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South Pasadena • Honors Chemistry Name Semester 1 Final Exam Period PART 1 • MULTIPLE CHOICE (PRACTICE) 1. Which measurement below shows the temperature to the correct precision? 20 mercury thread Date 5. The density of copper is known to be 8.96 g/mL. A student’s experimental result shows that the density of her copper cube is 8.79 g/mL. The percent error in this data is ______. (A) 0.17 % (B) 0.98 % (C) 1.90 % (D) 1.93 % 30 (A) 26 °C (B) 26.25 °C (C) 26.3 °C (D) 26.30 °C 2. In scientific notation, the number 3,020,000 should be written as: (A) 3.02 × 106 (B) 3.02 ×10–6 (C) 302 ×104 (D) 302 ×10–4 3. How should the following computation be recorded, with the correct number of significant figures? (1.15)(1.50) (0.08206)(315) (A) 0.0667 (B) 0.06673 (C) 0.067 (D) 6620 4. Which measurement is the most precise? (A) 4.2 .3 g (B) 4.3 .1 g (C) 4.5 .4 g (D) 4.6 .2 g 6. The average temperature on Venus is 460°C. What is this in Kelvin? (A) 187 K (B) –187 K (C) 273 K (D) 733 K 7. Which one of the following statements is true? (A) 1000 cm = 1 m 1 (B) 1 mm = 100 meter (C) 1 kg = 1000 g (D) each of these statements is true 8. What conversion factor would you use to convert milligrams to grams? 1000 mg (A) 1 g 1g (B) 1000 mg 1 mg (C) 1000 g 1000 g (D) 1 mg 9. A metal cube of metal measures 2 cm on each side. Its mass is 90.4 grams. What is the metal? (A) Al (density = 2.70 g/cm3) (B) Au (density = 19.3 g/ cm3) (C) Fe (density = 7.86 g/ cm3) (D) Pb (density = 11.3 g/ cm3) 10. What is the volume of a 5.08 gram sample of liquid bromine? (density of bromine = 3.10 g/mL) (A) 0.610 mL (B) 1.64 mL (C) 15.7 mL (D) 8.18 mL 16. In which of the following states of matter are the attractive forces between molecules strongest? (A) Solid (B) Liquid (C) Gas (D) Plasma 11. A gold block and a copper block both have a mass of 5.0 kg. Which occupies a greater volume? (Densities in g/cm3: gold = 19.3, copper = 8.94) (A) Copper block (B) Gold block (C) They have the same volume. (D) It cannot be determined. 17. Which set consists only of elements? (A) Na, Ca, H2 (B) H3O+, Cl–, I3– (C) NaCl, CH4, Br2 (D) H2S, CuCl2, KI 12. The atom represented by 57Co3+ has: (A) 27 protons, 30 neutrons, 24 electrons (B) 27 protons, 30 neutrons, 30 electrons (C) 27 protons, 57 neutrons, 3 electrons (D) 30 protons, 27 neutrons, 3 electrons 13. All of the following describe a neutron EXCEPT: (A) It determines the identity of the atom. (B) It does not carry a charge. (C) It is located in the nucleus. (D) It, along with the proton, makes us most of the atom’s mass. 14. Which of the following is an isotope of 40K? (A) 39K (B) 40K+ (C) 40Ar (D) 40Ca 15. The atomic mass of aluminum is 26.98. Which of the following is correct? (A) One aluminum atom has a mass of 26.98 amu. (B) One aluminum atom has a mass of 26.98 grams. (C) One mole of aluminum contains 26.98 atoms. (D) One mole of aluminum has a mass of 26.98 grams. 18. What do the elements phosphorous and sulfur have in common? (A) They are both alkali metals. (B) They are in the same family. (C) They are in the same period. (D) They both form ions with the same charges. 19. Which of the following is a liquid non-metal atom at room temperature? (A) Barium (B) Bromine (C) Mercury (D) Nitrogen 20. Which of the following compounds is ionic? (A) AlCl3 (B) HCl (C) SCl2 (D) SiCl4 21. What is the formula for the ionic compound formed when sodium ions and sulfide ions are combined? (A) Na2S (B) Na2SO4 (C) NaS (D) NaS2 22. An unknown element X forms a salt with the formula XO2. Which of the following could be X? (A) Al3+ (B) Ca2+ (C) Na+ (D) Sn4+ 23. Which one of the following is the correct formula for calcium phosphate? (A) Ca2(PO4)3 (B) Ca3(PO4)2 (C) CaPO4 (D) PO4Ca3 24. What is the name of the compound N2O3? (A) dinitride trioxide (B) dinitrogen trioxide (C) nitrate (D) nitrogen oxide 25. The formula for hydrosulfuric acid is: (A) H2S (B) H2SO4 (C) HS (D) HSO4 26. Which of the following is incorrect? (A) 1 mole of O2 molecules has 6.02 × 1023 oxygen atoms. (B) 1 mole of O2 molecules has a mass of 32 grams. (C) 1 mole of O2 molecules occupy 22.4 liters at STP. (D) All of the above statements are correct. 27. How many molecules are in 2.00 × 10–2 moles of carbon tetrachloride, CCl4? (molar mass = 154 g/mol) (A) 1.20 × 1023 (B) 3.01 × 1023 (C) 6.02 × 1023 (D) 1.20 × 1022 28. What is the percent of carbon in barium carbonate, BaCO3? (molar mass = 197.3 g/mol) (A) 3.04% (B) 6.09% (C) 14.0% (D) 20.0% 29. The general formula CnH2n describes the molecular composition of the hydrocarbon family known as the (A) alkadienes (B) alkanes (C) alkenes (D) alkynes 30. Structural formulas have advantages over molecular formulas because they show the (A) bonding arrangement of each carbon atom. (B) geometric arrangement of the atoms. (C) number of atoms of each element present. (D) percentage composition of the compound. 31. How many carbons make up the “parent chain” in the following molecule? (A) 4 (B) 5 (C) 6 (D) 7 32. The number of isomers of bromopropane, C3H7Br, is (A) 2 (B) 3 (C) 4 (D) 7 33. Which of the following is an isomer of the compound below: F H C (A) F F H H F H F F C C H (D) H F F H C C H F H 34. Which of the following is the correct name for the following compound: H H H Br C C C H H Br H (A) 1,1-dibromobutane (B) 1,1-dibromopropane (C) 2-bromopropane (D) 3,3-dibromopropane 35. Which functional group is found in the following compound? H H H C C H H O H 37. When the equation for the combustion of propene, C3H6, is balanced with the lowest whole-number coefficients, what is the coefficient of oxygen, O2? (A) 6 (B) 9 (C) 12 (D) 18 C F H (A) Grain alcohol (ethanol) (B) Isopropyl alcohol (2-propanol) (C) Nail polish remover (acetone, or propanone) (D) Vinegar (ethanoic acid) C C (C) F H C (B) H C H 36. The structure of which compound is given below? H H C C O (A) Aldehyde (B) Carboxylic Acid (C) Ether (D) Ketone H C H 38. When an alcohol reacts with a carboxylic acid, which of the following is formed? (A) A ketone (B) An ester (C) An ether (D) CO2 39. In a sample of salt water, the salt is called the (A) Precipitate (B) Solute (C) Solution (D) Solvent 40. Which of the following compounds is expected to be soluble in water? (A) CaSO4 (B) FeS (C) PbCl2 (D) SrBr2 41. How many grams of sodium hydroxide pellets, NaOH, are required to prepare 50.0 mL of a 0.150 M solution? [molar mass NaOH = 40.0 g/mol] (A) 0.300 (B) 2.00 (C) 3.00 (D) 200. 42. If 50 mL of a 200 mL sample of 0.10 M sodium chloride solution is spilled, what is the concentration of the remaining solution? (A) 0.025 M (B) 0.075 M (C) 0.10 M (D) 0.20 M 43. List the following solutions prepared with the same solute in order of increasing concentration: I. 30.0 g solute in a 240 mL solution II. 30.0 g solute in a 120 mL solution III. 60.0 g solute in a 120 mL solution (A) I < II < III (B) II < I < III (C) II < III <I (D) III < II < I 44. A 100 mL sample of a solution with a concentration of 5.00 M is diluted to a new volume of 400 mL with distilled water. The new concentration will be (A) 1.25 M (B) 1.66 M (C) 15.0 M (D) 20.0 M 45. A property of acids are that they (A) are caustic (B) feel slippery (C) neutralize water (D) taste sour 46. Which of the following represents the dissociation of CaI2 in solution? (A) CaI2 Ca + I2 (B) CaI2 Ca2+ + 2 I– (C) CaI2 Ca2+ + 2 I– (D) CaI2 is insoluble so it does not dissociate. 47. A solution that conducts electricity very well is called a: (A) liquid conductor (B) metallic solution (C) strong electrolyte (D) weak electrolyte 48. Which chemical is the conjugate base? NH3 + H2O NH4+ + OH– (A) H2O (B) NH3 (C) NH4+ (D) OH– 49. If a solution has [OH–] = 1.0 × 10–3 M, what is the pH? (A) 3 (B) 7 (C) 11 (D) 14 50. What is the [OH–] in a solution in which [H+] is 1.0 × 10–6 M? (A) 1.0 × 10–6 M (B) 1.0 × 10–7 M (C) 1.0 × 10–8 M (D) 1.0 × 10–9 M 51. A solution tested with cabbage juice turns green. Which of the following could be its pH? (A) 1 (B) 4 (C) 7 (D) 10 52. A substance that turns cabbage juice blue and slightly lights up a light bulb is a: (A) strong acid (B) strong base (C) weak acid (D) weak base 53. Which reaction below would be classified as a single replacement reaction? (A) 2 AgNO3 + Cu Cu(NO3)2 + 2 Ag (B) 2 H2 + O2 2 H2O (C) Ba(OH)2 + H2SO4 BaSO4 + 2 H2O (D) NaHCO3 NaOH + CO2 54. … H3PO3 … H3PO4 + …PH3 When the equation above is balanced, the coefficient for H3PO4 is: (A) 1 (B) 2 (C) 3 (D) 4 55. When solutions of potassium sulfate and calcium bromide are combined, which of the following precipitates? (A) KBr (B) CaS (C) CaSO4 (D) There is no precipitate. 56. Which of the following are products when magnesium metal is placed in hydrochloric acid? (A) H (B) H+ (C) Mg (D) MgCl2 57. Zn Zn2+ + 2e– In the half reaction above: (A) Zn is oxidized because it is gaining electrons. (B) Zn is oxidized because it is losing electrons. (C) Zn is reduced because it is gaining electrons. (D) Zn is reduced because it is losing electrons. 58. When we reacted AgNO3 and K2CrO4 to form Ag2CrO4 and KNO3, ________ was oxidized. (A) chromate ion (B) nitrate ion (C) silver ion (D) nothing (it wasn’t a redox reaction) 59. During the “ornament lab,” hydrogen gas was produced according to the following equation: Zn + 2 HCl ZnCl2 + H2 Which chemical was oxidized? (A) H2 (B) HCl (C) Zn (D) ZnCl2 60. What mass of sulfur dioxide, SO2 (64.0 g/mole), is produced when 245 g of sulfuric acid, H2SO4 (98.0 g/mole) reacts completely with zinc metal according to the balanced equation below? Zn + 2 H2SO4 ZnSO4 + SO2 + 2 H2O (A) 64.0 g (B) 80.0 g (C) 128 g (D) 160 g South Pasadena • Honors Chemistry Name Semester 1 Final Exam Period PART B Date SHORT ANSWER • (PRACTICE) Only answers will be graded. Unless otherwise stated, no partial credit will be awarded with the work. Numerical answers should be reported with the correct number of significant digits and with appropriate units. 1. 1 2 3 The length and width of a rectangular sheet of aluminum foil are measured as shown. Record the dimensions of the foil with correct number of significant figures. 4 1 2 3 4 5 cm 5 cm 2. Chlorine naturally exists in two isotopes: Cl-35 (isotopic mass 34.9689 amu) and Cl-37 (36.9659 amu). If chlorine has a molar mass of 35.453 g/mol, find the % abundance of each isotope. Abundance of Cl-35: Abundance of Cl-37: 3. 4. Name the following compounds. NH4ClO3 CuO H3PO3 IF7 A 12.3 g sample of a gas occupies 6.28 L at STP. Find the number of molecules in this sample. (Show your work using dimensional analysis.) Find the molar mass of this gas. (Show work here.) 5. Convert the density of copper, 8.96 g/cm3, to lb/in3. (Show your work using dimensional analysis.) [1 kg = 2.2046 lb, 1 in = 2.54 cm] 6. 7. Draw two isomers for C3H6I2. Draw two isomers for C2H2Cl2. 8. Identify the functional groups in the compound MMDA. 9. Write the structural formulas for the products when the following compounds are combined: Structure: Name: Structure: Name: Structure: Name: Structure: Name: H H H C C C C H 10. C C O H O H H C O H Consider a solution in which pH [OH–] = 6.5 × 10–7 M. Find its pH, pOH, and [H+], and determine whether the [H+] solution is acidic, basic, or neutral. pOH Acidic/Basic/Neutral 11. Write the balanced equations for the following reactions. States are not required. Propanol (C3H7OH) is burned in air. A sample of solid aluminum oxide is strongly heated. 12. Write the balanced equations for the following reactions. States are not required. Aluminum metal is placed in a solution of cupric chloride. Solid ammonium acetate is placed in water. Useful Formulas and Constants 1 mole = 6.022 × 1023 particles = 22.4 L gas at STP K = °C + 273 m D=V m Molar Mass = n n M=V Mc · V c = Md · V d [H+][OH–] = 1.0 × 10–14 pH + pOH = 14 pH = – log [H+] pOH = – log [OH–] Solubility Rules for Salts Always soluble: alkali ions, NH4+, NO3−, ClO3−, ClO4−, C2H3O2−, HCO3− Generally soluble: Cl−, Br−, I− Soluble except with Ag+, Pb2+, Hg22+ F− Soluble except with Pb2+, Ca2+, Ba2+, Sr2+, Mg2+ 2− SO4 Soluble except with Pb2+, Ca2+, Ba2+, Sr2+ Generally insoluble: O2−, OH− Insoluble except with Ca2+, Ba2+, Sr2+, alkali ions, NH4+ CO32−, PO43−, S2−, SO32−, CrO42−, C2O42− Insoluble except with alkali ions and NH4+ Strong Acids HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4, HIO4 Strong Bases LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 Gases that Form H2S (g) H2CO3 (aq) CO2 (g) + H2O (ℓ) H2SO3 (aq) SO2 (g) + H2O (ℓ) NH4OH (aq) NH3 (g) + H2O (ℓ) South Pasadena • Honors Chemistry Name Semester 1 Final Exam Period PART C • Date FREE RESPONSE (PRACTICE) For each question, write your response in the space provided. If the problem requires mathematical computation, show your work (steps) neatly, reporting your answer with the correct number of significant digits and units. Partial credit is given only when the process taken is clearly shown. Place a box around or circle your final answer. Unit conversions should be shown using dimensional analysis, showing how all units cancel out. Work for problems involving formulas should follow the I.E.S.A. form. 1. A particular compound containing only chlorine and oxygen is 52.56% chlorine by mass. The molar mass of the compound is found to be between 60 and 70 g/mol. a. Find the empirical formula for this compound. (4 points) b. Find the molecular formula for this compound. (2 points) 2. Samples of the HBr, Mg(OH)2, and NH3 are obtained. a. Complete the table for aqueous samples of each compound, predicting its color in cabbage juice and its conductivity with a light bulb, and writing its dissociation equation. (12 points) Compound (i) Cabbage Juice Color [red | green | purple] Conductivity [bright | dim | dark] Dissociation Equation HBr (ii) Mg(OH)2 (iii) NH3 b. How many mL of a 7.00 M HBr solution is required to prepare 250 mL of 0.140 M HBr? (4 points) c. The solubility of Mg(OH)2 at 20°C is 0.0014 g/100 g water. How many grams of water are needed to dissolve 0.0112 g Mg(OH)2? (2 points) 3. Consider the following balanced reaction for the combustion of isopropyl alcohol, or 2-propanol, C3H8O (ℓ) 2 C3H8O (ℓ) + 9 O2 (g) → 6 CO2 (g) + 8 H2O (ℓ) a. 4.05 g C3H8O is burned in air. i. What volume (in L) of CO2 at STP can be produced? (4 points) ii. If 4.25 L of CO2 was actually produced above, what was the percent yield of CO2? (2 points) b. Suppose 50.0 g C3H8O and 50.0 g O2 are combined? i. What is the theoretical yield of H2O in grams? (4 points) ii. Identify the limiting and excess reactants. (2 points) iii. How much (in grams) of the excess reactant remains if the reaction goes to completion? (4 points)