Chem 1 Chapter 8-9 review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. What information does a molecular formula provide?
a. the number and kind of atoms that are
c. information about a molecule’s structure
bonded by the transfer of electrons
b. the simplest whole-number ratio of atoms d. the number and kind of atoms present in a
that are bonded by the transfer of electrons
molecule
____
2. What is shown by the structural formula of a molecule or polyatomic ion?
a. the arrangement of bonded atoms
c. the number of metallic bonds
b. the number of ionic bonds
d. the shapes of molecular orbitals
____
3. Why do atoms share electrons in covalent bonds?
a. to become ions and attract each other
c. to become more polar
b. to attain a noble-gas electron
d. to increase their atomic numbers
configuration
____
4. Which of the following elements can form diatomic molecules held together by triple covalent bonds?
a. carbon
c. fluorine
b. oxygen
d. nitrogen
____
5. Which noble gas has the same electron configuration as the oxygen in a water molecule?
a. helium
c. argon
b. neon
d. xenon
____
6. Which elements can form diatomic molecules joined by a single covalent bond?
a. hydrogen only
c. halogens and members of the oxygen
group only
b. halogens only
d. hydrogen and the halogens only
____
7. What is the representative unit in a molecular compound?
a. a molecule
c. a formula unit
b. an ion
d. shared electrons
____
8. Which molecule has a single covalent bond?
a. CO
b. Cl
____
c. CO
d. N
9. Which of the following bonds is the least reactive?
a. C—C
c. O—H
b. H—H
d. H—Cl
____ 10. How many valid electron dot formulas—having the same number of electron pairs for a molecule or ion—can
be written when a resonance structure occurs?
a. 0
c. 2 only
b. 1 only
d. 2 or more
____ 11. A resonance structure, like the one above, represents
a. a difference in energy.
c. a difference in bond length, one shorter
than the other.
b. electron pairs resonating back and forth
d. a hybrid of the extremes represented by
between the extremes of the two
the resonance forms.
structures.
____ 12. Molecular orbital theory is based upon which of the following models of the atom?
a. classical mechanical model
c. quantum mechanical model
b. Bohr model
d. Democritus’s model
____ 13. A pair of molecular orbitals is formed by the
a. splitting of a single atomic orbital.
b. reproduction of a single atomic orbital.
c. overlap of two atomic orbitals from the
same atom.
d. overlap of two atomic orbitals from
different atoms.
____ 14. The side-by-side overlap of p orbitals produces what kind of bond?
a. alpha bond
c. pi bond
b. beta bond
d. sigma bond
____ 15. Where are the electrons most probably located in a molecular bonding orbital?
a. anywhere in the orbital
c. in stationary positions between the two
atomic nuclei
b. between the two atomic nuclei
d. in circular orbits around each nucleus
____ 16. Sigma bonds are formed as a result of the overlapping of which type(s) of atomic orbital(s)?
a. s only
c. d only
b. p only
d. s and p
____ 17. Which of the following bond types is normally the weakest?
a. sigma bond formed by the overlap of two c. sigma bond formed by the overlap of one s
s orbitals
and one p orbital
b. sigma bond formed by the overlap of two d. pi bond formed by the overlap of two p
p orbitals
orbitals
____ 18. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as
possible?
a. pairs of valence electrons
c. mobile electrons
b. inner shell electrons
d. the electrons closest to the nuclei
____ 19. What causes water molecules to have a bent shape, according to VSEPR theory?
a. repulsive forces between unshared pairs of c. ionic attraction and repulsion
electrons
b. interaction between the fixed orbitals of
d. the unusual location of the free electrons
the unshared pairs of oxygen
____ 20. Which of the following theories provides information concerning both molecular shape and molecular
bonding?
a. molecular orbital theory
b. VSEPR theory
c. orbital hybridization theory
d. Bohr atomic theory
____ 21. Experimental evidence suggests that the H—C—H bond angles in ethene, C H , are ____.
a. 90
c. 120
b. 109.5
d. 180
____ 22. What type of hybrid orbital exists in the methane molecule?
a. sp
c. sp
b. sp
d. sp d
____ 23. Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen?
a. C
c. O
b. Na
d. S
____ 24. Which of the following covalent bonds is the most polar?
a. H—F
c. H—H
b. H—C
d. H—N
____ 25. Which of the forces of molecular attraction is the weakest?
a. dipole interaction
c. hydrogen bond
b. dispersion
d. single covalent bond
____ 26. What causes dipole interactions?
a. sharing of electron pairs
b. attraction between polar molecules
c. bonding of a covalently bonded hydrogen
to an unshared electron pair
d. attraction between ions
____ 27. What are the weakest attractions between molecules?
a. ionic forces
c. covalent forces
b. Van der Waals forces
d. hydrogen forces
____ 28. What causes hydrogen bonding?
a. attraction between ions
b. motion of electrons
c. sharing of electron pairs
d. bonding of a covalently bonded hydrogen
atom with an unshared electron pair
____ 29. Which type of solid has the highest melting point?
a. ionic solid
c. metal
b. network solid
d. nonmetallic solid
____ 30. What type of ions have names ending in -ide?
a. only cations
c. only metal ions
b. only anions
d. only gaseous ions
____ 31. In which of the following are the symbol and name for the ion given correctly?
a. Fe : ferrous ion; Fe : ferric ion
c. Co : cobalt(II) ion; Co : cobaltous ion
b. Sn : stannic ion; Sn : stannous ion
d. Pb : lead ion; Pb : lead(IV) ion
____ 32. Which of the following determines that an element is a metal?
a. the magnitude of its charge
c. when it is a Group A element
b. the molecules that it forms
d. whether it loses valence electrons
____ 33. What is the Stock name for chromic ion?
a. chromium(I) ion
b. chromium(II) ion
c. chromium(III) ion
d. chromium(IV) ion
____ 34. In which of the following are the symbol and name for both of the ions given correctly?
a. NH : ammonia; H : hydride
c. OH : hydroxide; O : oxide
b. C H O
: acetate; C O
: oxalite
d. PO
: phosphate; PO
: phosphite
____ 35. Which of the following correctly provides the names and formulas of polyatomic ions?
a. carbonate: HCO ; bicarbonate: CO
c. sulfite: S ; sulfate: SO
b. nitrite: NO ; nitrate: NO
d. chromate: CrO
; dichromate: Cr O
____ 36. An -ate or -ite at the end of a compound name usually indicates that the compound contains
a. fewer electrons than protons.
c. only two elements.
b. neutral molecules.
d. a polyatomic anion.
____ 37. Systematic names are preferred over common names because common names
a. do not tell you the actual charge of the ion. c. were assigned by the scientist who
discovered the compound.
b. are derived from the method used to
d. are not very descriptive.
obtain the compound.
____ 38. How are chemical formulas of binary ionic compounds generally written?
a. cation on left, anion on right
c. Roman numeral first, then anion, then
cation
b. anion on left, cation on right
d. subscripts first, then ions
____ 39. Which of the following is true about the composition of ionic compounds?
a. They are composed of anions and cations. c. They are composed of cations only.
b. They are composed of anions only.
d. They are formed from two or more
nonmetallic elements.
____ 40. Which of the following formulas represents an ionic compound?
a. CS
c. N O
b. BaI
d. PCl
____ 41. In which of the following is the name and formula given correctly?
a. sodium oxide, NaO
c. cobaltous chloride, CoCl
b. barium nitride, BaN
d. stannic fluoride, SnF
____ 42. Which of the following compounds contains the lead(II) ion?
a. PbO
c. Pb2O
b. PbCl4
d. Pb2S
____ 43. Which set of chemical name and chemical formula for the same compound is correct?
a. iron(II) oxide, Fe O
c. tin(IV) bromide, SnBr
b. aluminum fluorate, AlF
d. potassium chloride, K Cl
____ 44. What is the correct formula for potassium sulfite?
a. KHSO
b. KHSO
c. K SO
d. K SO
____ 45. Which set of chemical name and chemical formula for the same compound is correct?
a. ammonium sulfite, (NH ) S
c. lithium carbonate, LiCO
b. iron(III) phosphate, FePO
d. magnesium dichromate, MgCrO
____ 46. What type of compound is CuSO ?
a. monotomic ionic
b. polyatomic covalent
c. polyatomic ionic
d. binary molecular
____ 47. Which polyatomic ion forms a neutral compound when combined with a group 1A monatomic ion in a 1:1
ratio?
a. ammonium
c. nitrate
b. carbonate
d. phosphate
____ 48. What is the ending for the names of all binary compounds, both ionic and molecular?
a. -ide
c. -ade
b. -ite
d. -ate
____ 49. Which of the following is a binary molecular compound?
a. BeHCO
c. AgI
b. PCl
d. MgS
____ 50. Which of the following formulas represents a molecular compound?
a. ZnO
c. SO
b. Xe
d. BeF
____ 51. What is the formula for sulfurous acid?
a. H SO
b. H SO
c. H SO
d. H S
____ 52. Which of the following are produced when a base is dissolved in water?
a. hydronium ions
c. hydrogen ions
b. hydroxide ions
d. ammonium ions
____ 53. How are bases named?
a. like monatomic elements
b. like polyatomic ions
c. like ionic compounds
d. like molecular compounds
____ 54. Select the correct formula for sulfur hexafluoride.
a. S F
c. F S
b. F SO
d. SF
____ 55. What is the correct name for the compound CoCl ?
a. cobalt(I) chlorate
c. cobalt(II) chlorate
b. cobalt(I) chloride
d. cobalt(II) chloride
____ 56. Suppose you encounter a chemical formula with H as the cation. What do you know about this compound
immediately?
a. It is a polyatomic ionic compound.
c. It is a base.
b. It is an acid.
d. It has a 1 charge.
____ 57. What is the correct formula for calcium dihydrogen phosphate?
a. CaH PO
c. Ca(H PO )
b. Ca H PO
d. Ca(H HPO )
____ 58. What does an -ite or -ate ending in a polyatomic ion mean?
a. Oxygen is in the formula.
c. Nitrogen is in the formula.
b. Sulfur is in the formula.
d. Bromine is in the formula.
____ 59. Which of the following is the correct name for N O ?
a. nitrous oxide
c. nitrogen dioxide
b. dinitrogen pentoxide
d. nitrate oxide
____ 60. What is the correct name for Sn (PO ) ?
a. tritin diphosphate
b. tin(II) phosphate
c. tin(III) phosphate
d. tin(IV) phosphate
Chem 1 Chapter 8-9 review
Answer Section
MULTIPLE CHOICE
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14. ANS:
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15. ANS:
D
PTS: 1
DIF: L2
REF: p. 222
8.1.1 Identify the information a molecular formula provides.
C.3.1 | C.3.2 | C.3.3
BLM: comprehension
A
PTS: 1
DIF: L1
REF: p. 227
8.2.1 Explain the result of electron sharing in covalent bonds.
C.3.1 | C.3.2 | C.3.3
BLM: comprehension
B
PTS: 1
DIF: L2
REF: p. 226
8.2.1 Explain the result of electron sharing in covalent bonds.
C.3.1 | C.3.2 | C.3.3
BLM: comprehension
D
PTS: 1
DIF: L2
REF: p. 230
8.2.1 Explain the result of electron sharing in covalent bonds.
C.3.1 | C.3.2 | C.3.3
BLM: comprehension
B
PTS: 1
DIF: L2
REF: p. 227
8.2.1 Explain the result of electron sharing in covalent bonds.
C.3.1 | C.3.2 | C.3.3
BLM: application
D
PTS: 1
DIF: L3
REF: p. 226 | p. 227
8.2.1 Explain the result of electron sharing in covalent bonds.
C.3.1 | C.3.2 | C.3.3
BLM: comprehension
A
PTS: 1
DIF: L2
REF: p. 226
8.1.2 Describe the representative units that define molecular compounds and ionic compounds.
C.3.1 | C.3.2 | C.3.3
BLM: comprehension
B
PTS: 1
DIF: L2
REF: p. 230
8.2.1 Explain the result of electron sharing in covalent bonds.
C.3.1 | C.3.2 | C.3.3
BLM: application
B
PTS: 1
DIF: L2
REF: p. 236 | p. 237
8.2.4 Explain how the strength of a covalent bond is related to its bond dissociation energy.
C.3.1 | C.3.2 | C.3.3
BLM: application
A
PTS: 1
DIF: L2
REF: p. 237
8.2.5 Describe how resonance structures are used.
STA: C.3.1 | C.3.2 | C.3.3
comprehension
D
PTS: 1
DIF: L2
REF: p. 237
8.2.5 Describe how resonance structures are used.
STA: C.3.1 | C.3.2 | C.3.3
comprehension
C
PTS: 1
DIF: L1
REF: p. 240
8.3.1 Describe the relationship between atomic and molecular orbitals.
C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: comprehension
D
PTS: 1
DIF: L2
REF: p. 240
8.3.1 Describe the relationship between atomic and molecular orbitals.
C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: comprehension
C
PTS: 1
DIF: L2
REF: p. 241
8.3.1 Describe the relationship between atomic and molecular orbitals.
C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: comprehension
B
PTS: 1
DIF: L2
REF: p. 241
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
OBJ: 8.3.1 Describe the relationship between atomic and molecular orbitals.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: comprehension
ANS: D
PTS: 1
DIF: L2
REF: p. 240 | p. 241
OBJ: 8.3.1 Describe the relationship between atomic and molecular orbitals.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: comprehension
ANS: D
PTS: 1
DIF: L2
REF: p. 241
OBJ: 8.3.1 Describe the relationship between atomic and molecular orbitals.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: comprehension
ANS: A
PTS: 1
DIF: L1
REF: p. 242
OBJ: 8.3.2 Describe how VSEPR theory helps predict the shapes of molecules.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: knowledge
ANS: A
PTS: 1
DIF: L2
REF: p. 243
OBJ: 8.3.2 Describe how VSEPR theory helps predict the shapes of molecules.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: comprehension
ANS: C
PTS: 1
DIF: L1
REF: p. 244
OBJ: 8.3.3 Identify the ways in which orbital hybridization is useful in describing molecules.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: knowledge
ANS: C
PTS: 1
DIF: L1
REF: p. 245
OBJ: 8.3.3 Identify the ways in which orbital hybridization is useful in describing molecules.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: knowledge
ANS: C
PTS: 1
DIF: L1
REF: p. 244
OBJ: 8.3.3 Identify the ways in which orbital hybridization is useful in describing molecules.
STA: C.3.1 | C.3.2 | C.3.3 | C.3.4
BLM: knowledge
ANS: C
PTS: 1
DIF: L2
REF: p. 248 | p. 249
OBJ: 8.4.1 Describe how electronegativity values determine the charge distribution in a polar molecule.
STA: C.3.1 | C.3.2 | C.3.3
BLM: application
ANS: A
PTS: 1
DIF: L3
REF: p. 248 | p. 249
OBJ: 8.4.1 Describe how electronegativity values determine the charge distribution in a polar molecule.
STA: C.3.1 | C.3.2 | C.3.3
BLM: application
ANS: B
PTS: 1
DIF: L1
REF: p. 251
OBJ: 8.4.2 Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and
covalent bonds.
STA: C.3.1 | C.3.2 | C.3.3
BLM: knowledge
ANS: B
PTS: 1
DIF: L1
REF: p. 251
OBJ: 8.4.2 Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and
covalent bonds.
STA: C.3.1 | C.3.2 | C.3.3
BLM: knowledge
ANS: B
PTS: 1
DIF: L1
REF: p. 250
OBJ: 8.4.2 Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and
covalent bonds.
STA: C.3.1 | C.3.2 | C.3.3
BLM: knowledge
ANS: D
PTS: 1
DIF: L2
REF: p. 251
OBJ: 8.4.2 Evaluate the strengths of intermolecular attractions compared with the strengths of ionic and
covalent bonds.
STA: C.3.1 | C.3.2 | C.3.3
BLM: comprehension
ANS: B
PTS: 1
DIF: L1
REF: p. 252
OBJ: 8.4.3 Explain why the properties of covalent compounds are so diverse.
STA: C.3.1 | C.3.2 | C.3.3
BLM: knowledge
ANS: B
PTS: 1
DIF: L2
REF: p. 265 | p. 267
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
STA: C.3.5
BLM: comprehension
ANS: A
PTS: 1
DIF: L2
REF: p. 265 | p. 266
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
STA: C.3.5
BLM: application
32. ANS: D
PTS: 1
DIF: L2
REF: p. 264
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
STA: C.3.5
BLM: comprehension
33. ANS: C
PTS: 1
DIF: L2
REF: p. 266
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
STA: C.3.5
BLM: application
34. ANS: C
PTS: 1
DIF: L2
REF: p. 264 | p. 265 | p. 268
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions. | 9.1.2 Explain how polyatomic ions
differ from and are similar to monatomic ions.
STA: C.3.5
BLM: application
35. ANS: D
PTS: 1
DIF: L2
REF: p. 268 | p. 269
OBJ: 9.1.2 Explain how polyatomic ions differ from and are similar to monatomic ions.
STA: C.3.5
BLM: application
36. ANS: D
PTS: 1
DIF: L2
REF: p. 268 | p. 269
OBJ: 9.1.2 Explain how polyatomic ions differ from and are similar to monatomic ions.
STA: C.3.5
BLM: application
37. ANS: A
PTS: 1
DIF: L2
REF: p. 266
OBJ: 9.1.1 Explain how to determine the charges of monatomic ions.
STA: C.3.5
BLM: comprehension
38. ANS: A
PTS: 1
DIF: L2
REF: p. 272
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
STA: C.3.5
BLM: comprehension
39. ANS: A
PTS: 1
DIF: L2
REF: p. 272
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
STA: C.3.5
BLM: comprehension
40. ANS: B
PTS: 1
DIF: L2
REF: p. 272 | p. 280
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds. | 9.3.1 Apply the
rules for naming and writing formulas for binary molecular compounds.
STA: C.3.5 | C.3.4 BLM: application
41. ANS: D
PTS: 1
DIF: L2
REF: p. 272 | p. 273 | p. 274 | p. 275
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
STA: C.3.5
BLM: application
42. ANS: A
PTS: 1
DIF: L2
REF: p. 272 | p. 273
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
STA: C.3.5
BLM: application
43. ANS: C
PTS: 1
DIF: L2
REF: p. 272 | p. 273 | p. 274 | p. 275
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds.
STA: C.3.5
BLM: application
44. ANS: C
PTS: 1
DIF: L2
REF: p. 276 | p. 277
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions.
STA: C.3.5
BLM: application
45. ANS: B
PTS: 1
DIF: L2
REF: p. 276 | p. 277 | p. 278
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions.
STA: C.3.5
BLM: application
46. ANS: C
PTS: 1
DIF: L2
REF: p. 268 | p. 278
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions.
STA: C.3.5
BLM: application
47. ANS: C
PTS: 1
DIF: L2
REF: p. 276 | p. 277
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions.
STA: C.3.5
BLM: analysis
ANS: A
PTS: 1
DIF: L2
REF: p. 265 | p. 275 | p. 280
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds. | 9.3.1 Apply the
rules for naming and writing formulas for binary molecular compounds.
STA: C.3.5 | C.3.4 BLM: comprehension
ANS: B
PTS: 1
DIF: L2
REF: p. 280 | p. 281
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds.
STA: C.3.4
BLM: application
ANS: C
PTS: 1
DIF: L2
REF: p. 280
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds.
STA: C.3.4
BLM: application
ANS: B
PTS: 1
DIF: L2
REF: p. 286 | p. 287
OBJ: 9.4.1 Determine the name and formula of an acid.
STA: C.3.4
BLM: application
ANS: B
PTS: 1
DIF: L1
REF: p. 287
OBJ: 9.4.2 Determine the name and formula of a base.
STA: C.3.4
BLM: knowledge
ANS: C
PTS: 1
DIF: L1
REF: p. 287
OBJ: 9.4.2 Determine the name and formula of a base.
STA: C.3.4
BLM: knowledge
ANS: D
PTS: 1
DIF: L2
REF: p. 282 | p. 283 | p. 293 | p. 294
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds. | 9.5.2 List the
general guidelines that can help you write the name and formula of a chemical compound.
STA: C.3.4
BLM: application
ANS: D
PTS: 1
DIF: L2
REF: p. 272 | p. 273 | p. 293 | p. 294
OBJ: 9.2.1 Apply the rules for naming and writing formulas for binary ionic compounds. | 9.5.2 List the
general guidelines that can help you write the name and formula of a chemical compound.
STA: C.3.5 | C.3.4 BLM: application
ANS: B
PTS: 1
DIF: L2
REF: p. 285 | p. 293
OBJ: 9.4.1 Determine the name and formula of an acid. | 9.5.2 List the general guidelines that can help you
write the name and formula of a chemical compound.
STA: C.3.4
BLM: comprehension
ANS: C
PTS: 1
DIF: L2
REF: p. 276 | p. 277 | p. 293 | p. 294
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions. | 9.5.2
List the general guidelines that can help you write the name and formula of a chemical compound.
STA: C.3.5 | C.3.4 BLM: application
ANS: A
PTS: 1
DIF: L2
REF: p. 268
OBJ: 9.1.2 Explain how polyatomic ions differ from and are similar to monatomic ions.
STA: C.3.5
BLM: comprehension
ANS: B
PTS: 1
DIF: L2
REF: p. 281 | p. 282 | p. 292 | p. 293
OBJ: 9.3.1 Apply the rules for naming and writing formulas for binary molecular compounds. | 9.5.2 List the
general guidelines that can help you write the name and formula of a chemical compound.
STA: C.3.4
BLM: application
ANS: B
PTS: 1
DIF: L2
REF: p. 278 | p. 279 | p. 292 | p. 293
OBJ: 9.2.2 Apply the rules for naming and writing formulas for compounds with polyatomic ions. | 9.5.2
List the general guidelines that can help you write the name and formula of a chemical compound.
STA: C.3.5 | C.3.4 BLM: application