Advanced Chemistry Final Exam Questions

Front 1

Forms monatomic ions with 2- charge in solution. (Cl, S, Mg, Ne, or Cu)

Back 1

S

Front 2

As "X" it forms an acid with the formula HXO4.

Back 2

Cl

Front 3

As an element, it exists as a diatomic molecule.

Back 3

Cl

Front 4

Will form an ionic compound with a single sodium ion.

Back 4

Cl

Front 5

Which of the following best represents a pair of isotopes?

Back 5

atomic: 7 mass: 13
atomic: 7 mass: 14

Front 6

Identify the respective proton number, neutron number, and number of electrons found in 63/29 Cu.

Back 6

29, 34, 29

Front 7

Which of the following statements is incorrect?

Back 7

Heterogeneous mixtures may not contain elements.

Front 8

The volume of a piece of topaz (a semiprecious gem) weighing 5.95 g is 1.7 mL. The densities of chloroform, carbon tetrachloride, and dibromomethane are 1.48, 1.59, and 2.50 g/cm3 respectively. On which liquid(s) will topaz float?

Back 8

on none of the liquids

Front 9

In one gram of carbon, one gram of sulfur, and one gram of helium, there are

Back 9

more atoms of helium than of sulfur or carbon

Front 10

How many oxygen atoms are present in 1.5 moles of glucose, C6H12O6?

Back 10

5.4 x 10^24

Front 11

Rubidium (atomic weight 85.4678) has two naturally-occurring isotopes, the predominant one being 85-Rb with isotopic weight 84.9117 and an abundance of 72.15%. which of the following isotopic weights is the most likely for the other isotope?

Back 11

86.9085

Front 12

Which formula is incorrect? (F2, Fe, Ca2, S8, Br2)

Back 12

Ca2

Front 13

Dividing the molar mass of a monatomic element by Avogadro's number gives the

Back 13

average mass of one atom of the element in grams

Front 14

All of the following are true except:

Back 14

Ions can be formed by changing the number of protons in an atom's nucleus

Front 15

Balanced chemical equations imply which of the following?

Back 15

Numbers of atoms are conserved in chemical change

Front 16

LiHCO3+H2SO4->Li2SO4+H2O+CO2
When the equation above is balanced and the coefficients are reduced to lowest whole-number terms, what is the coefficient of H2O(l)?

Back 16

2

Front 17

The limiting reactant in a reaction

Back 17

has the lowest ratio of moles available/coefficient in the balanced equation

Front 18

A reaction occurs between sodium bicarbonate and hydrochloric acid producing sodium chloride, carbon dioxide, and water. The correct set of coefficients, respectively, for the balanced reaction is

Back 18

none of these (1, 1, 1, 1, 1)

Front 19

2Ag+Br2->2AgBr
According to the equation above, the greatest mass of Ag(s) (molar mass 108 g/mol) that can react with 5.30mL of Br2 (molar mass 160g/mol, density 3.00g/mL) is closest to

Back 19

22g

Front 20

Which is the empirical formula of the compound that is 92.3 percent carbon and 7.7 percent hydrogen by mass?

Back 20

CH

Front 21

Forms monatomic ions that have a charge of +2

Back 21

Mg

Front 22

Forms an acid with the formula HXO4

Back 22

Cl

Front 23

Combines with oxygen gas to form compounds that are common in air pollution and that cause acid rain

Back 23

S

Front 24

Is the least chemically reactive

Back 24

Ne

Front 25

Which flask contains the smallest number of moles of gas?

Back 25

N2, 50°C, 0.5 atm

Front 26

In which flask to the molecules have the greatest average speed?

Back 26

N2, 50°C, 0.5 atm

Front 27

Which flask contains the sample with the greatest density?

Back 27

O2, 40°C, 2 atm

Front 28

C3H8+5O2->3CO2+4H2O
In the reaction represented above, what is the total number of moles of reactants consumed when 1.00 mole of CO2 is produced?

Back 28

2.00 mol

Front 29

Which of the following statements best accounts for the observation that per mole, calcium chloride is more effective than sodium chloride in preventing the formation of ice on surfaces in winter?

Back 29

One mole of calcium chloride produces more ions in solution than one mole of sodium chloride does.

Front 30

In the reaction represented by the balanced equation above, how many moles of electrons are transferred per mole of [Cr2O7]2-?

Back 30

6

Front 31

All of the following are assumptions of the kinetic molecular theory of gases EXCEPT

Back 31

The mass of the gas particles is zero.

Front 32

Which of the following metals produces bubbles of hydrogen gas when it is placed in 2.0 M HCl?

Back 32

Mg(s)

Front 33

What is the concentration of Cl- in 4.0L of a 0.12M solution of CaCl2?

Back 33

0.24 M

Front 34

A 1L flask containing oxygen gas and a 2L flask containing hydrogen gas are connected through a stopcock, as shown above. The oxygen gas is at 2atm and 25°C, and the hydrogen gas is at 3atm and 25°C. The stopcock is opened and the two gases are allowed to mix. After mixing, what are the partial pressures of oxygen gas and hydrogen gas at 25°C?

Back 34

Oxygen: 2/3 atm
Hydrogen: 2 atm

Front 35

For an experiment, a student needs 100mL of 0.422M NaCl. If the student starts with NaCl and distilled water, which of the following pieces of laboratory glassware should the student use to prepare the solution with the greatest accuracy?

Back 35

100 mL volumetric flask

Front 36

Cu+HNO3->Cu(NO3)2+NO2+H2O
When the equation above is balanced and the coefficients are reduced to lowest whole-number terms, what is the coefficient of H2O?

Back 36

2

Front 37

A student prepares a solution by dissolving 60.0g of glucose (180.2 g/mol) in enough distilled water to make 250.0mL of solution. The molarity of the solution should be reported as

Back 37

1.33 M

Front 38

Which of the following best describes what happens when a solution of BaCl2 is added to a solution of K2SO4?

Back 38

Ionic bonds are formed, and a solid is produced

Front 39

When equal volumes of the following pairs of solutions are mixed, which will produce a precipitate?

Back 39

1M Ba(NO3)2 and 1M Na2SO4 & 1M K2CrO4 and 1M Pb(NO3)2

Front 40

A hygroscopic substance requires special care when handling and when it is stored in a laboratory. Why does it need this special care?

Back 40

it absorbs water from the atmosphere

Front 41

Find Δ (in kJ/mol) for the reaction: CIF+F2->CIF3

Back 41

-108.7 kJ/mol

Front 42

H2+(1/2)O2->H2O
ΔH°=-286 kJ

Which of the following is the best statement?

Back 42

Both the reaction is exothermic and the enthalpy of the products is less than that of the reactants.

Front 43

Which of the following statements correctly describes the signs of q and w for the following exothermic process at 1atm pressure and 370K?
H2O(g)->H2O(l)

Back 43

q is negative and w is positive

Front 44

In an insulated cup of negligible heat capacity, 50g of water at 40°C is mixed with 30g of water at 20°C. The final temperature of the mixture is closest to

Back 44

33°C

Front 45

Which of the following statements must be true about a liquid that has been heated to its boiling point in a vessel that is open to the atmosphere?

Back 45

The vapor pressure of the liquid is equal to the atmospheric pressure.

Front 46

At 1atm, a solid, pure substance was heated at a constant rate to produce the heating curve above. As it was heated, the substance melted and then later boiled. On the basis of this heating curve, which of the following statements about the substance must be correct?

Back 46

The heat of vaporization is greater than the heat of fusion.

Front 47

The standard enthalpy of formation, ΔHf, of HI(g) is +26kJ/mol. Which of the following is the approximate mass of HI(g) that must decompose into H2 and I2 to release 500 kJ of energy?

Back 47

2,500g

Front 48

Given the information above, what is the enthalpy change ΔH°, for the reaction represented below?
2CO+O2->2CO2

Back 48

-568kJ/mol

Front 49

NaOH+HCl->H2O+NaCl
A student is trying to determine the heat of reaction for the acid-base neutralization reaction represented above. Which of the following situations, by itself, would most likely result in the LEAST error int he calculated value of the heat of reaction?

Back 49

The thermometer was incorrectly calibrated and read 0.5 Celsius degree too high during the procedure.

Front 50

Which of the following statements regarding atomic theory is NOT true?

Back 50

Heisenberg's uncertainty principle describes the equivalence of mass and energy.

Front 51

Electromagnetic radiation with the longest wavelength is

Back 51

microwave radiation

Front 52

Using the Aufbau principle of electron energy ordering, the correct electromagnetic configuration for the gold (III) ion is

Back 52

D (76) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 4f14 5d8

Front 53

Is in an excited state

Back 53

1s2 2s1 2p1

Front 54

Has exactly 5 valence electrons

Back 54

1s2 2s2 2p3

Front 55

Has the highest first ionization energy

Back 55

1s2

Front 56

A neutral atom has the following ground-state electron configuration: 1s2 2s2 2p6 3s2 3p5. The atom is that of an element that is best classified as a

Back 56

nonmetal

Front 57

For the element strontium, it can be correctly predicted that the greatest difference in ionization energies would be between the

Back 57

second and third ionization energies

Front 58

Which of the following species in the ground state has the largest number of unpaired electrons?

Back 58

Mn

Front 59

In which of the following are the chemical species correctly ordered from smallest radius to largest radius?

Back 59

Cl < S < [S]2-

Front 60

3C2H2->C6H6
What is the standard enthalpy change, ΔH°, for the reaction represented above? (ΔH°f of C2H2 is 230kJ/mol; ΔH°f of C6H6 is 83kJ/mol)

Back 60

-607 kJ

Front 61

Approximately what mass of CuSO4•5H2O (250g/mol) is required to prepare 250mL of 0.10M copper (II) sulfate solution?

Back 61

6.2 g

Front 62

2NO+O2->2NO2
A possible mechanism for the overall reaction represented above is the following.
(1) NO + NO -> N2O2 slow
(2) N2O2 + O2 -> 2 NO2 fast
Which of the following rate expressions agrees best with this possible mechanism?

Back 62

Rate = k[NO]2

Front 63

Of the following compounds, which is the most ionic?

Back 63

CaCl2

Front 64

The best explanation for the fact that diamond is extremely hard is that diamond crystals

Back 64

are giant molecules in which each atom forms strong covalent bonds with all of its neighboring atoms

Front 65

A solution is made by dissolving a nonvolatile solute in a pure solvent. Compared to the pure solvent, the solution

Back 65

has a higher normal boiling point

Front 66

[HCO3]-+[OH]-<->H2O+[CO3]2-
ΔH = -41.4

When the reaction represented by the equation above is at equilibrium at 1 atm and 25°C, the ratio [CO3 2-]/[HCO3 -] can be increased by doing which of the following?

Back 66

Decreasing the temperature

Front 67

An excess of Mg is added to 100. mL of 0.400 M HCl. At 0°C and 1 atm pressure, what volume of H2 gas can be obtained?

Back 67

448 mL

Front 68

H2+Br2<->2HBr
At a certain temperature, the value for the equilibrium constant, K, for the reaction represented above is 2.0x10^5. What is the value of K for the reverse reaction at the same temperature?

Back 68

5.0 x 10^-6

Front 69

The atomic mass of copper is 63.55. Given that there are onlyt wo naturally occuring isotopes of copper, 63Cu and 65Cu, the natural abundance of the 65Cu isotope must be approximately

Back 69

25%

Front 70

What is the mole fraction of ethanol, C2H5OH, in an aqueous solution that is 46 percent ethanol by mass? (The molar mass of C2H5OH is 46g/mol; the molar mass of H2O is 18g/mol)

Back 70

0.25

Front 71

The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following?

Back 71

Na has a lower first ionization energy than Ne

Front 72

Which of the following is a correct statement about reaction order?

Back 72

Reaction order can be determined only by experiment.

Front 73

Propane gas, C3H8, burns in excess oxygen gas. When the equation for this reaction is correctly balanced and all coefficients are reduced to their lowest whole-number terms, the coefficient for O2 is

Back 73

5

Front 74

According to the VSEPR model, the progressive decrease in bond angles in the series of molecules CH4, NH3, and H2O is best accounted for by the

Back 74

increasing number of unshared pairs of electrons

Front 75

Which of the following must be true for a reaction for which the activation energy is the same for both the forward and reverse reactions?

Back 75

ΔH for the reaction is zero.

Front 76

A reaction was observed for 20 days and the percentage of the reactant remaining after each day was recorded in the table above. Which of the following best describes the order and the half-life of the reaction?

Back 76

First, 3 days

Front 77

Rate = k[M][N]2
The rate of a certain chemical reaction between substances M and N obeys the rate law above. The reaction is first studied with [M] and [N] each 1 x 10^-3 molar. If a new experiment is conducted with [M] and [N] each 2 x 10^-3 molar, the reaction rate will increase by a factor of

Back 77

8

Front 78

2N2H4+N2O4->3N2+4H2O
When 8.0g of N2H4 (32g/mol) and 92g of N2O4 (92g/mol) are mixed together and react according to the equation above, what is the maximum mass of H2O that can be produced?

Back 78

9.0g

Front 79

Which of the following substances is LEAST soluble in water?

Back 79

BaCO3

Front 80

A precipitation reaction

Back 80

[Ca]2+ + [SO4]2- -> CaSO4 (D)

Front 81

A reaction in which the same reactant undergoes both oxidation and reduction

Back 81

3Br2 + 6OH- -> 5Br- + BrO3- + 3H2O (C)

Front 82

A combustion reaction

Back 82

S8 + 8O2 -> 8SO2 (B)

Front 83

In which of the following species does sulfur have the same oxidation number as it does in H2SO4?

Back 83

SO2Cl2

Front 84

2NH3 <-> [NH4]+ + [NH2]-
In liquid ammonia, the reaction represented above occurs. In the reaction [NH4]+ acts as

Back 84

the conjugate acid of NH3

Front 85

At 25°C aqueous solutions with a pH of 8 have a hydroxide ion concentration, [OH-], of

Back 85

1.0 x 10^-6

Front 86

Which of the following indicators is the best choice for this titration?

Back 86

Phenolphthalein (8.2-10.0)

Front 87

Which of the following represents a Bronsted-Lowry acid-base reaction?

Back 87

[NH4]+ + [OH]- -> NH3 + H2O

Front 88

When solid NH4SCN is mixed with solid Ba(OH)2 in a closed container, the temperature drops and a gas is produced. Which of the following indicates the correct signs for ΔG, ΔH, and ΔS for this process?

Back 88

ΔG: -
ΔH: +
ΔS: +

Front 89

[Cr2O7]2- + H2S + [H]+ -> [Cr]3+ + S + H2O

When the equation above is correctly balanced and all coefficients are reduced to lowest whole-number terms, the coefficient for [H]+ is

Back 89

8

Front 90

3Cu + 8[H]+ + 2[NO3]- -> 3[Cu]2+ + 2NO + 4H2O

True statements about the reaction represented above include which of the following?

Back 90

The oxidation state of nitrogen changes from +5 to +2.

Front 91

Which of the following must be true for a reaction for which the activation energy is the same for both the forward and the reverse reactions?

Back 91

ΔH for the reaction is zero.

Front 92

In the electroplating of nickel, 0.200 faraday of electrical charge is passed through a solution of NiSO4. What mass of nickel is deposited?

Back 92

5.87g

Front 93

Of the following compounds, which contains the smallest bond angle?

Back 93

SF6

Front 94

Which of the following molecules contains polar covalent bonds but is a nonpolar molecule?

Back 94

CCl4

Front 95

Resonance structures can be used to represent the bonding in which of the following species?

Back 95

O3 and NO2

Front 96

Is a polar molecule

Back 96

SF4

Front 97

Has a square-planar molecular geometry

Back 97

XeF4

Front 98

Contains more than one pi-bond

Back 98

CO2

Front 99

Which of the following species in the ground state has the largest number of unpaired electrons?

Back 99

Mn

Front 100

1s2 2s2 2p6 3s2 3p5
What is the lewis structure (electron-dot diagram) for the atom?

Back 100

..
:X:
.

Front 101

1s2 2s2 2p6 3s2 3p5
The atom is that of an element that is best classified as a

Back 101

nonmetal

Front 102

The hybridization of the lead atom in PbCl4 is

Back 102

none of these

Front 103

Given the following bond energies, estimate the enthalpy change (heat of reaction) for the combustion of methane (CH4)

Back 103

-808 kJ

Front 104

pi bonding occurs in each of the following species EXCEPT:

Back 104

CH4

Front 105

The geometry of the SO3 molecule is best described as

Back 105

trigonal planar

Front 106

The shape of XeF4 will be

Back 106

square planar

Front 107

In which of the following does sigma bonding NOT occur?

Back 107

none of the above

Front 108

How many unpaired electrons are there in an atom of sulfur in its ground state?

Back 108

2

Front 109

Sodium losing an electron is an ______ process and fluorine losing an electron is an ______ process.

Back 109

endothermic, endothermic

Front 110

Which of the following bonds would be the least polar yet still be considered polar covalent?

Back 110

N-O

Front 111

Atoms of an element "X" have the electronic configuration 1s2 2s2 2p6 3s2 3p3. The compound "X" will most likely form with Strontium, Sr, is

Back 111

Sr3X2

Front 112

The observed molecular geometry of BrF3 is

Back 112

T-shaped

Front 113

The hybridization that would occur in BrF3 would be

Back 113

sp3d

Front 114

How many of the following molecules possess dipole moments?

Back 114

2

Front 115

Which of the following has the smallest radius?

Back 115

[Ca]2+

Front 116

As indicated by Lewis structures, which of the following species could probably not exist as a stable molecule?

Back 116

N2H6

Front 117

Which of the molecules best obeys the octet rule?

Back 117

PCl3

Front 118

How many of the molecules have no dipole moment?

Back 118

NO2

Front 119

Which of these molecules shows resonance?

Back 119

NO2, O3

Front 120

The hybridization of I in IF- is

Back 120

d2sp3

Front 121

How many electrons are involved in pi bonding in benzene, C6H6?

Back 121

6