a. A mirror plane combined with an inversion ![]() |
||
b. Two proper rotation axes combined ![]() |
||
c. Identity combined with a mirror plane ![]() |
||
d. A proper rotation axis combined with a mirror plane ![]() |
||
e. The combination of two mirror planes ![]() |
a. Polarizability, dipole moment ![]() |
||
b. Magnetism, dipole moment ![]() |
||
c. Symmetry, magnetism ![]() |
||
d. Dipole moment, polarizability ![]() |
||
e. Magnetism, symmetry ![]() |
a. E ![]() |
||
b. C5 ![]() |
||
c. i ![]() |
||
d. S10 ![]() |
||
e. C6 ![]() |
a. IR active only ![]() |
||
b. Raman active only ![]() |
||
c. Both IR and Raman active ![]() |
||
d. Neither IR or Raman active ![]() |
||
e. The only spectroscopically active mode in the molecule ![]() |
a. IR active only ![]() |
||
b. Raman active only ![]() |
||
c. Both IR and Raman active ![]() |
||
d. Neither IR or Raman active ![]() |
||
e. The only spectroscopically active mode in the molecule ![]() |
a. Both the electronic and vibrational representations must be symmetric. ![]() |
||
b. Both the electronic and vibrational representations must be asymmetric. ![]() |
||
c. Only the electronic representations must be symmetric. ![]() |
||
d. Only the vibrational representations must be symmetric. ![]() |
||
e. Symmetry does not matter, as long as there is a change in dipole or polarizability. ![]() |
a. Closure (If A and B belong to the group, and A x B = C, then C also belongs to the group.) ![]() |
||
b. Associativity (A(BC) = (AB)C ) ![]() |
||
c. Identity (The symmetry element times its identity, E, remains unchanged.) ![]() |
||
d. Inverses (There must be an inverse symmetry element that returns the molecule to its original state; A x A-1 = E.) ![]() |
||
e. Continuity (If a molecule contains an n axis, then it also contains axes of n-1, n-2...) ![]() |
a. D2d ![]() |
||
b. Cs ![]() |
||
c. C2h ![]() |
||
d. S4 ![]() |
||
e. D4 ![]() |
a. H2O ![]() |
||
b. BrF5 ![]() |
||
c. BH3 ![]() |
||
d. PCl6 ![]() |
||
e. W(CO)6 ![]() |
a. SF6 ![]() |
||
b. O2 ![]() |
||
c. BF3 ![]() |
||
d. C2Cl4 ![]() |
||
e. All of the above ![]() |
a. Helium also has electrons in antibonding orbitals, resulting in a bond order of zero. ![]() |
||
b. Helium also has electrons in non-bonding orbitals, resulting in a bond order of zero. ![]() |
||
c. Helium is a noble gas and never forms bonds. ![]() |
||
d. Hydrogen also has electrons in nonbonding orbitals, resulting in a bond order of two. ![]() |
||
e. Hydrogen has no antibonding orbitals, resulting in a bond order of two. ![]() |
a. The amount of magnetic character is reduced in bonds. ![]() |
||
b. The electrons are shared between two elements. ![]() |
||
c. Nonbonding electrons decrease bond ability. ![]() |
||
d. The antibonding electrons interfere with bonding. ![]() |
||
e. None of the above ![]() |
a. 5 ![]() |
||
b. 1 ![]() |
||
c. 1.5 ![]() |
||
d. 2 ![]() |
||
e. 3 ![]() |
a. They should be at the same energy to indicate bond formation. ![]() |
||
b. They should be at the same energy to indicate allowed symmetry. ![]() |
||
c. They should be at different energies, relative to their difference in electronegativities. ![]() |
||
d. They should be at different energies, relative to their atomic radii. ![]() |
||
e. They should be at different energies, relative to the number of lone pairs of electrons. ![]() |
a. A maximum of two electrons per orbital is allowed. ![]() |
||
b. The orbitals with the lowest energy are filled first. ![]() |
||
c. Orbitals of the same energies are half-filled first; then electrons are allowed to pair up. ![]() |
||
d. Non-bonding orbitals are filled first. ![]() |
||
e. All of the above ![]() |
a. Nonbonding molecular orbitals ![]() |
||
b. Antibonding molecular orbitals ![]() |
||
c. Bonding molecular orbitals ![]() |
||
d. All of the above ![]() |
||
e. A and C only ![]() |
a. They must have constructive net interaction. ![]() |
||
b. They must have the correct symmetry to overlap ![]() |
||
c. They must be similar in energy ![]() |
||
d. There will be the same number of resultant molecular orbitals as atomic orbitals ![]() |
||
e. All of the above ![]() |
a. Sigma interactions occur along the internuclear axis. ![]() |
||
b. Pi interactions occur above and below the internuclear axis. ![]() |
||
c. Sigma bonds form first, followed by the subsequent formation of pi bonds. ![]() |
||
d. Two pi bonds are involved in a double bond. ![]() |
||
e. All of the above ![]() |
a. They are responsible for the formation of pi bonds. ![]() |
||
b. They are similar in energy to the atomic orbitals. ![]() |
||
c. They counteract bond formation in a molecule. ![]() |
||
d. They help hold the molecule together, once it is formed. ![]() |
||
e. They are responsible for the formation of sigma bonds. ![]() |
a. CO2 ![]() |
||
b. H2O ![]() |
||
c. CN- ![]() |
||
d. Cl2 ![]() |
||
e. N2 ![]() |
a. Mn2+ ![]() |
||
b. V ![]() |
||
c. Fe3+ ![]() |
||
d. All of the above ![]() |
||
e. A and C only ![]() |
a. An EPR spectrum shows that oxygen is paramagnetic; MO theory is correct. ![]() |
||
b. An EPR spectrum shows that oxygen is paramagnetic; VBT is correct. ![]() |
||
c. Infrared spectroscopy shows a double bond stretch; MO theory is correct. ![]() |
||
d. Infrared spectroscopy shows a double bond stretch; VBT is correct. ![]() |
||
e. There is no way to know which theory is correct in this matter. ![]() |
a. There is no actual difference; the orbitals involved are the same, only listed in a different order. ![]() |
||
b. The complex having d2sp3 hybridization is an “inner shell” complex, while the complex with sp3d2 hybridization is an “outer shell” complex. ![]() |
||
c. The complex having d2sp3 hybridization is an “outer shell” complex, while the complex with sp3d2 hybridization is an “inner shell” complex. ![]() |
||
d. The complex having sp3d2 hybridization does not exist; the electrons must fill the lowest energy orbitals first. ![]() |
||
e. The complex having d2sp3d2 hybridization does not exist; the electrons must fill the orbitals with the same principle quantum number. ![]() |
a. Octahedral ![]() |
||
b. Tetrahedral ![]() |
||
c. Square planar ![]() |
||
d. All of the above ![]() |
||
e. Both A and C ![]() |
a. They increase their ionization potential, rendering them most useful electrochemically. ![]() |
||
b. They reduce degenerate molecular orbitals, allowing a more stable molecule to exist. ![]() |
||
c. They undergo a strong magnetic transition, allowing easier detection by NMR and EPR. ![]() |
||
d. They increase their transition state energy, making them useful catalysts. ![]() |
||
e. They decrease shielding, allowing spectroscopically forbidden transitions to occur. ![]() |
a. Yes. The five electrons distribute themselves evenly in the five molecular orbitals, causing them to be degenerate. Axial elongation reduces this degeneracy. ![]() |
||
b. Yes. The five electrons distribute themselves evenly in the five molecular orbitals, causing them to be degenerate. Axial compression reduces this degeneracy. ![]() |
||
c. No. The five electrons distribute themselves evenly in the five molecular orbitals; no degeneracy exists. ![]() |
||
d. No. Four of the electrons are paired. Only one electron is unpaired and can only fill the one remaining orbital. No degeneracy exists. ![]() |
||
e. 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. ![]() |
a. mer-bis(cyclopentadienyl)iron(II) ![]() |
||
b. fac-bis(cyclopentadienyl)iron(II) ![]() |
||
c. bis(η5-cyclopentadienyl)iron(II) ![]() |
||
d. µ-bis(cyclopentadienyl)iron(II) ![]() |
||
e. (η5-cyclopentadienyl)iron(II) ![]() |
a. One would be a solid at room temperature, while the other would be a liquid. ![]() |
||
b. One would be highly colored, while the other would be colorless. ![]() |
||
c. One would be paramagnetic, while the other would be diamagnetic. ![]() |
||
d. One would rotate plane-polarized light clockwise, while the other would rotate it counterclockwise. ![]() |
||
e. All of the above ![]() |
a. 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 ![]() |
||
b. Because the 3d orbital is actually lower in energy than the 4s, so it fills first ![]() |
||
c. Because copper and chromium only exist as ions; never as neutral elements ![]() |
||
d. Because the atomic radii are so large that no effect is felt by the nucleus ![]() |
||
e. None of the above ![]() |
a. mu (µ) ![]() |
||
b. eta (η) ![]() |
||
c. chi (χ) ![]() |
||
d. xi (ξ) ![]() |
||
e. zeta (ζ) ![]() |
a. They are malleable and ductile. ![]() |
||
b. They have high melting points. ![]() |
||
c. They conduct heat and electricity. ![]() |
||
d. They are lustrous. ![]() |
||
e. They undergo irreversible oxidation. ![]() |
a. A low spin, d5 octahedral complex ![]() |
||
b. A high spin, d8 octahedral complex ![]() |
||
c. A low spin, d3 octahedral complex ![]() |
||
d. A d2 tetrahedral complex ![]() |
||
e. A d5 square planar complex ![]() |
a. Fe(CO)5 ![]() |
||
b. Ni(CO)5 ![]() |
||
c. Mo(CO)6 ![]() |
||
d. Re(CO)6 ![]() |
||
e. Ir(CO)5 ![]() |
a. The result is a low-spin complex, where electrons will pair up and fill the lowest energy level. ![]() |
||
b. The result is a high-spin complex, where electrons will be promoted to the next energy level before pairing. ![]() |
||
c. The result is an unstable complex, where electrons can either pair or be promoted to the next energy level. ![]() |
||
d. The result is a high-spin complex, where electrons will pair up and fill the lowest energy level. ![]() |
||
e. The result is a low-spin complex, where electrons will be promoted to the next energy level before pairing. ![]() |
a. BF3 ![]() |
||
b. ClF3 ![]() |
||
c. PF6 ![]() |
||
d. IF5 ![]() |
||
e. SbF5 ![]() |
a. Charge of the metal ion ![]() |
||
b. Nature of the ligands ![]() |
||
c. Geometry of the complex ![]() |
||
d. Size of the ligands ![]() |
||
e. All of the above ![]() |
a. [PtCl(H2O)3]Br and [Pt(Br)(H2O)3]Cl ![]() |
||
b. cis-[PtCl2(NH3)2] and trans-[PtCl2(NH3)2] ![]() |
||
c. [CrCl2(H2O)4]Cl•2H2O and [CrCl3(H2O)3]•3H2O ![]() |
||
d. [Co(NH3)6] [Cr(ac)3] and [Co(ac)3] [Cr(NH3)6] ![]() |
||
e. [Co(SCN)(NH3)5]- and [Co(NCS)(NH3)5]- ![]() |
a. Copper ![]() |
||
b. Iron ![]() |
||
c. Gold ![]() |
||
d. Titanium ![]() |
||
e. Tungsten ![]() |
a. It is highly polarizable. ![]() |
||
b. The ligand is relatively large. ![]() |
||
c. The ligand exhibits π donor ability. ![]() |
||
d. The ligand is acidic. ![]() |
||
e. All of the above ![]() |
a. Silver ![]() |
||
b. Rhodium ![]() |
||
c. Cadmium ![]() |
||
d. Molybdenum ![]() |
||
e. The melting points would be equivalent, because they are in the same period. ![]() |
a. Violet ![]() |
||
b. Blue ![]() |
||
c. Green ![]() |
||
d. Yellow ![]() |
||
e. Red ![]() |
a. Jahn-Teller distortion ![]() |
||
b. Mixing of the p and d orbitals ![]() |
||
c. MLCT ![]() |
||
d. LMCT ![]() |
||
e. All of the above ![]() |
a. The spectrum would show one very broad absorption band at 533 nm. ![]() |
||
b. The spectrum would show two weak absorption bands, one at 412 nm and the other at 654 nm. ![]() |
||
c. The spectrum would show two strong absorption bands, one at 412 nm and the other at 654 nm. ![]() |
||
d. The spectrum would show two weak absorption bands, one at 472 nm and the other at 594 nm. ![]() |
||
e. The spectrum would show two strong absorption bands, one at 472 nm and the other at 594 nm. ![]() |
a. The ligand field stabilization energy (LFSE) is insufficient to allow transitions to the left of the line. ![]() |
||
b. The transitions to the left are symmetry allowed, while the transitions to the right are spin allowed. ![]() |
||
c. The transitions to the left are spin allowed, while the transitions to the right are symmetry allowed. ![]() |
||
d. The transitions to the left are low-spin complexes, while the transitions to the right are high-spin complexes. ![]() |
||
e. The transitions to the left are high-spin complexes, while the transitions to the right are low-spin complexes. ![]() |
a. Two ![]() |
||
b. Three ![]() |
||
c. Nine ![]() |
||
d. Six ![]() |
||
e. Zero ![]() |
a. CT absorptions occur at higher wavelengths than d-d transitions. ![]() |
||
b. CT absorptions are less intense than d-d transitions. ![]() |
||
c. CT transitions are symmetry and spin allowed; d-d transitions are symmetry forbidden. ![]() |
||
d. CT transitions are spin allowed; d-d transitions are spin forbidden. ![]() |
||
e. CT transitions are symmetry and spin forbidden; d-d transitions are symmetry forbidden but spin allowed. ![]() |
a. Zn2+ has a completely filled d orbital, and Sc3+ has a completely empty d orbital. ![]() |
||
b. Zn2+ and Sc3+ always form high spin octahedral complexes. ![]() |
||
c. Zn2+ and Sc3+ always form low spin octahedral complexes. ![]() |
||
d. Zn2+ and Sc3+ are diamagnetic; the others are paramagnetic. ![]() |
||
e. Zn2+ and Sc3+ are paramagnetic; the others are diamagnetic. ![]() |
a. The transition in the high spin complex is symmetry and spin forbidden. The transition in the low spin complex is symmetry allowed. ![]() |
||
b. The transition in the high spin complex is symmetry and spin forbidden. The transition in the low spin complex is spin allowed. ![]() |
||
c. 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. ![]() |
||
d. 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. ![]() |
||
e. The transition in the high spin complex is symmetry and spin forbidden. The transition in the low spin complex is symmetry and spin allowed. ![]() |
a. 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. ![]() |
||
b. 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. ![]() |
||
c. 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. ![]() |
||
d. The solutions will both be similar in color; however, the complex with thiocyanate will be more intense. ![]() |
||
e. You cannot tell them apart; the experiment would need to be restarted. ![]() |
a. Dynamic fluxionality ![]() |
||
b. Spin-spin coupling interactions ![]() |
||
c. Integer quantum spin numbers (I = 1,2,3…) ![]() |
||
d. Fractional quantum spin numbers (I = 1/2, 3/2, 5/2) ![]() |
||
e. Low natural abundances of the 19F nucleus ![]() |
a. The asymmetric stretch of the C-O bonds creates a dipole moment that is IR active. ![]() |
||
b. The symmetric stretch of the C-O bonds creates a dipole moment that is IR active. ![]() |
||
c. The non-linear bending mode crates a net dipole, which is IR active. ![]() |
||
d. All of the above ![]() |
||
e. A and C only ![]() |
a. The chemical shift and resonance frequency also change. ![]() |
||
b. The chemical shift changes; the resonance frequency remains constant. ![]() |
||
c. The chemical shift remains constant; the resonance frequency changes. ![]() |
||
d. The chemical shift and resonance frequency remain constant. ![]() |
||
e. There is no way to predict the effect. ![]() |
a. The Zeeman effect ![]() |
||
b. Pauli exclusion principle ![]() |
||
c. Symmetry degeneracy ![]() |
||
d. Fermi contact interaction ![]() |
||
e. Bose-Einstein effect ![]() |
a. Dissociation and recoordination of the carbonyl ligands ![]() |
||
b. Rotation of a hindered carbonyl bond ![]() |
||
c. Opening and closing of bridging carbonyls ![]() |
||
d. Isomerism between trigonal bipyramidal and square pyramidal configurations ![]() |
||
e. Monmer-dimer formation with a bridging carbonyl ![]() |
a. NO2 radical ![]() |
||
b. CH3 radical ![]() |
||
c. CH2Cl radical ![]() |
||
d. CH2CH2 radical ![]() |
||
e. OH radical ![]() |
a. Paramagnetic transition metal complexes ![]() |
||
b. Diamagnetic transition metal complexes ![]() |
||
c. Free radicals in the solid state ![]() |
||
d. Free radicals in the liquid or gas state ![]() |
||
e. Complexes containing more than one unpaired electron ![]() |
a. An odd mass number and odd atomic number, such as 1H ![]() |
||
b. An odd mass number and an even atomic number, such as 13C ![]() |
||
c. An even mass number and an even atomic number, such as 16O ![]() |
||
d. An even mass number and an odd atomic number, such as 14N ![]() |
||
e. All of the above situations will result in a nonzero quantum spin number. ![]() |
a. A free electron ![]() |
||
b. An unpaired electron in an organic molecule ![]() |
||
c. An unpaired electron in a transition metal complex ![]() |
||
d. All of the above ![]() |
||
e. A and B only ![]() |
a. Cationic metal complexes experience less π backbonding than their neutral or anionic analogs. ![]() |
||
b. Pyridine is a good π acceptor and contributes to increased π backbonding. ![]() |
||
c. The carbonyl to metal bond strength is increased in the chloro complex. ![]() |
||
d. All of the above ![]() |
||
e. A and B only ![]() |
a. Two; through the lone pairs on the two nitrogen atoms ![]() |
||
b. Two; through the lone pairs on two of the oxygen atoms ![]() |
||
c. Four; through the lone pairs on the four oxygen atoms ![]() |
||
d. Four; through the anion on the four oxygen atoms ![]() |
||
e. Six; two through the lone pairs on the two nitrogen atoms and four through the lone pairs of the four oxygen atoms ![]() |
a. Associative mechanism, aided by a ring slip ![]() |
||
b. Dissociative mechanism, in which the Cp ring is lost ![]() |
||
c. Inversion of stereochemistry and loss of the Cp ring ![]() |
||
d. Dissociation of the Cp ligand, followed by re-association of Cp ![]() |
||
e. All of the above ![]() |
a. It is dependent on which ligands are a part of the primary valence and which ones are a part of the secondary valence. ![]() |
||
b. It depends on the charge of the metal ion present. ![]() |
||
c. It depends on the number of empty d orbitals. ![]() |
||
d. It depends on the nature of the ligands involved and whether they are mono or multi-dentate. ![]() |
||
e. All of the above ![]() |
a. 2 ![]() |
||
b. 5 ![]() |
||
c. 6 ![]() |
||
d. 8 ![]() |
||
e. 10 ![]() |
a. 2 ![]() |
||
b. 3 ![]() |
||
c. 4 ![]() |
||
d. 5 ![]() |
||
e. 6 ![]() |
a. +3 ![]() |
||
b. +2 ![]() |
||
c. +4 ![]() |
||
d. +7 ![]() |
||
e. +6 ![]() |
a. It plays an important role in insertion, polymerization, and metathesis reactions. ![]() |
||
b. It describes a complex with a coordination number less than 4. ![]() |
||
c. It generally means another ligand can be accommodated. ![]() |
||
d. All of the above ![]() |
||
e. A and C only ![]() |
a. [Co(Cl3)](NH3)6; AgCl is formed. ![]() |
||
b. [Co(Cl3)](NH3)6; NH4Cl is formed. ![]() |
||
c. [Co(NH3)6]Cl3; AgCl is formed. ![]() |
||
d. [Co(NH3)6]Cl3; NH4Cl is formed. ![]() |
||
e. Both will react with silver in water; AgCl and NH4Cl are formed. ![]() |
a. EDTA ![]() |
||
b. SCN- ![]() |
||
c. NH3 ![]() |
||
d. Hemoglobin ![]() |
||
e. Cl- ![]() |
a. Hydrophilic interactions ![]() |
||
b. Hydrophobic interactions ![]() |
||
c. Van der Waals interactions ![]() |
||
d. Lewis acid-base interactions ![]() |
||
e. Hydrogen bonding interactions ![]() |
a. Fe(s) ![]() |
||
b. Fe3+(aq) ![]() |
||
c. Fe(OH)2(s) ![]() |
||
d. Fe2+(aq) ![]() |
||
e. Fe(OH)3(s) ![]() |
a. The species on the left is readily reduced to the species on the right side of the arrow. ![]() |
||
b. The species on the lef tis a good reducing agent. ![]() |
||
c. The species under goes diproportionation. ![]() |
||
d. All of the above. ![]() |
||
e. None of the above. ![]() |
a. The heat of formation of the precursor complex ![]() |
||
b. The heat of fission of the successor complex ![]() |
||
c. The solvation energy of the transition complex ![]() |
||
d. The free energy of electron transfer ![]() |
||
e. All of the above ![]() |
a. The reaction does not proceed. ![]() |
||
b. The reaction is drastically slowed, requiring a spin flip to occur. ![]() |
||
c. The reaction proceeds quicker, because different spin states allow faster electron transfer. ![]() |
||
d. The reaction will proceed as inner sphere instead, because electrons with different spin will pair and form a bond. ![]() |
||
e. None of the above ![]() |
a. Even though a reaction is thermodynamically favorable, the reaction may be slow kinetically. ![]() |
||
b. All redox reactions are favorable at in alkaline media. ![]() |
||
c. All thermodynamically favorable reactions occur quickly on a kinetic scale. ![]() |
||
d. If a reaction is kinetically favorable, it will proceed even if it is thermodynamically unfavorable. ![]() |
||
e. No redox reactions occur in highly acidic media. ![]() |
a. Formation of the bridging ligand complex ![]() |
||
b. Formation of the precursor (cage) complex ![]() |
||
c. Electron transfer ![]() |
||
d. Solvent entering the coordination sphere ![]() |
||
e. Fission of the successor ligand complex ![]() |
a. Formation of the bridging ligand complex ![]() |
||
b. Fission of the successor ligand complex ![]() |
||
c. Electron transfer ![]() |
||
d. Solvent entering the coordination sphere ![]() |
||
e. Both B and C ![]() |
a. H3PO4 ![]() |
||
b. NH4+ ![]() |
||
c. HNO3 ![]() |
||
d. PH3 ![]() |
||
e. P & N (elemental) ![]() |
a. They experience Jahn-Teller distortion, making their axial bonds longer and easier to break. ![]() |
||
b. Their ground state structure resembles their transition state structure. ![]() |
||
c. Their electrons are distributed equally among the d-orbitals. ![]() |
||
d. Their large radii can accommodate a larger coordination sphere. ![]() |
||
e. Both A and B ![]() |
a. Tetragonal ![]() |
||
b. Trigonal bipyramidal ![]() |
||
c. Square pyramidal ![]() |
||
d. Both A and C ![]() |
||
e. All of the above ![]() |
a. The trans influence ![]() |
||
b. The trans effect ![]() |
||
c. The biphilic effect ![]() |
||
d. The solvolysis effect ![]() |
||
e. The anation effect ![]() |
a. Enthalpy of reaction ![]() |
||
b. Decreased activation energy ![]() |
||
c. Formation of dimeric species (bridging ligands) ![]() |
||
d. Entropy of reaction ![]() |
||
e. Outer sphere electron transfer ![]() |
a. 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. ![]() |
||
b. The chloride ions are anionic, and the metal centers cannot accommodate a larger negative charge; ammonia is a neutral species. ![]() |
||
c. Chloride ions precipitate the metals out of solution; ammonia complexes do not. ![]() |
||
d. The addition of excess chloride ions will actually result in hexa-chloro compounds. ![]() |
||
e. Chloride additions occur in acidic media; ammonia is alkaline. ![]() |
a. The entering group ![]() |
||
b. The leaving group ![]() |
||
c. Other ligands in the coordination sphere ![]() |
||
d. The metal center itself ![]() |
||
e. All of the above ![]() |
a. It is a kinetic phenomenon. ![]() |
||
b. It can influence M-L bond lengths. ![]() |
||
c. It can result in changes in NMR coupling constants. ![]() |
||
d. It can affect the vibrational frequency. ![]() |
||
e. It is purely thermodynamic. ![]() |
a. They occur via an associative mechanism with a five coordinate intermediate. ![]() |
||
b. They only proceed when bond formation is the rate determining step. ![]() |
||
c. They only proceed when bond breaking is the rate determining step. ![]() |
||
d. They only proceed when the transition energies of bond formation and bond breaking are similar. ![]() |
||
e. They occur via a dissociative mechanism with a three coordinate intermediate. ![]() |
a. k = [A][B] ![]() |
||
b. k = [A] ![]() |
||
c. k = [A]2[B] ![]() |
||
d. Both A and C ![]() |
||
e. The mechanism cannot be determined from the rate law. ![]() |
a. Activation energy ![]() |
||
b. Thermal energy ![]() |
||
c. Electron transfer ![]() |
||
d. Entropy ![]() |
||
e. Enthalpy ![]() |
a. Ammonia ![]() |
||
b. Sulfur trioxide ![]() |
||
c. Sulfuric acid ![]() |
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d. Margarine ![]() |
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e. Nitric acid ![]() |
a. Ammonia ![]() |
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b. Sulfur trioxide ![]() |
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c. Sulfuric acid ![]() |
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d. Margarine ![]() |
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e. Nitric acid ![]() |
a. It shifts the equilibrium toward the products based on LeChatlier’s principle. ![]() |
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b. It provides an alternate route with a lower activation energy for the reaction to proceed. ![]() |
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c. It donates electrons to break or form bonds as needed until it is entirely consumed. ![]() |
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d. It forms bridging complexes which align the molecular orbitals of the reactants. ![]() |
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e. All of the above ![]() |
a. The hydrogenation of vegetable oil in the presence of nickel to make margarine ![]() |
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b. The use of Pt, Pd or Rh in catalytic converters ![]() |
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c. The destruction of ozone in the atmosphere ![]() |
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d. The use of vanadium(V)oxide in the conversion of sulfur dioxide to sulfur trioxide ![]() |
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e. All of the above ![]() |
a. Ru ![]() |
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b. Ti ![]() |
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c. V ![]() |
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d. Fe ![]() |
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e. All of the above ![]() |
a. Doping allows the LED to harvest light from triplet states, increasing quantum efficiency. ![]() |
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b. Doping increases the overall number of singlet to singlet emission pathways. ![]() |
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c. It reduces the overall cost of producing an LED; the inorganic dopants are inexpensive. ![]() |
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d. All of the above ![]() |
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e. None of the above ![]() |
a. Metal ion complexes are unable to harvest light energy. ![]() |
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b. The cost of the metal ion complexes is prohibitive. ![]() |
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c. The storage of energy occurs by thermal or chemical means. ![]() |
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d. The energy produced can only be utilized in electrical grids. ![]() |
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e. All of the above ![]() |
a. Nickel-cadmium in portable electronics and toys ![]() |
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b. Lead acid batteries in automobiles ![]() |
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c. Silver-zinc button cells in hearing aides ![]() |
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d. Silver-cadmium batteries in satellites ![]() |
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e. Zinc-carbon dry cell batteries in flashlights ![]() |
a. The organometallic complexes are easier to synthesize than the inorganic salts. ![]() |
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b. The organometallic complexes are less toxic and more effective in lowering blood glucose levels. ![]() |
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c. The organometallic complexes are less expensive to synthesize and cost less on the market. ![]() |
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d. The effect of the inorganic salts was discovered after the organometallic complexes had established a successful history. ![]() |
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e. The FDA will not approve medicinal use of purely inorganic compounds for biological applications. ![]() |
a. Metals are nontoxic to humans. ![]() |
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b. Harmful stereoisomers do not exist. ![]() |
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c. They are soluble in water and easily administered. ![]() |
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d. They counteract drug resistance that has been built to purely organic molecules. ![]() |
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e. There are no current organometallic applications to antimicrobials. ![]() |