Question 1

Which of the following statements concerning octahedral coordination complexes is not correct?

Accepted Answer

A)  Strong field ligands produce large octahedral ligand field splittings. 
B)  Weak field ligands produce high spin complexes. 
C)  Halide ions are strong field ligands. 
D)  Weak field ligands result in relatively small values for Δo. 
E)  A relatively large value for Δo causes a complex ion to absorb relatively high energy (shorter wavelength) light. 
A)  Strong field ligands produce large octahedral ligand field splittings. 
B)  Weak field ligands produce high spin complexes. 
C)  Halide ions are strong field ligands. 
D)  Weak field ligands result in relatively small values for Δo. 
E)  A relatively large value for Δo causes a complex ion to absorb relatively high energy (shorter wavelength) light.

Question 2

All of the following complexes will be colored (in the visible) EXCEPT ____.

Accepted Answer

A)  [Co(en)3]2+ 
B)  [Fe(CN)6]4- 
C)  [Ni(H2O)6]2+ 
D)  [Sc(NH3)6]3+ 
E)  [Cu(NH3)4]2+ 
A)  [Co(en)3]2+ 
B)  [Fe(CN)6]4- 
C)  [Ni(H2O)6]2+ 
D)  [Sc(NH3)6]3+ 
E)  [Cu(NH3)4]2+

Question 3

Most copper minerals are mined as ________.

Accepted Answer

A)  fluorides 
B)  sulfides 
C)  oxides 
D)  nitrates 
E)  silicates 
A)  fluorides 
B)  sulfides 
C)  oxides 
D)  nitrates 
E)  silicates

Question 4

What is the formula for the pentaamminehydroxochromium(III) ion?

Accepted Answer

A)  [Cr(NH3)5(OH)5]2+ 
B)  [Cr(NH3)5(OH)5]3- 
C)  [Cr(NH3)5(OH)]2+ 
D)  [Cr(NH3)5(OH)]+ 
E)  [Cr(NH3)(OH)5]3- 
A)  [Cr(NH3)5(OH)5]2+ 
B)  [Cr(NH3)5(OH)5]3- 
C)  [Cr(NH3)5(OH)]2+ 
D)  [Cr(NH3)5(OH)]+ 
E)  [Cr(NH3)(OH)5]3-

Question 5

Which of the following may act as an ambidentate ligand, forming coordination isomers known as linkage isomers?

Accepted Answer

A)  NH3 
B)  OH- 
C)  SO42- 
D)  CO 
E)  H2S 
A)  NH3 
B)  OH- 
C)  SO42- 
D)  CO 
E)  H2S

Question 6

Which of the following salts would not be expected to have unpaired d-electrons?

Accepted Answer

A)  NiCl2 
B)  CoCl2 
C)  MnCl2 
D)  TiCl3 
E)  ZnCl2 
A)  NiCl2 
B)  CoCl2 
C)  MnCl2 
D)  TiCl3 
E)  ZnCl2

Question 7

Determine the number of unpaired electrons in an octahedral, high-spin Cr(II) complex.

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 8

All of the following metals are found in nature as free elements except _____.

Accepted Answer

A)  iridium 
B)  gold 
C)  platinum 
D)  titanium 
E)  rhodium 
A)  iridium 
B)  gold 
C)  platinum 
D)  titanium 
E)  rhodium

Question 9

The chemical formula of _____ is K2[PtCl4].

Accepted Answer

A)  potassium chloroplatinate(II) 
B)  potassium tetrachloroplatinate(II) 
C)  potassium chloroplatinate(IV) 
D)  potassium platanotetrachlorate(II) 
E)  dipotassium tetrachloroplatnum(II) 
A)  potassium chloroplatinate(II) 
B)  potassium tetrachloroplatinate(II) 
C)  potassium chloroplatinate(IV) 
D)  potassium platanotetrachlorate(II) 
E)  dipotassium tetrachloroplatnum(II)

Question 10

Identify the orbital shown below.

Accepted Answer

A)  $d _ { x ^ { 2 } } \cdot y ^ { 2 }$ 
B)  $\mathrm { d } _ { \mathrm { z }^2 }$ 
C)  $\mathrm { d } _ { \mathrm { xy } }$ 
D)  $d _ { y z }$ 
E)  $\mathrm { d } _ { x z }$ 
A)  $d _ { x ^ { 2 } } \cdot y ^ { 2 }$ 
B)  $\mathrm { d } _ { \mathrm { z }^2 }$ 
C)  $\mathrm { d } _ { \mathrm { xy } }$ 
D)  $d _ { y z }$ 
E)  $\mathrm { d } _ { x z }$

Question 11

Which of the following pairs of d-block metals will have approximately the same atomic radii owing to the lanthanide contraction?

Accepted Answer

A)  Iron and ruthenium 
B)  Ruthenium and rhodium 
C)  Ruthenium and osmium 
D)  Osmium and iridium 
E)  Cobalt and nickel 
A)  Iron and ruthenium 
B)  Ruthenium and rhodium 
C)  Ruthenium and osmium 
D)  Osmium and iridium 
E)  Cobalt and nickel

Question 12

Which of the following is not a transition-metal?

Accepted Answer

A)  scandium 
B)  gold 
C)  vanadium 
D)  silver 
E)  magnesium 
A)  scandium 
B)  gold 
C)  vanadium 
D)  silver 
E)  magnesium

Question 13

Which of the following complex ions has an optical isomer?

Accepted Answer

A)  [Cu(CN)4]2- 
B)  [Zn(phen)2]2+ 
C)  [Zn(NH3)2en]2+ 
D)  [Co(H2O)4en]2+ 
E)  [Ni(en)3]2+ 
A)  [Cu(CN)4]2- 
B)  [Zn(phen)2]2+ 
C)  [Zn(NH3)2en]2+ 
D)  [Co(H2O)4en]2+ 
E)  [Ni(en)3]2+

Question 14

Which of the following will not as a ligand to a transition metal cation?

Accepted Answer

A)  H2 
B)  NH4+ 
C)  NH3 
D)  Cl− 
E)  F− 
A)  H2 
B)  NH4+ 
C)  NH3 
D)  Cl− 
E)  F−

Question 15

Ions such as [Co(H2O)6]3+ and [Ag(CN)2]- are called ____.

Accepted Answer

A)  ligands 
B)  Lewis bases 
C)  chelates 
D)  alloys 
E)  coordination complexes 
A)  ligands 
B)  Lewis bases 
C)  chelates 
D)  alloys 
E)  coordination complexes

Question 16

The period 6 transition metals have greater densities than either the period 4 or 5 transition metals. An explanation concerns the 4f orbitals, which are filled with electrons just prior to the 5d orbitals. As the 4f orbitals are filled, the radii of the elements decrease. The decrease in size is referred to as the ________ contraction.

Accepted Answer

The answer of The period 6 transition metals have greater...

Question 17

EDTA4-, a hexadentate ligand, is most effective at chelating metal ions when the pH is greater than 12. Explain why low pH decreases the chelating ability of the ligand.

Accepted Answer

At low pH, EDTA^4- is protonated (in succes

Question 18

Consider the ions Co2+, Mn2+, and Fe3+. Which among them has/have an [Ar]3d5 electron configuration?

Accepted Answer

A)  Co2+ only 
B)  Mn2+ only 
C)  Fe3+ only 
D)  Co2+ and Fe3+ 
E)  Mn2+ and Fe3+ 
A)  Co2+ only 
B)  Mn2+ only 
C)  Fe3+ only 
D)  Co2+ and Fe3+ 
E)  Mn2+ and Fe3+

Question 19

In an octahedral complex, electrons in $d _ { z^2 }$ and $d _ { x ^ { 2 } - y ^ { 2 } }$ orbitals experience a greater repulsion from the lone pairs of electrons on ligands because these orbitals

Accepted Answer

A)  contain more electrons than the other three d orbitals. 
B)  each contain one unpaired electron. 
C)  are oriented directly toward the incoming ligand electron pairs. 
D)  are located a greater distance from the metal ion nucleus. 
E)  are roughly spherical in shape, much like an s orbital. 
A)  contain more electrons than the other three d orbitals. 
B)  each contain one unpaired electron. 
C)  are oriented directly toward the incoming ligand electron pairs. 
D)  are located a greater distance from the metal ion nucleus. 
E)  are roughly spherical in shape, much like an s orbital.

Question 20

When 7.9 moles of [Co(NH3)5Cl]Cl2 is dissolved in water, how many moles of ions are in solution?

Accepted Answer

A)  71 
B)  24 
C)  4.9 
D)  2.6 
E)  5.9 
A)  71 
B)  24 
C)  4.9 
D)  2.6 
E)  5.9

Exam 23: The Chemistry of the Transition Elements

Which of the following statements concerning octahedral coordination complexes is not correct?

All of the following complexes will be colored (in the visible) EXCEPT ____.

Most copper minerals are mined as ________.

What is the formula for the pentaamminehydroxochromium(III) ion?

Which of the following may act as an ambidentate ligand, forming coordination isomers known as linkage isomers?

Which of the following salts would not be expected to have unpaired d-electrons?

Determine the number of unpaired electrons in an octahedral, high-spin Cr(II) complex.

All of the following metals are found in nature as free elements except _____.

The chemical formula of _____ is K2[PtCl4].

Identify the orbital shown below.

Which of the following pairs of d-block metals will have approximately the same atomic radii owing to the lanthanide contraction?

Which of the following is not a transition-metal?

Which of the following complex ions has an optical isomer?

Which of the following will not as a ligand to a transition metal cation?

Ions such as [Co(H2O)6]3+ and [Ag(CN)2]- are called ____.

EDTA4-, a hexadentate ligand, is most effective at chelating metal ions when the pH is greater than 12. Explain why low pH decreases the chelating ability of the ligand.

Consider the ions Co2+, Mn2+, and Fe3+. Which among them has/have an [Ar]3d5 electron configuration?

In an octahedral complex, electrons in dz2d _ { z^2 }dz2​ and dx2−y2d _ { x ^ { 2 } - y ^ { 2 } }dx2−y2​ orbitals experience a greater repulsion from the lone pairs of electrons on ligands because these orbitals

When 7.9 moles of [Co(NH3)5Cl]Cl2 is dissolved in water, how many moles of ions are in solution?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

The chemical formula of _____ is K₂[PtCl₄].

Ions such as [Co(H₂O)₆]³⁺ and [Ag(CN)₂]^- are called ____.

EDTA^4-, a hexadentate ligand, is most effective at chelating metal ions when the pH is greater than 12. Explain why low pH decreases the chelating ability of the ligand.

Consider the ions Co²⁺, Mn²⁺, and Fe³⁺. Which among them has/have an [Ar]3d⁵ electron configuration?

In an octahedral complex, electrons in $d _ { z^2 }$ and $d _ { x ^ { 2 } - y ^ { 2 } }$ orbitals experience a greater repulsion from the lone pairs of electrons on ligands because these orbitals

When 7.9 moles of [Co(NH₃)₅Cl]Cl₂ is dissolved in water, how many moles of ions are in solution?