Honors Chemistry
Mr. Trubic
St. John’s College High School
Chapter 6 Review
Solutions
Name ________________________________________
Date ______________
HONORS CHEMISTRY
CHAPTER 6 REVIEW
NO CALCULATOR MAY BE USED.
(Why would you need one anyway?)
PART A: MULTIPLE CHOICE
Directions: Each of the questions or incomplete statements below is followed by four suggested answers or completions.
Select the one that is best in each case and then write the letter on the line USING CAPITAL LETTERS.
B
Mg3N2(?) + 6 H2O(l) → 3 Mg(OH)2(aq) + 2 NH3(g)
A
______
______
3. Which of the following is a strong acid?
(A) H3PO4
1. If the reaction above is carried out at
298 K, what is the physical state of
magnesium nitride?
(B) HCl
(C) HNO2
(A) solid
(D) HC2H3O2
(B) liquid
(C) gas
C
______
(D) aqueous
D
______
4. Which of the following correctly shows
the ions present in an aqueous solution of
sodium carbonate?
(A) Na2+, CO32−
2. Solid aluminum reacts with gaseous
oxygen to form solid aluminum oxide.
Which of the following correctly
represents this chemical reaction?
(B) Na2+, C2−, O3
(C) Na+, CO32−
(D) Na+, C4+, O32−
(A) Al(s) + O(g) → AlO(s)
(B) Al(s) + O2(g) → AlO2(s)
A
(C) Al2(s) + O3(g) → Al2O3(s)
______
(D) 4 Al(s) + 3 O2(g) → 2 Al2O3(s)
5. Which of the following compounds is
soluble in water?
(A) (NH4)3PO4
(B) Ca3(PO4)2
(C) AlPO4
(D) Ag3PO4
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Honors Chemistry
Mr. Trubic
D
______
St. John’s College High School
Chapter 6 Review
C
6. When a precipitation reaction occurs, the
ions that do NOT form the precipitate
______ 10. If 100 formula units of aluminum sulfate
are placed in 1.0 L of water, how many
aluminum ions will be in solution?
(A) evaporate
(B) are cations only
(A) Zero; aluminum sulfate is insoluble.
(C) form a second insoluble compound in
the solution
(B)
50
(C) 200
(D) are left dissolved in the solution
(D) 300
B
______
7. The common constituent in all acid
solutions is
A
______ 11. An aqueous solution of potassium
chromate is allowed to react with an
aqueous solution of lead(II) nitrate. The
net ionic equation contains which of the
following species (when balanced using
lowest whole numbers)?
(A) H2
(B) H+
(C) OH−
(D) Cl−
A
______
Note: The solubility of chromates is the
same as that of phosphates.
8. What is the correct formula of the salt
formed in the neutralization reaction of
phosphoric acid and barium hydroxide?
(A) Pb2+(aq)
(B) Cr2O72−(aq)
(A) Ba3(PO4)2
(C) 2 K+(aq)
(B) Ba2(PO4)3
(D)
NO3−(aq)
(C) Ba3(PO3)2
(D) Ba2(PO3)3
D
______
B
______ 12. What are the products of the reaction
shown below?
9. When solutions of ZnSO4(aq) and
MgCl2(aq) are mixed,
(A) ZnCl2 will precipitate; Mg2+ and
SO42− will be spectator ions
Ca(s) + Zn(ClO3)2(aq) → ?
(B) ZnSO4 will precipitate; Mg2+ and
Cl− will be spectator ions
(A) CaZn(ClO3)2(aq)
(B) Zn(s) + Ca(ClO3)2(aq)
(C) MgSO4 will precipitate; Zn2+ and
Cl− will be spectator ions
(C) CaCl2(aq) + ZnO(aq)
(D) CaO(aq) + Zn(ClO2)2(aq)
(D) no precipitate will form
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Honors Chemistry
Mr. Trubic
St. John’s College High School
Chapter 6 Review
PART B: FREE-RESPONSE
13. Balance the following chemical equations using lowest whole numbers. If the coefficient is 1, you may write the
number ‘1’ or leave the line blank.
(a)
2 C3H8O(l) + _____
9 O2(g)
_____
6 CO2(g) + _____
8 H2O(g)
_____
→
2 KI(aq)
(b) _____ Cl2(g) + _____
→
2 KCl(aq) + _____ I2(s)
_____
3 Cl2(g)
_____ CS2(g) + _____
→
_____ CCl4(l) + _____ S2Cl2(g)
(c)
16 Cr(s) + _____
3 S8(s)
(d) _____
8 Cr2S3(s)
_____
→
(e)
3 O2(g)
_____
(f)
2 H2SO4(aq)
_____ Cu(s) + _____
→
2 O3(g)
_____
4 NH3(g) + _____
3 F2(g)
(g) _____
→
→
2 H2O(l)
_____ CuSO4(aq) + _____ SO2(g) + _____
3 NH4F(s) + _____ NF3(g)
_____
6 KI(aq) + _____
6 HCl(aq)
(h) _____ As2O3(s) + _____
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→
2 AsI3(s) + _____
6 KCl(aq) + _____
3 H2O(l)
_____
Honors Chemistry
Mr. Trubic
Cu
Al
St. John’s College High School
Chapter 6 Review
Fe
Ag
Au
14. A student prepares an aqueous solution of tin(II) chloride and obtains samples of
each of the five metals shown above.
(a) Circle the metal or metals that will react with the tin(II) chloride solution.
(b) Write the balanced molecular equation for the reaction between the metal circled
in part (a) and the tin(II) chloride solution. (If more than one metal was circled in
part (a), choose one.) Balance the equation using lowest whole numbers and be
sure to include states.
2 Al(s) + 3 SnCl2(aq) → 2 AlCl3(aq) + 3 Sn(s)
OR
Fe(s) + SnCl2(aq) → FeCl2(aq) + Sn(s)
(c) Write the total (complete) ionic equation for the reaction described in part (b).
Balance the equation using lowest whole numbers and be sure to include states.
2 Al(s) + 3 Sn2+(aq) + 6 Cl−(aq) → 2 Al3+(aq) + 6 Cl−(aq) + 3 Sn(s)
OR
Fe(s) + Sn2+(aq) + 2 Cl−(aq) → Fe2+(aq) + 2 Cl−(aq) + Sn(s)
(d) Write the net ionic equation for the reaction described in part (b). Balance the
equation using lowest whole numbers and be sure to include states.
2 Al(s) + 3 Sn2+(aq) → 2 Al3+(aq) + 3 Sn(s)
OR
Fe(s) + Sn2+(aq) → Fe2+(aq) + Sn(s)
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Honors Chemistry
Mr. Trubic
St. John’s College High School
Chapter 6 Review
15. Aqueous solutions of sodium hydroxide and copper(II) acetate are mixed.
(a) Write the balanced molecular equation for the reaction that occurs. Balance the equation using lowest whole
numbers and be sure to include states.
2 NaOH(aq) + Cu(C2H3O2)2(aq) → 2 NaC2H3O2(aq) + Cu(OH)2(s)
(b) Write the total (complete) ionic equation for the reaction that occurs. Balance the equation using lowest whole
numbers and be sure to include states.
2 Na+(aq) + 2 OH−(aq) + Cu2+(aq) + 2 C2H3O2−(aq) → 2 Na+(aq) + 2 C2H3O2−(aq) + Cu(OH)2(s)
(c) Write the net ionic equation for the reaction that occurs. Balance the equation using lowest whole numbers and
be sure to include states.
2 OH−(aq) + Cu2+(aq) → Cu(OH)2(s)
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Honors Chemistry
Mr. Trubic
St. John’s College High School
Chapter 6 Review
16. Write the balanced molecular equation for each of the laboratory situations described below. In all cases, a reaction
occurs. Balance the equations using lowest whole numbers and be sure to include states.
(a) Magnesium bromide is formed from its constituent elements.
Mg(s) + Br2(ℓ) → MgBr2(s)
(b) Aqueous solutions of ammonium sulfide and manganese(II) iodide are mixed.
(NH4)2S(aq) + MnI2(aq) → 2 NH4I(aq) + MnS(s)
(c) Liquid C6H12O (hexanal) is combusted in air.
2 C6H12O(ℓ) + 17 O2(g) → 12 CO2(g) + 12 H2O(g)
(d) Electric current is applied to a sample of calcium fluoride.
CaF2(s) → Ca(s) + F2(g)
(e) A piece of solid chromium is placed in sulfuric acid.
2 Cr(s) + 3 H2SO4(aq) → Cr2(SO4)3(aq) + 3 H2(g)
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