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Introduction to Chemistry > Quest #1 > Flashcards

Quest #1 Flashcards

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1
Q

Reaction

H2 + O2 –> H2O

A

Combination - Redox

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2
Q

Reaction

S8 + O2 –> SO3

A

Combination - Redox

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3
Q

Reaction

HgO –> Hg + O2

A

Decomposition - Gas - Forming, Redox

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4
Q

Reaction

Zn + HCl –> ZnCl2 + H2

A

Displacement - Gas-Forming, Redox

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5
Q

Reaction

Na + H2O –> NaOH + H2

A

Displacement - Gas-Forming, Redox

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6
Q

Reaction

C10H16 + Cl2 –> C + HCl

A

Displacement - Redox

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7
Q

Reaction

Si2H3 + O2 –> SiO2 + H2O

A

Displacement - Redox

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8
Q

Reaction

C7H6O2 + O2 –> CO2 + H2O

A

Displacement - Combustion - Gas-Forming - Redox

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9
Q

Reaction

Fe2O3 + H2 –> Fe + H2O

A

Displacement - Redox

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10
Q

Reaction

K + Br2 –> KBr

A

Combination - Redox

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11
Q

Reaction

C2H2 + O2 –> CO2 + H2O

A

Displacement - Combustion, Gas-Forming, Redox

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12
Q

Reaction

H2O2 –> H2O + O2

A

Decomposition - Gas-Forming, Redox

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13
Q

Reaction

C7H16 + O2 –> CO2 + H2O

A

Displacement - Combustion, Gas-Forming, Redox

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14
Q

Reaction

SiO2 + HF –> SiF4 + H2O

A

Exchange

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15
Q

Reaction

KCIO3 –> KCl + O2

A

Decomposition - Gas-Forming, Redox

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16
Q

Reaction

P4O10 + H2O –> H3PO4

A

Combination

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17
Q

Reaction

Sb + O2 –> Sb4O6

A

Combination - Redox

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18
Q

Reaction

Fe2O3 + CO –> Fe + CO2

A

Displacement - Redox, Gas-Forming

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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)

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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

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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

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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-

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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+

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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

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25
Q

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)

A

Mg - Oxidized

O - Reduced

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26
Q

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)

A

Ca - Oxidized

F2 - Reduced

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27
Q

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)

A

Fe - Oxidized

Cl2 - Reduced

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28
Q

Balance each of the following oxidation-reduction chemical reactions

A

P4(s) + 5O2(g) –> P4O10(s)

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29
Q

Balance each of the following oxidation-reduction chemical reactions

A

MgO(s) + C(s) –> Mg(s) + CO(g)

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30
Q

Balance each of the following oxidation-reduction chemical reactions

A

Sr(s) + 2H2O(l) –> Sr(OH)2(aq) + H2(g)

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31
Q

Balance each of the following oxidation-reduction chemical reactions

A

Co(s) + 2HCl(aq) –> CoCl2(aq) + H2(g)

32
Q

What is a net ionic equation? What species are shown in such an equation, and which species are not shown?

A

A net ionic equation indicates only those ions involved in making a precipitate spectating ion are not included.

33
Q

What are spectator ions? Write an example of an equation in which spectator ions are present and identify them.

A

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
Q

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

A

Ag+ + Cl - –> AgCl

35
Q

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

A

Ba+2 + SO4 2- –> BaSO4

36
Q

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

A

3Ca+2 + 2PO4 2- –> Ca3(PO4)2

37
Q

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

A

No Reaction

38
Q

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

A

Ca+2 + SO4 2- –> CaSO4

39
Q

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

A

Pb+2 + 2Cl- –> PbCl2

40
Q

What is meant by a strong acid? Are the strong acids also strong electrolytes? Explain

A

Strong acids ionize completely in water.

They are also strong electrolytes.

41
Q

What is meant by a strong base? Are the strong bases also strong electrolytes? Explain.

A

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
Q

The same net ionic process takes place when any strong acid reacts with a strong base. Write the equation for this process

A

H+ + OH - –> H2O

43
Q

What is a salt? Give one balanced chemical equation showing how a salt is formed when an acid reacts with a base.

A

A salt is an ionic product remaining in a solution when an acid neutralizes a base.

HCl + NaOH –> NaCl + H2O

44
Q

What salt would form when each of the following strong acid/strong base reactions takes place?
HCl(aq) + KOH(aq)

A

KCl

45
Q

What salt would form when each of the following strong acid/strong base reactions takes place?
RbOH(aq) + HNO3(aq)

A

RbNO3

46
Q

What salt would form when each of the following strong acid/strong base reactions takes place?
HClO4(aq) + NaOH(aq)

A

NaClO4

47
Q

What salt would form when each of the following strong acid/strong base reactions takes place?
HBr(aq) + CsOH(aq)

A

CsBr

48
Q

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

A

HCl + KOH –> KCl + H2O

49
Q

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

A

HClO4 + NaOH –> NaClO4 + H2O

50
Q

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

A

HNO3 + CsOH –> CsNO3 + H2O

51
Q

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

A

H2SO4 + 2KOH –> K2SO4 + 2H20

52
Q

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

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
Q

When two solutions of ionic substances are mixed and a precipitate forms, what is the net charge of the precipitate? Why?

A
  1. The net positive charge = the net negative charge
54
Q

Describe briefly what happens when an ionic substance is dissolved in water.

A

The ions separate, become hydrated, and behave independently.

55
Q

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?

A

It is soluble

56
Q

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

A

Soluble

57
Q

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

A

insoluble

58
Q

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

A

insoluble

59
Q

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

A

Soluble

60
Q

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

A

Soluble

61
Q

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

A

insoluble

62
Q

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

A

soluble

63
Q

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

A

insoluble

64
Q

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

A

Insoluble - most OH- are insoluble

65
Q

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

A

Insoluble - most SO4 2- are insoluble

66
Q

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

A

insoluble - most CO3 2- are insoluble

67
Q

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

A

insoluble - most S2- salts are insoluble

68
Q

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

A

MnCO3

69
Q

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

A

potassium salts + sulfates are soluble

70
Q

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.

A

Hg2Cl2

71
Q

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

A

nitrates + sodium salts are soluble

72
Q

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

A

Ni(OH)2

73
Q

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

A

Chlorides and sulfates are soluble

74
Q

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

A

Na2S(aq) + CuCl2(aq) –> CuS(s) + 2NaCl(aq)

75
Q

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

A

K3PO4(aq) + AlCl3(aq) –> 3KCl(aq) + AlPO4(s)

76
Q

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

A

2NaCl(aq) + Hg2(NO3)2(aq) –> Cr2(CO3)3(s) + 6KC2H3O2(aq)

Introduction to Chemistry (1 decks)

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