Physical Science - Chapter 6 Practice Test

39. The metallic bonds in a transition metal, such as tungsten, are stronger than the metallic bonds in a(an) ____________________ metal, such as sodium.

Alkali

57. Mixing magnesium and aluminum together produces an excellent lightweight material from which to make airplane parts. What is this type of mixture called?

An alloy

28. In an ionic compound, the attractions between cations and ____________________ hold the compound together.

Anions

53. How do you know that magnesium is the more metallic element in the compound magnesium oxide, MgO?

Because the symbol for magnesium comes first in the chemical formula and name

51. In potassium bromide, KBr, which element forms anions?

Bromine

42. In a metal lattice, ____________________ are surrounded by a pool of shared electrons.

Cation

30. The chemical formula for calcium chloride, CaCl2, shows that the compound contains two ____________________ ions for every ____________________ ion.

Chloride, Calcium

48. Sodium, an alkali metal, and chlorine, a halogen, are both in Period 3 of the periodic table. Which element has a higher ionization energy? Explain your answer.

Chlorine, it gains electrons rather losing them

44. To produce stainless steel, steelmakers add ____________________ to iron.

Chromium

43. In its simplest form, the alloy brass consists of zinc and ____________________.

Copper

63. Classifying What type of bond belongs in box (3) in Figure 6-2?

Covalent

67. Comparing and Contrasting What kind of bond forms between the elements in row B of Figure 6-3? How is this type of bond different from the type of bond that forms between the elements in row A?

Covalent bonds form between the nonmetals carbon and oxygen. In a covalent bond, atoms share electrons. When potassium and iodine react, electrons are transferred from potassium atoms to iodine atoms. Ionic bonds form between potassium cations and iodide anions. There is no sharing of electrons in an ionic bond.

32. The ions in solid sodium chloride are arranged in a structure called a(an) ____________________ lattice.

Crystal

33. If there are two long dashes between two atoms in a structural formula, molecules of the compound contain a(an) ____________________ bond.

Double

34. A polar covalent bond forms when ____________________ are not shared equally between atoms.

Electrons

35. When cesium and fluorine react, they form an ionic compound called cesium ____________________.

Flourine

45. In a periodic table that included electron dot diagrams, in which column would the diagrams contain more dots—Group 2A (the alkaline metals) or Group 6A (the oxygen family)?

Group 6A, the Oxygen Family

50. Are covalent bonds more likely to be found in compounds containing both metals and nonmetals or compounds containing only nonmetals?

In Compounds, containing only nonmetals

59. Compare the lattice in an ionic compound, such as sodium chloride, with the lattice in a metal, such as tungsten. How do any differences affect the malleability of these solids?

In both lattices, positively charged cations are attracted to negatively charged particles. In an ionic lattice, the negative particles are anions. In a metal lattice, the negative particles are electrons. Because the electrons are mobile, electrons still separate cations when the shape of the metal changes. When an ionic lattice is struck, ions with similar charges are pushed near one another. Repulsions between these ions cause the crystal to shatter.

65. Comparing and Contrasting How are metallic bonds and ionic bonds similar? How are they different?

In both metallic and ionic bonds, there are attractions between particles with positive and negative charges — cations and electrons in a metallic bond, and cations and anions in an ionic bond. Ionic bonds are found in compounds. Metallic bonds are found in a single metal or in alloys.

49. In the binary ionic compound lithium iodide, LiI, which element forms anions?

Iodine

41. Among the elements potassium, lithium, and iron, the metallic bonds are likely to be strongest in ____________________.

Iron

70. Predicting Suppose you could substitute sulfur, S, for iodine in row A in Figure 6-3. What would the formula for the resulting compound be? Explain your answer.

K2S; because sulfur has six valence electrons, its atoms gain two electrons when they form ionic compounds. Potassium atoms donate one valence electron when they form ionic compounds. It takes two potassium atoms to donate two electrons to one sulfur atom.

47. Study the electron dot diagrams in Figure 6-1. Which of the elements are most likely to react and form a compound? What type of compound are they likely to form?

Li + F, an Ionic Compound

54. The structure in a metal lattice can be described as cations surrounded by a pool of shared electrons. What two properties of metals can be explained by this structure?

Malleability and the ability to conduct an electric current

60. How does the ability of metals such as copper and alloys such as steel to be drawn into wires affect the possible uses of these materials?

Metal wires are used to carry electric current. The cables on suspension bridges are made from thin strands of steel.

64. Classifying What type of bond belongs in box (4) in Figure 6-2?

Metallic

55. Why are metals good conductors of electric current?

Metals contain a shared pool of electrons that are free to move

31. KBr is the formula for an ionic compound. The fact that neither symbol is followed by a subscript means that there is a(an) ____________________ ratio of ions in the compound.

One - One

36. A(An) ____________________ ion is a covalently bonded group of atoms that has a positive or negative charge.

Polyatomic

29. In the binary ionic compound potassium bromide, KBr, the element that forms cations is ____________________.

Potassium

46. In an electron dot diagram of potassium, there is one dot. In an electron dot diagram of silicon, there are four dots. Which element would you expect to be more reactive?

Potassium

66. Applying Concepts How does the saying "Opposites attract" apply to the bonding in the compound shown in row A of Figure 6-3?

Potassium is a highly reactive metal with one valence electron. Iodine is a highly reactive nonmetal with seven valence electrons. When electrons are transferred from potassium atoms to iodine atoms, there is an attraction between the oppositely charged ions that form. Thus, opposites do attract in an ionic bond.

58. How is an electron dot diagram a useful model for focusing on the chemical properties of an element?

Shows the number of V. Electrons. The chemical properties of an element depend on the number of V. Electrons in its atoms

56. Which material is most likely to shatter if you strike it with a hammer—sodium chloride or bronze?

Sodium Chloride

62. Using Tables and Graphs What compound name belongs in box (1) in Figure 6-2?

Sodium Chloride

52. In sodium chloride, NaCl, are the cations sodium ions or chloride ions?

Sodium Ions

61. Using Tables and Graphs Write a description to place in box (2) in Figure 6-2.

The atoms of a metal lose one or more valence electrons and form cations. The atoms of a nonmetal gain one or more electrons and form anions. There is an attraction between the oppositely charged ions.

69. Inferring A hydroxide ion has a charge of 1-. What is the charge on the aluminum ion? Explain your answer. Use Figure 6-3 to answer this question.

The charge on the aluminum ion is 3+. The formula Al(OH)3 indicates that there are three hydroxide ions for each aluminum ion in aluminum hydroxide. Since each hydroxide ion has a 1- charge, each aluminum ion must have a charge of 3+ for the overall charge on the compound to be zero.

68. Comparing and Contrasting How are the compounds in rows A and C in Figure 6-3 similar? How are they different?

The compounds in rows A and C are both ionic compounds. However, KI is a binary ionic compound, which forms between a metal and a nonmetal. The compound in row C contains a polyatomic hydroxide ion (OH-). The atoms within a polyatomic ion are joined by covalent bonds.

38. The compound whose formula is SO3 is called sulfur ____________________.

Trioxide

27. In an electron dot diagram, each dot represents a(an) ____________________.

Valence Electrons

40. In general, the more ____________________ a metal has, the stronger its metallic bonds will be.

Valence Electrons

37. In ionic compounds, the sum of the charges of all the cations and anions must be ____________________.

Zero

____ 26. How does increasing the amount of carbon in steel affect its properties? a. Carbon makes the lattice harder and stronger. b. Carbon forms an oxide that protects the steel from rusting. c. Carbon makes the steel light enough to use for airplane parts. d. Carbon makes the steel softer and easier to cut.

a. Carbon makes the lattice harder and stronger.

____ 14. Which of the following formulas represents a compound whose molecules contain a triple bond? a. N≡N b. O=O=O c. O3 d. SO3

a. N≡N

____ 23. Many metals can be drawn into thin wires without breaking because... a. cations are still surrounded by electrons when they shift their positions in the lattice. b. metals generally have low melting points. c. when a metal is struck with a hammer, the positions of the anions do not change. d. electrons have fixed positions in a metallic lattice.

a. cations are still surrounded by electrons when they shift their positions in the lattice.

____ 6. The formation of an ionic bond involves the a. transfer of electrons. b. transfer of neutrons. c. transfer of protons. d. sharing of electrons.

a. transfer of electrons.

____ 16. The elements most likely to form more than one type of ion are the ... a. transition metals. b. alkali metals. c. halogens. d. alkaline earth metals.

a. transition metals.

____ 11. Which of the following compounds does NOT contain molecules? a. H2 b. NaCl c. CO2 d. H2O

b. NaCl

____ 7. Which of the following statements correctly describes the substance with the formula KI? a. Molecules of potassium iodide contain one atom of potassium and one atom of iodine. b. There is a one-to-one ratio of potassium ions to iodide ions. c. Potassium iodide is a molecular compound. d. Potassium iodide is a polyatomic ion.

b. There is a one-to-one ratio of potassium ions to iodide ions.

____ 13. You see a structural formula in which the symbols for elements are connected by a long dash. You can assume that the chemical bonds in the compound are ... a. ionic. b. covalent. c. metallic. d. unstable.

b. covalent.

____ 18. The name iron(II) indicates that a compound contains ... a. iron ions with an 11+ charge. b. iron ions with a 2+ charge. c. iron ions with a negative charge. d. two types of iron ions.

b. iron ions with a 2+ charge.

____ 17. Fluorine, F, forms a binary ionic compound with lithium, Li. What is the name of this compound? ... a. fluorine lithide b. lithium fluoride c. lithium fluorine d. fluorine lithium

b. lithium fluoride

____ 20. In the name carbon dioxide, the prefix of the second word indicates that a molecule of carbon dioxide contains... a. two carbon atoms. b. two oxygen atoms. c. a polyatomic ion. d. an ionic bond.

b. two oxygen atoms.

____ 19. Beryllium, Be, and chlorine, Cl, form a binary ionic compound with a one-to-two ratio of beryllium ions to chloride ions. The formula for the compound is ... a. Be2Cl. b. 2BeCl. c. BeCl2. d. Be2Cl2.

c. BeCl2.

____ 24. Which statement about metals is true? a. A metal lattice is extremely rigid. b. The bonds within a metal lattice are weak. c. Electrons in a metal lattice are free to move. d. Generally, metals have a low melting point.

c. Electrons in a metal lattice are free to move.

____ 2. Typically, atoms gain or lose electrons to achieve... a. an exchange of energy. b. ionization. c. a stable electron configuration. d. vaporization.

c. a stable electron configuration

____ 12. When two atoms of the same nonmetal react, they often form a(an) ... a. ionic bond. b. polyatomic ion. c. diatomic molecule. d. polar molecule.

c. diatomic molecule.

____ 5. Ionization energies tend to... a. decrease from left to right across a period. b. increase from the top of a group to the bottom. c. increase from left to right across a period. d. decrease from the bottom of a group to the top.

c. increase from left to right across a period.

____ 10. Which of the following is a typical property of an ionic compound? a. low melting point b. poor conductor of electric current when melted c. tendency to shatter when struck d. all of the above

c. tendency to shatter when struck

____ 9. Which statement best describes the properties of sodium chloride? a. Sodium chloride is a malleable solid. b. Solid sodium chloride is a good conductor of electric current. c. Sodium chloride has a low melting point. d. Liquid sodium chloride is a good conductor of electric current.

d. Liquid sodium chloride is a good conductor of electric current.

____ 4. Study the electron dot diagrams for lithium, carbon, fluorine, and neon in Figure 6-1. Choose the statement that correctly identifies the most stable of the elements. a. Lithium is the most stable element because it has to lose only one electron to achieve a stable configuration. b. Carbon is the most stable element because it can form four bonds. c. Fluorine is the most stable element because it has to gain only one electron to achieve... a. stable configuration. d. Neon is the most stable element because its highest occupied energy level is filled.

d. Neon is the most stable element because its highest occupied energy level is filled.

____ 15. In a polar covalent bond, a. electrons are shared equally between atoms. b. a cation is bonded to an anion. c. electrons are transferred between atoms. d. electrons are not shared equally between atoms.

d. electrons are not shared equally between atoms.

____ 1. Which of the following groups contain three elements with stable electron configurations? a. lithium, krypton, argon b. argon, neon, barium c. xenon, neon, boron d. helium, xenon, neon

d. helium, xenon, neon

____ 25. An alloy that contains mainly iron and carbon is a. sterling silver. b. bronze. c. brass. d. stainless steel.

d. stainless steel.

____ 21. Which phrase best describes a metallic bond? a. a bond that is formed by a metal b. the attraction between a metal anion and a shared pool of electrons c. a bond that forms between a metal and a nonmetal d. the attraction between a metal cation and a shared pool of electrons

d. the attraction between a metal cation and a shared pool of electrons

____ 3. In an electron dot diagram, the symbol for an element is used to represent... a. the nucleus. b. the nucleus and all electrons. c. the nucleus and valence electrons. d. the nucleus and all non-valence electrons.

d. the nucleus and all non-valence electrons

____ 8. In the compound MgCl2, the subscript 2 indicates that... a. there are two magnesium ions for each ion of chlorine b. the chloride ion is twice the size of the magnesium ion. c. magnesium and chlorine form a double covalent bond. d. there are two chloride ions for each magnesium ion.

d. there are two chloride ions for each magnesium ion.

____ 22. Metallic bonding is similar to ionic bonding because... a. electrons are transferred between atoms. b. electrons are shared between atoms. c. the lattice that forms contains anions and cations. d. there is an attraction between positively charged and negatively charged particles.

d. there is an attraction between positively charged and negatively charged particles.