Chapter 6 and 7 Practice MC

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Preston Harper
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1 Chapter 6 and 7 Practice MC MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Ammonium fluoride is considered which of the following? 1) A) molecular compound B) ionic compound C) atomic element D) molecular element 2) Which molecule listed below is a polar molecule? 2) A) NH3 B) HCN C) H2O D) all of the compounds E) none of the compounds 3) Oxidation typically involves: 3) A) the gain of electrons. B) the loss of oxygen. C) the loss of electrons. D) the gain of water. 4) A 15.5 gram sample of diphosphorous pentoxide contains how many grams of phosphorous? 4) A) 6.76 B) 13.5 C) 3.38 D) ) Which of the following statements are TRUE about the BF3 molecule? 5) A) BF3 has a trigonal planar molecular geometry. B) BF3 is nonpolar. C) BF3 violates the octet rule for the central atom. D) All of the above statements are true. E) None of the above are true. 6) How many moles of Cu are in Cu atoms? 6) A) B) C) D)

2 7) Which of the following is an example of a combination reaction? 7) A) 2 Na + Cl2 2NaCl B) Mg + HCl H2 + MgCl2 C) KClO3 KCl + O2 D) HCl + NaOH NaCl + H2O 8) Carbon monoxide is considered which of the following? 8) A) molecular element B) atomic element C) ionic compound D) molecular compound 9) Reduction typically involves: 9) A) the gain of electrons. B) the gain of oxygen. C) the loss of electrons. D) the gain of water. 10) What is the molecular geometry if you have a double bond, a single bond and 1 lone pair around the central atom? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information 11) What is the molecular geometry if you have 3 single bonds and 1 lone pair around the central atom? A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information 10) 11) 12) The charge of a vanadium ion in the compound V2O5 is: 12) A) 2+ B) 10- C) 5+ D) ) Determine the theoretical yield of C when 3 units of A and 10 units of B are reacted in the following generic chemical equation: 2A + 5B 4C. A) 8 B) 3 C) 6 D) 4 13) 2

3 14) Nonpolar molecules may exhibit. 14) A) hydrogen bonding B) dipolar forces C) London forces D) all of the above 15) One mole of oxygen gas has a mass of g. 15) A) 32.0 B) 16.0 C) 8 D) ) Which of the following reactions is a single replacement reaction? 16) A) KClO3 KCl + O2 B) HCl + NaOH NaCl + H2O C) CaCl2 + H2O CaCl2 2H2O D) Mg + HCl H2 + MgCl2 17) Which of the following reactions is a double replacement reaction? 17) A) KClO3 KCl + O2 B) CaC12 + H2O CaCl2 2H2O C) Mg + HCl H2 + MgCl2 D) HCl + NaOH NaCl + H2O 18) Any reaction that absorbs 150 kilojoules of energy can be classified as 18) A) exothermic. B) activated. C) oxidation. D) reduction. E) endothermic. 19) In comparing a balloon containing 25 grams of helium to a balloon containing 25 grams of neon, which one of the following statements is TRUE? A) The neon balloon has more atoms. B) Each balloon has an equal number of atoms. C) This scenario cannot happen because gases have no mass. D) The helium balloon has more atoms. 19) 20) The name trisodium phosphate is incorrect for the compound Na3PO4 because: 20) A) this compound should be called trisodium monophosphate. B) the sodium has a negative 3 charge. C) you cannot use a prefix for the first element of an ionic compound. D) you cannot use a prefix for the first element in a molecular compound. 21) The electronegativity value for Mg is 1.2 and the value for O is 3.5. Based on these values, what type of bond is expected for a compound formed between Mg and O? A) ionic B) polar covalent C) pure covalent D) not enough information 21) 3

4 22) Which formula shown is incorrect for the name given? 22) A) magnesium nitrite: Mg(NO2)3 B) sodium hydrogen carbonate: NaHCO3 C) calcium carbonate: CaCO3 D) potassium hydroxide: KOH E) aluminum sulfate: Al2(SO4)3 23) Which molecule listed below is a nonpolar molecule? 23) A) CO2 B) CCl4 C) BH3 D) all of the compounds E) none of the compounds 24) What is the correct formula for potassium dichromate? 24) A) K2Cr2O7 B) KCr2O7 C) K2CrO4 D) K(CrO4)2 25) What are the coefficients for the following reaction when it is properly balanced? 25) potassium iodide + lead (II) acetate lead (II) iodide + potassium acetate A) 3, 2, 2, 1 B) 2, 1, 1, 1 C) 1, 1, 2, 2 D) 2, 1, 1, 2 26) A reaction that releases energy as it occurs is classified as a(n) 26) A) exothermic reaction. B) oxidation-reduction reaction. C) endothermic reaction. D) catalyzed reaction. E) decomposition reaction. 27) The strongest interactions between molecules of hydrogen chloride are 27) A) dipole-dipole interactions. B) dispersion forces. C) covalent bonds. D) hydrogen bonds. E) ionic bonds. 4

5 28) The electronegativity value for N is 3.0 and that for O is 3.5. Based on these values, which of the following statements is TRUE about the compound NO? A) NO is a pure covalent compound. B) NO is an ionic compound. C) NO is a polar covalent compound. D) There is not enough enough information to determine the nature of NO. E) None of the above statements is true. 28) 29) Which of the following statements is FALSE? 29) Actual Yield A) The percent yield = Theoretical Yield 100%. B) The limiting reactant is completely consumed in a chemical reaction. C) The theoretical yield is the amount of product that can be made based on the amount of limiting reagent. D) The actual yield is the amount of product actually produced by a chemical reaction. E) All of the above are true statements. 30) What is the sum of all coefficients after the following equation is balanced? K2CrO4 + Al(NO3)3 Al2(Cr O4)3 + KNO3 A) 15 B) 8 C) 12 D) 4 30) 31) How many atoms are in 1.50 moles of fluorine gas? 31) A) B) C) D) ) How many moles of H2 can be made from complete reaction of 3.0 moles of Al? Given: 2 Al + 6 HCl 2 AlCl3 + 3 H2 A) 3.0 moles B) 9.0 moles C) 3 moles D) 4.5 moles 32) 33) What is the molar mass of aluminum sulfate? 33) A) g/mol B) g/mol C) g/mol D) g/mol E) g/mol 34) Which among the following elements does NOT exist as a diatomic molecule in nature? 34) A) neon B) hydrogen C) fluorine D) nitrogen 5

6 35) Which of the following chemical substances would you expect to exhibit hydrogen bonding? 35) A) NH3 B) HF C) CH3OH D) all of the above 36) Which of the following reactions is a decomposition reaction? 36) A) CaCl2 + H2O CaCl2 2H2O B) KClO3 KCl + O2 C) HCl + NaOH NaCl + H2O D) Mg + HCl H2 + MgCl2 37) What would the formula of diiodine pentasulfide be? 37) A) I2S7 B) I5S2 C) I4S9 D) I2S5 38) How many atoms are in 15.6 grams of silicon? 38) A) B) C) D) ) The theoretical yield of a reaction is 75.0 grams of product and the actual yield is 42.0g. What is the percent yield? A) 178 B) 56.0 C) 75.0 D) ) 40) What is the molecular geometry of SCl2? 40) A) bent B) linear C) tetrahedral D) trigonal pyramidal E) not enough information 6

7 Answer Key Testname: CH 6 & 7 PRACTICE MC 1) B 2) D 3) C 4) A 5) D 6) D 7) A 8) D 9) A 10) A 11) D 12) C 13) C 14) C 15) A 16) D 17) D 18) E 19) D 20) C 21) A 22) A 23) D 24) A 25) D 26) A 27) A 28) C 29) E 30) C 31) A 32) D 33) B 34) A 35) D 36) B 37) D 38) C 39) B 40) A 7

Honors Chemistry Semester 2 Final Exam MC Practice

Honors Chemistry Semester 2 Final Exam MC Practice Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1. What do the alkali metals all have in common?