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WorksheetsAdvanced Inorganic Chemistry
Total questions: 100
Worksheet time: 2hrs 40mins
An improper rotation axis, S, arises from which of the following situations?
A mirror plane combined with an inversion
Two proper rotation axes combined
Identity combined with a mirror plane
A proper rotation axis combined with a mirror plane
The combination of two mirror planes
Choose the best answer to fill in the blanks. Raman activity is dictated by a change in the _____________ of a molecule, while IR activity is related to a change in the ____________.
Polarizability, dipole moment
Magnetism, dipole moment
Symmetry, magnetism
Dipole moment, polarizability
Magnetism, symmetry
Dodecaborate (B12H12) does NOT contain which of the following symmetry elements?
E
C5
i
S10
C6
Fill in the blank. The character table for a C3v molecule, such as PCl3, lists three symmetry labels: A1, A2, and E. The A1 mode transforms z, z2, and x2 + y2. This means that the A1 mode is ________________.
IR active only
Raman active only
Both IR and Raman active
Neither IR or Raman active
The only spectroscopically active mode in the molecule
Fill in the blank. The character table for a D3h ion, such as CO32-, lists six symmetry labels: A1', A2', E', A1'', A2'', and E''. The A2' mode transforms Rz. This means that the A2' mode is _________________.
IR active only
Raman active only
Both IR and Raman active
Neither IR or Raman active
The only spectroscopically active mode in the molecule
In symmetry terms, which of the following MUST be true for an allowed transition?
Both the electronic and vibrational representations must be symmetric.
Both the electronic and vibrational representations must be asymmetric.
Only the electronic representations must be symmetric.
Only the vibrational representations must be symmetric.
Symmetry does not matter, as long as there is a change in dipole or polarizability.
Symmetry elements within a group must display which of the following?
Closure (If A and B belong to the group, and A x B = C, then C also belongs to the group.)
Associativity (A(BC) = (AB)C )
Identity (The symmetry element times its identity, E, remains unchanged.)
Inverses (There must be an inverse symmetry element that returns the molecule to its original state; A x A-1 = E.)
Continuity (If a molecule contains an n axis, then it also contains axes of n-1, n-2...)
Using the flow chart provided, determine which point group a tennis ball would belong to.
D2d
Cs
C2h
S4
D4
Which of the following has C4v symmetry?
H2O
BrF5
BH3
PCl6
W(CO)6
Which of the following does NOT contain an inversion center?
SF6
O2
BF3
C2Cl4
All of the choices
Hydrogen and helium both have two electrons (completely filled) bonding molecular orbitals. Hydrogen exists as a diatomic molecule; helium does not. Why?
Helium also has electrons in antibonding orbitals, resulting in a bond order of zero.
Helium also has electrons in non-bonding orbitals, resulting in a bond order of zero.
Helium is a noble gas and never forms bonds.
Hydrogen also has electrons in nonbonding orbitals, resulting in a bond order of two.
Hydrogen has no antibonding orbitals, resulting in a bond order of two.
The bond order of a molecule is given by the equation: ½ (bonding electrons – antibonding electrons). What accounts for the ½?
The amount of magnetic character is reduced in bonds.
The electrons are shared between two elements.
Nonbonding electrons decrease bond ability.
The antibonding electrons interfere with bonding.
None of the choices
What is the bond order for dinitrogen, N2?
5
1
1.5
2
3
When drawing the MO diagram of a heteronuclear diatomic molecule, at what relative positions should the atomic orbitals appear?
They should be at the same energy to indicate bond formation.
They should be at the same energy to indicate allowed symmetry.
They should be at different energies, relative to their difference in electronegativities.
They should be at different energies, relative to their atomic radii.
They should be at different energies, relative to the number of lone pairs of electrons.
When filling molecular orbitals, which of the following is FALSE?
A maximum of two electrons per orbital is allowed.
The orbitals with the lowest energy are filled first.
Orbitals of the same energies are half-filled first; then electrons are allowed to pair up.
Non-bonding orbitals are filled first.
All of the choices
Which of the following minimizes nucleus-nucleus repulsion and promotes electron-nucleus interaction?
Nonbonding molecular orbitals
Antibonding molecular orbitals
Bonding molecular orbitals
All of the choices
Nonbonding molecular orbitals and bonding molecular orbitals only
Which of the following must be true when atomic orbitals combine to form molecular orbitals?
They must have constructive net interaction.
They must have the correct symmetry to overlap
They must be similar in energy
There will be the same number of resultant molecular orbitals as atomic orbitals
All of the choices
Which of the following statements concerning sigma and pi molecular orbitals is FALSE?
Sigma interactions occur along the internuclear axis.
Pi interactions occur above and below the internuclear axis.
Sigma bonds form first, followed by the subsequent formation of pi bonds.
Two pi bonds are involved in a double bond.
All of the choices
Which of the following statements is true of nonbonding molecular orbitals?
They are responsible for the formation of pi bonds.
They are similar in energy to the atomic orbitals.
They counteract bond formation in a molecule.
They help hold the molecule together, once it is formed.
They are responsible for the formation of sigma bonds.
What compound is represented by this MO diagram? (Pay attention to the number of electrons and their respective energies.)
CO2
H2O
CN-
Cl2
N2
1s22s22p63s23p63d5 is the electron configuration for which element/ion?
Mn2+
V
Fe3+
All of the choices
Mn2+ and Fe3+ only
According to valence bond theory(VBT), O2 has no unpaired electrons. MO theory shows two unpaired electrons in a 2π* molecular orbital. Which of the following experiments supports the correct electron configuration?
An EPR spectrum shows that oxygen is paramagnetic; MO theory is correct.
An EPR spectrum shows that oxygen is paramagnetic; VBT is correct.
Infrared spectroscopy shows a double bond stretch; MO theory is correct.
Infrared spectroscopy shows a double bond stretch; VBT is correct.
There is no way to know which theory is correct in this matter.
According to valence bond theory, what is the difference between a complex with d2sp3 hybridization and sp3d2 hybridization?
There is no actual difference; the orbitals involved are the same, only listed in a different order.
The complex having d2sp3 hybridization is an “inner shell” complex, while the complex with sp3d2 hybridization is an “outer shell” complex.
The complex having d2sp3 hybridization is an “outer shell” complex, while the complex with sp3d2 hybridization is an “inner shell” complex.
The complex having sp3d2 hybridization does not exist; the electrons must fill the lowest energy orbitals first.
The complex having d2sp3d2 hybridization does not exist; the electrons must fill the orbitals with the same principle quantum number.
Analysis of a high spin d6 complex reveals that it is diamagnetic. What is the probable molecular geometry of the complex?
Octahedral
Tetrahedral
Square planar
All of the choices
Both Octahedral and Square planar
Compounds with octahedral molecular geometries sometimes elongate or compress through Jahn-Teller distortion. In doing so, which of the following occurs?
They increase their ionization potential, rendering them most useful electrochemically.
They reduce degenerate molecular orbitals, allowing a more stable molecule to exist.
They undergo a strong magnetic transition, allowing easier detection by NMR and EPR.
They increase their transition state energy, making them useful catalysts.
They decrease shielding, allowing spectroscopically forbidden transitions to occur.
Do high spin d5 octahedral complexes experience Jahn-Teller distortion? Why, or why not?
Yes. The five electrons distribute themselves evenly in the five molecular orbitals, causing them to be degenerate. Axial elongation reduces this degeneracy.
Yes. The five electrons distribute themselves evenly in the five molecular orbitals, causing them to be degenerate. Axial compression reduces this degeneracy.
No. The five electrons distribute themselves evenly in the five molecular orbitals; no degeneracy exists.
No. Four of the electrons are paired. Only one electron is unpaired and can only fill the one remaining orbital. No degeneracy exists.
Yes. Four electrons are paired in the lower energy orbitals. The fifth electron can position itself into any of the remaining three orbitals, making it triply degenerate.
Ferrocene consists of two cyclopentadienyl rings bound through 5 carbons to an iron center. What is the IUPAC name for ferrocene?
mer-bis(cyclopentadienyl)iron(II)
fac-bis(cyclopentadienyl)iron(II)
bis(η5-cyclopentadienyl)iron(II)
µ-bis(cyclopentadienyl)iron(II)
(η5-cyclopentadienyl)iron(II)
How would the complexes Λ-[Co(en)3]3+ and Δ-[Co(en)3]3+ differ?
One would be a solid at room temperature, while the other would be a liquid.
One would be highly colored, while the other would be colorless.
One would be paramagnetic, while the other would be diamagnetic.
One would rotate plane-polarized light clockwise, while the other would rotate it counterclockwise.
All of the choices
In chromium and copper, the 3d orbital fills before the 4s orbital is filled. Why?
Because the stability gained from having a fully-filled or evenly, half-filled set of d orbitals is greater than the need to fill all lower energy orbitals first
Because the 3d orbital is actually lower in energy than the 4s, so it fills first
Because copper and chromium only exist as ions; never as neutral elements
Because the atomic radii are so large that no effect is felt by the nucleus
None of the choices
Phosphines are often used as molecular bridges between two metal centers. How should these phosphines be notated according to IUPAC nomenclature?
mu (µ)
eta (η)
chi (χ)
xi (ξ)
zeta (ζ)
Transition metals exhibit all of the following general characteristics, EXCEPT:
They are malleable and ductile.
They have high melting points.
They conduct heat and electricity.
They are lustrous.
They undergo irreversible oxidation.
Using ligand field theory, which of the following would you predict to be the most paramagnetic?
A low spin, d5 octahedral complex
A high spin, d8 octahedral complex
A low spin, d3 octahedral complex
A d2 tetrahedral complex
A d5 square planar complex
Using the valence bond theory and the 18 electron rule, which of the following would you predict to be the most stable?
Fe(CO)5
Ni(CO)5
Mo(CO)6
Re(CO)6
Ir(CO)5
What happens when the electron pairing energy is larger than the octahedral field splitting energy?
The result is a low-spin complex, where electrons will pair up and fill the lowest energy level.
The result is a high-spin complex, where electrons will be promoted to the next energy level before pairing.
The result is an unstable complex, where electrons can either pair or be promoted to the next energy level.
The result is a high-spin complex, where electrons will pair up and fill the lowest energy level.
The result is a low-spin complex, where electrons will be promoted to the next energy level before pairing.
Which of the following has T-shaped molecular geometry?
BF3
ClF3
PF6
IF5
SbF5
Which of the following influences the amount of crystal field splitting in a metal complex?
Charge of the metal ion
Nature of the ligands
Geometry of the complex
Size of the ligands
All of the choices
Which of the following sets of complexes represents a set of stereoisomerism (not structural isomerism)?
[PtCl(H2O)3]Br and [Pt(Br)(H2O)3]Cl
cis-[PtCl2(NH3)2] and trans-[PtCl2(NH3)2]
[CrCl2(H2O)4]Cl•2H2O and [CrCl3(H2O)3]•3H2O
[Co(NH3)6] [Cr(ac)3] and [Co(ac)3] [Cr(NH3)6]
[Co(SCN)(NH3)5]- and [Co(NCS)(NH3)5]-
Which of the following would have the largest ionization energy?
Copper
Iron
Gold
Titanium
Tungsten
You discover a new metal complex that exhibits high spin characteristics. What ligand properties can you predict?
It is highly polarizable.
The ligand is relatively large.
The ligand exhibits π donor ability.
The ligand is acidic.
All of the choices
Which of the following would have the highest melting point?
Silver
Rhodium
Cadmium
Molybdenum
The melting points would be equivalent, because they are in the same period.
If a complex has a maximum absorption at 423 nm, what color would the complex appear to the human eye?
Violet
Blue
Green
Yellow
Red
Some tetrahedral metal complexes exhibit weak electronic transitions even though they are symmetry forbidden. Why?
Jahn-Teller distortion
Mixing of the p and d orbitals
MLCT
LMCT
All of the choices
The UV spectrum of metal complex A has a strong absorption at 412 nm. The UV spectrum of metal complex B has a strong absorption at 654 nm. If equal quantities of the two solutions of metal complexes are mixed, what would the resulting UV spectrum look like?
The spectrum would show one very broad absorption band at 533 nm.
The spectrum would show two weak absorption bands, one at 412 nm and the other at 654 nm.
The spectrum would show two strong absorption bands, one at 412 nm and the other at 654 nm.
The spectrum would show two weak absorption bands, one at 472 nm and the other at 594 nm.
The spectrum would show two strong absorption bands, one at 472 nm and the other at 594 nm.
The vertical line (located at Δ/B = 2 for a d6 system) in the Tanabe-Sugano diagram corresponds to which of the following?
The ligand field stabilization energy (LFSE) is insufficient to allow transitions to the left of the line.
The transitions to the left are symmetry allowed, while the transitions to the right are spin allowed.
The transitions to the left are spin allowed, while the transitions to the right are symmetry allowed.
The transitions to the left are low-spin complexes, while the transitions to the right are high-spin complexes.
The transitions to the left are high-spin complexes, while the transitions to the right are low-spin complexes.
Using the spin selection rules and the Tanabe-Sugano diagram provided, how many electronic transitions would you expect to see in the spectrum of a d8complex if Δ/B = 1.5?
Two
Three
Nine
Six
Zero
Which of the following is true with regard to charge transfer (ligand-to-metal or metal-to-ligand) absorption bands in relation to d-d transition bands?
CT absorptions occur at higher wavelengths than d-d transitions.
CT absorptions are less intense than d-d transitions.
CT transitions are symmetry and spin allowed; d-d transitions are symmetry forbidden.
CT transitions are spin allowed; d-d transitions are spin forbidden.
CT transitions are symmetry and spin forbidden; d-d transitions are symmetry forbidden but spin allowed.
Which of the following would be a spin allowed transition?
3T1 → 1T1
5E → 2E
3T1 → 3A2
1A2 → 3A2
4T2 → 2T4
Why are the hexaaqua complexes of Sc3+ and Zn+2 colorless, while the hexaaqua complexes of Fe2+, Cr3+, Co2+, Ni2+, and Cu2+ are intensely colored?
Zn2+ has a completely filled d orbital, and Sc3+ has a completely empty d orbital.
Zn2+ and Sc3+ always form high spin octahedral complexes.
Zn2+ and Sc3+ always form low spin octahedral complexes.
Zn2+ and Sc3+ are diamagnetic; the others are paramagnetic.
Zn2+ and Sc3+ are paramagnetic; the others are diamagnetic.
Why does a high spin d5 octahedral complex exhibit a very pale color, while a low spin d5 octahedral complex is more highly colored?
The transition in the high spin complex is symmetry and spin forbidden. The transition in the low spin complex is symmetry allowed.
The transition in the high spin complex is symmetry and spin forbidden. The transition in the low spin complex is spin allowed.
The transition in the high spin complex is symmetry forbidden but spin allowed. The transition in the low spin complex is symmetry and spin allowed.
The transition in the high spin complex is spin forbidden but symmetry allowed. The transition in the low spin complex is symmetry and spin allowed.
The transition in the high spin complex is symmetry and spin forbidden. The transition in the low spin complex is symmetry and spin allowed.
You have two solutions of chromium ions. Your lab partner has added potassium thiocyanate to one and potassium cyanide to the other, but does NOT remember which one contains which anion. Just by appearance, how can you tell them apart?
The solution containing cyanide ion will give a larger crystal field splitting, causing a blue shift in the color of the complex. The complex with thiocyanate ion will appear as more red shifted.
The solution containing cyanide ion will give a smaller crystal field splitting, causing a blue shift in the color of the complex. The complex with thiocyanate ion will appear as more red shifted.
The solution containing cyanide ion will give a larger crystal field splitting, causing a red shift in the color of the complex. The complex with thiocyanate ion will appear as more blue shifted.
The solutions will both be similar in color; however, the complex with thiocyanate will be more intense.
You cannot tell them apart; the experiment would need to be restarted.
A 19F NMR spectrum at room temperature reveals on well defined peak. When cooled slightly, the peak becomes broadened. At N2(l) temperatures, two well defined peaks are apparent. What is responsible for these observations?
Dynamic fluxionality
Spin-spin coupling interactions
Integer quantum spin numbers (I = 1,2,3…)
Fractional quantum spin numbers (I = 1/2, 3/2, 5/2)
Low natural abundances of the 19F nucleus
Carbon dioxide is a linear molecule with no dipole moment. Which of the following interactions is responsible for the observed IR spectrum of CO2?
The asymmetric stretch of the C-O bonds creates a dipole moment that is IR active.
The symmetric stretch of the C-O bonds creates a dipole moment that is IR active.
The non-linear bending mode crates a net dipole, which is IR active.
All of the choices
The asymmetric stretch of the C-O bonds creates a dipole moment that is IR active and the non-linear bending mode crates a net dipole (which is IR active) only
In NMR spectroscopy, what happens to the chemical shift and resonance frequency of a compound when the spectrometer frequency changes?
The chemical shift and resonance frequency also change.
The chemical shift changes; the resonance frequency remains constant.
The chemical shift remains constant; the resonance frequency changes.
The chemical shift and resonance frequency remain constant.
There is no way to predict the effect.
The splitting of energy levels in the presence of a magnetic field is caused by which of the following?
The Zeeman effect
Pauli exclusion principle
Symmetry degeneracy
Fermi contact interaction
Bose-Einstein effect
What is the most likely cause of fluxional behavior in the NMR spectrum of Fe(CO)5, iron pentacarbonyl?
Dissociation and recoordination of the carbonyl ligands
Rotation of a hindered carbonyl bond
Opening and closing of bridging carbonyls
Isomerism between trigonal bipyramidal and square pyramidal configurations
Monmer-dimer formation with a bridging carbonyl
What molecule most likely produced this EPR spectrum?
NO2 radical
CH3 radical
CH2Cl radical
CH2CH2 radical
OH radical
Which of the following cannot be studied by EPR?
Paramagnetic transition metal complexes
Diamagnetic transition metal complexes
Free radicals in the solid state
Free radicals in the liquid or gas state
Complexes containing more than one unpaired electron
Which of the following conditions does NOT result in a nonzero quantum spin number (I)?
An odd mass number and odd atomic number, such as 1H
An odd mass number and an even atomic number, such as 13C
An even mass number and an even atomic number, such as 16O
An even mass number and an odd atomic number, such as 14N
All of the mentioned situations will result in a nonzero quantum spin number.
Which of the following would be predicted to have a g-factor value close to 2?
A free electron
An unpaired electron in an organic molecule
An unpaired electron in a transition metal complex
All of the choices
A free electron and an unpaired electron in an organic molecule only
Why does Re(CO)5Cl exhibit lower carbonyl stretching frequencies (νco) than [Re(CO)5(py)]+?
Cationic metal complexes experience less π backbonding than their neutral or anionic analogs.
Pyridine is a good π acceptor and contributes to increased π backbonding.
The carbonyl to metal bond strength is increased in the chloro complex.
All of the choices
Cationic metal complexes experience less π backbonding than their neutral or anionic analogs and pyridine is a good π acceptor and contributes to increased π backbonding only
EDTA4- is a polydentate ligand. How many coordination sites does it contain and through what moieties?
Two; through the lone pairs on the two nitrogen atoms
Two; through the lone pairs on two of the oxygen atoms
Four; through the lone pairs on the four oxygen atoms
Four; through the anion on the four oxygen atoms
Six; two through the lone pairs on the two nitrogen atoms and four through the lone pairs of the four oxygen atoms
How do Cp complexes and derivatives of metal ions undergo ligand substitution reaction?
Associative mechanism, aided by a ring slip
Dissociative mechanism, in which the Cp ring is lost
Inversion of stereochemistry and loss of the Cp ring
Dissociation of the Cp ligand, followed by re-association of Cp
All of the choices
How is it possible to form different transition metal complexes when mixed with the same two ligands?
It is dependent on which ligands are a part of the primary valence and which ones are a part of the secondary valence.
It depends on the charge of the metal ion present.
It depends on the number of empty d orbitals.
It depends on the nature of the ligands involved and whether they are mono or multi-dentate.
All of the choices
Using the neutral (covalent) method of electron counting, how many electrons are donated to a metal center by a cyclopentadiene ring?
2
5
6
8
10
What is the coordination number of [Cu(NH3)4][Cl-]2?
2
3
4
5
6
What is the oxidation state of chromium in [Cr(NH3)2(C2O4)2]- ?
+3
+2
+4
+7
+6
What is true about coordinative unsaturation?
It plays an important role in insertion, polymerization, and metathesis reactions.
It describes a complex with a coordination number less than 4.
It generally means another ligand can be accommodated.
All of the choices
It plays an important role in insertion, polymerization, and metathesis reactions and it generally means another ligand can be accommodated only
Which compound will react with Ag+ ion in water: [Co(NH3)6]Cl3 or [Co(Cl3)](NH3)6? What is formed?
[Co(Cl3)](NH3)6; AgCl is formed.
[Co(Cl3)](NH3)6; NH4Cl is formed.
[Co(NH3)6]Cl3; AgCl is formed.
[Co(NH3)6]Cl3; NH4Cl is formed.
Both will react with silver in water; AgCl and NH4Cl are formed.
Which of the following is an ambidentate ligand?
EDTA
SCN-
NH3
Hemoglobin
Cl-
The interaction between the metal and ligands in coordination complexes can best be described as which of the following?
Hydrophilic interactions
Hydrophobic interactions
Van der Waals interactions
Lewis acid-base interactions
Hydrogen bonding interactions
A natural spring containing manganese is found to be highly acidic. Using this diagram, what form of iron would you predict to be most abundant?
Fe(s)
Fe3+(aq)
Fe(OH)2(s)
Fe2+(aq)
Fe(OH)3(s)
In Latimer diagrams, what does a large positive standard reduction potential indicate?
The species on the left is readily reduced to the species on the right side of the arrow.
The species on the lef tis a good reducing agent.
The species under goes diproportionation.
All of the choices.
None of the choices.
Marcus theory is used to approximate which of the following?
The heat of formation of the precursor complex
The heat of fission of the successor complex
The solvation energy of the transition complex
The free energy of electron transfer
All of the choices
What happens to an outer sphere redox reaction, if the spin multiplicity is different?
The reaction does not proceed.
The reaction is drastically slowed, requiring a spin flip to occur.
The reaction proceeds quicker, because different spin states allow faster electron transfer.
The reaction will proceed as inner sphere instead, because electrons with different spin will pair and form a bond.
None of the choices
What implication does overpotential have on a redox reaction?
Even though a reaction is thermodynamically favorable, the reaction may be slow kinetically.
All redox reactions are favorable at in alkaline media.
All thermodynamically favorable reactions occur quickly on a kinetic scale.
If a reaction is kinetically favorable, it will proceed even if it is thermodynamically unfavorable.
No redox reactions occur in highly acidic media.
What is considered the rate determining step in an outer sphere redox reaction?
Formation of the bridging ligand complex
Formation of the precursor (cage) complex
Electron transfer
Solvent entering the coordination sphere
Fission of the successor ligand complex
What is considered the rate determining step in an outer sphere redox reaction?
Formation of the bridging ligand complex
Fission of the successor ligand complex
Electron transfer
Solvent entering the coordination sphere
Both fission of the successor ligand complex and electron transfer
Which of the following is a properly balanced half reaction in acidic media?
Cr2O72- + 8 H+ + 3 H2C2O4 → 2 Cr3+ + 7 H2O + 6 CO2
12 H+ + 5 I- + IO3- → 3 I2 + 6H2O
2 Fe(OH)2 + H2O2 → 2 Fe(OH)3
3 Cd + 8 H+ + 2 NO3- → 3 Cd2+ + 2 NO + 8 H2O
2 Au3+ + 6I- → 2 Au + 3 I2
Which of the following is a properly balanced half reaction in basic media?
Cr2O72- + 8 H+ + 3 H2C2O4 → 2 Cr3+ + 7 H2O + 6 CO2
12 OH- + 5 I- + IO3- → 3 I2 + 6H2O
Fe(OH)2 + OH- → Fe(OH)3
2 Cr(OH)3 + ClO3− + 4 OH− → 2 CrO42− + Cl− + 5 H2O
2 Au3+ + 6I− → 2 Au + 3 I2
Given the Frost diagram for phosphorus and nitrogen in acidic conditions, which of the following species is the most thermodynamically favored?
H3PO4
NH4+
HNO3
PH3
P & N (elemental)
Cr2+ (d4 system) and Cu2+ (d9 system) are kinetically labile with respect to substitution reactions. Why?
They experience Jahn-Teller distortion, making their axial bonds longer and easier to break.
Their ground state structure resembles their transition state structure.
Their electrons are distributed equally among the d-orbitals.
Their large radii can accommodate a larger coordination sphere.
They experience Jahn-Teller distortion, making their axial bonds longer and easier to break and their ground state structure resembles their transition state structure.
In D or Id mechanisms for substitution in octahedral metal complexes, stereochemistry is retained when the intermediate’s molecular geometry is which of the following?
Tetragonal
Trigonal bipyramidal
Square pyramidal
Both Tetragonal and Square pyramidal
All of the choices
The effect of a coordinated ligand upon the rate of substitution of ligands opposite it is referred to as which of the following?
The trans influence
The trans effect
The biphilic effect
The solvolysis effect
The anation effect
What is responsible for the increased stability of formation of a complex containing two chelating ligands as compared to four monodentate ligands?
Enthalpy of reaction
Decreased activation energy
Formation of dimeric species (bridging ligands)
Entropy of reaction
Outer sphere electron transfer
When hexaaqua complexes of cobalt react with chloride ion, they undergo a change in the coordination chemistry. Why is this NOT the case when they react with ammonia?
The chloride ions are larger than the water molecules, only allowing four to coordinate around the central metal ion; ammonia is similar in size to water, so six will coordinate.
The chloride ions are anionic, and the metal centers cannot accommodate a larger negative charge; ammonia is a neutral species.
Chloride ions precipitate the metals out of solution; ammonia complexes do not.
The addition of excess chloride ions will actually result in hexa-chloro compounds.
Chloride additions occur in acidic media; ammonia is alkaline.
Which of the following affects substitution at square planar metal centers?
The entering group
The leaving group
Other ligands in the coordination sphere
The metal center itself
All of the choices
Which of the following is about the trans influence is FALSE?
It is a kinetic phenomenon.
It can influence M-L bond lengths.
It can result in changes in NMR coupling constants.
It can affect the vibrational frequency.
It is purely thermodynamic.
Which of the following is true of substitutions at square planar metal centers?
They occur via an associative mechanism with a five coordinate intermediate.
They only proceed when bond formation is the rate determining step.
They only proceed when bond breaking is the rate determining step.
They only proceed when the transition energies of bond formation and bond breaking are similar.
They occur via a dissociative mechanism with a three coordinate intermediate.
Which of the following rate laws indicates a dissociative mechanism?
k = [A][B]
k = [A]
k = [A]2[B]
Both k = [A][B] and k = [A]2[B]
The mechanism cannot be determined from the rate law.
Fill in the blank to complete the following analogy. Thermodynamics : free energy :: kinetics : ________________.
Activation energy
Thermal energy
Electron transfer
Entropy
Enthalpy
Fill in the blank. The Haber process is used for the production of _______________.
Ammonia
Sulfur trioxide
Sulfuric acid
Margarine
Nitric acid
What is the end product of the Contact Process?
Ammonia
Sulfur trioxide
Sulfuric acid
Margarine
Nitric acid
What is the role of a catalyst in a reaction?
It shifts the equilibrium toward the products based on LeChatlier’s principle.
It provides an alternate route with a lower activation energy for the reaction to proceed.
It donates electrons to break or form bonds as needed until it is entirely consumed.
It forms bridging complexes which align the molecular orbitals of the reactants.
All of the choices
Which of the following is an example of a homogeneous catalysis?
The hydrogenation of vegetable oil in the presence of nickel to make margarine
The use of Pt, Pd or Rh in catalytic converters
The destruction of ozone in the atmosphere
The use of vanadium(V)oxide in the conversion of sulfur dioxide to sulfur trioxide
All of the choices
The anticancer drug cisplatin is a platinum based complex, which works by destroying the DNA within cancer cells. Which of the following transition metals have anticancer applications?
Ru
Ti
V
Fe
All of the choices
What advantage does doping an LED with a transition metal have?
Doping allows the LED to harvest light from triplet states, increasing quantum efficiency.
Doping increases the overall number of singlet to singlet emission pathways.
It reduces the overall cost of producing an LED; the inorganic dopants are inexpensive.
All of the choices
None of the choices
Which of the following describes a challenge in the production of effective metal-based dye-sensitized solar cell?
Metal ion complexes are unable to harvest light energy.
The cost of the metal ion complexes is prohibitive.
The storage of energy occurs by thermal or chemical means.
The energy produced can only be utilized in electrical grids.
All of the choices
Which of the following is NOT an application of a secondary cell battery?
Nickel-cadmium in portable electronics and toys
Lead acid batteries in automobiles
Silver-zinc button cells in hearing aides
Silver-cadmium batteries in satellites
Zinc-carbon dry cell batteries in flashlights
Why are organometallic vanadium complexes being used to treat diabetes instead of the inorganic vanadium salts?
The organometallic complexes are easier to synthesize than the inorganic salts.
The organometallic complexes are less toxic and more effective in lowering blood glucose levels.
The organometallic complexes are less expensive to synthesize and cost less on the market.
The effect of the inorganic salts was discovered after the organometallic complexes had established a successful history.
The FDA will not approve medicinal use of purely inorganic compounds for biological applications.
Which of the following is true of organometallic pharmaceuticals as antimicrobials?
Metals are nontoxic to humans.
Harmful stereoisomers do not exist.
They are soluble in water and easily administered.
They counteract drug resistance that has been built to purely organic molecules.
There are no current organometallic applications to antimicrobials.
