Name:______________________________Class: _________________ Date: _________________
Assessment
Chapter Test B
Teacher Notes and Answers
7
Chemical Formulas and
Chemical Compounds
TEST B
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
c
d
d
a
d
d
c
b
+6
1
+2
+4
SiO2
CI4
Sn(CrO4)2
Ba(OH)2
phosphorus(III) iodide
dinitrogen tetroxide
iron(II) nitrite
carbon tetrachloride
carbon monoxide
copper(II) carbonate
CaCl2, calcium chloride
PbCrO4, lead(II) chromate
Al2(SO4)3, aluminum sulfate
Sn3(PO4)4, tin(IV) phosphate
cyanide ion
oxide ion
hydroxide ion
S2 Cu+
CO 32
H, +1; O, 1
C, +4; O, 2
N, 3; H, +1
323.5 g/mol
134.45 amu
47.27% Cu, 52.73% Cl
43.2 g
CF4
C4H10
C2H6
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
1
Chapter Test
Name:______________________________Class: _________________ Date: _________________
Assessment
Chapter Test B
Chapter: Chemical Formulas and Chemical Compounds
PART I In the space provided, write the letter of the term or phrase that best
completes each statement or best answers each question.
_____ 1. Changing a subscript in a correctly written chemical formula will
a. change the electron configuration of that element.
b. change the charges on the other ions in the compound.
c. change the formula so that it no longer represents the same
compound.
d. have no effect on the formula.
_____ 2. Using the Stock system of nomenclature, Cr2(SO4)3 is named
a. chromium(II) sulfate.
b. chromic sulfate.
c. dichromium trisulfate.
d. chromium(III) sulfate.
_____ 3. In a polyatomic ion, the algebraic sum of the oxidation numbers of all
atoms is equal to
a. 0.
b. 10.
c. the number of atoms in the ion.
d. the charge on the ion.
_____ 4. The first part of the name of a binary ionic compound is the
a. cation.
b. polyatomic ion.
c. oxyanion.
d. anion.
_____ 5. The empirical formula may not represent the actual composition of a(n)
a. ionic compound.
b. crystal.
c. salt.
d. molecular compound.
_____ 6. The formula for phosphoric acid is
a. HPO4.
b. H(PO4)2.
c. H2PO3.
d. H3PO4.
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
2
Chapter Test
Name:______________________________Class: _________________ Date: _________________
Chapter Test B, continued
_____ 7. The term formula mass can be applied to both ionic compounds and
molecular compounds because
a. ionic compounds exist as individual molecules.
b. not all molecular formulas are empirical formulas.
c. not all formulas represent individual molecules.
d. all molecular formulas are Lewis formulas.
_____ 8. To determine the correct molecular formula of a compound from an
empirical formula, one must determine the
a. density.
b. formula mass.
c. structural formula.
d. crystal lattice.
PART II
Write the oxidation number for the given element in the space provided.
9. Sulfur in H2SO4
____________________
10. Oxygen in peroxides
____________________
11. Magnesium in MgO
____________________
12. Silicon in SiCl4
____________________
Write the formulas for the following compounds in the space provided.
13. Silicon dioxide
_____________________
14. Carbon tetriodide
_____________________
15. Tin(IV) chromate
_____________________
16. Barium hydroxide
_____________________
Write the names of the following compounds in the space provided. Use the Stock
system or prefixes, as indicated.
17. PI3, Stock system
____________________________
18. N2O4, prefixes
____________________________
19. Fe(NO2)2, Stock system
____________________________
20. CCl4, prefixes
____________________________
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
3
Chapter Test
Name:______________________________Class: _________________ Date: _________________
Chapter Test B, continued
21. CO, prefixes
____________________________
22. CuCO3, Stock system
____________________________
Write the formulas and give the names of the compounds formed by the following
ions in the space provided.
2+
23. Ca
2+
24. Pb
3+
25. Al
4+
26. Sn
and Cl
____________________________________
2
and CrO 4
____________________________________
and
SO 24 ____________________________________
and
PO 34
____________________________________
Name each of the following ions in the space provided.
27. CN
28. O
2
29. OH
____________________________
____________________________
____________________________
Write the formulas and indicate the charges for the following ions in the space
provided.
30. sulfide ion
___________________
31. copper(I) ion
___________________
32. carbonate ion
___________________
Write each atom and its oxidation number in the space provided.
33. H2O2
___________________________
34.
___________________________
35.
CO 32
NH +4
___________________________
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
4
Chapter Test
Name:______________________________Class: _________________ Date: _________________
Chapter Test B, continued
PART III Use the table of atomic masses to answer the following questions. Write
your answer on the line to the left, and show your work in the space provided.
Element
Symbol Atomic mass Element
Symbol
Atomic mass
Aluminum
Al
26.98 u
Lead
Pb
Bromine
Br
79.90 u
Li
Carbon
C
12.01 u
Mg
24.30 u
Chlorine
Cl
35.45 u
Lithium
Magnesiu
m
Manganes
e
Mn
54.94 u
Chromium
Cr
52.00 u
Nitrogen
N
14.01 u
Copper
Cu
63.55 u
Oxygen
O
16.00 u
Fluorine
Hydrogen
F
H
19.00 u
1.01 u
Sodium
Sulfur
Na
S
22.99 u
32.07 u
207.2 u
6.94 u
36. ________________ What is the molar mass of tetraethyl lead, Pb(C2H5)4?
37. ________________ What is the formula mass of copper(II) chloride, CuCl2?
38. ________________ What is the percentage composition of CuCl2 by mass?
39. ________________ What is the mass of 0.240 mol glucose, C6H12O6?
40. ________________ What is the empirical formula for a sample of a
compound that contains 259.2 g F and 40.8 g C?
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
5
Chapter Test
Name:______________________________Class: _________________ Date: _________________
Chapter Test B, continued
41. ________________ The empirical formula for a compound is C2H5 and its
formula mass is 58 u. What is its molecular formula?
42. ________________ A sample of a compound is 80% carbon and 20%
hydrogen by mass. Its formula mass is 30 u. What is its
molecular formula?
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
6
Chapter Test
Name:______________________________Class: _________________ Date: _________________
CHAPTER 7 REVIEW
Chemical Formulas and Chemical
Compounds
Teacher Notes and Answers
SHORT ANSWER
1. a.
b.
c.
d.
e.
2. a.
b.
c.
d.
e.
CuCO3
Na2SO3
(NH4)3PO4
SnS2
HNO2
magnesium perchlorate
iron(II) nitrate
iron(III) nitrite
cobalt(II) oxide
nitrogen(V) oxide
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
1
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
CHAPTER 7 REVIEW
Chemical Formulas and Chemical
Compounds
MIXED REVIEW
SHORT ANSWER Answer the following questions in the space provided.
1. Write formulas for the following compounds:
__________________ a. copper(II) carbonate
__________________ b. sodium sulfite
__________________ c. ammonium phosphate
__________________ d. tin(IV) sulfide
__________________ e. nitrous acid
2. Write the Stock system names for the following compounds:
__________________________ a. Mg(ClO4)2
__________________________ b. Fe(NO3)2
__________________________ c. Fe(NO2)3
__________________________ d. CoO
__________________________ e. dinitrogen pentoxide
3. ___________________ a. How many atoms are represented by the formula
Ca(HSO4)2?
__________________ b. How many moles of oxygen atoms are in a 0.50
mol sample of this compound?
__________________ c. Assign the oxidation number to sulfur in the HSO 4
anion.
4. Assign the oxidation number to the element specified in each of the following:
_______ a. hydrogen in H2O2
_______ b. hydrogen in MgH2
_______ c. sulfur in S8
_______ d. carbon in (CO3)2
_______ e. chromium in Na2Cr2O7
_______ f. nitrogen in NO2
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
2
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
MIXED REVIEW continued
PROBLEMS Write the answer on the line to the left. Show all your work in the
space provided.
5. ___________________ Following are samples of four different compounds.
Arrange them in order of increasing mass, from
smallest to largest.
a. 25 g of oxygen gas c. 3 1023 molecules of C2H6
b. 1.00 mol of H2O
d. 2 1023 molecules of C2H6O2
6. ___________________ a. What is the formula for sodium hydroxide?
__________________ b. What is the formula mass of sodium hydroxide?
__________________ c. What is the mass in grams of 0.25 mol of sodium
hydroxide?
7. ___________________ What is the percentage composition of ethane gas,
C2H6, to the nearest whole number?
8. __________________
Ribose is an important sugar (part of RNA),with a
molar mass of 150.15 g/mol. If its empirical formula
is CH2O, what is its molecular formula?
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
3
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
MIXED REVIEW continued
9. Butane gas, C4H10, is often used as a fuel.
__________________ a. What is the mass in grams of 3.00 mol of butane?
__________________ b. How many molecules are present in that 3.00 mol
sample?
__________________ c. What is the empirical formula of the gas?
10. __________________
Naphthalene is a soft covalent solid that is often used
in mothballs. Its molar mass is 128.18 g/mol and it
contains 93.75% carbon and 6.25% hydrogen.
Determine the molecular formula of napthalene from
this information.
11. Nicotine has the formula CxHyNz. To determine its composition, a sample is
burned in excess oxygen, producing the following results:
1.0 mol of CO2
0.70 mol of H2O
0.20 mol of NO2
Assume that all the atoms in nicotine are present as products.
__________________ a. Determine the number of moles of carbon present
in the products of this combustion.
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
4
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
MIXED REVIEW continued
__________________ b. Determine the number of moles of hydrogen
present in the combustion products.
__________________ c. Determine the number of moles of nitrogen present
in the combustion products.
__________________ d. Determine the empirical formula of nicotine based
on your calculations.
__________________ e. In a separate experiment, the molar mass of
nicotine is found to be somewhere between 150
and 180 g/mol. Calculate the molar mass of
nicotine to the nearest gram.
12. When MgCO3(s) is strongly heated, it produces solid MgO as gaseous CO2 is
driven off.
__________________________ a. What is the percentage loss in mass as
this reaction occurs?
__________________________ b. Assign the oxidation number to each
atom in MgCO3.
__________________________ c. Does the oxidation number of carbon
change upon the formation of CO2?
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
5
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
CHAPTER 7 REVIEW
Chemical Formulas and Chemical
Compounds
Teacher Notes and Answers
SECTION 2
Chapter 7
SECTION 1
SHORT ANSWER
1. a. +4
b. +6
c. 2
d. +1
e. +6
f. +5
g. +4
h. 3
2. a. SCl2
b. nitrogen(IV) oxide
3. a. fluorine
b. 0; F2
4. a. tin(IV) oxide
b. SnO
5. a. NO, NO2
b. ClO
6. a. N2O3
b. +3
c. The three oxygen atoms have oxidation
states of 6 total, and because the algebraic
sum of the oxidation states in a neutral
compound must be zero, the two nitrogen
atoms must have oxidation states of +6 total,
therefore +3 each.
nitrogen(III) oxide
7. a. Carbon is +4 and each oxygen is 2.
b. Carbon is 4 and each hydrogen is +1.
c. Each carbon is 0, each hydrogen is +1,
and each oxygen is 2.
d. Each carbon is 8/3 and each hydrogen
is +1.
8. a. Each iron is +3 and each oxygen is 2.
b. Nitrogen is +4 and each oxygen is 2.
c. Chromium is +4 and each oxygen is 2.
SHORT ANSWER
1. c
2. c
3. a. 4 elements
b. 6 oxygen atoms
c. 21 atoms
d. 4.2 1024 atoms
4. a. 11 atoms
b. 45 atoms
c. 10 atoms
d. 9 atoms
5. a. N2O5
b. iron(II) oxide
c. H2SO3
d. phosphoric acid
6. a. True
b. True
7. a. In general, if the anion name ends in ate, the corresponding acid name will end
in a suffix of -ic. In general, if the anion
name ends in -ite, the corresponding acid
name will end in a suffix of -ous.
b. In general, if the anion name ends in ide, the corresponding acid name will end
in a suffix of -ic and begin with a prefix of
hydro-. The prefix hydro- is never used for
anions ending in -ate or -ite.
8.
Compound name
Formula
Aluminum sulfide
Al2S3
Cesium carbonate
Cs2CO3
Lead(II) chloride
PbCl2
Ammonium phosphate
(NH4)3PO4
Hydroiodic acid
HI
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
1
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
SECTION 3
2. C4H8
3. a. Na2S2O3
b. neither
4. a. 36%
b. 5
c. The second heating is to ensure that all
the water in the sample has been driven off.
If the mass is less after the second heating,
water was still present after the first heating.
5. a. CF2
b. C4F8
6. a. CuClO3
b. copper(I) chlorate
SHORT ANSWER
1. a. True
b. False
c. True
2. 10 mol of calcium, 20 mol of nitrogen, 60
mol of oxygen
3. a. 0.250 mol
b. 1.50 1023 molecules
c. 4.51 1023 carbon atoms
d. 10.1%
4. a. 52.9%
b. 2100 lb
5. a. 20 g
b. 0.17 mol
c. 4.0 mol
SECTION 4
SHORT ANSWER
1. a. CH3O2
b. N2O5
c. HgCl
d. CH2
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
2
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
CHAPTER 7 REVIEW
Chemical Formulas and Chemical
Compounds
SECTION 1
SHORT ANSWER Answer the following questions in the space provided.
1. _____ In a Stock system name such as iron(III) sulfate, the Roman numeral
tells us
(a) how many atoms of Fe are in one formula unit.
(b) how many sulfate ions can be attached to the iron atom.
(c) the charge on each Fe ion.
(d) the total positive charge of the formula unit.
2. _____ Changing a subscript in a correctly written chemical formula
(a) changes the number of moles represented by the formula.
(b) changes the charges on the other ions in the compound.
(c) changes the formula so that it no longer represents the compound it
previously represented.
(d) has no effect on the formula.
3. The explosive TNT has the molecular formula C7H5(NO2)3.
__________________ a. How many elements make up this compound?
__________________ b. How many oxygen atoms are present in one
molecule of C7H5(NO2)3?
__________________ c. How many atoms in total are present in one
molecule of C7H5(NO2)3?
__________________ d. How many atoms are present in a sample of 2.0 1023 molecules of C7H5(NO2)3?
4. How many atoms are present in each of these formula units?
__________________ a. Ca(HCO3)2
__________________ b. C12H22O11
__________________ c. Fe(ClO2)3
__________________ d. Fe(ClO3)2
5. ___________________ a. What is the formula for the compound dinitrogen
pentoxide?
__________________ b. What is the Stock system name for the compound
FeO?
__________________ c. What is the formula for sulfurous acid?
__________________ d. What is the name for the acid H3PO4?
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
2
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
SECTION 1 continued
6. Some binary compounds are ionic, others are covalent. The type of bond
favored partially depends on the position of the elements in the periodic table.
Label each of these claims as True or False; if False, specify the nature of the
error.
a. Covalently bonded binary molecular compounds are typically composed of
nonmetals.
_______________________________________________________________
_______________________________________________________________
b. Binary ionic compounds are composed of metals and nonmetals, typically
from opposite sides of the periodic table.
_______________________________________________________________
_______________________________________________________________
7. Refer to the text for examples of names and formulas for polyatomic ions and
acids.
a. Derive a generalization for determining whether an acid name will end in
the suffix -ic or -ous.
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
b. Derive a generalization for determining whether an acid name will begin
with the prefix hydro- or not.
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
8. Fill in the blanks in the table below.
Compound name
Formula
Aluminum sulfide
Cesium carbonate
PbCl2
(NH4)3PO4
Hydroiodic acid
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
3
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
CHAPTER 7 REVIEW
Chemical Formulas and Chemical
Compounds
SECTION 2
SHORT ANSWER Answer the following questions in the space provided.
1. Assign the oxidation number to the specified element in each of the following
examples:
_______ a. S in H2SO3
_______ b. S in MgSO4
_______ c. S in K2S
_______ d. Cu in Cu2S
_______ e. Cr in Na2CrO4
_______ f. N in HNO3
_______ g. C in (HCO3)
_______ h. N in (NH4)+
2. ___________________ a. What is the formula for the compound sulfur(II)
chloride?
__________________ b. What is the Stock system name for NO2?
3. ___________________ a. Use electronegativity values to determine the one
element that always has a negative oxidation
number when it appears in any binary compound.
__________________ b. What is the oxidation number and formula for the
element described in part a when it exists as a pure
element?
4. Tin has possible oxidation numbers of +2 and +4 and forms two known
oxides. One of them has the formula SnO2.
__________________ a. Give the Stock system name for SnO2.
__________________ b. Give the formula for the other oxide of tin.
5. Scientists think that two separate reactions contribute to the depletion of the
ozone, O3, layer. The first reaction involves oxides of nitrogen. The second
involves free chlorine atoms. The equations that represent the reactions follow.
When a compound is not stated as a formula, write the correct formula in the
blank beside its name.
a. ______ (nitrogen monoxide) + O3 ______ (nitrogen dioxide) + O2
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
4
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
SECTION 2 continued
b. Cl + O3 ______ (chlorine monoxide) + O2
6. Consider the covalent compound dinitrogen trioxide when answering the
following:
__________________ a. What is the formula for dinitrogen trioxide?
__________________ b. What is the oxidation number assigned to each
nitrogen atom in this compound? Explain your
answer.
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_________________ c. Give the Stock name for dinitrogen trioxide.
7. The oxidation numbers assigned to the atoms in some organic compounds
have unexpected values. Assign oxidation numbers to each atom in the
following compounds: (Note: Some oxidation numbers may not be whole
numbers.)
a. CO2
_______________________________________________________________
b. CH4 (methane)
_______________________________________________________________
c. C6H12O6 (glucose)
_______________________________________________________________
d. C3H8 (propane gas)
_______________________________________________________________
8. Assign oxidation numbers to each element in the compounds found in the
following situations:
a. Rust, Fe2O3, forms on an old nail.
_______________________________________________________________
b. Nitrogen dioxide, NO2, pollutes the air as a component of smog.
_______________________________________________________________
c. Chromium dioxide, CrO2, is used to make recording tapes.
_______________________________________________________________
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
5
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
CHAPTER 7 REVIEW
Chemical Formulas and Chemical
Compounds
SECTION 3
SHORT ANSWER Answer the following questions in the space provided.
1. Label each of the following statements as True or False:
__________________ a. If the formula mass of one molecule is x u, the
molar mass is x g/mol.
__________________ b. Samples of equal numbers of moles of two
different chemicals must have equal masses as
well.
__________________ c. Samples of equal numbers of moles of two
different molecular compounds must have equal
numbers of molecules as well.
2. How many moles of each element are present in a 10.0 mol sample of
Ca(NO3)2?
_______________________________________________________________
PROBLEMS Write the answer on the line to the left. Show all your work in the
space provided.
3. Consider a sample of 10.0 g of the gaseous hydrocarbon C3H4 to answer the
following questions.
__________________________ a. How many moles are present in this
sample?
__________________________ b. How many molecules are present in the
C3H4 sample?
__________________________ c. How many carbon atoms are present in
this sample?
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
6
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
SECTION 3 continued
__________________ d. What is the percentage composition of hydrogen in
the sample?
4. One source of aluminum metal is alumina, Al2O3.
__________________ a. Determine the percentage composition of Al in
alumina.
__________________ b. How many pounds of aluminum can be extracted
from 2.0 tons of alumina.?
5. Compound A has a molar mass of 20 g/mol, and compound B has a molar
mass of 30 g/mol.
__________________ a. What is the mass of 1.0 mol of compound A, in
grams?
__________________ b. How many moles are present in 5.0 g of compound
B?
__________________ c. How many moles of compound B are needed to
have the same mass as 6.0 mol of compound A?
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
7
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
CHAPTER 7 REVIEW
Chemical Formulas and Chemical
Compounds
SECTION 4
SHORT ANSWER Answer the following questions in the space provided.
1. Write empirical formulas to match the following molecular formulas:
__________________ a. C2H6O4
__________________ b. N2O5
__________________ c. Hg2Cl2
__________________ d. C6H12
2. ___________________ A certain hydrocarbon has an empirical formula of
CH2 and a molar mass of 56.12 g/mol. What is its
molecular formula?
3. A certain ionic compound is found to contain 0.012 mol of sodium, 0.012 mol
of sulfur, and 0.018 mol of oxygen.
__________________ a. What is its empirical formula?
__________________ b. Is this compound a sulfate, sulfite, or neither?
PROBLEMS Write the answer on the line to the left. Show all your work in the
space provided.
4. Water of hydration was discussed in Sample Problem K in Section 4 of the
text. Strong heating will drive off the water as a vapor in hydrated copper(II)
sulfate. Use the data table below to answer the following:
Mass of the empty crucible
Mass of the crucible plus hydrate sample
4.00 g
4.50 g
Mass of the system after heating
4.32 g
Mass of the system after a second heating
4.32 g
__________________ a. Determine the mass percentage of water in the
original sample.
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
8
Chemical Bonding
Name:______________________________Class: _________________ Date: _________________
SECTION 4 continued
__________________ b. The compound has the formula CuSO4 • xH2O.
Determine the value of x.
c. What might be the purpose of the second heating?
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
_______________________________________________________________
5. Gas X is found to be 24.0% carbon and 76.0% fluorine by mass.
__________________ a. Determine the empirical formula of gas X.
__________________ b. Given that the molar mass of gas X is 200.04
g/mol, determine its molecular formula.
6. A compound is found to contain 43.2% copper, 24.1% chlorine, and 32.7%
oxygen by mass.
__________________ a. Determine its empirical formula.
b. What is the correct Stock system name of the compound in part a?
_______________________________________________________________
Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor.
Modern Chemistry
9
Chemical Bonding