CEM 26897 | Course Paper

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Which of the following statements concerning structural isomers is/are correct?

1/ Structural isomers have the same elemental composition, but the atoms are linked in

different ways.

2/ Structural isomers have identical physical properties, but different chemical

properties.

3/ Structural isomers have identical structures, but contain different isotopes of the

same elements.

A.1 only

B.2 only

C.3 only

D.1 and 2

E.1, 2, and 3

For which of the following transitions would a hydrogen atom emit the lowest energy

photon?

A.n = 4 to n = 5

B.n = 5 to n = 2

C.n = 4 to n = 3

D.n = 3 to n = 1

E.n = 3 to n = 2

Which of the following substances is never a Brnsted-Lowry acid in an aqueous

solution?

A.sodium dihydrogen phosphate, NaH2PO4(s)

B.sodium acetate, NaCH3CO2(s)

C.ammonium nitrate, NH4NO3(s)

D.hydrogen bromide, HCl(g)

E.sodium bicarbonate, NaHCO3(s)

What is the distance, in atomic radii, along any edge of a body-centered unit cell?

B.2 r

C.4 r

E.r

Ammonia, NH3, is used as a refrigerant. At its boiling point of “33 C, the standard

enthalpy of vaporization of ammonia is 23.3 kJ/mol. How much heat is released when

50.0 g of ammonia is condensed at “33 C?

A.”0.466 kJ

B.”7.94 kJ

C.”36.6 kJ

D.”68.4 kJ

E.”1.17 103 kJ

Given the following equilibria,

Ni2+(aq) + 2 OH“(aq) Ni(OH)2(s) K1 = 1.8 1015

Ni2+(aq) + 4 CN“(aq) Ni(CN)4

2″(aq) K2 = 2.0 1031

determine the equilibrium constant, Kc, for the following reaction.

Ni(OH)2(s) + 4 CN“(aq) Ni(CN)4

2″(aq) + 2 OH“(aq)

A.2.8 10“47

B.9.0 10“17

C.1.8 1015

D.1.1 1016

E.3.6 1046

Which of the following ions have the same ground state electron configuration: S2″,

N3″, Mg2+, and Br“?

A.N3″ and Mg2+

B.S2″, N3″, and Br“

C.S2″ and Br“

D.Mg2+ and Br“

E.S2″, N3″, Mg2+, and Br“

The conjugate base of HPO4

2″ is ____.

A.OH“

B.PO4

3″

C.H2PO4

“

D.H2O

E.H3O+

Metals react with oxygen gas to produce oxides with the general formula MxOy. Write a

balanced chemical equation for the reaction of titanium with oxygen to yield

titanium(IV) oxide.

A.4 Ti(s) + O2(g) 2 Ti2O(s)

B.Ti(s) + O2(g) TiO2(s)

C.2 Ti(s) + O2(g) 2 TiO(s)

D.Ti(s) + O(g) TiO(s)

E.8 Ti(s) + O2(g) 2 Ti4O(s)

For the reaction A B, the rate law is

What are the units of the rate constant where time is measured in seconds?

What is the name of the following compound?

A.3-methyl-2-isopropylacetylene

B.cis-4-methylhexyne

C.4-methyl-2-hexyne

D.1-methy-2-ethyl-4-butyne

E.trans-3-methyl-4-hexyne

One statement of the first law of thermodynamics is that

A.the amount of work done on a system is dependent of the pathway.

B.the total work done on a system must equal the heat absorbed by the system.

C.the total work done on a system is equal in magnitude, but opposite in sign of the heat

absorbed by the system.

D.the total energy change for a system is equal to the sum of the heat transferred to or

from the system and the work done by or on the system.

E.in any chemical process the heat flow must equal the change in enthalpy.

According to the effective atomic number rule, Mo(0) should coordinate to ____

carbonyl ligands.

A.4

B.5

C.6

D.7

E.8

What is the classification of the molecule below?

A.polymer

B.fatty acid

C.saccharide

D.carbohydrate

E.triglyceride

Diagram 9-1

The molecular orbital diagram below may be used for the following problem(s). For

oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However,

the diagram will still yield correct bond order and magnetic behavior for these

molecules.

Energy ________ s*2p

________ ________ p*2p

________ s2p

________ ________ p2p

________ s*2s

________ s2s

________ s*1s

________ s1s

Refer to Diagram 9-1. What is the molecular orbital configuration of N2

2+?

A.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2 (p*2p)2

B.[core electrons] (s2s)2 (s*2s)2 (p2p)4

C.[core electrons] (s2s)2 (s*2s)2 (p2p)2 (s2p)2

D.[core electrons] (s2s)4 (s*2s)4

E.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2 (p*2p)4

Xenon has an enthalpy of vaporization of 12.6 kJ/mol and a vapor pressure of 1.00 atm

at “108.0 C. What is the vapor pressure of xenon at -148.0 C? (R = 8.314 J/Kmol)

A.0.053 atm

B.0.73 atm

C.0.93 atm

D.0.99 atm

E.19 atm

What is the correct cell notation for a voltaic cell based on the reaction below?

Cu2+(aq) + Fe(s) Cu(s) + Fe2+(aq)

A.Cu(s) | Cu2+(aq) || Fe2+(aq) | Fe(s)

B.Fe(s) || Fe2+(aq), Cu2+(aq) | Cu(s)

C.Cu(s) || Cu2+(aq), Fe2+(aq) || Fe(s)

D.Cu(s) | Fe2+(aq) || Cu2+(aq) | Fe(s)

E.Fe(s) | Fe2+(aq) || Cu2+(aq) | Cu(s)

What is the product of the addition of excess F2 to acetylene?

A.1,2-difluoroethane

B.ethylene

C.1,1,2,2-tetrafluoroethane

D.ethane

E.1,1-difluoroethylene

Which of the following statements is/are CORRECT?

1/ Complex ions with the structure [ML2]n are always linear.

2/ Complex ions with the structure [ML6]n are always octahedral.

3/ Complex ions with the structure [ML4]n are always square planar.

A.1 only

B.2 only

C.3 only

D.1 and 2

E.2 and 3

Calculate for the reaction below,

2 AgBr(aq) + 2 Hg(l) 2 Ag(s) + Hg2Br2(s)

given the following standard reduction potentials.

Hg2Br2(s) + 2 e“ 2 Hg(l) + 2 Br“(aq) E = +0.140 V

AgBr(aq) + e“ Ag(s) + Br“(aq) E = +0.071 V

A.”0.211 V

B.”0.069 V

C.+1.97 V

D.+0.069 V

E.+0.211 V

How many electrons can be described by the quantum numbers n = 4, = 2, = 0?

A.0

B.1

C.2

D.5

E.10

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of

boron tribromide, BBr3.

A.The electron-pair geometry is trigonal-pyramidal, the molecular geometry is

trigonal-pyramidal.

B.The electron-pair geometry is trigonal-planar, the molecular geometry is

trigonal-planar.

C.The electron-pair geometry is trigonal-planar, the molecular geometry is bent.

D.The electron-pair geometry is tetrahedral, the molecular geometry is

trigonal-pyramidal.

E.The electron-pair geometry is trigonal-pyramidal, the molecular geometry is t-shaped.

For a reaction, DrH = “208.8 kJ and DrS = “308.2 J/K. At what temperature will DrG =

0.00 kJ?

A.0.68 K

B.677.5 K

C.1476 K

D.6435 K

E.DG is less than 0.00 kJ at any temperature.

Which one of the following is not an SI base unit?

A.liter

B.mole

C.calorie

D.ampere

E.second

How much energy (in kJ) is required to change the temperature of 325 g aluminum

from 32 C to 815 C? The specific heat capacity of aluminum is 0.897 J/gK.

A.238 kJ

B.284 kJ

C.46.3 kJ

D.228 kJ

E.2.16 kJ

Which of the following types of radiation has the greatest quality factor?

A.beta particles

B.alpha particles emitted within the body

C.gamma rays

D.low energy protons

E.low energy neutrons

Write the expression for K for the reaction below.

Al3+(aq) + 4 OH“(aq) Al(OH)4

“(aq)

Determine the heat of evaporation of carbon disulfide,

CS2( ) CS2(g)

given the enthalpies of reaction below.

C(s) + 2 S(s) CS2( ) DrH = +89.4 kJ/mol-rxn

C(s) + 2 S(s) CS2(g) DrH = +116.7 kJ/mol-rxn

A.”206.1 kJ

B.”27.3 kJ

C.+27.3 kJ

D.+206.1 kJ

E.+1.31 kJ

Metal oxides react with water to produce ____.

A.bases

B.hydrogen gas

C.oxygen gas

D.acids

E.hydronium ions

Rank F, Cl, and Br in order of increasing first ionization energy.

A.F < Cl < Br

B.Cl < F < Br

C.Cl < Br < F

D.Br < F < Cl

E.Br < Cl < F