Quest #1 Flashcards
1
Q
Reaction
H2 + O2 –> H2O
A
Combination - Redox
2
Q
Reaction
S8 + O2 –> SO3
A
Combination - Redox
3
Q
Reaction
HgO –> Hg + O2
A
Decomposition - Gas - Forming, Redox
4
Q
Reaction
Zn + HCl –> ZnCl2 + H2
A
Displacement - Gas-Forming, Redox
5
Q
Reaction
Na + H2O –> NaOH + H2
A
Displacement - Gas-Forming, Redox
6
Q
Reaction
C10H16 + Cl2 –> C + HCl
A
Displacement - Redox
7
Q
Reaction
Si2H3 + O2 –> SiO2 + H2O
A
Displacement - Redox
8
Q
Reaction
C7H6O2 + O2 –> CO2 + H2O
A
Displacement - Combustion - Gas-Forming - Redox
9
Q
Reaction
Fe2O3 + H2 –> Fe + H2O
A
Displacement - Redox
10
Q
Reaction
K + Br2 –> KBr
A
Combination - Redox
11
Q
Reaction
C2H2 + O2 –> CO2 + H2O
A
Displacement - Combustion, Gas-Forming, Redox
12
Q
Reaction
H2O2 –> H2O + O2
A
Decomposition - Gas-Forming, Redox
13
Q
Reaction
C7H16 + O2 –> CO2 + H2O
A
Displacement - Combustion, Gas-Forming, Redox
14
Q
Reaction
SiO2 + HF –> SiF4 + H2O
A
Exchange
15
Q
Reaction
KCIO3 –> KCl + O2
A
Decomposition - Gas-Forming, Redox
16
Q
Reaction
P4O10 + H2O –> H3PO4
A
Combination
17
Q
Reaction
Sb + O2 –> Sb4O6
A
Combination - Redox
18
Q
Reaction
Fe2O3 + CO –> Fe + CO2
A
Displacement - Redox, Gas-Forming
19
Q
What is an oxidation-reduction reaction? What is transferred during such a reaction?
A
One species loses electrons (oxidation); another species gains electrons (reduction)
20
Q
If atoms of a metallic element (such as sodium) react with atoms of a nonmetallic element (such as sulfur), which element loses electrons and which element gains them?
A
Metals lose electrons
Nonmetals gain electrons
21
Q
If atoms of the metal calcium were to react with molecules of the nonmetal fluorine, F2, how many electrons would each calcium atom lose? How many electrons would each fluorine atom gain? How many calcium atoms would be needed to react with one fluorine molecule? What chares would the resulting calcium and fluoride ions have?
A
Calcium would lose 2e - + become Ca+2
Fluorine would gain le - + becomes F-
CaF2
22
Q
For the reaction Mg(s) + Cl2(g) –> MgCl2(s), illustrate how electrons are gained and lost during the reaction
A
Cl Cl-
Mg ——–> Mg+2
Cl Cl-
23
Q
For the reaction, 2K(s) + S(g) –> K2S (s), show how electrons are gained and lost by the atoms.
A
K K+
S –> S2-
K K+
24
Q
Balance each of the following oxidation-reduction reactions. In each, indicate which substance is being oxidized and which is being reduced.
2Na(s) + S(s) –> Na2S(s)
A
Na - Oxidized
S - Reduced
25
Balance each of the following oxidation-reduction reactions. In each, indicate which substance is being oxidized and which is being reduced.
2Mg(s) + O2(g) --> 2MgO(s)
Mg - Oxidized
| O - Reduced
26
Balance each of the following oxidation-reduction reactions. In each, indicate which substance is being oxidized and which is being reduced.
Ca(s) + F2(g) --> CaF2(s)
Ca - Oxidized
| F2 - Reduced
27
Balance each of the following oxidation-reduction reactions. In each, indicate which substance is being oxidized and which is being reduced.
2Fe(s) + 3Cl2(g) --> 2FeCl3(s)
Fe - Oxidized
| Cl2 - Reduced
28
Balance each of the following oxidation-reduction chemical reactions
P4(s) + 5O2(g) --> P4O10(s)
29
Balance each of the following oxidation-reduction chemical reactions
MgO(s) + C(s) --> Mg(s) + CO(g)
30
Balance each of the following oxidation-reduction chemical reactions
Sr(s) + 2H2O(l) --> Sr(OH)2(aq) + H2(g)
31
Balance each of the following oxidation-reduction chemical reactions
Co(s) + 2HCl(aq) --> CoCl2(aq) + H2(g)
32
What is a net ionic equation? What species are shown in such an equation, and which species are not shown?
A net ionic equation indicates only those ions involved in making a precipitate spectating ion are not included.
33
What are spectator ions? Write an example of an equation in which spectator ions are present and identify them.
Spectator ions are ions that remain in solution during a precipitation/double displacement reaction.
NaCl(ag) + AgNO3(ag) --> AgCl(s) + NaNO3 (ag) - Na+
NO3-
34
Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely (i.e. there is no driving force), so indicate)
Silver nitrate, AgNO3, and potassium chloride, KCl
Ag+ + Cl - --> AgCl
35
Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely (i.e. there is no driving force), so indicate)
nickel (II) sulfate, NiSO4, and barium chloride, BaCl2
Ba+2 + SO4 2- --> BaSO4
36
Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely (i.e. there is no driving force), so indicate)
ammonium phosphate, (NH4)3 PO4, and calcium chloride, CaCl2
3Ca+2 + 2PO4 2- --> Ca3(PO4)2
37
Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely (i.e. there is no driving force), so indicate)
hydrofluoric acid, HF, and potassium sulfate, K2SO4
No Reaction
38
Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely (i.e. there is no driving force), so indicate)
calcium chloride, CaCl2, and ammonium sulfate, (NH4)2SO4
Ca+2 + SO4 2- --> CaSO4
39
Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely (i.e. there is no driving force), so indicate)
lead (II) nitrate, Pb(NO3)2, and barium chloride, BaCl2
Pb+2 + 2Cl- --> PbCl2
40
What is meant by a strong acid? Are the strong acids also strong electrolytes? Explain
Strong acids ionize completely in water.
They are also strong electrolytes.
41
What is meant by a strong base? Are the strong bases also strong electrolytes? Explain.
Strong bases are the hydroxide compounds that dissociate fully when dissolved in water.
The hydroxides that are highly soluble in water are strong electrolytes.
42
The same net ionic process takes place when any strong acid reacts with a strong base. Write the equation for this process
H+ + OH - --> H2O
43
What is a salt? Give one balanced chemical equation showing how a salt is formed when an acid reacts with a base.
A salt is an ionic product remaining in a solution when an acid neutralizes a base.
HCl + NaOH --> NaCl + H2O
44
What salt would form when each of the following strong acid/strong base reactions takes place?
HCl(aq) + KOH(aq)
KCl
45
What salt would form when each of the following strong acid/strong base reactions takes place?
RbOH(aq) + HNO3(aq)
RbNO3
46
What salt would form when each of the following strong acid/strong base reactions takes place?
HClO4(aq) + NaOH(aq)
NaClO4
47
What salt would form when each of the following strong acid/strong base reactions takes place?
HBr(aq) + CsOH(aq)
CsBr
48
Below are the formulas of some salts. Such salts could form by the reaction of the appropriate strong acid with the appropriate strong base (with the other product of the reaction being, of course, water). For each salt, write an equation showing the formation for the salt from the reaction of the appropriate strong acid and strong base.
KCl
HCl + KOH --> KCl + H2O
49
Below are the formulas of some salts. Such salts could form by the reaction of the appropriate strong acid with the appropriate strong base (with the other product of the reaction being, of course, water). For each salt, write an equation showing the formation for the salt from the reaction of the appropriate strong acid and strong base.
NaClO4
HClO4 + NaOH --> NaClO4 + H2O
50
Below are the formulas of some salts. Such salts could form by the reaction of the appropriate strong acid with the appropriate strong base (with the other product of the reaction being, of course, water). For each salt, write an equation showing the formation for the salt from the reaction of the appropriate strong acid and strong base.
CsNO3
HNO3 + CsOH --> CsNO3 + H2O
51
Below are the formulas of some salts. Such salts could form by the reaction of the appropriate strong acid with the appropriate strong base (with the other product of the reaction being, of course, water). For each salt, write an equation showing the formation for the salt from the reaction of the appropriate strong acid and strong base.
K2SO4
H2SO4 + 2KOH --> K2SO4 + 2H20
52
What is a "driving force"? What are some of the driving forces discussed in this section that tend to make reactions likely to occur? Can you think of any other possible driving forces?
A driving force is a type of change in a system that pulls a reaction in the direction of product formation
Formation of a solid, formation of water, formation of a gas, transfer of e-
53
When two solutions of ionic substances are mixed and a precipitate forms, what is the net charge of the precipitate? Why?
0. The net positive charge = the net negative charge
54
Describe briefly what happens when an ionic substance is dissolved in water.
The ions separate, become hydrated, and behave independently.
55
When aqueous solutions of sodium chloride, NaCl, and silver nitrate, AgNO3, are mixed, a precipitate forms, but this precipitate is not sodium nitrate. What does this reaction tell you about the solubility of NaNO3 in water?
It is soluble
56
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
manganese (II) chloride
Soluble
57
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
lead (ll) sulfide
insoluble
58
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
iron (III) hydroxide
insoluble
59
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
potassium fluoride
Soluble
60
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
magnesium sulfate
Soluble
61
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
iron (II) sulfide
insoluble
62
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
potassium carbonate
soluble
63
On the basis of the general solubility rules, predict which of the following substances would not be expected to be appreciably soluble in water.
calcium carbonate
insoluble
64
On the basis of the general solubility rules, for each of the following compounds, indicate why the compound is not likely to be soluble in water. Indicate which of the solubility rules covers each substance's particular situation.
chromium (III) hydroxide
Insoluble - most OH- are insoluble
65
On the basis of the general solubility rules, for each of the following compounds, indicate why the compound is not likely to be soluble in water. Indicate which of the solubility rules covers each substance's particular situation.
silver phosphate
Insoluble - most SO4 2- are insoluble
66
On the basis of the general solubility rules, for each of the following compounds, indicate why the compound is not likely to be soluble in water. Indicate which of the solubility rules covers each substance's particular situation.
manganese (II) carbonate
insoluble - most CO3 2- are insoluble
67
On the basis of the general solubility rules, for each of the following compounds, indicate why the compound is not likely to be soluble in water. Indicate which of the solubility rules covers each substance's particular situation.
barium sulfide
insoluble - most S2- salts are insoluble
68
On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply.
sodium carbonate, Na2CO3, and manganese (II) chloride, MnCl2
MnCO3
69
On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply.
potassium sulfate, K2SO4, and calcium acetate, Ca(C2H3O2)2
potassium salts + sulfates are soluble
70
On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply.
hydrochloric acid, HCl and mercurous acetate, Hg2(C2H3O2)2.
Hg2Cl2
71
On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply.
sodium nitrate, NaNO3, and lithium sulfate, Li2SO4
nitrates + sodium salts are soluble
72
On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply.
potassium hydroxide, KOH, and nickel (II) chloride, NiCl2
Ni(OH)2
73
On the basis of the general solubility rules, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply.
Sulfuric acid, H2SO4, and barium chloride, BaCl2
Chlorides and sulfates are soluble
74
On the basis of the general solubility rules, write a balanced molecular equation for the precipitation reactions that place when the following aqueous solutions are mixed. Underline the precipitate (solid) that forms. If not precipitation reaction is likely for the solutes given, so indicate.
sodium sulfide, Na2S, and copper (II) chloride, CuCl2
Na2S(aq) + CuCl2(aq) --> CuS(s) + 2NaCl(aq)
75
On the basis of the general solubility rules, write a balanced molecular equation for the precipitation reactions that place when the following aqueous solutions are mixed. Underline the precipitate (solid) that forms. If not precipitation reaction is likely for the solutes given, so indicate.
potassium phosphate, K3PO4, and aluminum chloride, AlCl3
K3PO4(aq) + AlCl3(aq) --> 3KCl(aq) + AlPO4(s)
76
On the basis of the general solubility rules, write a balanced molecular equation for the precipitation reactions that place when the following aqueous solutions are mixed. Underline the precipitate (solid) that forms. If not precipitation reaction is likely for the solutes given, so indicate.
sodium chloride, NaCl, and mercurous nitrate, Hg2(NO3)2
2NaCl(aq) + Hg2(NO3)2(aq) --> Cr2(CO3)3(s) + 6KC2H3O2(aq)
