Free Printable Chem Final Review Test 1401

1.

Give the composition of water

a)

two hydrogen atoms and two oxygen atoms

b)

one hydrogen and one oxygen atom

c)

two hydrogen atoms and one oxygen atom

d)

three hydrogen atoms and one oxygen atom

e)

one hydrogen atom and two oxygen atoms

2.

The atomic number (Z) is the number of _______ found in the nucleus of an atom.

a)

Neutrons

b)

Electrons

c)

Protons and Neutrons

d)

Protons

e)

Protons and Electrons

3.

A sample of a compound containing only nitrogen and oxygen decomposes and produces 24.50 g of nitrogen and 32.59 g of oxygen. What is the mass of the original sample of the compound?

a)

32.59 g

b)

55.90 g

c)

57.09 g

d)

24.50 g

e)

90.57 g

4.

An atom that has gained an electron is:

a)

a cation

b)

unlikely to be found in homogenous mixtures

c)

electrically neutral

d)

likely to behave like other atoms

e)

an anion

5.

What does "X" represent in the following symbol? $_{35}^{80}X$

a)

mercury

b)

chlorine

c)

scandium

d)

bromine

e)

selenium

6.

Calculate the atomic mass of element "X" if it has two naturally occurring isotopes with the following masses and natural abundances.

X-10, 10.0129 amu, 19.78%

X-11, 11.0093 amu, 80.22%

a)

10.195 amu

b)

10.002 amu

c)

10.797 amu

d)

10.323 amu

e)

10.812 amu

7.

Two or more substances in variable proportions are added together, where the composition is nonuniform throughout are:

a)

a solution

b)

a homogenous mixture

c)

a compound

d)

an element

e)

a heterogenous mixture

8.

Which ion is represented by the following information?

$p^+$ = 79, $n^0$ = 118, $e^-$ = 78

a)

$Au^+$

b)

$Pt^+$

c)

$Au^{2+}$

d)

$Au^{3+}$

e)

$Pt^{2+}$

9.

When waves of equal amplitude from two sources are in phase when they interact, it is called:

a)

destructive interferance

b)

frequency

c)

constructive interference

d)

diffraction

e)

amplitude

10.

Give the possible values for the angular momentum quantum number (ml) of a d-orbital.

a)

0

b)

-1, 0, 1

c)

0, 1, 2

d)

-2, -1, 0, 1 , 2

e)

-3, -2, -1, 0, 1, 2, 3

11.

Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of $6.88\times10^{14}$ Hz.

a)

229 nm

b)

436 nm

c)

206 nm

d)

485 nm

e)

675 nm

12.

Calculate the frequency of light associated with the transition from n=4 to n=2 in the hydrogen atom.

a)

$6.17\times10^{14}s^{-1}$

b)

$5.59\times10^{14}s^{-1}$

c)

$4.57\times10^{14}s^{-1}$

d)

$1.79\times10^{14}s^{-1}$

e)

$3.28\times10^{14}s^{-1}$

13.

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 377.2 nm.

a)

$4.73\times10^{-19}J$

b)

$2.06\times10^{-19}J$

c)

$1.23\times10^{-19}J$

d)

$8.13\times10^{-19}J$

e)

$5.27\times10^{-19}J$

14.

Determine a ball's mass with a wavelength of $3.45\times10^{-36}m$ and a velocity of 6.55 m/s.

a)

29.3 kg

b)

12.6 kg

c)

28.9 kg

d)

34.6 kg

e)

3.41 kg

15.

Rutherford's Gold Foil experiment helped prove:

a)

The diameter of a gold atom

b)

That the mass of an atom is concentrated in a tiny space.

c)

The exact mass of a gold atom.

d)

The exact charge of an electron

e)

The mass-to-charge ratio of an electron.

16.

Electrons fill lower-energy atomic orbitals before filling higher-energy ones is known as the:

a)

Pauli exclusion principle

b)

Hund's rule

c)

Schrodinger Equation

d)

Heisenberg uncertainty principle

e)

Aufbau principle

17.

The mass number (A) is equal to:

a)

The sum of the number of electrons and protons

b)

The sum of the number of neutrons and electrons

c)

The sum of the number of protons, neutrons and electrons

d)

The sum of the number of neutrons and protons

e)

the sum of the number of the number of protons

18.

The element that corresponds to the complete electronic configuration $1s^22s^22p^63s^23p^64s^13d^5$ is:

a)

Titanium

b)

Vanadium

c)

Chromium

d)

Manganese

e)

Iron

19.

Choose the "short" electron configuration for Po.

a)

$\left[Xe\right]6s^25d^{10}6p^4$

b)

$\left[Xe\right]5d^{10}6p^4$

c)

$\left[Xe\right]6s^24f^{14}5d^{10}6p^4$

d)

$\left[Xe\right]6p^4$

e)

$\left[Xe\right]6d^96p^4$

20.

Isotopes are formed when atoms differ in their number of:

a)

Electrons

b)

Neutrons

c)

Protons

d)

Neutrons and Protons

e)

Electrons and Protons

21.

Which of the following elements is a mettaloid?

a)

Ir

b)

Ta

c)

As

d)

Sn

e)

Rb

22.

Give the complete electron configuration of Ge.

a)

1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2

b)

1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 4p^6

c)

1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^10, 4p^2

d)

1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 3d^10, 4p^6

e)

1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 4s^2, 4p^6

23.

Choose the orbital diagram that represents the ground state of a N-atom

a)

b)

c)

d)

e)

24.

What is the maximum number of possible orbitals in the n=4 energy level (or shell)?

a)

1

b)

5

c)

7

d)

9

e)

16

25.

How many moles of H2O are contained in 85.6 mg of H2O

a)

$4.75\times10^{-3}$ mol

b)

33.4 mol

c)

$2.21\times10^{-2}$ mol

d)

$2.99\times10^{-3}$ mol

e)

$1.10\times10^{-4}$ mol

26.

An atom that has lost an electron is:

a)

a cation.

b)

unlikely to be found in homogeneous mixtures.

c)

electrically neutral.

d)

likely to behave exactly like the parent atom.

e)

an anion

27.

What does "X" represent in the following symbol?

$_{14}^{28}X$

a)

Silicon

b)

Sulfur

c)

Zinc

d)

Ruthenium

e)

Nickel

28.

Calculate the atomic mass of element "X," if it has 2 naturally occurring isotopes with the following masses and natural abundances:

X-45, 44.8776 amu, 32.88%

X-47, 46.9443 amu, 67.12%

a)

46.26 amu

b)

45.91 amu

c)

46.34 amu

d)

46.84 amu

e)

44.99 amu

29.

When waves of equal amplitude from two sources are out-of-phase when they interact, it is called:

a)

destructive interference

b)

diffraction

c)

constructive interference

d)

effusion

e)

amplitude

30.

Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of $1.33\times10^{-35}$ m.

a)

8.81 m/s

b)

12.3 m/s

c)

2.21 m/s

d)

4.98 m/s

e)

6.44 m/s

31.

Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen atom.

a)

103 nm

b)

155 nm

c)

646 nm

d)

971 nm

e)

136 nm

32.

Only two electrons, with opposing spins, are allowed in each orbital is known as the

a)

Pauli exclusion principle.

b)

Hund's rule.

c)

Aufbau principle.

d)

Heisenberg uncertainty principle.

33.

Place the following in order of increasing 1st Ionization Energy (IE1):

N, F, As

a)

N < As < F

b)

As < N < F

c)

F < N < As

d)

As < F < N

e)

F < As < N

34.

Choose the valence orbital diagram that represents the ground state of Se2⁻

a)

b)

c)

d)

e)

35.

Identify the element that has a ground state electronic configuration of [Ar]4s23d7.

a)

tungsten

b)

zinc

c)

rhenium

d)

cobalt

e)

calcium

36.

Determine the name for W(SO3)2

a)

Tungsten (II) Sulfate

b)

Tungsten (IV) Sulfite

c)

Tungsten (IV) Sulfide

d)

Tungsten (II) Sulfite

e)

Tungsten (IV) sulfate

37.

Give the correct formula for Barium Nitride

a)

BaN2

b)

Ba(NO3)

c)

Ba3N2

d)

Ba2N3

e)

Ba(NO2)

38.

Calculate the molar mass of Al(ClO3)3

a)

87.05 g/mol

b)

121.95 g/mol

c)

310.18 g/mol

d)

277.33 g/mol

e)

148.93 g/mol

39.

How many molecules are contained in 17.4 mg of Na(NO3)?

a)

$1.23\times10^{20}$ molecules

b)

$2.96\times10^{21}$ molecules

c)

$2.87\times10^{22}$ molecules

d)

$1.10\times10^{21}$ molecules

e)

$3.37\times10^{20}$ molecules

40.

Determine the empirical formula for a compound that contains C, H, and O. It has 18.75% C and 74.94% O by mass.

a)

C2H6O

b)

CHO

c)

C4H13O2

d)

CH4O3

e)

CH3O

41.

Write the chemical name for P2O5

a)

Phosphorous (IV) Oxide

b)

Diphosphorous Pentoxide

c)

Phosphorous Pentoxide

d)

Phosphorus (II) Oxide

e)

Diphosphorous oxide

42.

Which of the following represents the Lewis dot structure for $Ca^{2+}$ ?

a)

b)

c)

d)

e)

43.

How many pi ( $\pi$ ) bonds are present in the following molecule?

a)

1

b)

2

c)

3

d)

4

e)

5

44.

Give the number of valence electrons for XeI2.

a)

22

b)

20

c)

18

d)

24

e)

16

45.

Choose the best Lewis structure for SF4.

a)

b)

c)

d)

e)

46.

Write the formula for Titanium (II) cyanide dihydrate

a)

Ti2(CN)2 • H2

b)

Ti2(CN) • 2H2O

c)

TiN • 2H2O

d)

Ti(CN)2 • H2

e)

Ti(CN)2 • 2H2O

47.

Draw the best Lewis structure for azide ion, $N_3^-$ . What is the formal charge on the N-atom

a)

0

b)

+1

c)

-1

d)

+2

e)

-2

48.

Identify the bond with the lowest bond energy

a)

$C-C$

b)

$N=N$

c)

$C=C$

d)

$C=O$

e)

$O=O$

49.

The bond angle in NH3 is:

a)

107°

b)

180°

c)

120°

d)

109.5°

e)

90°

50.

How many of the following molecules are polar?

XeF4, CS2, BCl3, SeH2

a)

2

b)

0

c)

1

d)

3

e)

4

51.

How many of the following molecules have sp3 hybridization on the central atom?

CH2O, SO2, OCl2, CH2I2

a)

4

b)

3

c)

2

d)

1

e)

0

52.

Give the hybridization for the Br in BrF3

a)

$sp^3d^2$

b)

$sp^3d$

c)

$sp^3$

d)

$sp^2$

e)

sp

53.

Consider the molecule below. Determine the molecular geometry at each of the two labeled carbons.

a)

C1 = Tetrahedral, C2 = Linear

b)

C1 = Trigonal Planar, C2 = Bent

c)

C1 = Trigonal Planar, C2 = Tetrahedral

d)

C1 = Bent, C2 = Trigonal Planar

e)

C1 = Trigonal pyramidal, C2 = See-saw

54.

Place the following in order of increasing (smallest-to-largest) atomic radius (AR).

P, Al, F

a)

$Al<F<P$

b)

$P<Al<F$

c)

$F<Al<P$

d)

$Al<P<F$

e)

$P<F<Al$

55.

Place the following in order of decreasing (most-to-least) 1st Ionization energy (IE1)

a)

$Mg>K>Cs$

b)

$Cs>Mg>K$

c)

$Mg>Cs>K$

d)

$Cs>K>Mg$

e)

$K>Mg>Cs$

56.

Which element is diamagnetic?

a)

Cd

b)

Se

c)

Zr

d)

Ni

e)

Rb

57.

Choose the bond below that is the most polar

a)

$N-C$

b)

$C-C$

c)

$O-C$

d)

$F-C$

e)

$F-F$

58.

Calculate the mass percent of composition of Potassium in K3(PO4)

a)

26.75%

b)

17.98%

c)

30.72%

d)

55.26%

e)

20.82%

59.

Identify the number of bonding pairs and lone pairs of electrons in water.

a)

1 bonding pair and 1 lone pair

b)

1 bonding pair and 2 lone pairs

c)

2 bonding pairs and 2 lone pairs

d)

2 bonding pairs and 1 lone pair

e)

3 bonding pairs and 2 lone pairs

60.

Determine the Electron Geometry (EG) and the Molecular Geometry (MG) of $ClO_4^-$ .

a)

EG = Tetrahedral, MG = Tetrahedral

b)

EG = Tetrahedral, MG = Trigonal Pyramidal

c)

EG = Trigonal Planar, MG = Bent

d)

EG = Trigonal Planar, MG = Trigonal Planar

e)

EG = Tetrahedral, MG = Trigonal Planar

61.

Determine the name for CoCl2 · 6H2O. Remember that Co forms several ions.

a)

Cobalt chloride hydrate

b)

Cobalt(I) chloride heptahydrate

c)

Cobalt(II) chloride heptahydrate

d)

Cobalt(II) chloride hexahydrate

e)

Cobalt(I) chloride

62.

Calculate the molar mass of Al(C2H3O2)3

a)

86.03 g/mol

b)

204.13 g/mol

c)

56.00 g/mol

d)

258.09 g/mol

e)

139.99 g/mol

63.

Determine the molecular formula of a compound that is 49.48% carbon, 5.19% hydrogen,28.85% nitrogen, and 16.48% oxygen. The molecular weight is 194.19 g/mol

a)

C8H12N4O2

b)

C4H5N2O

c)

C8H10N4O2

d)

C8H10N2O

e)

C16H20N8O4

64.

Choose the best Lewis structure for OCl2.

a)

b)

c)

d)

e)

65.

Give the number of valence electrons for $SO4^{-2}$ .

a)

32

b)

30

c)

34

d)

28

e)

36

66.

Draw the best Lewis structure for BrO4⁻ and determine the formal charge on bromine.

a)

-1

b)

+1

c)

0

d)

+2

e)

+3

67.

Determine the Electron Geometry (EG), Molecular Geometry (MG), and polarity of SF4.

a)

EG = Trigonal bipyramidal, MG = Trigonal bipyramidal, and Nonpolar

b)

EG = Tetrahedral, MG = Tetrahedral, and Polar

c)

EG = Trigonal bipyramidal, MG = See-saw, and Polar

d)

EG = Octahedral, MG = Trigonal bipyramidal, and Nonpolar

e)

EG = Octahedral, MG = Octahedral, and Nonpolar

68.

How many of the following molecules are polar?

PCl5 COS XeO3 SeBr2

a)

2

b)

0

c)

1

d)

3

e)

4

69.

Calculate the mass percent composition of sulfur in Al2(SO4)3.

a)

28.12%

b)

9.372%

c)

42.73%

d)

21.38%

e)

35.97%

70.

How many of the following molecules have sp3d hybridization on the central atom?

SiCl4 BrF5 AsF5 BrF3

a)

2

b)

0

c)

4

d)

1

e)

3

71.

Give the complete Ionic equation for the reaction (if any) that occurs when aqueous Na2S and Zn(NO3)2 are mixed.

a)

Na+ (aq) + NO3- (aq) -> Na(NO3) (s)

b)

Na+ (aq) + S-2 (aq) + Zn+2 (aq) + 2NO3- (aq) -> ZnS (s) + 2Na+ (aq) + 2NO3- (aq)

c)

Na+ (aq) + S-2 (aq) + Zn+2 (aq) + 2NO3- (aq) -> Zn+2 (aq) + S-2 (aq) + 2Na(NO3) (s)

d)

Zn+2 (aq) + S-2 (aq) -> ZnS (s)

e)

No Reaction

72.

Determine the specific heat capacity of a metal alloy that requires 3.44 kJ to raise the temperature of 90.0 g of alloy from 25.0 Celsius to 41.7 Celsius.

a)

4.38 J/g•°C

b)

2.29 J/g•°C

c)

3.95 J/g•°C

d)

2.53 J/g•°C

e)

1.87J/g•°C

73.

The law of_______ states that energy can be neither created nor destroyed.

a)

Kinetic Energy

b)

The Consecration of Energy

c)

Potential Energy

d)

The Conservation of Energy

e)

Thermochemistry

74.

Determine the limiting reactant and the mass (in grams) of nitrogen gas that can be formed from 11.5 g N2O4 and 10.2 g N2H4.

$N_2O_4\left(l\right)+2N_2H_4\left(l\right)\longrightarrow\ 3N_2\left(g\right)+4H_2O\left(g\right)$

a)

Limiting reactant is N2H4, and 59.0 g N2 is formed.

b)

Limiting reactant is N2O4 and 10.5 g N2 formed

c)

Limiting reactant is N2O4 and 45.7 g N2 formed

d)

Limiting reactant is N2H4 and 13.4 g N2 formed

e)

No limiting reactant, and 45.0 g N2 formed

75.

What is the name of an aqueous solution of HBrO?

a)

Hydrobromic acid

b)

Hypobromous acid

c)

Bromous acid

d)

Bromic acid

e)

Perbromic acid

76.

Use the information provided to determine ΔH_rxfor the following reaction:

$CH_4\left(g\right)\ +3Cl_2\left(g\right)\longrightarrow\ 3CHCl_3\left(l\right)+3HCl\left(g\right)$

ΔH_rx(KJ/mol)

CH4 (g) = -75, CHCl3 (l) = -134, HCl (g) = -92

a)

-151 kJ/mol

b)

-335 kJ/mol

c)

+662 kJ/mol

d)

+117 kJ/mol

e)

-217 kJ/mol

77.

All of the following compounds are soluble in water except:

a)

Ba(OH)2

b)

PbCl2

c)

Zn(SO4)

d)

Ag(NO3)

e)

Cu(C2H3O2)2

78.

Identify acetic acid, H(C2H3O2) (aq)

a)

Weak acid

b)

Weak base

c)

Strong base

d)

Strong acid

e)

Not acid or base

79.

Determine the oxidation state of phosphorous in $P_2O_5$ .

a)

+5

b)

+3

c)

0

d)

+2

e)

+4

80.

The titration of 25.0 mL of an unknown concentration of H2(SO4) solution requires 83.6 mL of 0.12 M Na(OH) solution. What is the concentration of H2(SO4) solution (in M)?

a)

0.20 M

b)

0.40 M

c)

0.13 M

d)

0.36 M

e)

0.25 M

81.

In 11.52 g sample of N2 reacts with 3.03 g of H2 to form ammonia (NH3) If ammonia is the only product, what mass of ammonia is formed?

a)

17.03 g

b)

11.00 g

c)

14.01 g

d)

32.76 g

e)

23.07 g

82.

Which of the following is a single-replacement (or single-displacement) reaction?

a)

C(s) + O2(g) $\rightarrow$ CO2 (g)

b)

2H(ClO4)(aq) + Ca(OH)2(aq) $\rightarrow$ 2H2O(l) + Ca(ClO4)2(aq)

c)

Fe(s) + 2Ag(NO3)(aq) $\rightarrow$ 2Ag(s) + Fe(NO3)2(aq)

d)

Mg(SO4)(aq) + Ba(NO3)2(aq) $\rightarrow$ Mg(NO3)2(aq) + Ba(SO4)(s)

e)

None of the above are acid-base reactions

83.

Determine the oxidation state of manganese in MnO4- ion.

a)

+1

b)

+3

c)

+5

d)

+7

e)

0

84.

Use the bond energies provided to estimate ΔH_rxfor the reaction below:

$PCl_3\left(g\right)+Cl_2\left(g\right)\rightarrow\ PCl_5\left(l\right)$

Bond energy table:

Cl-Cl = 243, P-Cl = 331

a)

-243 kJ/mol

b)

-419 kJ/mol

c)

-662 kJ/mol

d)

-67 kJ/mol

e)

-905 kJ/mol

85.

Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M LiBr to 250.0 mL

a)

1.13 M

b)

0.0887 M

c)

0.0313 M

d)

0.0160 M

e)

0.0501 M

86.

Balance the following equation:

$\ldots C_2H_6\left(g\right)+\ldots\ O_2\left(g\right)\longrightarrow\ldots CO_2\left(g\right)+\ldots H_2O\left(g\right)$

What is the stoichiometric coefficient for carbon dioxide?

a)

1

b)

2

c)

3

d)

4

e)

6

87.

According to the following reaction, what volume (in mL) of 0.244 M Pb(NO3)2 solution is required to react exactly with 50.0 mL of 0.210 M CaCl2 solution?

$CaCl_2\left(aq\right)+Pb\left(NO_3\right)_2\left(aq\right)\longrightarrow\ PbCl_2\left(s\right)+Ca\left(NO_3\right)_2\left(aq\right)$

a)

97.4 mL

b)

21.5 mL

c)

43.0 mL

d)

86.1 mL

e)

58.1 mL

88.

Determine the percent yield of a reaction that produces 20.04 g of Fe when 50.00 g of Fe2O3 reacts with excess Al, according to the following reaction:

$Fe_2O_3\left(s\right)+2Al\left(s\right)\longrightarrow\ Al_2O_3\left(s\right)+2Fe\left(s\right)$

a)

61.03%

b)

28.65%

c)

57.31%

d)

20.02%

e)

81.93%

89.

Using Hess' Law and the reaction enthalpies given below, determine the ΔH_rxfor the following reaction:

$2S\left(s\right)+3O_2\left(g\right)\longrightarrow\ 2SO_3\left(g\right)$

Given:

$SO_2\left(g\right)\longrightarrow S\left(s\right)+O_2\left(g\right)$ , ΔHrxn = -296.8 kJ/mol

$2SO_2\left(g\right)+O_2\left(g\right)\rightarrow\ 2SO_3\left(g\right)$ , ΔHrxn = -197.8 kJ/mol

a)

-494.6 kJ/mol

b)

-692.4 kJ/mol

c)

-791.4 kJ/mol

d)

1583 kJ/mol

e)

-293.0 kJ/mol

90.

What element is undergoing reduction (if any) in the following reaction?

$Cu\left(s\right)+2Sn\left(NO_3\right)_2\left(aq\right)\rightarrow\ Cu\left(NO_3\right)_2\left(aq\right)+2Sn\left(s\right)$

a)

Cu

b)

Sn

c)

N

d)

O

e)

This is not an oxidation-reduction reaction.

91.

According to the reaction below, how much energy is released with the consumption of 51.2 g of Al?

$Fe_2O_3\left(s\right)+2Al\left(s\right)\rightarrow\ Al_2O_3\left(s\right)+2Fe\left(s\right)$ , ΔHrxn = -472 kJ/mol

a)

51.2 kJ

b)

448 kJ

c)

224 kJ

d)

1617 kJ

e)

808 kJ

92.

What is one of the reactants of a combustion reaction?

a)

Carbon Dioxide

b)

Hydrogen Gas

c)

Oxygen Gas

d)

Water

e)

Sulfur

93.

Give the theoretical yield, in mol, of CO2 from the reaction of 0.400 mol of C8H18 with 4.00 mol of O2.

$2C_8H_{18}\left(l\right)+25O_2\left(g\right)\rightarrow\ 16CO_2\left(g\right)+18H_2O\left(g\right)$

a)

2.88 mol

b)

3.20 mol

c)

2.56 mol

d)

16.0 mol

e)

5.12 mol

94.

Which compounds will undergo a gas-evolving reaction in an aqueous reaction?

a)

H(C2H3O2) (aq)

b)

HF (aq)

c)

HCl (aq)

d)

H2(SO3) (aq)

e)

H(ClO3) (aq)

95.

Choose the reaction that represents the decomposition of C6H12O2

a)

C6H12O2 (l) + 8O2 (g) -> 6CO2 (g) + 6H2O (g)

b)

Mg (s) + C6H12O2 (l) -> Mg(C6H12O2) (aq)

c)

6C (s) + 6H2 (g) + O2 (g) -> C6H12O2 (l)

d)

C6H12O2 (l) -> 6C (s) + 6H2 (g) + O2 (g)

e)

None of the above represents the combustion of C6H12O2

96.

A chemical change

a)

occurs when methane gas is burned.

b)

occurs when paper is shredded.

c)

occurs when water is vaporized.

d)

occurs when salt is dissolved in water.

e)

occurs when powdered lemonade is stirred into water.

97.

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed

a)

30.15 g

b)

54.93 g

c)

140.01 g

d)

79.71 g

e)

91.86 g

98.

Why are the halogens among the most active nonmetals?

a)

Their valence electrons are more effectively shielded.

b)

All halogens have low electron affinities.

c)

They all have smaller diameters than other nonmetals.

d)

Their d-orbitals are completely filled.

e)

They only need one electron needed to attain a noble gas configuration

99.

Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles ofC8H18 with 8.000 moles of O2.

2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

a)

20.00%

b)

25.00%

c)

50.00%

d)

12.50%

e)

75.50%

100.

Choose the reaction that represents the combustion of C6H12O2

a)

C6H12O2(l) + 8 O2(g) → 6 CO2(g) + 6 H2O(g)

b)

Mg(s) + C6H12O2(l) → MgC6H12O2(aq)

c)

6 C(s) + 6 H2(g) + O2(g) → C6H12O2(l)

d)

C6H12O2(l) → 6 C(s) + 6 H2(g) + O2(g)

e)

None of the above represent the combustion of C6H12O2.

101.

According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of0.227 M LiOH solution? Assume that there is excess FeCl2.

FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq)

a)

3.97 × 10-2 mol

b)

2.52 × 10-2 mol

c)

1.99 × 10-2 mol

d)

5.03 × 10-2 mol

e)

6.49 × 10-2 mol

102.

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed.

a)

Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s)

b)

Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s)

c)

Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s)

d)

3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3(s)

e)

No reaction occurs.

103.

What element is undergoing oxidation (if any) in the following reaction?

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

a)

O

b)

H

c)

C

d)

C and H

e)

None of the elements is undergoing oxidation.

104.

Which of the following compounds will undergo a gas-evolving reaction in an aqueous solution?

a)

CH3COOH

b)

HF

c)

HCl

d)

H2SO4

e)

H2CO3

105.

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?

a)

50.0 g Al, CAl = 0.903 J/g.°C

b)

50.0 g Cu, CCu = 0.385 J/g.°C

c)

25.0 g granite, Cgranite = 0.79 J/g.°C

d)

25.0 g Au, CAu = 0.128 J/g.°C

e)

25.0 g Ag, CAg = 0.235 J/g.°C

Chem Final Review Test 1401

Total questions: 105

Worksheet time: 2hrs 45mins

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