is true? a. The limiting reactant in a reaction that limits the amount of product that can be produced b. The limiting reactant in a reaction has the smallest coefficient after an equation has been balanced c. The limiting reactant in a reaction is the reactant that you have the smallest number of moles of… d. Equations need to be balanced because otherwise, the reaction will not proceed e. A balanced reaction predicts how many moles can be produced given a certain number of moles of reactants f. Both a and b are true g. Both a and c are true h. Both a and d are true i. Both a and e are true