Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

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1 MYP hemistry Final Exam Review Practice Questions ( ) Multiple hoice Identify the letter of the choice that best completes the statement or answers the question. / 1. Which of the following is NOT one of the key characteristics of a true experiment? a. Holding everything constant apart from the variable being manipulated. b. ll participants experience all experimental conditions. c. The measurement of changes caused by the manipulation of a variable. d. The manipulation of a variable. 2. In an experiment, the variable that is manipulated is called the a. Independent variable. c. Independent variable. b. onfounding variable. d. ependent variable. 3. In an experiment, the variable that is being measured is referred to as the a. Measurement variable. c. ependent variable. b. Independent variable. d. onstant variable. 4. What is a hypothesis? a. The right answer to an experiment. c. The manipulation of a variable. b. n educated guess. d. Is determined after the experiment. 5. n experiment is performed on plants to see how different liquids affect plant growth. Each plant in the experiment is given a different liquid; water, apple juice, or milk. Each plant has the same amount of soil, same amount of sunlight, and the same amount of liquid. In this investigation, what is the independent variable? a. Type of plant. c. ifferent liquids. b. Plant growth. d. mount of sunlight. 6. What is the dependent variable in an experiment in which the mass of a ball affects the distance it rolls off a ramp? a. istance traveled by the ball. c. Height of the ramp. b. Mass of the ball. 7. Praise is typically used as a reward when training a dog. In order to determine the best way to train a do, an experiment was set up to find out if there is a better way to get a dog to respond to commands. What is the dependent variable in this experiment? a. Type of reward. c. Praise. b. Type of dog. d. mount of time the dog follows commands. 8. In a controlled experiment, the variable that is changed to test the hypothesis is called the a. ontrolled variable. c. Responsive variable. b. ependent variable. d. Independent variable. 9. Which of the following represents qualitative data? a. olor. c. ensity. b. Mass. d. Volume. 10. golf ball has more mass than a tennis ball because it a. Takes up more space. c. ontains different kinds of matter. b. ontains more matter. d. Has a definite composition. 11. n example of an extensive property of matter is a. Temperature. c. Mass. b. Pressure. d. Hardness.

2 12. Which of the following is a heterogeneous mixture? a. ir. c. Steel. b. Salt water. d. Soil. 13. substance that can be separated into two or more substances only by a chemical change is a(n) a. Solution. c. Mixture. b. Element. d. ompound. 14. The chemical symbol for iron is a. fe c. Fe b. FE d. Ir 15. Which of the following is a chemical property? a. olor. c. Freezing point. b. Hardness. d. bility to react with oxygen. 16. Which of the following is NOT a physical change? a. Grating cheese. c. Fermenting of cheese. b. Melting cheese. d. Mixing two cheeses in a bowl. 17. chemical change occurs when a piece of wood a. Is split. c. ecays. b. Is painted. d. Is cut. 18. When an iron nail is ground into powder, its mass a. Stays the same. c. Increases. b. ecreases. d. annot be determined. 19. The expression of 5008 km in scientific notation is a km c km b km d km 20. The closeness of a measurement to its true value is a measure of its a. Precision. c. Reproducibility. b. ccuracy. d. Usefulness. 21. What is the density of an object having a mass of 8.0 g and a volume of 25 cm? a g/cm c. 3.1 g/cm b. 2.0 g/cm d. 200 g/cm 22. The smallest particle of an element that retains the properties of that element is a(n) a. tom. c. Proton. b. Electron. d. Neutron. 23. Which of the following is true about subatomic particles? a. Electrons are negatively charged and are the heaviest subatomic particle. b. Protons are positively charged and the lightest subatomic particle. c. Neutrons have no charge and are the lightest subatomic particle. d. The mass of a neutron nearly equals the mass of a proton. 24. The particles that are found in the nucleus of an atom are a. Neutrons and electrons. c. Protons and neutrons. b. Electrons only. d. Protons and electrons.

3 25. s a consequence of discovery of the nucleus by Rutherford, which model of the atom is thought to be true? a. Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom. b. The nucleus is made of protons, electrons, and neutrons. c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom. d. The nucleus is made of electrons and protons. 26. The nucleus of an atom is a. The central core and is composed of protons and neutrons. b. Positively charged and has more protons than neutrons. c. Negatively charged and has a high density. d. Negatively charged and has a low density. 27. The atomic number of an element is the total number of which particles in the nucleus? a. Neutrons. c. Electrons. b. Protons. d. Protons and electrons. 28. n element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are a. 152 protons and 76 electrons c. 38 protons and 38 electrons b. 76 protons and 0 electrons d. 76 protons and 76 electrons 29. The sum of the protons and neutrons in an atom equals the a. tomic number. c. tomic mass. b. Nucleus number. d. Mass number. 30. What does the number 84 in the name krypton-84 represent? a. The atomic number. c. The sum of the protons and electrons. b. The mass number. d. Twice the number of protons. 31. ll atoms of the same element have the same a. Number of neutrons. c. Mass numbers. b. Number of protons. d. Mass. 32. Isotopes of the same element have different a. Numbers of neutrons. c. Numbers of electrons. b. Numbers of protons. d. tomic numbers. 33. Which of the following sets of symbols represents isotopes of the same element? a. J J J c. M M M b. L L L d. Q Q Q 34. In which of the following is the number of neutrons correctly represented? a. F has 0 neutrons. c. Mg has 24 neutrons. b. s has 108 neutrons. 35. What unit is used to measure weighted average atomic mass? a. mu. c. ngstrom. b. Gram. d. Nanogram. 36. In the ohr model of the atom, an electron in an orbit has a fixed a. Position. c. Energy. b. olor. d. Size. d. U has 146 neutrons.

4 37. How does the energy of an electron change when the electron moves closer to the nucleus? a. It decreases. c. It stays the same. b. It increases. d. It doubles. 38. The average isotopic mass of chlorine is Which mixture of isotopes produces this average mass? a. 50% l-35 and 50% l-37. c. 75% l-35 and 25% l-37. b. 50% -12 and 50% -13. d. 75% -12 and 25% sample of element X contains 90% x-35 atoms, 8% x-37 atoms, and 2% x-38 atoms. The average isotopic mass is closest to a. 37 c. 38 b. 35 d What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p? a. 2d c. 3f b. 3d d. 4s 41. ccording to the aufbau principle a. n orbital may be occupied by only two electrons. b. Electrons in the same orbital must have opposite spins. c. Electrons enter orbitals of highest energy first. d. Electrons enter orbitals of lowest energy first. 42. What is the electron configuration of potassium? a. 1s 2s 2p 3s 3p 4s c. 1s 2s 3s 3p 3d b. 1s 2s 2p 3s 3p d. 1s 2s 2p 3s 3p 4s 43. [r] 4s 2 3d 2 is the noble gas notation for a. Scandium. c. Vanadium. b. Titanium. d. Zirconium. 44. [Kr] 5s 2 4d 10 is the noble gas notation for a. r c. t b. I d. d 45. How many unpaired electrons are in a sulfur atom (atomic number 16)? a. 0 c. 2 b. 1 d Which color of visible light has the shortest wavelength? a. Yellow. c. lue. b. Green. d. Violet. 47. Which of the following electromagnetic waves have the highest frequencies? a. Ultraviolet light waves. c. Microwaves. b. X-rays. d. Gamma rays. 48. How are the frequency and wavelength of light related? a. They are inversely proportional to each other. b. Frequency equals wavelength divided by the speed of light. c. Wavelength is determined by dividing frequency by the speed of light. d. They are directly proportional to each other.

5 49. Which scientist developed the quantum mechanical model of the atom? a. lbert Einstein. c. Niels ohr. b. Erwin Schrodinger. d. Ernest Rutherford. 50. Which of the following elements is in the same period as phosphorus? a. arbon. c. Nitrogen. b. Magnesium. d. Oxygen. 51. Each period in the periodic table corresponds to a. principal energy level. c. n orbital. b. n energy sublevel. d. suborbital. 52. The modern periodic table is arranged in order of increasing atomic a. Mass. c. Number. b. harge. d. Radius. 53. Of the elements Pt, V, Li, and Kr, which is a nonmetal? a. Pt c. Li b. V d. Kr 54. To what category of elements does an element belong if it is a poor conductor of electricity? a. Transition elements. c. Nonmetals. b. Metalloids. d. Metals. 55. What element has the electron configuration 1s 2s 2p 3s 3p? a. Nitrogen. c. Silicon. b. Selenium. d. Silver. 56. Which subatomic particle plays the greatest part in determining the properties of an element? a. Proton. c. Neutron. b. Electron. d. None of the above. 57. Which of the following elements is a transition metal? a. esium. c. Tellurium. b. opper. d. Tin. 58. How does atomic radius change from top to bottom in a group in the periodic table? a. It tends to decrease. c. It first increases, then decreases. b. It tends to increase. d. It first decreases, then increases. 59. How does atomic radius change from left to right across a period in the periodic table? a. It tends to decrease. c. It first increases, then decreases. b. It tends to increase. d. It first decreases, then increases. 60. What element in the second period has the largest atomic radius? a. arbon. c. Potassium. b. Lithium. d. Neon. 61. What is the charge of a cation? a. positive charge. b. No charge. c. negative charge. d. The charge depends on the size of the nucleus.

6 62. The metals in Groups 1, 2, and 3 a. Gain electrons when they form ions. c. ll have ions with a 1 charge. b. ll form ions with a negative charge. d. Lose electrons when they form ions. 63. What is the element with the lowest electronegativity value? a. esium. c. alcium. b. Helium. d. Fluorine. 64. What is the element with the highest electronegativity value? a. esium. c. alcium. b. Helium. d. Fluorine. 65. What is the energy required to remove an electron from an atom in the gaseous state called? a. Nuclear energy. c. Shielding energy. b. Ionization energy. d. Electronegative energy. 66. ompared with the electronegativities of the elements on the left side of a period, the electronegativities of the elements on the right side of the same period tend to be a. Lower. c. The same. b. Higher. d. Unpredictable. 67. Which of the following describes the net positive charge experience by valence electrons by the nucleus. a. Electronegativity. c. Ionization energy. b. tomic radius. d. Effective nuclear charge. 68. How many valence electrons are in an atom of phosphorus? a. 2 c. 4 b. 3 d What is the electron configuration of the gallium ion? a. 1s 2s 2p 3s 3p c. 1s 2s 2p 3s 3p 4s 4p b. 1s 2s 2p 3s 3p 4s d. 1s 2s 2p 3s 3p 3d 70. The octet rule states that, in chemical compounds, atoms tend to have a. The electron configuration of a noble gas. b. More protons than electrons. c. Eight electrons in their principal energy level. d. More electrons than protons. 71. compound held together by ionic bonds is also called a a. iatomic molecule. c. ovalent molecule. b. Polar compound. d. Salt. 72. What is the formula unit of aluminum oxide? a. lo c. lo b. l O d. l O 73. Which of these elements does not exist as a diatomic molecule? a. Ne c. H b. F d. I

7 74. Which of the following is the name given to the pairs of valence electrons that do not participate in bonding in diatomic oxygen molecules? a. Unvalenced pair. c. Inner pair. b. Outer pair. d. Unshared pair. 75. Which of the following diatomic molecules is joined by a double covalent bond? a. c. b. d. 76. bond formed between a silicon atom and an oxygen atom is likely to be a. Ionic. c. Polar covalent. b. oordinate covalent. d. Nonpolar covalent. 77. Which of the following covalent bonds is the most polar? a. H F c. H H b. H d. H N 78. What type of ions have names ending in -ide? a. Only cations. c. Only metal ions. b. Only anions. d. Only gaseous ions. 79. When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a a. Prefix. c. Roman numeral following the name. b. Suffix. d. Superscript after the name. 80. n -ate or -ite at the end of a compound name usually indicates that the compound contains a. Fewer electrons than protons. c. Only two elements. b. Neutral molecules. d. polyatomic anion. 81. Which of the following compounds contains the Mn ion? a. MnS c. Mn O b. Mnr d. MnO 82. How are chemical formulas of binary ionic compounds generally written? a. ation on left, anion on right. b. nion on left, cation on right. c. Roman numeral first, then anion, then cation. d. Subscripts first, then ions. 83. Which of the following formulas represents an ionic compound? a. S c. N O b. ai d. Pl 84. Which element, when combined with fluorine, would most likely form an ionic compound? a. Lithium. c. Phosphorus. b. arbon. d. hlorine. 85. Which of the following compounds contains the lead(ii) ion? a. PbO c. Pb 2O b. Pbl 4 d. Pb 2S

8 86. What is the correct formula for potassium sulfite? a. KHSO c. K SO b. KHSO d. K SO 87. In naming a binary molecular compound, the number of atoms of each element present in the molecule is indicated by a. Roman numerals. c. Prefixes. b. Superscripts. d. Suffixes. 88. What SI unit is used to measure the number of representative particles in a substance? a. Kilogram. c. Kelvin. b. mpere. d. Mole. 89. vogadro's number of representative particles is equal to one a. Kilogram. c. Kelvin. b. Gram. d. Mole. 90. How many molecules are in 2.10 mol O? a molecules c molecules b molecules d molecules 91. What is the molar mass of (NH ) O? a. 144 g c. 96 g b. 138 g d. 78 g 92. What is the mass in grams of 5.90 mol H? a g c. 389 g b g d. 673 g 93. What is the number of moles in 432 g a(no )? a mol c mol b mol d mol 94. In the chemical equation H O (aq) H O(l) O (g), the is a a. atalyst. c. Product. b. Solid. d. Reactant. 95. What are the coefficients that will balance the skeleton equation below? ll + NaOH l(oh) Nal a. 1, 3, 1, 3 c. 1, 1, 1, 3 b. 3, 1, 3, 1 d. 1, 3, 3, When the equation Fe l Fel is balanced, what is the coefficient for l? a. 1 c. 3 b. 2 d hemical equations must be balanced to satisfy a. The law of definite proportions. c. The law of conservation of mass. b. The law of multiple proportions. d. vogadro s principle. 98. In every balanced chemical equation, each side of the equation has the same number of a. toms of each element. c. Moles. b. Molecules. d. oefficients.

9 99. What are the missing coefficients for the skeleton equation below? l (SO ) (aq) KOH(aq) l(oh) (aq) K SO (aq) a. 1, 3, 2, 3 c. 4, 6, 2, 3 b. 2, 12, 4, 6 d. 1, 6, 2, The type of reaction that takes place when one element reacts with a compound to form a new compound and a different element is a a. ombination reaction. c. Single-replacement reaction. b. ecomposition reaction. d. ouble-replacement reaction The type of reaction that forms carbon dioxide and water as products is a. ombustion reaction. c. Single-replacement reaction. b. ecomposition reaction. d. ouble-replacement reaction The type of reaction shown by, 2NaOH + al 2 a(oh) 2 + 2Nal a. ombination reaction. c. Single-replacement reaction. b. ecomposition reaction. d. ouble-replacement reaction Which of the following is a balanced equation representing the decomposition of lead(iv) oxide? a. PbO Pb 2O c. Pb O 2Pb O b. PbO Pb O d. PbO Pb O 104. If a combination reaction takes place between rubidium and bromine, the chemical formula for the product is.. a. Rur c. Rbr b. Rb r d. Rbr 105. The calculation of quantities in chemical equations is called a. Stoichiometry. c. Percent composition. b. imensional analysis. d. Percent yield Which of the following is not an indicator of a chemical reaction? a. hange in temperature. c. Increase in volume after combination. b. Formation of bubbles. d. Formation of a precipitate Which of the following defines the formation of a precipitate. a. Formation of a solid. c. hange in color. b. Formation of bubbles. d. hange in temperature How many moles of aluminum are needed to react completely with 1.2 mol of FeO? 2l(s) + 3FeO(s) 3Fe(s) + l O (s) a. 1.2 mol c. 1.6 mol b. 0.8 mol d. 2.4 mol 109. Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum? 2l(s) + 3H SO (aq) l (SO ) (aq) + 3H (g) a mol c mol b mol d mol 110. The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO is formed? a g c g b g d g

10 111. Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe O are formed when 16.7 g of Fe reacts completely with oxygen? a g c g b g d g 112. How many grams of chromium are needed to react with an excess of uso to produce 27.0 g u? 2r(s) + 3uSO (aq) r (SO ) (aq) + 3u(s) a g c g b g d g 113. The charge of magnesium in magnesium chloride is a. 1 c. +1 b. 0 d The charge of hydroxide in sodium hydroxide is a. 1 c. +1 b. 0 d The charge of aluminum in aluminum chloride is a. +3 c. -1 b. 0 d. +2 / 116. What term defines delocalized electrons within certain molecules where bonding cannot be expressed by a single Lewis structure? a. Lewis dot structure. c. Electron orbitals. b. ohr diagram. d. Resonance Which of the following compounds has a tetrahedral geometry? a. l 4 c. NH 3 b. SO 2 d. H 2O 118. Which of the following compounds has a bent geometry? a. l 4 c. NH 3 b. O 2 d. H 2O 119. Which of the following compounds has a trigonal pyramidal geometry? a. l 4 c. NH 3 b. SO 2 d. H 2O 120. Which of the following compounds has hydrogen bonds? a. H 2O c. H 4 b. NH 3 d. l Which of the following compounds has dispersion forces? a. H 2O c. H 4 b. NH 3 d. ll of the above Which of the following intermolecular forces are specific to polar molecules? a. Hydrogen bonds. c. The dark force. b. ipole-dipole interactions. d. ispersion forces.