Chemistry--Unit 2: Chemical Names and Formulas Test Review

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Horace Garrison
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1 vocab anion binary compound cation chemical formula formula unit ion ionic compound law of definite proportions law of multiple proportions molecular formula polyatomic ion representative particle ternary compound know o how to I.D. ions, molecular compounds, ionic compounds, acids, and diatomic molecules o how to name ions, molecular compounds, ionic compounds, acids, and diatomic molecules o how to write formulas for ions, molecular compounds, ionic compounds, acids, and diatomic molecules o trend in oxidation numbers (charges) across the periodic table o characteristics of molecular compounds, ionic compounds, and acids o cations (+) lose electrons, anions ( ) gain electrons questions to try Completion Every substance is either an element or a(n) (1). A compound is either (2) or ionic in nature. Molecular compounds are composed of two or more (3). The representative particle of a molecular compound is a (4). Ionic compounds are composed of oppositely charged (5) combined in electrically neutral groupings. Molecular compounds tend to have (6) melting and boiling points, while ionic compounds tend to have (7) melting and boiling points. Ions form when atoms or groups of atoms (8) or (9) electrons. Chemists have identified more than ten million chemical (10). A (11) shows the numbers and kinds of atoms in the smallest representative unit of a substance. The chemical formula of a molecular compound is called a (12). If there is more than one atom of a given element in a molecule, a (13) is used to indicate the number of atoms. For an ionic compound, the smallest whole-number ratio of atoms in the compound is called a (14). The law of (15) proportions states that the masses of elements in a compound are always in the same proportions. This is consistent with Dalton s theory that atoms combine in (16) ratios. Ions that consist of a single atom are called (17) ions. Metallic elements tend to (18) electrons. Group 1 ions have a (19) charge, while Group 2 metals form with a (20) charge and Group 13 metals form ions with a (21) charge. The charge of an ion of the representative elements can be determined from the (22) number. Many of the (23) have more than one common ionic charge. The ions are named using (24). Ions containing more than

2 one atom are called (25) ions. The names of most common polyatomic ions end in either (26) or (27). Binary ionic compounds are named by writing the name of the (28) followed by the name of the (29). Names of binary compounds end in (30). For example, NaI is (31). When a cation has more than one ionic charge, a (32) is used in the name. Ternary compounds contain at least one (33) ion. In writing the formula of an ionic compound, the net ionic charge must be (34). Binary molecular compounds are composed of two (35) elements. The name of this type of compound ends in (36). Prefixes are used to show how many (37) of each element are present in a molecule of the compound. For example, As 2 S 5 is (38). Compounds of the general form HX, where X is an anion, are named as (39) when in water solution. HBr, named as an acid, is (40) acid. H 3 PO 4 is a(n) (41). It is named (42). CCl 4 is not a(n) (43). It contains two elements, so it is a (44) compound. It does not contain a metal, so it is a (45) (46) compound. The compound is named (47). Pb(C 2 H 3 O 3 ) 2 is not a(n) (48). It contains more than two (49). C 2 H 3 O 2 1 is a (50) ion. Pb is a group (51) metal. The compound is called (52). True-False 53. In forming an ionic compound, an atom of an element can only gain more electrons. 54. An anion is any atom or group of atoms with a positive charge. 55. For metallic ions, the name of the ion is the same as the name of the element. 56. For ions of nonmetals, the name of the ion is the same as the name of the element. 57. A molecule can only contain two atoms. 58. The molecular formula for table salt is NaCl. 59. Whenever two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in ratios of small whole numbers. 60. The proportions of elements in a sample of a compound vary with the mass of the sample. 61. A subscript in a chemical formula is used to indicate the number of atoms of a given element in the smallest representative unit of the substance. 62. A chemical formula is the same as a molecular formula. 63. The names of all polyatomic ions end in ite or ate. 64. Polyatomic ions can only be anions. 65. The charge of ions from representative elements can be determined from the group number. 66. Group 16 ions have a charge of The IUPAC name for baking soda (NaHCO 3 ) is sodium bicarbonate. 68. In writing a formula for an ionic compound, the net ionic charge of the formula must be zero. 69. The cation name is placed first when naming ionic compounds. 70. Binary molecular compounds must contain carbon. 71. Charges must be balanced when writing formulas for molecular compounds. 72. Acids produce hydrogen cations in aqueous solution. 73. Roman numerals are used when naming multiple-charge transition metals. 74. Names of all compounds containing polyatomic ions end in ide. 75. Prefixes are used when naming binary ionic compounds. 76. Compounds containing two non-metals are called binary ionic compounds.

3 Matching 77. molecule 78. molecular compounds 79. ions 80. cations 81. anions 82. ionic compounds 83. chemical formula 84. molecular formula 85. formula unit 86. subscript 87. law of definite proportions 88. monatomic ions 89. polyatomic ions 90. binary ionic compounds 91. ternary ionic compounds 92. transition metals 93. binary molecular compound 94. prefix 95. acid 96. mono- 97. tetra- a. compound that produces hydrogen cations in aqueous solution b. negatively charged ions c. positively charged ions d. ions that consist of a single atom e. ions that consist of more than one atom f. non-ionic compound containing atoms of two elements g. ionic compounds composed of three elements h. ionic compounds composed of two elements i. elements of Groups 3-12, many of which have more than one possible ionic charge j. prefix indicating four atoms in a molecule k. prefix indicating one atom in molecule l. compounds composed of molecules m. compounds composed of cations and anions n. atoms or groups of atoms with a positive or negative charge o. smallest electrically neutral unit of a substance that retains the properties of the substance p. chemical formula for a molecular compound q. lowest whole number ratio of ions in an ionic compound r. in any sample of a compound, the masses of the elements are always in the same proportion s. shows the numbers and kinds of atoms in the smallest representative unit of a substance t. used to indicate the number of atoms of each element present in a chemical compound u. used when naming binary molecular compounds to indicate the number of atoms of an element present in a molecule

4 Br 1 Short Answer 98. State the number of electrons lost or gained in forming each of these ions. a. Mg +2 b. Ca +2 c. Br 1 d. Ag Name each ion and tell whether it is an anion or cation. a. Mg +2 c. b. Ca +2 d. Ag Classify each particle as an atom, cation, anion, or molecule. a. Fe +3 b. F 1 c. CH 4 d. Ne e. O 2 f. O 2 g. Na +1 h. He i. CO 2 j. Ca Classify each of the following chemical formulas as a molecule or a formula unit. Name them. a. NaBr d. K 2 S b. CaCl 2 e. CCl 4 c. C 2 H 6 f. H 2 O 102.What is the charge on a typical ion for each of the following groups? a. 1 b. 16 c. 17 d Write the name of each of the following polyatomic ions. 1 2 a. HCO 3 c. MnO 4 +1 b. NH 4 d. OH Name the following compounds and tell what type of compound they are (binary ionic or ternary ionic). a. FeBr 3 b. KOH c. Na 2 Cr 2 O Write the formulas for the following compounds. a. sodium chlorate b. lead (II) phosphate c. magnesium hydrogen carbonate 106.Classify the following compounds as either binary molecular or acids. Name them. a. HI b. CF 4 c. HC 2 H 3 O 2 d. CO Name each of the following compounds. a. PCl 5 c. SO 2 b. HBr d. P 4 S Write formulas for the following compounds. a. hydrofluoric acid b. carbon tetrachloride 109.Name the following compounds. a. Pb(C 2 H 3 O 2 ) 4 b. HCN 110.Write formulas for the following compounds. a. phosphorus heptachloride b. iron (II) oxide c. nitrous acid c. dinitrogen tetroxide d. nitric acid c. P 2 O 5 d. LiBr d. potassium chloride e. calcium nitrate

5 answers to questions to try 1. compound 24. roman numerals 2. molecular 25. polyatomic 3. nonmetals 26. ate/ ite 4. molecule 27. ite/ ate 5. ions 28. cation 6. low 29. anion 7. high 30. ide 8. gain/lose 31. sodium iodide 9. lose/gain 32. roman numeral 10. compounds 33. polyatomic 11. chemical 34. zero formula 35. nonmetal 12. molecular 36. ide formula 37. atoms 13. subscript 38. diarsenic 14. formula unit pentasulfide 15. definite 39. acids 16. small whole 40. hydrobromic number 41. acid 17. monatomic 42. phosphoric acid 18. lose 43. acid binary binary molecular 22. group 47. carbon 23. transition metals tetrachloride 48. binary compound 49. elements 50. polyatomic lead (II) acetate 53. F 54. F 55. T 56. F 57. F 58. F 59. T 60. T 61. F 62. F 63. F 64. F 65. T 66. T 67. T 68. T 69. T 70. F 71. F 72. T 73. T 74. F 75. F 76. F 77. o 78. l 79. n 80. c 81. b 82. m 83. s 84. p 85. q 86. t 87. r 88. d 89. e 90. h 91. g 92. i 93. f 94. u 95. a 96. k 97. j 98. a. lost 2 b. lost 2 c. gained 1 d. lost a. magnesium ion, cation b. calcium ion, cation c. bromide ion, anion d. silver ion, cation 100. a. cation, b. anion, c. molecule, d. atom, e. molecule, f. anion, g. cation, h. atom, i. molecule, j. cation 101. a. formula unit, sodium bromide b. formula unit, calcium chloride c. molecule, dicarbon hexahydride d. formula unit, potassium sulfide e. molecule, carbon tetrachloride f. molecule, dihydrogen monoxide 102. a. +1 b. 2 c. 1 d a. bicarbonate ion or hydrogen carbonate ion b. ammonium ion c. manganate ion d. hydroxide ion 104. a. iron (III) bromide, binary ionic b. potassium hydroxide, ternary ionic c. sodium dichromate, ternary ionic 105. a. NaClO 3 b. Pb 3 (PO 4 ) 2 c. Mg(HCO 3 ) a. acid, hydroiodic acid b. binary molecular, carbon tetrafluoride c. acid, acetic acid d. binary molecular, carbon dioxide 107. a. phosphorus pentachloride b. hydrobromic acid c. sulfur dioxide d. tetraphosphorus decasulfide 108. a. HF b. CCl 4 c. N 2 O 4 d. HNO a. lead (IV) acetate b. hydrocyanic acid c. diphosphorus pentoxide d. lithium bromide 110. a. PCl 7 b. FeO c. HNO 2 d. KCl e. Ca(NO 3 ) 2

Name Date Class. 3 charge, whereas Group 2A metals form ions with a 4 3. charge, and Group 3A metals form ions with a 5 charge. 4.

Name Date Class. 3 charge, whereas Group 2A metals form ions with a 4 3. charge, and Group 3A metals form ions with a 5 charge. 4. 9.1 NAMING IONS Section Review Objectives Determine the charges of monatomic ions by using the periodic table and write the names of the ions Define a polyatomic ion and write the names and formulas of