Advanced Chemistry Final Exam Questions

Front 1

Which of the following best represents a pair of isotopes?

Back 1

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

Front 2

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

Back 2

more atoms of helium than of sulfur or carbon

Front 3

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

Back 3

5.4 x 10^24

Front 4

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 4

86.9085

Front 5

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

Back 5

Ca2

Front 6

Balanced chemical equations imply which of the following?

Back 6

Numbers of atoms are conserved in chemical change

Front 7

The limiting reactant in a reaction

Back 7

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

Front 8

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 8

22g

Front 9

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

Back 9

CH

Front 10

Which flask contains the smallest number of moles of gas?

Back 10

N2, 50°C, 0.5 atm

Front 11

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 11

2.00 mol

Front 12

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 12

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

Front 13

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

Back 13

0.24 M

Front 14

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 14

2

Front 15

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 15

1.33 M

Front 16

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 16

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

Front 17

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

Back 17

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

Front 18

Electromagnetic radiation with the longest wavelength is

Back 18

microwave radiation

Front 19

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

Back 19

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

Front 20

Has the highest first ionization energy

Back 20

1s2

Front 21

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 21

nonmetal

Front 22

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

Back 22

second and third ionization energies

Front 23

Of the following compounds, which is the most ionic?

Back 23

CaCl2

Front 24

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

Back 24

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

Front 25

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 25

0.25

Front 26

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 26

Na has a lower first ionization energy than Ne

Front 27

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 27

9.0g

Front 28

Which of the following substances is LEAST soluble in water?

Back 28

BaCO3

Front 29

A combustion reaction

Back 29

S8 + 8O2 -> 8SO2 (B)

Front 30

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

Back 30

1.0 x 10^-6

Front 31

Contains more than one pi-bond

Back 31

CO2

Front 32

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

Back 32

N-O

Front 33

How many of the following molecules possess dipole moments?

Back 33

2

Front 34

Which of the following has the smallest radius?

Back 34

[Ca]2+

Front 35

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

Back 35

N2H6

Front 36

Which of the molecules best obeys the octet rule?

Back 36

PCl3

Front 37

How many of the molecules have no dipole moment?

Back 37

NO2

Front 38

Which of these molecules shows resonance?

Back 38

NO2, O3