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Review Multiple Choice Questions Chapter 2 – Matter and Changes 1. The random molecular motion of a substance is greatest when the substance is a. condensed b. a liquid c. frozen d. a gas 2. After elements A & B react to completion in a closed container, the ratio of masses of A and B in the container will be the same as before the reaction. This is true because of the law of a. definite proportion b. multiple proportions c. conservation of mass d. conservation of energy 3. Which one of the following is not a PHYSICAL change? a. ice melting b. salt dissolving in water c. iron rusting d. a rock being crushed 4. Which of the following is not a chemical reaction? a. dissolving salt in water b. fading of a black sweater by sunlight
c. combustion of wood in a fireplace d. curdling of milk.
5. When atoms of a substance are geometrically arranged in a predictable, non-random pattern, the substance is a: a. gas b. liquid c. solid d. plasma 6. All of the following are physical properties of sucrose EXCEPT: a. forms solid crystals are room temp b. appears as white crystals
c. breaks down into C and H2O(g) when heated d. tastes sweet
Chapter 4 – Atomic Structure 7. Which is the following is the correct ranking of increasing size of the following examples of sodium: atom, ion, nucleus, proton, neutron and electron. (The first is the smallest, the last is the largest.) a. Ion, atom, proton, neutron, electron, nucleus b. Nucleus, proton, neutron, electron, atom, ion. c. Electron, neutron, proton, nucleus, atom, ion. d. Electron, neutron, proton, nucleus, ion, atom. e. Neutron, electron, proton, nucleus, atom, ion. 8. An atom has no net electrical charge because a. its subatomic particles carry no electrical charges b. the positively charged protons cancel out the negatively charged neutrons. c. The positively charged neutrons cancel out the negatively charged electrons. d. The positively charged protons cancel out the negatively charged electrons. 9. In the reaction 49 Be + X Æ 126 C + 01 n , the X represents a. an alpha particle b. a beta particle c. an electron
d. a proton
10. When an atom emits a ß-particle from its nucleus the resulting nucleus contains a. one less proton and one more neutron b. one more proton and one more neutron c. one less proton and the same number of neutrons d. one more proton and one less neutron 11. How many total electrons does Cl- have? a. 17 b. 18 c. 16
12. Which of the following is a product of α decay of 238 92 U ? a.
Chapter 5 - Electrons in Atoms 13. Which of the following atoms has six valence electrons? a. Magnesium b. Silicon c. Sulfur d. Argon 14. Using noble gas notation, the ground state electrons configuration for Cd is a. [Kr]4d104f2 b. [Ar]4s23d10 c. [Kr]5s24d10 d. [Xe]5s24d10 15. The complete electron configuration of a scandium atom is a. 1s22s22p63s23p64s23d1 b. 1s22s22p73s23p74s23d1 c. 1s22s22p53s23p54s23d1 d. 1s22s12p73s13p74s23d1 16. How many valance electrons does Zr have? a. 2
17. Which of the following is the electron configuration for Mn? a. [He] 2s2 2p3
b. [Ar] 4s2 3d5
c. [Ne] 3s2
d. [Ar] 4s2 3d8
18. What element has the electron configuration: 1s22s22p63s23p64s23d104p65s24d105p4? a. Se
19. Which of the following elements has the same Lewis dot structure as silicon a. Germanium b. Aluminum c. Arsenic d. Gallium
Chapter 6 - The Periodic Table 20. Two different elements are located in different portions of the periodic table. Element A is on the far upper left side (not Hydrogen); element B is a halogen. Which statement(s) is/are true? a. Element A is a metal and B is a non-metal. b. The combination of A & B results in an ionic compound. c. Element A has a smaller atomic number than element B. d. Element B has fewer valence electrons than A. e. Element A is an alkali earth metal. 21. Which of the following are incorrectly paired? a. Na, alkali metal b. Mg, alkaline earth metal c. Br, halogen d. Ar, noble gas e. Sn, transition metal 22. Consider the following orderings. Al < Si < P < Cl Be < Mg < Ca < Sr I < Br < Cl < F Which of these give(s) a correct trend in ionization energy? a. III b. I, II c. I d. I, III
e. none of them
23. Which of the following statements is false? a. b. c. d. e.
A sodium atom has a smaller radius than a potassium atom. A neon atom has a smaller radius than an oxygen atom. A fluorine atom has a smaller first ionization energy than an oxygen atom. A cesium atom has a smaller first ionization energy than a helium atom. All are true.
24. The elements of group 2 a. Are in the same horizontal row of the periodic table b. Are generally different in their chemical reactivity c. Have different number of valance electrons d. Are generally similar in their chemical and physical properties e. Have different outer electron configurations 25. Arrange the following elements in order of increasing atomic radii: K, Na, Mg, Cs, Cl a. Na, Mg, Cl, K, Cs b. Cl, Mg, Na, K, Cs c. Cs, K, Cl, Mg, Na d. Cl, Mg, Cs, K, Na e. Cl, Mg, Na, Cs, K 26. Which of the following is INCORRECTLY classified? a. Se / metal
b. Cr / metal
c. Ag / metal
d. Si / metalloid e. C / nonmetal
Chapter 7 & 9 - Ionic Compounds 27. The anion in AlPO4 has a charge of a. 2+ b. 3+ c. 2d. 3e. cannot determine without more information. 28. Which of the following pairs is incorrect? a. NH4Br, ammonium bromide b. K2CO3, potassium carbonate c. BaPO4, barium phosphate d. CuCl, copper (I) chloride e. MgO, magnesium oxide 29. A compound in which the nitrate to metal ion ratio is 2:1 has the following formula? a. M(NO3)2 b. M(NO3)4
30. When the calcium ion is combined with the sulfate ion, the following neutral compound is produced a. CaS
31. The combination of a positively charged metal to a negatively charged non-metal which results in a neutrally charged substance is a(n): a. polyatomic ion c. molecular compound b. monatomic ion d. ionic compound 32. The correct formula for iron (II) oxide is a. Fe2O3 b. IrO c. FeO
33. The correct formula for calcium phosphate is a. CaPO4 b. Ca(PO4) c. Ca3(PO4)2
34. Which of the following ion formulas is NOT correctly stated? a. NO3-1 b. CO23c. Fe3+ d. MnO4-1 35. Which of the following formulas for magnesium hydroxide is correctly written? c. MgOH2 d. Mg2OH a. Mg(OH)2 b. MgOH 36. Which of the following does not represent an ionic compound? a. LiNO3 b. MgO c. KF d. CO2 Chapter 8 & 9 - Covalent Bonding 37. The proper name for the molecular compound N2Cl5 is a. Dinitride pentachloride b. Dinitrogen pentachlorine c. Dinitride pentachlorine d. Dinitrogen pentatchloride e. Nitrogen chloride
38. Which of the following molecules contains a double bond? a. CO2
39. How many total lone pairs of electrons are on the molecule, NF3? a. 0
40. How many of the 6 valance electrons in sulfur are used in covalent bonding in sulfur tetrachloride and sulfur difluoride? a. 3 and 2
b. 6 and 1
c. 4 and 2
d. 2 and 2
Chapter 11 - Chemical Reactions 41. On a separate piece of paper, balance the following equation using the coefficient of 1 already given to Al4C3. C
Al2O3 Æ 1 Al4C3 +
In the correctly balanced equation, the coefficient of carbon, C, is a. 3 b. 6 c. 9 d. 12 42. On a separate piece of paper, balance the equation below and choose the correct coefficient. Pb(NO3)2 +
a. 2, 2, 1, 2 b. 1, 2, 2, 1
KNO3 + c. 1, 2, 1, 2
d. 2, 1, 2, 1
43. Which of the following displacement reactions will NOT occur? (use activity series) a. CuSO4(aq) + Zn(s) ---> Cu(s) + ZnSO4(aq) b. 2NaNO3(aq) + Zn(s) ---> 2Na(s) + Zn(NO3)2(aq) c .2AgNO2(aq) + Zn(s) ---> 2Ag(s) + Zn(NO3)2(aq) d. 2HCl(aq) + Zn(s) ---> H2(g) + ZnCl2(aq) Chapter 10- Chemical Quantities: The Mole 44. Two moles of (NH4)2S has a mass of a. 76 g
b. 100 gc. 136 g d. 2 x (6 x 1023) g
45. Which one of the following is NOT a valid CHEMICAL example of a mole? a. 6.02 x 1023 particles b. Avagadro’s number of particles
c. the number of atoms in 12.0 grams of carbon 12 d. a small, burrowing, gopher-like animal
46. How many moles of NaOH are in 10.0 grams of NaOH? Molar mass of NaOH = 40 g/mol a. 0.25 mol
c. 0.25 x 1023 mol
b. 400 mol
d. 1.5 x 1023 mol
47. How many molecules are present in 22.0 grams of CO2? (molar mass of CO2 = 44 g/mol) a. 0.5 molecules
b. 2.0 molecules
c. 3.0 x 1023 molecules
d. 2.0 x 1023 molecules
48. How many grams of CO2 are present in 0.20 moles of CO2? Molar mass = 44 g/mol a. 44 g
b. 8.8 g c. 220 g d. 4.4 g
Classify the chemical reactions in questions 49-55, using the following key: a. single displacement c. combustion b. double displacement d. synthesis
49. 2 Al + Fe3N2 → 2 AlN + 3Fe 50. 2 Na + Cl2 → NaCl 51. C7H8 + 9 O2 → 4 H2O + 7 CO2 52. 8 Ag2S → 16 Ag + 1 S8 53. 3 KBr + Fe(OH)3 → 3 KOH + FeBr3 54. 2 H2O2 → 2 H2O + O2 55. 3 ZnS + 2 AlP → Zn3P2 + Al2S3 Ch 12 - Stoichiometry 56. Given the following balanced equation, how many grams of aluminum oxide are formed from 13.5 g of aluminum? Molar mass: Al: 27.0, Al2O3 102 g/mol 4 Al + 3 O2 → 2 Al2O3 a. 7.25 g
b. 13.5 g
c. 25.5 g
d. 51.0 g
Questions 57-60 refer to the following: A lab experiment was run in which material X was reacted with material Y to produce material Z as shown in the below equation. A stoichiometry calculation showed that 50.0 g of Z should be produced, but in the lab only 45.0 g were obtained. 1X+1Y→1Z 57. The theoretical yield was a. 50.0 g
b. 45.0 g
c. 5.0 g
d. 95.0 g
58. The actual, or experimental yield was a. 50.0 g
b. 45.0 g
c. 5.0 g
d. 95.0 g
b. 95.0 %
c. more than 100 %
59. The % yield was a. 90.0 %
d. less than 50 %
60. The balanced equation for the reaction between zinc and sulfur is Zn + S → ZnS. The only statement below which is consistent between zinc and sulfur is: a. 1 mol Zn + 1 mol S → 2 mol ZnS c. 1 g Zn + 1 g S → 1 g ZnS b. 20 atoms Zn + 20 atoms S → 40 atoms of ZnS d. 65.4 g Zn + 32.0g S → 97.4 g ZnS Chapter 13/14 - Gases 61. Which of the following variables (amount, pressure, temperature, volume) have an indirect mathematical relationship? a. amount and volume b. volume and pressure
c. pressure and temperature d. temperature and volume
62. If a rigid container of oxygen is submerged in sixty feet of water, it does not crush. Which of the following is NOT correct? a. the pressure of the oxygen does not change b. the container exerts a pressure outward on the water c. the water pressure is nearly 2 atmospheres d. the oxygen molecules are closer together under water 63. 75 L of a gas at 27 atm will occupy what volume at 30 atm? a. 67.5 L
b. 83.3 L
c. 75 L d. 10.8 L
64. At 250 K a gas had a pressure of 0.853 atm. At what temperature would it be at 1.32 atm? a. 162 K