Name Midterm Review Date 1. In which process does a solid change directly into a vapor? A) sublimation B) deposition C) condensation D) solidification 2. What is the molecular formula of a compound that has a molecular mass of 54 and the empirical formula C2H3? A) C4H6 B) C2H3 C) C8H12 D) C6H9 3. Two substances, A and Z, are to be identified. Substance A can not be broken down by a chemical change. Substance Z can be broken down by a chemical change. What can be concluded about these substances? A) Substance A is a compound and substance Z is an element. B) Both substances are compounds. C) Both substances are elements. D) Substance A is an element and substance Z is a compound. 4. The element in Group 14, Period 3 on the Periodic Table is classified as a A) nonmetal B) metalloid C) metal D) noble gas 5. In which compound is the percent composition by mass of chlorine equal to 42%? A) HClO4 (gram-formula mass = 100. g/mol) B) HClO3 (gram-formula mass = 84 g/mol) C) HClO2 (gram-formula mass = 68 g/mol) D) HClO (gram-formula mass = 52 g/mol) 6. Which particles are found in the nucleus of an atom? A) electrons, only B) protons and electrons C) neutrons, only D) protons and neutrons 7. Given the particle diagram representing four molecules of a substance: Which particle diagram best represents this same substance after a physical change has taken place? A) B) C) D) 8. A mixture of crystals of salt and sugar is added to water and stirred until all solids have dissolved. Which statement best describes the resulting mixture? A) The mixture is homogeneous and can be B) The mixture is homogeneous and cannot be C) The mixture is heterogeneous and can be D) The mixture is heterogeneous and cannot be
9. Which must be a mixture of substances? A) liquid B) gas C) solid D) solution 10. A sample of an element has a mass of 34.261 grams and a volume of 3.8 cubic centimeters. To which number of significant figures should the calculated density of the sample be expressed? A) 3 B) 2 C) 4 D) 5 11. Which of these elements has an atom with the most stable outer electron configuration? A) Cl B) Ca C) Ne D) Na 12. What is the chemical formula for copper(ii) hydroxide? A) Cu(OH)2 B) CuOH C) Cu2(OH) D) CuOH2 13. A sample of a gas is contained in a closed rigid cylinder. According to kinetic molecular theory, what occurs when the gas inside the cylinder is heated? A) The number of gas molecules increases. B) The number of collisions between gas molecules per unit time decreases. C) The volume of the gas decreases. D) The average velocity of the gas molecules increases. 14. A sample of helium gas has a volume of 900. milliliters and a pressure of 2.50 atm at 298 K. What is the new pressure when the temperature is changed to 336 K and the volume is decreased to 450. milliliters? A) 0.177 atm B) 5.64 atm C) 14.1 atm D) 4.43 atm 15. Which element is a noble gas? A) krypton B) chlorine C) manganese D) antimony 16. What is the chemical formula for sodium sulfate? A) NaSO4 B) Na2SO4 C) NaSO3 D) Na2SO3 17. Which conclusion is based on the gold foil experiment and the resulting model of the atom? A) An atom is mainly empty space, and the nucleus has a negative charge. B) An atom has hardly any empty space, and the nucleus has a negative charge. C) An atom is mainly empty space, and the nucleus has a positive charge. D) An atom has hardly any empty space, and the nucleus has a positive charge. 18. Which element is an alkali metal? A) sodium B) calcium C) hydrogen D) zinc 19. Which element has chemical properties that are most similar to those of calcium? A) N B) Sr C) K D) Co 20. Which mass measurement contains four significant figures? A) 0.431 g B) 0.086 g C) 1003 g D) 3870 g 21. Which trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom? A) Their metallic properties increase and their atomic radii decrease. B) Their metallic properties increase and their atomic radii increase. C) Their metallic properties decrease and their atomic radii increase. D) Their metallic properties decrease and their atomic radii decrease. 22. Which list consists of types of chemical formulas? A) empirical, molecular, structural B) synthesis, decomposition, neutralization C) atoms, ions, molecules D) metals, nonmetals, metalloids 23. A correct name for N2O3 is A) nitrogen (I) oxide B) nitrogen (II) oxide C) nitrogen (III) oxide D) nitrogen (IV) oxide
24. Which symbol represents a particle that has the same total number of electrons as S 2? A) Ar B) O 2 C) Si D) Se 2 25. What is the mass number of an atom that has six protons, six electrons, and eight neutrons? A) 6 B) 14 C) 12 D) 20 26. If 4.00 moles of oxygen gas, 3.00 moles of hydrogen gas, and 1.00 mole of nitrogen gas are combined in a closed container at standard pressure, what is the partial pressure exerted by the hydrogen gas? A) 1.00 atm B) 0.125 atm C) 3.00 atm D) 0.375 atm 27. During a laboratory activity to investigate reaction rate, a student reacts 1.0-gram samples of solid zinc with 10.0-milliliter samples of HCl(aq). The table below shows information about the variables in five experiments the student performed. Which two experiments can be used to investigate the effect of the concentration of HCl(aq) on the reaction rate? A) 1 and 3 B) 4 and 3 C) 1 and 5 D) 4 and 2 28. The average kinetic energy of water molecules is greatest in which of these samples? A) 100 g of water at 45 C B) 100 g of water at 25 C C) 10 g of water at 55 C D) 10 g of water at 35 C 29. Which trends are observed when the elements in Period 3 on the Periodic Table are considered in order of increasing atomic number? A) The atomic radius decreases, and the first ionization energy generally decreases. B) The atomic radius decreases, and the first ionization energy generally increases. C) The atomic radius increases, and the first ionization energy generally increases. D) The atomic radius increases, and the first ionization energy generally decreases. 30. A metal, M, forms an oxide compound with the general formula M2O. In which group on the Periodic Table could metal M be found? A) Group 2 B) Group 1 C) Group 16 D) Group 17 31. What is the empirical formula of a compound that contains 28% iron, 24% sulfur, and 48% oxygen by mass? A) FeSO3 B) Fe2(SO3)3 C) Fe2(SO4)3 D) FeSO4 32. Which statement concerning elements is true? A) Different elements must have different numbers of isotopes. B) All atoms of a given element must have the same mass number. C) All atoms of a given element must have the same atomic number. D) Different elements must have different numbers of neutrons. 33. What occurs when an atom of chlorine and an atom of hydrogen become a molecule of hydrogen chloride? A) A chemical bond is broken and energy is released. B) A chemical bond is formed and energy is absorbed. C) A chemical bond is broken and energy is absorbed. D) A chemical bond is formed and energy is released.
34. Which compound forms a green aqueous solution? A) RbCl B) NiCl2 C) ZnCl2 D) CaCl2 35. The temperature of a sample of a substance changes from 10. C to 20. C. How many Kelvin does the temperature change? A) 20. B) 10. C) 283 D) 293 36. Which element forms an ion that is larger than its atom? A) aluminum B) sodium C) magnesium D) chlorine 37. Which properties are most common in nonmetals? A) low ionization energy and high B) high ionization energy and high C) high ionization energy and low D) low ionization energy and low 38. Which group contains elements composed of diatomic molecules at STP? A) 11 B) 2 C) 7 D) 17 39. Which process is a chemical change? A) decomposing of water B) subliming of ice C) melting of ice D) boiling of water 40. The gram formula mass of NH4Cl is A) 22.4 g/mole B) 28.0 g/mole C) 53.5 g/mole D) 95.5 g/mole 41. Which phase change results in the release of energy? A) H2O( ) H2O(g) B) H2O(s) H2O(g) C) H2O(s) H2O( ) D) H2O(g) H2O( ) 42. How many electrons are in the outermost principal energy level (shell) of an atom of carbon in the ground state? A) 6 B) 2 C) 3 D) 4 43. Which set of procedures and observations indicates a chemical change? A) Ethanol is added to an empty beaker and the ethanol eventually disappears. B) Large crystals are crushed with a mortar and pestle and become powder. C) A solid is gently heated in a crucible and the solid slowly turns to liquid. D) A cool, shiny metal is added to water in a beaker and rapid bubbling occurs. 44. What is the total number of oxygen atoms in the formula MgSO4 7 H2O? [The represents seven units of H2O attached to one unit of MgSO4.] A) 11 B) 7 C) 5 D) 4 45. The temperature of a sample of water changes from 10. C to 20. C when the water absorbs 420 Joules of heat. What is the mass of the sample? A) 1.0 g B) 10. g C) 100 g D) 1000 g 46. Which notation represents an atom of sodium with an atomic number of 11 and a mass number of 24? 47. Based on bond type, which compound has the highest melting point? A) C6H14 B) CaCl2 C) CH3OH D) CCl4
48. A student investigated the physical and chemical properties of a sample of an unknown gas and then identified the gas. Which statement represents a conclusion rather than an experimental observation? A) When placed in the gas, a flaming splint stops burning. B) When the gas is bubbled into limewater, the liquid becomes cloudy. C) The gas is carbon dioxide. D) The gas is colorless. 49. A student calculated the percent by mass of water in a sample of to be, but the accepted value is. What was the student's percent error? 50. What is the formula of titanium(ii) oxide? A) TiO2 B) TiO C) Ti2O3 D) Ti2O 51. Which Lewis electron-dot diagram is correct for a S 2 ion? 54. In comparison to an atom of in the ground state, an atom of in the ground state has A) three more valence electrons B) three more neutrons C) three fewer valence electrons D) three fewer neutrons 55. The molecular formula of glucose is C6H12O6. What is the empirical formula of glucose? A) CH2O B) C12H24O12 C) CHO D) C6H12O6 56. A sample of a compound contains 65.4 grams of zinc, 12.0 grams of carbon, and 48.0 grams of oxygen. What is the mole ratio of zinc to carbon to oxygen in this compound? A) 1:4:6 B) 1:1:2 C) 5:1:4 D) 1:1:3 57. Which diagram represents the nucleus of an atom of? 52. Under which conditions of temperature and pressure would helium behave most like an ideal gas? A) 50 K and 20 kpa B) 750 K and 600 kpa C) 50 K and 600 kpa D) 750 K and 20 kpa 53. When a quantity of electricity is converted to heat, the heat energy produced is measured in A) volts B) amperes C) degrees D) joules 58. The modern model of the atom is based on the work of A) one scientist over a short period of time B) many scientists over a long period of time C) many scientists over a short period of time D) one scientist over a long period of time 59. Which element is malleable and can conduct electricity in the solid phase? A) iodine B) phosphorus C) tin D) sulfur 60. What amount of heat is required to completely melt a 29.95-gram sample of H2O(s) at 0 C? A) 334 J B) 2260 J C) 1.00 10 4 J D) 1.00 10 3 J
61. Element X is a solid that is brittle, lacks luster,and has six valence electrons. In which group on the Periodic Table would element X be found? A) 16 B) 15 C) 1 D) 2 62. What is the total number of orbitals containing only one electron in an atom of nitrogen in the ground state? A) 1 B) 2 C) 3 D) 4 63. A gas occupies a volume of 444 ml at 273 K and 79.0 kpa. What is the final kelvin temperature when the volume of the gas is changed to 1880 ml and the pressure is changed to 38.7 kpa? A) 31.5 K B) 2360 K C) 566 K D) 292 K Midterm Review 64. The data table below gives the temperature and pressure of four different gas samples, each in a 2-liter container. Which two gas samples contain the same total number of particles? A) CH4 and CO2 B) He and Ne C) CH4 and Ne D) He and CO2
65. Which substance contains bonds that involved the transfer of electrons from one atom to another? 67. The diagram below represents a Celsius thermometer recording a certain temperature. A) KBr B) CO2 C) NH3 D) Cl2 66. The graph below represents the uniform heating of a substance, starting below its melting point, when the substance is solid. Which line segments represent an increase in average kinetic energy? A) and B) and C) and D) and What is the correct reading of the thermometer? A) 5 C B) 4.3 C C) 0.3 C D) 4 C 68. Which is a binary compound? A) MgSO4 B) KOH C) NaNO3 D) CaCl2 69. A compound is made up of iron and oxygen, only. The ratio of iron ions to oxide ions is 2:3 in this compound. The IUPAC name for this compound is A) iron(ii) oxide B) iron(iii) oxide C) iron trioxide D) triiron dioxide 70. Which quantity of heat is equal to 200. joules? A) 20.0 kj B) 2.00 kj C) 0.200 kj D) 0.0200 kj