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Chem 3A > Exam #1 > Flashcards

Exam #1 Flashcards

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1
Q

Name the following compound

FeCO3 :

A

iron(II) carbonate

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2
Q

Name the following compound

Fe2(CO3)3 :

A

iron(III) carbonate

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3
Q

Name the following compound

Na3(PO4) :

A

sodium phosphate

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4
Q

Name the following compound

N2O :

A

dinitrogen monoxide

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5
Q

Name the following compound

SF6 :

A

sulfur hexafluoride

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6
Q

Name the following compound

Na2O2 :

A

sodium peroxide

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7
Q

Name the following compound

Ca(OH)2 :

A

calcium hydroxide

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8
Q

Name the following compound

NO :

A

nitrogen monoxide

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9
Q

Name the following compound

Fe(NO3)3 :

A

iron(III) nitrate

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10
Q

Name the following compound

MgCl2 :

A

magnesium chloride

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11
Q

Name the following compound

NaClO4 :

A

sodium perchlorate

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11
Q

Give the formulas for the following compound

sodium phosphate :

A

Na3PO4

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12
Q

Give the formulas for the following compound

sodium hydrogen phosphate :

A

Na2HPO4

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13
Q

Give the formulas for the following compound

iron (III) chloride :

A

FeCl3

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14
Q

Give the formulas for the following compound

silver nitrate :

A

AgNO3

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15
Q

Give the formulas for the following compound

diphosphorus pentoxide :

A

P2O5

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16
Q

Give the formulas for the following compound

iron (II) hydroxide :

A

Fe(OH)2

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17
Q

Give the formulas for the following compound

calcium phosphate :

A

Ca3(PO4)2

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18
Q

Give the formulas for the following compound

titanium (III) chloride :

A

TiCl3

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19
Q

Give the formulas for the following compound

sodium hypochlorite :

A

NaClO

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20
Q

Give the formulas for the following compound

xenon tetrafluoride :

A

XeF4

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21
Q

Give the formulas for the following compound

carbon tetrachloride :

A

CCl4

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22
Q

Give the formulas for the following compound

lithium carbonate :

A

Li2CO3

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23
Q

Perform the following conversion

0.52 g aluminum to moles aluminum:

A

0.019 mol Al

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24
Q

Perform the following conversion

3.62x10-7 m to nm:

A

362 nm

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25
Q

Perform the following conversion

65 miles per hour to m/s:

A

29 m/s

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26
Q

Perform the following conversion

11.4 g to kg:

A

0.0114 kg

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27
Q

Perform the following conversion

100.0 cm to m:

A

1.000 m

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28
Q

Perform the following conversion

34.21 μs to s:

A

0.00003421 s

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29
Q

Perform the following conversion

0.0523 moles of calcium phosphate to grams of calcium phosphate:

A

16.2 g

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30
Q

Perform the following conversion

0.0523 moles of lithium fluoride to grams of lithium fluoride:

A

1.36 g

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31
Q

Perform the following conversion

0.0523 moles of iron (II) hydroxide to grams of iron (II) hydroxide:

A

4.70 g

32
Q

Perform the following conversion

1.54 g of some metal to cm3 of that metal (if the density of the metal is 13.0 g/cm3):

A

0.118 cm

33
Q

7Li+

-# of protons
-# of electrons
-# of neutrons

A

of protons:
3
# of electrons:
2
# of neutrons:
4

34
Q

108Ag
-#of protons:
-#of electrons:
-#of neutrons:

A

of protons:

47
#of electrons:
47
#of neutrons:
61

35
Q

128Te2-
-#of protons:
-#of electrons:
-#of neutrons:

A

of protons:

52
#of electrons:
54
#of neutrons:
76

36
Q

40Ca2+
-#of protons:
-#of electrons:
-#of neutrons:

A

of protons:

20
#of electrons:
18
#of neutrons:
20

37
Q

1H-
-# of protons:
-# of electrons:
-# of neutrons:

A

of protons:

1
#of electrons:
2
#of neutrons:
0

38
Q

-103Rh3+
#of protons:
-#of electrons:
-#of neutrons:

A

of protons:

45
#of electrons:
42
#of neutrons:
58

39
Q

Oxygen (O2) reacts with propane (C3H8) to produce carbon dioxide gas (CO2) and
water (H2O).
a) Write the balanced equation for this reaction.

b) If 39.11 g of oxygen reacts with 40.74 g of propane, how many grams of carbon
dioxide are formed?

c) If the density of carbon dioxide is 1.96 g/L, what volume of carbon dioxide is
produced in part b?

A

a) C3H8 + 5 O2 à 3CO2 + 4H2O

b) 32.27 g

c) 16.5 L

40
Q

Tetraethyllead, a gasoline additive that is no longer used in the United States, has the formula PbC8H20. What is its percent composition (by mass)?

A

64.06% Pb, 29.71% C, 6.232% H

41
Q

When Rutherford bombarded gold foil with alpha particles, some of the
particles were deflected. What conclusion did he make based on this
result?

A

He concluded that atoms were mostly empty space, but they contained a
the dense, positively charged center, which he called the nucleus.

42
Q

J.J. Thomson showed that “cathode rays” were deflected by an electric
field. What particles made up the cathode rays, and why were they
deflected?

A

The particles were electrons, and they were deflected because they possess an electric charge.

43
Q

What was Millikan able to measure in his oil drop experiment?

A

He measured the charge of an electron and then, combining his results with Thomson’s, was able to calculate the mass of an electron.

44
Q

If protons and neutrons each weigh approximately 1 amu, why is the
the atomic mass of chlorine (Cl) 35.45 amu?

A

The atomic mass of chlorine is not a whole number because it is the weighted average of all the naturally occurring isotopes of chlorine. The isotopes themselves weigh 35.0 amu and 37.0 amu; their average is in between.

45
Q

Give the atomic symbols for 2 nonmetals.

A

C, N, S, H, etc.

46
Q

List 2 properties of metals.

A

Malleable, electrically conductive, and high thermal conductivity tend to
form positive ions in ionic compounds.

47
Q

Give the atomic symbols for 2 elements that commonly form +2 ions.

A

Ca, Mg, etc. Also Co, Fe.

48
Q

A compound is composed of 30.80% carbon (C), 41.03% oxygen (O), and
28.18% manganese (Mn) (by mass). What is the empirical formula of this
compound? If the molecular weight is 389.976 g/mol, what is the molecular
formula of this compound?

A

Empirical: MnC5O5

Molecular: Mn2C10O10

49
Q

CaCO3 reacts with HCl to yield CaCl2, H2O, and CO2. When 2.35 g of HCl reacts
with 2.35 g of CaCO3, how many liters of CO2 are formed? (Assume that 1.00
mol of CO2 has a volume of 22.4 L under the conditions of this reaction.)

A

0.526 L

50
Q

a) How many molecules are there in a 5.88 mg sample of chlorine trifluoride?

b) How many fluorine atoms are present in the same sample?

A

a) 3.83x1019 ClF3 molecules

b) 1.15x1020 F atoms

51
Q

Hydrogen gas can be produced by the reaction of water with methane
(CH4) at very high temperatures. The other product of this reaction is
carbon monoxide.

A

H2O + CH4 à 3H2 + CO

52
Q

When aqueous solutions of barium chloride and sodium sulfate are mixed,
a white precipitate of barium sulfate is formed.

A

BaCl2(aq) + Na2SO4(aq) à 2NaCl(aq) + BaSO4(s)

53
Q

Classify each of the following reactions as acid/base, redox, or precipitation.

a) CH4(g) + O2(g) à CO2(g) + H2O(g)

b) H2SO4(aq) + NaOH(aq) à H2O(l) + Na2SO4(aq)

c) H2O(l) à H2(g) + O2(g)

d) 2F2(g) + 2H2O(l) à 4HF(aq) + O2(g)

e) Ag+(aq) + Cl-(aq) à AgCl(s)

A

a) CH4(g) + O2(g) à CO2(g) + H2O(g) Redox

b) H2SO4(aq) + NaOH(aq) à H2O(l) + Na2SO4(aq) Acid-base

c) H2O(l) à H2(g) + O2(g) Redox

d) 2F2(g) + 2H2O(l) à 4HF(aq) + O2(g) Redox

e) Ag+(aq) + Cl-(aq) à AgCl(s) Precipitation

54
Q

For the acid-base reactions in part 54), state which reactant is acid and which reactant is the base. For the redox reactions, state which element is oxidized and which is reduced, and state which reactant is the reducing agent and which is the oxidizing agent.

A

a) C is oxidized. O2 is the oxidizing agent. O is reduced. CH4 is the
reducing agent.

b) H2SO4 is the acid. NaOH is the base.

c) H is reduced. O is oxidized. In this case, there is no oxidizing or reducing agent.

d) F is reduced. H2O is the reducing agent. O is oxidized. F2 is the oxidizing agent.

55
Q

Predict the products for each reaction below.

Mg(OH)2(aq) + HClO3(aq)

A

(acid-base)
Mg(OH)2(aq) + 2HClO3(aq) à Mg(ClO3)2(aq) + 2H2O(l)
or
OH-(aq) + HClO3(aq) à H2O(l) + ClO3-(aq)

56
Q

Predict the products for each reaction below.

H2C2O4(aq) + NaOH(aq)

A

(acid-base)
H2C2O4(aq) + 2NaOH(aq) à Na2C2O4(aq) + 2H2O(l)
or
H2C2O4(aq) + 2OH-(aq) à C2O42-(aq) + 2H2O(l)

57
Q

Predict the products for each reaction below.

Hg2(NO3)2(aq) + CuCl2(aq)

A

(precipitation)
Hg2(NO3)2(aq) + CuCl2(aq) à Hg2Cl2(s) + Cu(NO3)2(aq)
or
Hg22+(aq) + 2Cl-(aq) à Hg2Cl2(s)

58
Q

J.J. Thomson measured the charge/mass ratio of *cathode rays,” which were emitted by different metals, by observing their behavior as they passed through magnetic fields. What are cathode rays?

A

Electrons

59
Q

A N-15 anion (15N3-‘) has
protons, neutrons, and electrons.

A

7, 8, 10

60
Q

Which subatomic particles have approximately equal masses?

A

protons and neutrons

61
Q

A ‘133^ 55Cs* ion has protons, neutrons, and electrons.

A

55, 78, 54

62
Q

Calculate the number of hydrogen atoms in 0.25 moles of strychnine, CaH22N202.

A

3.3 x 1024 atoms

63
Q

What is the formula of the precipitate that forms when aqueous Fe(NOg) and aqueous NazCO; are mixed?

A

Fe3(CO3)3

64
Q

When ammonia (NHs, a base) is dissolved in water, which of the following best represents the resulting solution?

A

NHa(ag) + H20(c) = NE (ag) + OH
(ag)

65
Q

What is the oxidation number of carbon in the bicarbonate ion (HCO3-)?

A

+4

66
Q

How many moles of nitrate ions are present in exactly 475 mL of a 1.27 M iron(III) nitrate solution, Fe(NO3)з(aq)?

A

1.81 mol

67
Q

Co2(HPO4)3

A

cobalt (III) hydrogenphosphate

68
Q

CBr4

A

carbon tetrabramide

69
Q

NH4CI

A

ammonium chloride

70
Q

Mg3N2

A

magnesium nitride

71
Q

H2SO4

A

sulfuric acid

72
Q

PbO2

A

lead(IV) oxide

73
Q

A 13 g piece of dark chocolate is found to contain 14 mg caffeine, while the caffeine content in a 20-fluid-ounce mug of coffee is 415 mg. How many pounds of chocolate would you have to eat to consume the amount of caffeine in exactly 2 mugs in this particular coffee?(1lb=453.6g)

A

(2 mugs) [(415 cof. ms)/(mug)] [(13g choc.)/(14mg caf)] [(1 lb)/(453.6g) = 1.7 lb

74
Q

What is the volume of a 35 kg piece of aluminum (if the density of aluminum is 2.70 g/cm^3)

A

(35 kg) [(1000)/(1kg)] [(1cm^3)/(2.70g)]= 13,000 cm^3

75
Q

A graduated cylinder is filled with water to the 25.0 mL mark. After 27.5 g of titanium dioxide (TiOs) is added, the volume is 31.5 mL. Calculate the density of TiOs.

A

31.5 mL
-25.0 mL
= 6.5 m L

d = [(2 7.5 g)/(6.5 m L)]= 4.2 g/L

76
Q

The radius of a gold atom is approximately 190 pm. Convert this to meters.

A

(190 pm) [(1m)/(1 x 10^2 pm)]= 1.9 x10
^-10 m

77
Q

8 IT (ag) + 3 Cu(s) + 2 NOs (ag) - 3 Cu? (ag) + 2 NO(s) + 4 H.O(D
a. What element is oxidized?
b. What is the oxidizing agent?
c. In the balanced equation, how many electrons are transferred?

A

a) Cu

b) No3-

c) 6

78
Q

Add coefficients to balance the following redox reaction:
____Ag+ (ag) +____Mg (s) -> ___ Ag (s) + ___ Mg^2+ (aq)

A

2 Ag+ (ag) + 1Mg (s) -> 2 Ag (s) + 1 Mg^2+ (aq)

Chem 3A (7 decks)

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