Chapter 5 Review/Practice Test
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1 Chapter 5 Review/Practice Test Name Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Electrons involved in bonding between atoms are a. closest to the nucleus. b. valence electrons. c. inside the nucleus. d. positively charged. 2. When an atom loses an electron, it becomes a a. neutral atom. b. negative ion. c. positive ion. d. neutral ion. 3. Ions that are made of more than one atom are examples of a. negative ions. b. positive ions. c. polyatomic ions. d. neutral ions. 4. Magnesium bromide is an ionic compound with the chemical formula MgBr 2. What does the 2 tell you? a. There are two magnesium ions to every bromide ion. b. There are two bromide ions for every magnesium ion. c. Bromide has a 2 charge. d. Bromide has a 2+ charge. 5. Which of the following is a characteristic property of ionic compounds? a. They have low melting points. b. They contain no charged particles. c. They form hard, brittle crystals with characteristic shapes. d. They have low boiling points. 6. A chemical bond formed when two atoms share electrons is called a(n) a. ionic bond. b. polyatomic bond. c. crystal bond. d. covalent bond. 7. A mixture that is made of two or more elements one that is a metal that has the properties of metal is a(n) a. alloy. b. monomer. c. ceramic. d. polymer. 8. The attraction between a positive metal ion and the sea of electrons surrounding it is a(n) a. metallic bond. b. chemical bond. c. ionic bond. d. covalent bond.
2 9. Water is polar and oil is nonpolar. What happens when the two liquids are poured into the same container? a. Both liquids become nonpolar. b. The liquids mix well. c. A gas is produced. d. The liquids do not mix. 10. Each family in the periodic table has its own characteristic properties based on the number of a. ions. b. valence electrons. c. neutrons. d. protons. 11. Molecular compounds do not conduct electricity because they a. do not break up into ions. b. do not dissolve in water. c. break up into ions. d. have high melting points. 12. A covalent bond in which electrons are shared unequally is a. polyatomic. b. a double bond. c. polar. d. ionic. 13. Which of the following best describes a metallic crystal? a. positive metal ions surrounded by freely moving valence electrons b. metal atoms held together by ionic bonds c. metal atoms held together by covalent bonds d. neutral metal atoms surrounded by freely moving valence electrons 14. Which of the following terms means that metals can be rolled into thin sheets, as in aluminum foil, or beaten into complex shapes? a. alloy b. malleable c. polar d. ductile. 15. How many valence electrons does calcium have? a. 1 b. 2 c. 6 d Which of the following elements has 7 valence electrons? a. Beryllium c. Lithium b. Oxygen d. Chlorine 17. A negative ion is called a a. anion c. polar ion b. cation d. covalent ion
3 18. Sodium is combined with sulfur to produce sodium sulfide. What will be the charge of a sodium atom after it bonds with a sulfur atom? a. +1 c. +2 b. -1 d Nitrogen bonds with sulfur in a chemical reaction. What type of bond will be present? a. ionic c. metallic b. covalent 20. Potassium bonds with chlorine in a chemical reaction. What type of bond will be present? a. ionic c. metallic b. covalent 21. Rubidium is combined with oxygen in a chemical reaction. The formula of the compound created, rubidium oxide, is a. RbO c. RbO 2 b. Rb 2 O d. Rb 2 O The type of compound formed when calcium combines with sulfur. a. Metallic compound c. Ionic Compound b. Molecular compound 23. Consider this chemical formula: Li 2 (CF 2 ) 4. How many fluorine atoms are there? a. 2 c. 8 b. 4 d Consider this chemical formula: 3 Au NCl 4 How many chlorine atoms are there? a. 1 c. 12 b. 2 d Which Lewis Dot Formula is incorrect? a. b. c. d. e.
4 Which of the following represent the Lewis dot diagram for ammonia (NH 3 )? Modified True/False Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true. 28. The attraction between a positive ion and a negative ion results in a covalent bond. _ 29. When electrons are transferred between two atoms, a covalent bond is formed. _ 30. A nonpolar bond is formed when two atoms share electrons unequally. _ Completion Complete each statement. 31. Ionic compounds have melting points because a lot of energy is needed to break the bonds between the ions. 32. Solid metals are good conductors of heat and.
5 Short Answer Use the diagram to answer each question. 33. List three elements from the group containing the most reactive nonmetals. 34. How many atoms of a Group 17 element would be needed to react with one atom of a Group 2 element? Explain. Essay 35. How do valence electrons relate to the chemical reactions of an element? 36. Explain what makes the Group 1 elements the most reactive metals.
6 37. Draw a Lewis dot reaction diagram for combining sodium and sulfur to form sodium sulfide. 38. Draw a Lewis dot diagram for carbon tetrafluoride (CF 4 )?
7 Chapter 5 Review/Practice Test Answer Section MULTIPLE CHOICE 1. ANS: B PTS: 1 DIF: L2 OBJ: CaPS Explain how the reactivity of elements is related to valence electrons in atoms. STA: S 8.3.a BLM: comprehension 2. ANS: C PTS: 1 DIF: L1 OBJ: CaPS Explain how ions form bonds. STA: S 8.3.a BLM: knowledge 3. ANS: C PTS: 1 DIF: L1 OBJ: CaPS Explain how ions form bonds. STA: S 8.3.b BLM: knowledge 4. ANS: B PTS: 1 DIF: L2 OBJ: CaPS Explain how the formulas and names of ionic compounds are written. STA: S 8.3.b BLM: application 5. ANS: C PTS: 1 DIF: L2 OBJ: CaPS Identify the properties of ionic compounds. STA: S 8.7.c BLM: comprehension 6. ANS: D PTS: 1 DIF: L1 OBJ: CaPS State what holds covalently bonded atoms together. STA: S 8.3.b BLM: knowledge 7. ANS: A PTS: 1 DIF: L1 OBJ: CaPS Explain how the properties of metals and alloys compare. STA: S 8.7.c BLM: knowledge 8. ANS: A PTS: 1 DIF: L1 OBJ: CaPS Describe how metal atoms are bonded in solid metal. STA: S 8.3.a S 8.3.b BLM: knowledge 9. ANS: D PTS: 1 DIF: L2 OBJ: CaPS Explain how unequal sharing of electrons occurs and how it affects molecules. STA: S 8.3.b S 8.7.c BLM: application 10. ANS: B PTS: 1 DIF: L2 OBJ: CaPS State what the periodic table tells you about atoms and the properties of elements. STA: S 8.3.a BLM: comprehension 11. ANS: A PTS: 1 DIF: L2
8 OBJ: CaPS Identify the properties of molecular compounds. STA: S 8.3.b S 8.7.c BLM: application 12. ANS: C PTS: 1 DIF: L1 OBJ: CaPS Explain how unequal sharing of electrons occurs and how it affects molecules. STA: S 8.3.b BLM: knowledge 13. ANS: A PTS: 1 DIF: L2 OBJ: CaPS Describe how metal atoms are bonded in solid metal. STA: S 8.3.c BLM: comprehension 14. ANS: B PTS: 1 DIF: L1 OBJ: CaPS Explain how metallic bonding results in useful properties of metals. STA: S 8.7.c BLM: knowledge MODIFIED TRUE/FALSE 15. ANS: F, an ionic PTS: 1 DIF: L1 OBJ: CaPS Explain how ions form bonds. STA: S 8.3.b BLM: knowledge 16. ANS: F, shared PTS: 1 DIF: L2 OBJ: CaPS State what holds covalently bonded atoms together. STA: S 8.3.b BLM: comprehension 17. ANS: F, polar PTS: 1 DIF: L1 OBJ: CaPS Explain how unequal sharing of electrons occurs and how it affects molecules. STA: S 8.3.b BLM: knowledge COMPLETION 18. ANS: high PTS: 1 DIF: L2 OBJ: CaPS Identify the properties of ionic compounds. STA: S 8.3.b BLM: comprehension 19. ANS: electricity PTS: 1 DIF: L2 OBJ: CaPS Explain how metallic bonding results in useful properties of metals. STA: S 8.7.c BLM: comprehension SHORT ANSWER 20. ANS: Accept any three elements from Group 17: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At). PTS: 1 DIF: L2 OBJ: CaPS State what the periodic table tells you about atoms and the properties of elements. STA: S 8.7.a BLM: analysis 21. ANS: Two. Atoms of elements in Group 17 form ions with a charge of 1, and atoms of elements in Group 2 form ions with a charge of 2+. It would take two ions of a Group 17 element to balance the charge of one ion of a Group 2 element.
9 PTS: 1 DIF: L3 OBJ: CaPS Explain how ions form bonds. STA: S 8.7.a BLM: synthesis ESSAY 22. ANS: Valence electrons are the electrons that are most loosely held by the atom and the ones that are involved in chemical reactions. Chemical reactions occur whenever valence electrons are shared or transferred between atoms. The number of valence electrons determines how these reactions take place and what kind of bonds atoms can form. PTS: 1 DIF: L3 OBJ: CaPS Explain how the reactivity of elements is related to valence electrons in atoms. STA: S 8.3.a BLM: synthesis 23. ANS: Atoms of Group 1 elements each have a single valence electron. These atoms easily lose their valence electron, reacting with other elements that can gain electrons, and therefore becoming more chemically stable. The easy loss of the one valence electron makes the Group 1 elements more reactive than metals that must lose two or three electrons in reactions. PTS: 1 DIF: L3 OBJ: CaPS State what the periodic table tells you about atoms and the properties of elements. STA: S 8.7.a BLM: synthesis
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