Ch 8 Review
Modified True/False
Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true.
____
1. Every compound can be identified by a chemical formula which shows the ratio of the atoms of each element
in the compound. _________________________
____
2. In the formula for magnesium chloride, MgCl2, there are two ions of magnesium.
_________________________
____
3. Negative polyatomic ions behave like metals when forming compounds. _________________________
____
4. Brackets and a subscript are used around a metal ion if there is more than one in a chemical formula.
_________________________
____
5. The total number of electrons transferred to form a single unit of a compound will be the lowest common
multiple of the two ion charges. _________________________
____
6. To determine the formula for the compound produced when Pb4+ and N3- combine, it is necessary to find the
lowest common multiple of 2+ and 3–. _________________________
____
7. The ratio of ions in a compound is 1:1; for example, NaCl and MgO, when the outermost electrons of the two
elements are balanced. _________________________
____
8. When a single unit of the compound Al2S3 is formed, six electrons are transferred.
_________________________
____
9. On the periodic table, elements with similar chemical properties are found in vertical columns called periods.
_________________________
____ 10. When metals have more than one ion charge they are called monovalent. _________________________
____ 11. Lead has two ion charges, 1+ and 3+. _________________________
____ 12. Gold is a monovalent metal. _________________________
____ 13. Elements forming nonmetals ions are given the suffix “ide” when naming ionic compounds.
_________________________
____ 14. Metallic elements are written second in the names of ionic compounds. _________________________
____ 15. Negative polyatomic ions are written second in the chemical formulae of ionic compounds.
_________________________
____ 16. The name of the compound, NaOH, is sodium hydroxide. _________________________
____ 17. The name of the compound, Cr2(CO3)3 is chromium(II) carbonate. _________________________
____ 18. The chemical formula for the compound tin(IV) phosphate is Sn3(PO4)4. _________________________
____ 19. The chemical formula for the compound sodium sulphide is Na2SO4. _________________________
____ 20. The chemical formula for the ionic compound strontium oxide is SrO. _________________________
____ 21. The element with atomic number 11 is most likely to have similar chemical properties to the element with
atomic number 20. _________________________
____ 22. All members of the halogen group form ions with a 1+ charge when they react.
_________________________
____ 23. An iodine atom is larger than a fluorine atom because iodine has more electron shells than fluorine.
_________________________
____ 24. Alkali metals are stored in oil because they react with air to produce hydrogen gas and an alkaline solution.
_________________________
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 25. Which of the following describes a polyatomic ion?
a. It has an electrical charge.
b. It is a group of different atoms.
c. It is often unchanged in a chemical reaction.
d. all of the above
____ 26. What are the proportions of metal ions to nonmetal ions in the compound K2CO3?
a. 1 potassium to 1 carbonate
b. 1 potassium to 2 carbonate
c. 2 potassium to 1 carbonate
d. 2 potassium to 3 carbonate
____ 27. What are the proportions of metal ions to nonmetal ions in the compound BaSO4?
a. 1 barium to 1 sulphate
b. 1 barium to 4 sulphate
c. 2 barium to 1 sulphate
d. 2 barium to 4 sulphate
____ 28. What is the total number of atoms in a single unit of the compound Ga(OH)3?
a. 3
b. 5
c. 6
d. 7
____ 29. How many carbonate ions are in a single unit of the compound Pb(CO3)2?
a. 1
b. 2
c. 3
d. 6
____ 30. How many atoms of oxygen are in the compound Ba(OH)2?
a. 0
b. 1
c. 2
d. 3
____ 31. How many atoms of magnesium, hydrogen, carbon, and oxygen are in the compound Mg(HCO3)2?
a. 1 magnesium, 1 hydrogen, 1 carbon and 3 oxygen
b. 1 magnesium, 2 hydrogen, 2 carbon and 3 oxygen
c. 1 magnesium, 2 hydrogen, 2 carbon and 6 oxygen
d. 2 magnesium, 6 hydrogen, 6 carbon and 6 oxygen
____ 32. What is the chemical formula when 3 ammonium ions combine with 1 phosphate ion?
a. NH4PO4
b. NH4(PO4)3
c. (NH4)3PO4
d. (NH4)3(PO4)1
____ 33. How are the ion charges balanced when beryllium and oxygen form a compound?
a. one ion of beryllium balances one ion of oxygen
b. two ions of beryllium balance one ion of oxygen
c. one ion of beryllium balances two ions of oxygen
d. all of the above
____ 34. The ion charges of magnesium and bromine are 2+ and 1– respectively. When ions of these elements
combine, what is the chemical formula?
a. MgBr
b. MgBr2
c. Mg2Br
d. Mg2Br
____ 35. A compound of chlorine and potassium is sometimes used as a substitute for table salt (NaCl) when people
are on a sodium restricted diet. What is the name of this compound?
a. chlorine potassium
b. potassium chlorine
c. potassium chloride
d. potassium chlorate
____ 36. What is the name of the ionic compound (NH4)2SO4?
a. ammonium sulphide
b. ammonium sulphate
c. ammonium(I) sulphide
d. ammonium(I) sulphate
____ 37. What is the name of the ionic compound Cu(OH)2.?
a. copper(I) hydroxide
b. copper(I) hydrogen oxide
c. copper(II) hydroxide
d. copper(II) hydrogen oxide
____ 38. What is the chemical formula for the ionic compound tin(IV) iodide?
a. SnI
b. Sn4I
c. SnI2
d. SnI4
____ 39. Which group in the periodic table contains the noble gases?
a. 1
b. 2
c. 17
d. 18
____ 40. Which of the following sets of elements belong to the same group on the periodic table?
a.
b.
c.
d.
oxygen, nitrogen, sulphur
calcium, iron, magnesium
lithium, potassium, sodium
carbon, manganese, silicon
____ 41. Which of the following elements would react in a manner most similar to nitrogen?
a.
b.
c.
d.
neon
sodium
oxygen
phosphorus
____ 42. How many electrons is an atom of the element with an atomic number of 116 likely to have in its outermost
shell?
a.
b.
c.
d.
2
6
16
116
Completion
Complete each statement.
43. One of the few positive polyatomic ions is ____________________.
44. A group of elements that occur in compounds, and as a group have a positive or negative charge is called a(n)
______________________________.
45. The nitrate ion contains ____________________ atoms of oxygen.
46. The phosphate ion has a ____________________ charge.
47. A ____________________ always contains the same elements in definite proportions.
48. Positive ions are attracted to negative ions through ____________________ attraction.
49. When an atom becomes a negative ion, it has had an electron transferred to it from another atom which has
become a(n) ____________________ ion.
50. When calcium and selenium combine to form a compound, each calcium atom will transfer
____________________ electrons to each selenium atom.
51. Iron is ____________________ because it has two ion charges, 2+ and 3+.
52. The names of the two ions in the ionic compound, Al2(SO4)3 are ____________________ and
____________________.
53. The chemical formula for the compound potassium sulphide is ____________________.
54. The chemical formula for the compound tin(II) chloride is ____________________.
55. The name of the ionic compound, LiI, is ______________________________.
56. The name of the ionic compound, Au2O3, is ______________________________.
57. The name of the ionic compound, Al2(SO4)3, is ______________________________.
58. The most reactive elements on the periodic table are found in Groups _________________________ and
____________________.
59. The elements in the _________________________ group are unreactive because their outermost electron
shells are filled.
60. All members of the _________________________ group form ions with a 1+ charge when they react.
61. Elements with two electrons in their outermost shell belong to the ______________________________.
Ch 8 Review
Answer Section
MODIFIED TRUE/FALSE
1. ANS: T
OBJ: 8.1
2. ANS: F, chlorine
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI1
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
3. ANS: F, nonmetals
OBJ: 8.1
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
4. ANS: F, polyatomic ion
OBJ: 8.1
LOC: Unit B - PLC3
1
REF: U/A
OBJ: 8.1
Unit B - Ch. 08 KI1
T
PTS: 1
8.2
LOC: Unit B - PLC3
F, 4+ and 3–
LOC: Unit B - PLC3
PTS:
TOP:
5. ANS:
OBJ:
6. ANS:
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
7. ANS: F, ion charges
REF: K
TOP: Unit B - Ch. 08 KI1
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: U/A
OBJ: 8.2
TOP: Unit B - Ch. 08 KI1
8. ANS: T
PTS: 1
OBJ: 8.2
LOC: Unit B - PLC3
9. ANS: F
groups
families
LOC: Unit B - PLC3
REF: U/A
TOP: Unit B - Ch. 08 KI1
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
10. ANS: F, multivalent
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
11. ANS: F, 2+ and 4+
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
12. ANS: F, multivalent
OBJ: 8.2
LOC: Unit B - PLC3
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: K
TOP:
13. ANS:
OBJ:
14. ANS:
Unit B - Ch. 08 KI1
T
PTS: 1
8.3
LOC: Unit B - PLC3
F, nonmetallic
PTS:
TOP:
15. ANS:
OBJ:
16. ANS:
OBJ:
17. ANS:
1
REF: K
OBJ: 8.3
Unit B - Ch. 08 KI3
T
PTS: 1
8.3
LOC: Unit B - PLC3
T
PTS: 1
8.3
LOC: Unit B - PLC3
F, chromium(III) carbonate
LOC: Unit B - PLC3
PTS:
TOP:
18. ANS:
OBJ:
19. ANS:
1
REF: U/A
OBJ: 8.3
Unit B - Ch. 08 KI3
T
PTS: 1
8.3
LOC: Unit B - PLC3
F, Na2S
LOC: Unit B - PLC3
PTS:
TOP:
20. ANS:
OBJ:
21. ANS:
1
REF: U/A
OBJ: 8.3
Unit B - Ch. 08 KI2
T
PTS: 1
8.2
LOC: Unit B - PLC3
F, atomic number 12
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI4
22. ANS: F, alkali metal
PTS:
TOP:
23. ANS:
OBJ:
24. ANS:
REF: U/A
TOP: Unit B - Ch. 08 KI3
REF:
TOP:
REF:
TOP:
K
Unit B - Ch. 08 KI2
U/A
Unit B - Ch. 08 KI3
REF: U/A
TOP: Unit B - Ch. 08 KI2
REF: U/A
TOP: Unit B - Ch. 08 KI2
OBJ: 8.4
LOC: Unit B - PLC2
1
REF: U/A
OBJ: 8.4
Unit B - Ch. 08 KI4
T
PTS: 1
8.4
LOC: Unit B - PLC2
F, water
LOC: Unit B - PLC2
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI4
OBJ: 8.4
REF: U/A
TOP: Unit B - Ch. 08 KI4
LOC: Unit B - PLC2
MULTIPLE CHOICE
25. ANS:
LOC:
26. ANS:
LOC:
27. ANS:
LOC:
28. ANS:
LOC:
29. ANS:
D
PTS:
Unit B - PLC3
C
PTS:
Unit B - PLC3
A
PTS:
Unit B - PLC3
D
PTS:
Unit B - PLC3
B
PTS:
1
1
1
1
1
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
K
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
8.1
8.1
8.1
8.1
8.1
LOC:
30. ANS:
LOC:
31. ANS:
LOC:
32. ANS:
LOC:
33. ANS:
LOC:
34. ANS:
LOC:
35. ANS:
LOC:
36. ANS:
LOC:
37. ANS:
LOC:
38. ANS:
LOC:
39. ANS:
LOC:
40. ANS:
LOC:
41. ANS:
LOC:
42. ANS:
LOC:
Unit B - PLC3
C
PTS:
Unit B - PLC3
C
PTS:
Unit B - PLC3
C
PTS:
Unit B - PLC3
A
PTS:
Unit B - PLC3
B
PTS:
Unit B - PLC3
C
PTS:
Unit B - PLC3
B
PTS:
Unit B - PLC3
C
PTS:
Unit B - PLC3
D
PTS:
Unit B - PLC3
D
PTS:
Unit B - PLC2
C
PTS:
Unit B - PLC2
D
PTS:
Unit B - PLC2
B
PTS:
Unit B - PLC2
1
1
1
1
1
1
1
1
1
1
1
1
1
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
REF:
TOP:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI1
U/A
OBJ:
Unit B - Ch. 08 KI3
U/A
OBJ:
Unit B - Ch. 08 KI3
U/A
OBJ:
Unit B - Ch. 08 KI3
U/A
OBJ:
Unit B - Ch. 08 KI2
K
OBJ:
Unit B - Ch. 08 KI4
U/A
OBJ:
Unit B - Ch. 08 KI4
U/A
OBJ:
Unit B - Ch. 08 KI4
U/A
OBJ:
Unit B - Ch. 08 KI4
8.1
8.1
8.1
8.2
8.2
8.3
8.3
8.3
8.3
8.4
8.4
8.4
8.4
COMPLETION
43. ANS: ammonium
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI1
44. ANS: polyatomic ion
OBJ: 8.1
LOC: Unit B - PLC3
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI1
45. ANS:
three
3
OBJ: 8.1
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
46. ANS: 3–
OBJ: 8.1
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
47. ANS: compound
OBJ: 8.1
LOC: Unit B - PLC3
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI1
48. ANS:
electrical
electrostatic
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI1
49. ANS: positive
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI1
50. ANS:
two
2
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI1
51. ANS: multivalent
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: K
TOP: Unit B - Ch. 08 KI1
52. ANS: aluminum, sulphate
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 2
REF: K
TOP: Unit B - Ch. 08 KI3
53. ANS: K2S
OBJ: 8.2
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI2
54. ANS: SnCl2
OBJ: 8.3
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI2
55. ANS: lithium iodide
OBJ: 8.3
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI3
56. ANS: gold(III) oxide
OBJ: 8.3
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI3
57. ANS: aluminum sulphate
OBJ: 8.3
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI3
58. ANS:
1, 17
alkali metals, halogens
OBJ: 8.3
LOC: Unit B - PLC3
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI4
59. ANS:
noble gas
18
OBJ: 8.4
LOC: Unit B - PLC2
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI4
60. ANS:
alkali metal
1
OBJ: 8.4
LOC: Unit B - PLC2
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI4
61. ANS:
Group 2 elements
alkaline earth metals
OBJ: 8.4
LOC: Unit B - PLC2
PTS: 1
REF: U/A
TOP: Unit B - Ch. 08 KI4
OBJ: 8.4
LOC: Unit B - PLC2