Download Ch. 20 - Chemical Bonds - Study Guide

Name: ________________________ Class: ___________________ Date: __________
ID: B
Ch. 20 - Chemical Bonds - Study Guide
Essay
1. Write the names of these compounds: KCl, CR2O3, Ba(ClO3)2, NH4Cl, PCl3
.
2. Explain how the formula for a binary compound is written.
.
3. Lithium's atomic number is 3. Fluorine's is 9. Explain how an atom of lithium and an atom of fluorine
combine by ionic bonding.
.
4. Write the formula for dinitrogen trioxide & carbon pentachloride.
.
1
Name: ________________________
ID: B
5. Identify a physical property that might be used to tell whether a compound is ionic or covalent. Explain why
this physical property is a good indicator.
.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
1 - mono
8 - octa
NH4 1+ - Ammonium
ClO3 1- - Chlorate
2 - di
3 - tri
OH 1- - Hydroxide
NO3 1- - Nitrate
4 - tetra
5 - penta
CO3 2- - Carbonate
2SO4 - Sulfate
6 - hexa
PO4 3- - Phosphate
7 - hepta
____
6. In a covalent bond, electrons are __________.
a. gained
c.
b. shared
d.
destroyed
lost
____
7. A polyatomic ion is another name for a __________ ion.
a. negative
c. neutral
b. positive
d. complex
____
8. A covalent compound made of one sulfur and two oxygen atoms would be named
a. sulfur oxide.
c. sulfur dioxide.
b. disulfur oxide.
d. sulfide oxygen.
____
9. The chemical formula for an ionic compound of boron and chlorine is
a. B3Cl.
c. BCl3.
b. ClB.
d. BCl.
____ 10. Why do the noble gases NOT form compounds readily?
a. They have no electrons.
b. Their outer energy levels are completely filled with electrons.
c. They have seven electrons in the outer energy levels.
d. They have empty outer energy levels.
2
Name: ________________________
ID: B
____ 11.
According to this information, a polyatomic ion is a _________________.
a. group of ionically bonded atoms with
c. group of covalently bonded atoms
a net charge of zero
with a net charge of zero
b. charged, ionically bonded group of
d. charged, covalently bonded group of
atoms
atoms
____ 12. What is Neon’s oxidation number?
a. 0
b. 8-
c.
d.
1+
8+
____ 13. The chemical formula for an ionic compound of sodium and oxygen is
a. NaO2.
c. Na2O.
b. NaO.
d. Na2O2.
____ 14. The elements that make up a compound and the exact number of atoms of each element in a unit of the
compound can be shown in a ____.
a. subscript
c. chemical formula
b. chemical symbol
d. superscript
____ 15. Cu2O is named copper (I) oxide because it contains
a. three oxygen atoms.
c. Cu1+ ions.
b. three iron atoms.
d. O3+ ions.
____ 16. The oxidation number of an atom is shown with a ____.
a. special symbol
c. superscript
b. subscript
d. coefficient
____ 17. Which is the correct name for the following formula: Ca(NO3)2 •3H2O
a. Calcium Nitride Hydrate
c. Calcium Nitrate Trihydrate
b. Calcium Nitride Trihydrate
d. Calcium Nitrate Hydrate
____ 18. When elements form bonds, it changes their __________ properties.
a. mass
c. chemical
b. chemical and physical
d. physical
____ 19. What is Beryllium’s oxidation number?
a. 2+
b. 1+
c.
d.
12-
____ 20. Which of the following is the correct formula for calcium nitrate?
a. Ca(NO3)2
c. Ca2(NO3)2
b. CaNO3
d. Ca2NO3
3
Name: ________________________
ID: B
____ 21. When an atom's outer energy levels are not filled completely, the atom __________.
a. can gain, lose, or share electrons
c. is a noble gas
b. cannot form a compound
d. is very stable
____ 22. What is the correct name for K2SO4?
a. dipotassium sulfate
b. potassium sulfide
c.
d.
potassium disulfide
potassium sulfate
____ 23. What is the number of potassium atoms compared to oxygen atoms in a binary compound made from these
two elements?
a. Three potassium atoms to one oxygen atom.
b. One potassium atom to two oxygen atoms.
c. One potassium atom to three oxygen atoms.
d. Two potassium atoms to one oxygen atom.
____ 24. How many atom of Carbon are present in TWO molecules of Cane Sugar, C12H22O11
a. 6
c. 12
b. 11
d. 24
____ 25. Which of these is a binary ionic compound?
a. H2O
b. NaF
c.
d.
O2
CO
____ 26. Sodium has one electron in its outer shell and chlorine has seven electrons in its outer shell. The atoms will
form a(n) _____ bond by _____ their electrons.
a. covalent, sharing
c. ionic, transferring
b. covalent, transferring
d. ionic, sharing
____ 27. What is the difference between carbon monoxide and carbon dioxide?
a. Carbon monoxide has only one oxygen atom.
b. Carbon dioxide has two carbon atoms.
c. Carbon dioxide has only one oxygen atom.
d. Carbon monoxide has two carbon atoms.
____ 28. The sum of the oxidation numbers in a neutral compound is always ____.
a. zero
c. a negative number
b. one
d. a positive number
____ 29. In sodium chloride, which atom loses an electron?
a. both
c. chloride
b. sodium
d. neither
____ 30. A compound __________.
a. is composed of only metals
c.
b. is a combination of two or more elements d.
has the same properties as its parts
is a pure element
____ 31. Most elements require ____ electrons in the outer energy level.
a. 0
c. 8
b. 2
d. 16
4
Name: ________________________
ID: B
____ 32. Which of the following correctly shows the formula for a hydrate?
c. MgSO4 • 7H2O
a. H2O
b. H2O2
d. MgSO4(H2O)7
____ 33. Which statement best describes what happens to sodium and chlorine atoms when they combine to form
sodium chloride?
a. The sodium atom becomes a negative chloride ion, and the chlorine atom becomes a
positive sodium ion.
b. The sodium atom becomes a positive chloride ion, and the chlorine atom becomes a
negative sodium ion.
c. The sodium atom becomes a positive sodium ion, and the chlorine atom becomes a
negative chloride ion.
d. The sodium atom becomes a negative sodium ion, and the chlorine atom becomes a
positive chloride ion.
____ 34. How many hydrogen atoms are present in TWO molecules of ammonium acetate, NH4C2H3O2?
a. 6
c. 8
b. 24
d. 14
____ 35. How many electron(s) are shared in a triple bond?
a. three pairs
c. three electrons
b. one electron
d. one pair
____ 36. A group of covalently bonded atoms that acts together as one charged atom is a ____.
a. polyatomic ion
c. molecule
b. negative ion
d. crystal
____ 37.
The picture shows models of polar molecules. Which of these is the major characteristic of polar molecules?
a. They have a triangular shape created by the large size of negative oxygen molecules.
b. They contain a metal and a nonmetal.
c. They have a slightly positive end and a slightly negative end.
d. They contain at least two hydrogen atoms.
____ 38. What is the name of a binary compound made up of lithium and chlorine?
a. chlorine lithium
c. lithium chloride
b. lithium chlorate
d. chlorine lithiate
____ 39. How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically
stable?
a. 6
c. 4
b. 8
d. 2
5
Name: ________________________
ID: B
____ 40. In general, noble gases react with __________.
a. metals
c.
b. nothing
d.
other noble gases
water
____ 41. The ____ tells you how many electrons an atom must gain, lose, or share to become stable.
a. ionic number
c. oxidation number
b. atomic number
d. atomic mass
____ 42. Compounds that are hydrates contain what ingredient?
a. water
c. chlorine
b. hydrogen chloride
d. nitrogen
____ 43. What is the correct formula for magnesium oxide?
a. Mg2O2
c. MgO
b. MgO2
d. Mg2O
____ 44. Which is the correct name for N2O 4?
a. Dinitrogen Tetroxide
b. Nitrogen Oxide
c.
d.
Nitrous
Dinitrogen Oxide
____ 45. Ca3N2 is the formula for __________.
a. Calcium Nitride
b. Calcium Nitrogen
c.
d.
Calicitride
Tricalcium Dinitrogen
____ 46. The covalent compound NO5 would be named
a. nitrogen pentoxide.
c.
b. dinitrogen oxide.
d.
dinitrogen pentoxide.
nitrogen oxide.
____ 47. Which of the following is a compound?
a. paint
b. salt
air
soup
c.
d.
____ 48. All of these atoms lend electrons and form positive ions EXCEPT —
a.
c.
b.
d.
6
Name: ________________________
ID: B
____ 49.
Which process is taking place in these chemical combinations?
a. electron sharing
c. electron transfer
b. electron gain
d. electron loss
____ 50. What is the charge of potassium in K3PO4?
a. 1+
b. 7-
c.
d.
4+
3-
____ 51. In a chemical formula, the number of each type of atom in the compound is shown by numbers called ____.
a. superscripts
c. oxidation numbers
b. chemical symbols
d. subscripts
____ 52. An ionic compound made of copper (Cu2+) and oxygen would be named
a. copper oxygen.
c. copper oxide.
b. dicopper oxide.
d. copper(II) oxide.
____ 53. The name for the compound with the formula CuBr2 would be written as
a. copper bromide.
c. copper(II) bromide.
b. copper(I) bromide.
d. copper(III) bromide.
____ 54. What kind of chemical bond is formed when a metal donates electrons to a nonmetal?
a. magnetic
c. ionic
b. covalent
d. hydrate
____ 55. What is Aluminum’s oxidation number?
a. 1+
b. 3-
c.
d.
7
12+
ID: B
Ch. 20 - Chemical Bonds - Study Guide
Answer Section
ESSAY
1. ANS:
1. potassium chloride
2. chromium (III) oxide
3. barium chlorate
4. ammonium chloride
5. phosphorus trichloride
PTS: 1
2. ANS:
First, write the symbol for the element that has the positive oxidation number. Second, write the symbol for
the element that has the negative oxidation number. Third, add subscripts so that the sum of the oxidation
numbers of all atoms in the formula is zero.
Score
Description
Student clearly and correctly explains all three steps in writing a formula for a
4
binary compound.
Student explains all three steps in writing a formula for a binary compound with a
3
minor error in explaining one of the steps.
Student explains all three steps in writing a formula for a binary compound with
2
errors in two of the steps.
OR
Student explains only two of the three steps in writing a formula for a binary
compound.
Student explains only one of the steps in writing a formula for a binary compound.
1
OR
Student has major explanation errors in the steps for writing a formula for a binary
compound.
Student’s response is totally incorrect or irrelevant.
0
No student response.
Blank
PTS: 1
DIF:
DOK 2
OBJ: 8-3
1
STA: C4.2B
ID: B
3. ANS:
Lithium's atomic number of 3 indicates that a lithium atom has three electrons. Two of these electrons fill an
inner energy level; the third electron is in an almost empty outer energy level. A fluorine atom has nine
electrons. Two of fluorine's electrons fill the inner energy level, and seven are in the outer energy level.
Lithium gives an electron to fluorine. Lithium becomes positive, and fluorine becomes negative. Both lithium
and fluorine then have full and therefore relatively stable outer energy levels.
Score
Description
Student clearly explains how lithium and fluorine atoms combine by ionic bonding
4
by discussing filling of energy levels by giving and taking electrons. Student
identifies that lithium becomes positive and fluorine becomes negative and
discusses the stability of their outer energy levels.
Student explains how lithium and fluorine atoms combine by ionic bonding by
3
discussing filling of energy levels by giving and taking electrons, the resulting
charge for the atoms, and their outer energy levels with one or two minor errors.
Student explains how lithium and fluorine atoms combine by ionic bonding by
2
discussing filling of energy levels by giving and taking electrons, the resulting
charge for the atoms, and their outer energy levels with multiple errors.
Student explains how lithium and fluorine atoms combine by ionic bonding by
1
discussing filling of energy levels by giving and taking electrons, the resulting
charge for the atoms, and their outer energy levels with major errors.
Student’s response it totally incorrect or irrelevant.
0
No student response.
Blank
PTS: 1
DIF:
DOK 2
OBJ: 5-2
2
STA: C4.3g | C5.5A
ID: B
4. ANS:
The bond between the calcium ion, Ca2+, and the polyatomic carbonate ion, CO32-, is an ionic bond. The
bonds within the carbonate ion are covalent bonds.
.
Score
4
3
2
1
0
Blank
Description
Student clearly explains the bond between the calcuim ion and polyatomic
carbonate ion as ionic and the bonds within the carbonate ion as covalent.
Student explains the bonds between the two ions are ionic and the bonds between
one ion as being covalent.
Student explains the covalent bond, but is incorrect in explaining the ionic bond.
OR
Student explains the ionic bond, but is incorrect in explaining the covalent bond.
Student only explains the covalent bond.
OR
Student only explains the ionic bond.
Student’s response is totally incorrect or irrelevant.
No student response.
PTS: 1
DIF: DOK 3
OBJ: 5-2
STA: C4.2d | C4.3g | C5.5A
5. ANS:
The state of matter at room temperature can be used to classify most ionic and covalent compounds. Most
covalent compounds are liquids or gases at room temperature. Most ionic compounds are crystalline solids
with high melting points.
Score
Description
Student provides a physical property that can be used to tell whether a compound
4
is ionic or covalent and clearly explains his or her reasoning.
Student provides a physical property that can be used to tell whether a compound
3
is ionic or covalent, but does not clearly explain his or her reasoning.
Student provides an incorrect physical property that can be used to tell whether a
2
compound is ionic or covalent, but does explain his or her reasoning.
Student provides an incorrect physical property that can be used to tell whether a
1
compound is ionic or covalent and does not explain his or her reasoning.
Student’s response is totally incorrect or irrelevant.
0
No student response.
Blank
PTS: 1
DIF:
DOK 3
OBJ: 5-2
MULTIPLE CHOICE
6. ANS: B
7. ANS: D
PTS: 1
PTS: 1
3
STA: C4.3d | C4.3e
ID: B
8. ANS:
OBJ:
9. ANS:
OBJ:
10. ANS:
11. ANS:
12. ANS:
13. ANS:
OBJ:
14. ANS:
STA:
15. ANS:
OBJ:
16. ANS:
STA:
17. ANS:
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20. ANS:
21. ANS:
22. ANS:
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24. ANS:
25. ANS:
26. ANS:
OBJ:
27. ANS:
28. ANS:
STA:
29. ANS:
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31. ANS:
32. ANS:
33. ANS:
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35. ANS:
36. ANS:
STA:
37. ANS:
38. ANS:
39. ANS:
STA:
40. ANS:
41. ANS:
STA:
42. ANS:
C
PTS: 1
2
C
PTS: 1
1
B
PTS: 1
D
PTS: 1
A
PTS: 1
C
PTS: 1
1
C
PTS: 1
SCI.IV.2.MS.2 | SCI.IV.2.MS.3
C
PTS: 1
1
C
PTS: 1
SCI.IV.2.MS.2 | SCI.IV.2.MS.3
C
PTS: 1
B
PTS: 1
A
PTS: 1
A
PTS: 1
A
PTS: 1
D
PTS: 1
D
PTS: 1
D
PTS: 1
B
PTS: 1
C
PTS: 1
4
A
PTS: 1
A
PTS: 1
SCI.IV.2.MS.2 | SCI.IV.2.MS.3
B
PTS: 1
B
PTS: 1
C
PTS: 1
C
PTS: 1
C
PTS: 1
D
PTS: 1
A
PTS: 1
A
PTS: 1
SCI.IV.2.MS.2 | SCI.IV.2.MS.3
C
PTS: 1
C
PTS: 1
B
PTS: 1
SCI.IV.2.MS.2 | SCI.IV.2.MS.3
B
PTS: 1
C
PTS: 1
SCI.IV.2.MS.2 | SCI.IV.2.MS.3
A
PTS: 1
DIF:
1
REF: 3
DIF:
1
REF: 3
DIF:
B
OBJ: 3/1
DIF:
1
REF: 3
DIF:
B
OBJ: 2/1
DIF:
2
REF: 3
DIF:
B
OBJ: 8/3
DIF:
A
OBJ: 8/3
DIF:
DIF:
A
B
OBJ: 8/3
OBJ: 2/1
DIF:
1
REF: 1
DIF:
B
OBJ: 8/3
DIF:
B
OBJ: 9/3
DIF:
B
OBJ: 2/1
DIF:
B
OBJ: 10/3
DIF:
DIF:
A
B
OBJ: 8/3
OBJ: 3/1
DIF:
B
OBJ: 8/3
4
ID: B
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
STA:
ANS:
C
PTS: 1
A
PTS: 1
A
PTS: 1
A
PTS: 1
2
B
PTS: 1
2
B
PTS: 1
A
PTS: 1
A
PTS: 1
D
PTS: 1
D
PTS: 1
1
C
PTS: 1
1
C
PTS: 1
SCI.IV.2.MS.2 | SCI.IV.2.MS.3
B
PTS: 1
DIF:
A
OBJ: 8/3
DIF:
1
REF: 3
DIF:
1
REF: 1
DIF:
DIF:
DIF:
A
B
1
OBJ: 8/3
OBJ: 2/1
REF: 3
DIF:
1
REF: 3
DIF:
B
OBJ: 5/2
5