End of Semester 1 Review

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1 Name: ate: 1. In the modern Periodic Table, the elements are arranged in order of increasing. atomic number. mass number. oxidation number. valence number 5. Which element within any given period of the Periodic Table would always have the lowest first ionization energy?. an alkali metal. a halogen. an alkaline earth metal. a noble gas 2. More than two-thirds of the elements are classified as. nonmetals. metals. metalloids. noble gases 6. Element X is in Group 2 (II) and element Y is in Group 17 (VII). compound formed between these two elements is most likely to have the formula 3. Which is the most active nonmetal in the Periodic Table of the Elements?. X 2 Y. XY 2. X 2 Y 7. X 7 Y 2. Na. F. I. l 4. Which element in Period 2 has the greatest tendency to form a negative ion?. lithium. carbon 7. In the ground state, how many electrons are in the outermost s sublevel of each element in Group VII? neon. fluorine page 1

2 8. erylium is classified as. an alkaline earth metal. an alkali metal. a transition metal 11. ll of the elements in Period 3 have a total of 2 electrons in the. 2s sublevel. 3s sublevel. 2p sublevel. 3p sublevel. a noble gas 12. Which element would have properties characteristic of both a metal and a nonmetal? 9. s the elements are considered from the top to the bottom of Group V, which sequence in properties occurs?. g. K. Si. Xe. metal metalloid nonmetal. metal nonmetal metalloid. metalloid metal nonmetal. nonmetal metalloid metal 13. The chemical properties of elements are periodic functions of their. ionic charges. oxidation states. atomic numbers. mass numbers 10. ll the elements in Period 3 have the same number of. occupied sublevels. principal energy levels. electrons. protons 14. Which characteristic describes most nonmetals in the solid phase?. good conductors of electricity. good conductors of heat. malleable. brittle page 2

3 15. Two basic properties of the gas phase are. a definite shape and a definite volume. a definite shape but no definite volume. no definite shape but a definite volume. no definite shape and no definite volume 18. Which is the electron configuration of a neutral atom in the ground state with a total of six valence electrons?. 1s 2 2s 2 2p 2. 1s 2 2s 2 2p 4. 1s 2 2s 2 2p 6. 1s 2 2s 2 2p 6 3s 2 3p Which list of particles is in order of increasing mass? 19. What is the total number of valence electrons in an atom with the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 3? proton electron alpha particle. proton alpha particle electron. electron proton alpha particle. alpha particle electron proton 20. The number of valence electrons in an atom with an electron configuration of 1s 2 2s 2 2p 6 3s 2 3p 4 is Which terms are used to identify pure substances?. an element and a mixture. an element and a compound. a solution and a mixture. a solution and a compound 21. What is the electron configuration for e 2+ ions?. 1s 1. 1s 2. 1s 2 2s 1. 1s 2 2s 2 page 3

4 22. n atom has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 5. The electron dot symbol for this element is. X:.. X:.... X:. :... X: 25. Which electron-dot formula represents a substance that contains a nonpolar covalent bond? Which is the electron dot symbol for a chlorine atom in the ground state?. : l:..... l:. :...l:....l: 26. What is the correct Lewis electron-dot structure for the compound magnesium fluoride? The correct electron dot formula for hydrogen chloride is. H : l. : H:.... l. H : l:..... : H: l: Which electron dot symbol could represent a metalloid?. X.. X:. :..X:.....X. page 4

5 28. Which represents the electron configuration of an atom of an alkaline earth metal?. [r]4s 1. [r]4s 2. [r]3d 10 4s 1. [r]3d 10 4s Which compound contains ionic bonds?. Nar(s). Hr(g). 6 H 12 O 6 (s). O 2 (g) 33. characteristic of ionic solids is that they 29. n atom that has an electron configuration of 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 2 is classified as. an alkali metal. an alkaline earth metal. a transition element. have high melting points. have low boiling points. conduct electricity. are noncrystalline. a noble gas element 34. Which type of bond is formed by the transfer of electrons from one atom to another? 30. Which ion has the electron configuration of a noble gas?. u 2+. Fe 2+. a 2+. Hg 2+. a covalent bond. a coordinate covalent bond. a hydrogen bond. an ionic bond 31. Which pair of elements form an ionic bond with each other?. Kl. Il. Pl. Hl 35. Which compound has the least ionic character?. Kl. al 2. ll 3. l 4 page 5

6 36. When ionic bonds are formed, metallic atoms tend to 39. Which of the following elements is most likely to form a compound with radon?. lose electrons and become negative ions. lose electrons and become positive ions. iodine. fluorine. sodium. calcium. gain electrons and become negative ions. gain electrons and become positive ions 40. Which molecule contains a nonpolar covalent bond?. Hl. F 2. O 2. NH When a metal atom combines with a nonmetal atom, the nonmetal atom will. lose electrons and decrease in size. lose electrons and increase in size. gain electrons and decrease in size. gain electrons and increase in size 41. Which type of bond is predominant in a water molecule?. coordinate covalent. polar covalent. ionic. metallic 38. Which kind of bond is formed when two atoms share electrons to form a molecule?. ionic. metallic. electrovalent. covalent 42. Which element is composed of atoms that can form more than one covalent bond with each other?. hydrogen. helium. carbon. calcium page 6

7 43. The four single bonds of a carbon atom are directed in space toward the corners of a 46. Given the compound:. regular tetrahedron. regular octahedron. square plane. trigonal bipyramid The symbol = represents. one pair of shared electrons. two pairs of shared electrons. a single covalent bond. a coordinate covalent bond 44. In a nonpolar covalent bond, electrons are. located in a mobile sea shared by many ions. transferred from one atom to another. shared equally by two atoms. shared unequally by two atoms 47. What is the maximum number of covalent bonds that a carbon atom can form? Which pair of atoms is held together by a covalent bond?. Hl. Lil. Nal. Kl 45. Which type of bond if formed between the two chlorine atoms in a chlorine molecule?. polar covalent. nonpolar covalent. metallic. ionic 49. Which molecule contains a triple covalent bond?. H 2. N 2. O 2. l 2 page 7

8 50. Metallic bonding occurs between atoms of 53. Most metals have the properties of. fluorine. neon. sulfur. copper. brittleness and high ionization energy. brittleness and low ionization energy. ductility and high ionization energy. ductility and low ionization energy 51. Mobile electrons are a distinguishing characteristic of. an ionic bond. an electrovalent bond. a metallic bond. a covalent bond 54. Which type of bond is found between atoms of solid cobalt?. nonpolar covalent. polar covalent. metallic. ionic 52. When combining with nonmetallic atoms, metallic atoms generally will 55. Which is the predominate type of attraction between molecules of HF in the liquid state?. lose electrons and form negative ions. lose electrons and form positive ions. gain electrons and form negative ions. gain electrons and form positive ions. hydrogen bonding. electrocovalent bonding. ionic bonding. covalent bonding page 8

9 56. Which atom has the least attraction for the electrons in a bond between that atom and an atom of hydrogen?. carbon. nitrogen 59. The P l bond in a molecule of Pl 3 is. nonpolar covalent. polar covalent. coordinate covalent. electrocovalent. oxygen. fluorine 60. Which molecule is a dipole?. He. H 2. NH 3. H Oxygen, nitrogen, and fluorine bond with hydrogen to form molecules. Theses molecules are attracted to each other by. ionic bonds. hydrogen bonds. electrovalent bonds 61. Which electron dot formula represents a nonpolar molecule?. coordinate covalent bonds. H H :..: l:.... H. H H :..: H H. H H :...Ṇ: H. H :.Ọ: H 58. The unusually high boiling point of water is due to the. network bonds between the molecules. hydrogen bonds between the molecules. linear structure of the molecules. nonpolar character of the molecules 62. The bond between hydrogen and oxygen in a water molecule is classified as. ionic and nonpolar. ionic and polar. covalent and nonpolar. covalent and polar page 9

10 63. Which substance is correctly paired with its type of bonding?. Nar nonpolar covalent. Hl nonpolar covalent. NH 3 polar covalent. r 2 polar covalent 66. Why is NH 3 classified as a polar molecule?. NH 3 is a gas at STP.. N H bonds are nonpolar.. Nitrogen and hydrogen are both nonmetals.. NH 3 molecules have asymmetrical charge distribution. 64. Which statement explains why a molecule of H 4 is nonpolar?. The bonds between the atoms in a H 4 molecule are polar. 67. What is the correct name of the compound with the formula NH 4 NO 2?. ammonia nitrite. ammonium nitrite. ammonia nitrate. ammonium nitrate. The bonds between the atoms in a H 4 molecule are ionic.. The geometric shape of a H 4 molecule distributes the charges symmetrically.. The geometric shape of a H 4 molecule distributes the charges asymmetrically. 68. The correct formula for sodium oxide is. SO 2. S 2 O. NaO 2. Na 2 O 65. Which formula represents a molecule with the most polar bond?. O. NO. HI. Hl 69. Which formula represents tetrahedral molecule?. H 4. al 2. Hr. r 2 page 10

11 70. What is the correct formula of potassium hydride? 74. ll of the atoms of argon have the same. KH. KH 2. KOH. K(OH) 2. mass number. atomic number. number of neutrons. number of nucleons 71. Which formula correctly represents iron (III) oxide?. Fe 2 O 3. Fe 3 O 2. FeO 3. Fe 3 O 75. n atom of an element contains 20 protons, 20 neutrons, and 20 electrons. This element is. an alkali metal 72. Which is the correct formula for iron (III) sulfate?. Fe 3 SO 4. Fe 2 SO 4. an alkaline earth metal. a halogen. a noble gas. Fe(SO4) 3. Fe 2 (SO 4 ) The atomic number of an atom is always equal to the total number of. neutrons in the nucleus. protons in the nucleus. neutrons plus protons in the atom 76. Which atom has a nucleus that contains 13 protons and 14 neutrons?. Mg. e. l. N. protons plus electrons in the atom page 11

12 77. particle of matter contains 6 protons, 7 neutrons, and 6 electrons. This particle must be a. neutral carbon atom. neutral nitrogen atom. positively charged carbon ion. positively charged nitrogen ion 80. The nucleus is the part of the atom that. consist mostly of empty space. has a negative charge. occupies most of the atom s total volume. contains most of the atom s total mass 78. The mass number of an atom is equal to the number of. neutrons, only. protons, only. neutrons plus protons. electrons plus protons 81. n atom that contains 8 protons, 8 electrons, and 9 neutrons has. an atomic number of 9. an atomic number of 16. a mass number of 17. a mass number of n atom of 226 Rn contains protons and 138 neutrons. 88 protons and 138 electrons. 88 electrons and 226 neutrons. 88 electrons and 226 protons 82. The atomic mass of an element is defined as the weighted average mass of that element s. most abundant isotope. least abundant isotope. naturally occurring isotopes. radioactive isotopes page 12

13 83. Which symbol represents a proton? 87. Which atom contains exactly 15 protons?. 1 1 H. 0 1 H. 1 0 H. 0 0 H. phosphorus-32. sulfur-32. oxygen-15. nitrogen How many protons are present in an atom of P? Which statement is true about a proton and an electron?. They have the same masses and the same charges.. They have the same masses and different charges. 85. n experiment using alpha particles to bombard a thin sheet of gold foil indicated that most of the volume of the atoms in the foil is taken up by. They have different masses and the same charges.. They have different masses and different charges.. electrons. protons. neutrons. empty space 89. What is the total number of orbitals in a p sublevel? 86. In an experiment, alpha particles were used to bombard gold foil. s a result of this experiment, the conclusion was made that the nucleus of an atom is smaller than the atom and positively charged. smaller than the atom and negatively charged. larger than the atom and positively charged. larger than the atom and negatively charged 90. The maximum number of electrons that can occupy a principal energy level (n) of an atom is equal to. n 2. 2n 2. n + 2. n page 13

14 91. Which principal energy level can hold a maximum of 18 electrons? 95. Which orbital notation represents an atom of beryllium in the ground state? s 2s 2p {}}{ ). 1s 2s 2p {}}{,, ) ) ). 1s 2s 2p {}}{, + + ) ). 1s 2s 2p {}}{ + ) The total number of d orbitals in the third principal energy level is Which orbital notation correctly represents the outermost principal energy level of a nitrogen atom in the ground state?. S P {}}{. S P {}}{ 93. What is the total number of sublevels in the second principal energy level?. S P {}}{. S P {}}{ What is the maximum number of electrons that can occupy an orbital? Which atom has the strongest attraction for electrons?. l. F. r. I page 14

15 98. Hydrogen bonds are most likely to form between molecules in which hydrogen is covalently bonded to an element of. small atomic radius and low electronegativity. small atomic radius and high electronegativity 102. Which element exists as diatomic molecules at STP?. argon. sulfur. nitrogen. helium. large atomic radius and low electronegativity. large atomic radius and high electronegativity 103. What is the total number of electrons in a Mg 2+ ion? Which of the following atoms has the least tendency to lose electrons?. s. Na. a. Mg 104. K atom differs from a K + ion in that the K atom has one. more electron. less electron 100. The formula H 2 represents one. more proton. less proton. gram. liter. atom. molecule 105. sodium atom and a sodium ion must have the same number of. neutrons 101. Which element is a noble gas?. W. r. N. Er. protons. occupied principal energy levels. outermost electrons page 15

16 106. n isotope of which element has an atomic number of 6 and a mass number of 14?. carbon. magnesium. nitrogen. silicon 110. Element X has two isotopes. If 72.0% of the element has an isotopic mass of 84.9 atomic mass units, and 28.0% of the element has an isotopic mass of 87.0 atomic mass units, the average atomic mass of element X is numerically equal to. ( ) ( ). ( ) ( ). ( ) ( ) If X is the symbol of an element, which pair correctly represents isotopes of X?. ( ) + ( ) X and X X and X and X X and X 65 X 111. The average isotopic mass of chlorine is Which mixture of isotopes (shown as percents) produces this average mass? 108. ifferent isotopes of the same element must have a different. mass number. atomic number. 50% 12 and 50% % 35 l and 50% 37 l. 75% 35 l and 25% 37 l. 75% 12 and 25% 13. number of protons. number of electrons 112. Which statement best explains why most atomic masses on the Periodic Table are decimal numbers? 109. toms of every isotope of calcium have the same. atomic mass. atomic number. number of neutrons. number of nucleons. tomic masses are determined relative to an H 1 standard.. tomic masses are determined relative to an O 16 standard.. tomic masses are a weighted average of the naturally occurring isotopes.. tomic masses are an estimated average of the artificially produced isotopes. page 16

17 113. ase your answer(s) to the following question(s) on the data table below, which shows three isotopes of neon. Isotope tomic Mass (atomic mass units) Percent Natural bundance 20Ne % 21Ne % 22Ne % 117. In the reaction U n 239 Np + X, the species 93 represented by X is. 1 1 H. 1 0 n. 4 2 He. 0 1 e ased on natural abundances, the average atomic mass of neon is closest to which whole number? 114. n 80 milligram sample of a radioactive isotope decays to 5 milligrams in 32 days. What is the half-life of this element?. 8 days. 2 days. 16 days. 4 days 118. The graph shown represents the decay of a radioactive isotope. What is the half-life of this isotope?. 1 hour. 2 hours. 3 hours. 6 hours 115. What is the number of hours required for potassium-42 to undergo 3 half-life periods?. 6.2 hours hours hours hours 119. What is the mass of 42 K remaining in a 16-gram sample of 42 K after 37.2 hours? 116. In the reaction X H 6 3 Li + 4 He, the nucleus 2 represented by X is. 1.0 g. 2.0 g. 8.0 g. 4.0 g. 9 3 Li e page 17

18 120. Given the reaction: 24Na Mg e. This reaction is best described as. alpha decay. beta decay. fission. fusion 123. Gamma rays are most similar to. positively charged hydrogen nuclei. positively charged helium nuclei. high-energy X-rays. high-speed electrons 121. Which nuclear reaction is classified as alpha decay? N e K a e 226. Ra Rn He. 3 1 H 0 1 e He 124. Which two characteristics do radioisotopes have that are useful in medical diagnosis?. long half-lives and slow elimination from the body. short half-lives and slow elimination from the body. long half-lives and quick elimination from the body. short half-lives and quick elimination from the body 122. The structure of an alpha particle is the same as a. lithium atom. neon atom. hydrogen nucleus. helium nucleus 125. Gamma rays are emanations that have. mass but no charge. charge but no mass. neither mass nor charge. both mass and charge page 18

19 126. Which product of nuclear decay has mass but no charge? 129. nuclear fission reaction and a nuclear fusion reaction are similar because both reactions. alpha particles. neutrons. gamma rays. beta positrons. form heavy nuclides from light nuclides. form light nuclides from heavy nuclides. release a large amount of energy. absorb a large amount of energy 127. Given the reaction: 2 1 H H 4 He + energy 2 The process represented by the reaction is called. fission 130. When a uranium nucleus breaks up into fragments, which type of nuclear reaction occurs?. fusion. fission. replacement. redox. fusion. artificial transmutation. alpha decay 131. diagram of the electromagnetic spectrum is shown below Given the nuclear equation: Es + X 1 0 n Md Which particle is represented by X?. 4 2 He. 0 1 e. 1 0 n e Sunscreen is a lotion used to protect skin from exposure to the Sun. This sunscreen protects a person s skin from wavelengths that are. longer than radio waves but shorter than x-rays.. longer than x-rays but shorter than infrared waves.. longer than microwaves but shorter than infrared waves.. longer than visible light waves but shorter than radio waves. page 19

20 132. Which of the following choices best explains why grass on a distant hillside appears green? Grass reflects all colors except green.. Grass absorbs only green light from the sun.. Grass reflects green light more than any other color.. Grass transmits green light in the same way that green-colored cellophane does. Iodine would have chemical properties most like. manganese (Mn).. tellurium (Te).. chlorine (l).. xenon (Xe) The atomic theories of alton, Thomson, Rutherford, and ohr all support which of the following statements?. toms are mostly composed of empty space.. ll matter is composed of tiny, discrete particles called atoms.. Electrons orbit the nucleus of an atom at distinct energy levels.. toms are composed of positively and negatively charged particles Which of the following elements is classified as a metal?. bromine. helium. sulfur. lithium 134. Which of the following statements explains why oxygen is classified as a pure substance and air is classified as a mixture?. Oxygen is more reactive than air.. Oxygen has a higher density than air.. Oxygen undergoes phase changes, whereas air is always a gas When cations and anions join, they form what kind of chemical bond?. ionic. hydrogen. metallic. covalent. Oxygen contains only one substance, but air contains several substances. page 20

21 138. Some of the molecules found in the human body are NH 2 H 2 OOH (glycine), 6 H 12 O 6 (glucose), and H 3 (H 2 ) 16 OOH (stearic acid). The bonds they form are 139. Water is a polar solvent, while hexane is a nonpolar solvent.. nuclear.. metallic.. ionic.. covalent. Which of the examples above illustrates a nonpolar solute in a polar solvent?. NH 4 l in water. 10 H 8 in water. 2 H 5 OH in hexane. O(NH 2 ) 2 in hexane page 21

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