Which trend is observed for atomic size as you move from left to right across a period on the Periodic Table?

Atomic size first increases, then decreases

Which trend is observed for atomic size as you move down a group on the Periodic Table?

Atomic size fluctuates randomly

How and why does the typical trend relate to transition metals across the period?

The trend is due to increasing nuclear charge, which causes a decrease in atomic radius and an increase in ionization energy.

The trend is due to decreasing nuclear charge, which causes an increase in atomic radius and a decrease in ionization energy.

The trend is due to increasing electron shielding, which causes a decrease in atomic radius and a decrease in ionization energy.

The trend is due to decreasing electron shielding, which causes an increase in atomic radius and an increase in ionization energy.

How and why does the typical trend relate to transition metals down the group?

The trend is due to increasing atomic number, which causes an increase in atomic radius and a decrease in ionization energy.

The trend is due to decreasing atomic number, which causes a decrease in atomic radius and an increase in ionization energy.

The trend is due to increasing electron shielding, which causes a decrease in atomic radius and an increase in ionization energy.

The trend is due to decreasing electron shielding, which causes an increase in atomic radius and a decrease in ionization energy.

Describe the lanthanide contraction:

The gradual decrease in the size of the lanthanide ions as the atomic number increases.

The gradual increase in the size of the lanthanide ions as the atomic number increases.

The sudden decrease in the size of the lanthanide ions as the atomic number decreases.

The sudden increase in the size of the lanthanide ions as the atomic number decreases.

Describe the trends for ionization energy across and down the Periodic Table for main group elements:

Ionization energy increases across a period and decreases down a group.

Ionization energy decreases across a period and increases down a group.

Ionization energy remains constant across a period and down a group.

Ionization energy decreases both across a period and down a group.

Describe how this trend correlates to the transition metals:

Transition metals show a slight increase in ionization energy across the period and a decrease down the group.

Transition metals show a sharp decrease in ionization energy across the period and an increase down the group.

Transition metals show no change in ionization energy across the period or down the group.

Transition metals show a sharp increase in ionization energy across the period and a decrease down the group.

Describe the trends for electronegativity across and down the Periodic Table for Main Group elements:

Electronegativity increases across a period and decreases down a group.

Electronegativity decreases across a period and increases down a group.

Electronegativity remains constant across a period and down a group.

Electronegativity decreases both across a period and down a group.

Which of the following best defines a complex ion?

A charged species consisting of a central metal atom bonded to one or more molecules or ions

A neutral molecule with no metal atoms

A simple ion with only one atom

A molecule with only nonmetal atoms

What is a ligand in the context of coordination compounds?

An ion or molecule that binds to a central metal atom to form a complex

Which statement best describes a coordination compound?

A compound containing a complex ion and counter ions

A compound made only of nonmetals

A compound that does not contain any ions

A compound that is always a gas at room temperature

What does the term "primary valence" refer to in coordination chemistry?

The oxidation state of the central metal atom in a complex

The number of ligands attached to the metal

The color of the coordination compound

The physical state of the compound

What is meant by "secondary valence" in coordination compounds?

The number of ligands directly attached to the central metal atom

The number of electrons in the outer shell

The melting point of the compound

What is the definition of a coordination number in coordination chemistry?

The number of ligands attached to the central metal ion in a complex

The number of atoms bonded to the central atom in a molecule

The number of electrons in the outer shell of an atom

The number of protons in the nucleus of an atom

Which of the following best describes a coordinate covalent bond?

A bond where both electrons in the shared pair come from the same atom

A bond formed by the sharing of two pairs of electrons between atoms

A bond formed by the transfer of electrons from one atom to another

A bond formed by the overlap of atomic orbitals

Which statement correctly describes a monodentate ligand?

A ligand that can form only one bond to a central metal ion

A ligand that can form two bonds to a central metal ion

A ligand that can form multiple bonds to several metal ions

A ligand that cannot form any bonds to a metal ion

What is a bidentate ligand?

A ligand that forms two bonds to a metal ion

A ligand that forms one bond to a metal ion

A ligand that forms three bonds to a metal ion

A ligand that forms no bonds to a metal ion

Which of the following best describes a polydentate ligand?

A ligand that can form multiple bonds to a single metal ion

A ligand that can form only one bond to a metal ion

A ligand that can form two bonds to a metal ion

A ligand that cannot bond to a metal ion

What is a chelate in coordination chemistry?

A complex in which a ligand forms a ring by bonding to a metal ion at two or more points

A compound with only one ligand

A compound with only ionic bonds

Which of the following is a chelating agent?

A ligand that forms a ring structure with a metal ion by bonding at multiple points

A ligand that forms only one bond to a metal ion

A ligand that cannot bond to a metal ion

A ligand that forms only ionic bonds

Describe one characteristic of coordination numbers in coordination compounds.

Coordination numbers determine the geometry of the complex

Coordination numbers are always equal to the number of protons in the metal ion

Coordination numbers are always less than 2

Coordination numbers are unrelated to the structure of the compound

Which of the following is the correct way to identify the cation and anion in the complex compound [Cr(H₂O)₅Cl]Cl₂?

[Cr(H₂O)₅Cl]²⁺ is the complex cation; Cl⁻ is the chloride anion.

[Cr(H₂O)₅Cl]⁻ is the complex anion; Cl₂ is the cation.

Cr²⁺ is the cation; [H₂O)₅Cl] is the anion.

Cl₂ is the cation; [Cr(H₂O)₅Cl] is the anion.

When naming the ligands in a coordination compound, what is the correct order?

List each ligand in alphabetical order.

List each ligand in order of increasing charge.

List each ligand in order of decreasing size.

List each ligand in order of color.

Which of the following is the correct way to name the complex ion [Cr(H₂O)₅Cl]²⁺?

Pentachlorohydroxochromium(III)

How is the complete name of the compound [Cr(H₂O)₅Cl]Cl₂ written?

Pentaquochlorochromium(III) chloride

Pentaquochlorochromium(II) chloride

Pentaquochlorochromate(III) chloride

Pentaquochlorochromium(III) dichloride

Which of the following is the correct name for K₃[Fe(CN)₆]?

Potassium hexacyanoferrate(III)

Potassium hexacyanochromate(III)

Potassium hexachloroferrate(III)

Why is Fe³⁺ called ferrate(III) in the name of the complex ion [Fe(CN)₆]³⁻?

Because the complex ion is anionic.

Because the complex ion is cationic.

Because Fe³⁺ is always called ferrate.

Because CN⁻ is present as a ligand.

Which of the following best describes the difference between structural isomers and stereoisomers?

Structural isomers have different connectivity of atoms; stereoisomers have the same connectivity but differ in spatial arrangement.

Structural isomers have the same connectivity but different spatial arrangement; stereoisomers have different connectivity.

Both have the same connectivity and spatial arrangement.

Structural isomers and stereoisomers are identical in all aspects.

What is structural isomerism?

Compounds with the same molecular formula but different connectivity of atoms.

Compounds with the same molecular formula but different spatial arrangement of atoms.

Compounds with different molecular formulas.

Compounds with the same structure but different physical states.

Which of the following is an example of a coordination isomer?

[Co(NH3)6][Cr(CN)6] and [Cr(NH3)6][Co(CN)6]

cis-2-butene and trans-2-butene

Describe coordination isomers and provide an example.

Isomers in which the composition of the complex ion varies between cation and anion; e.g., [Co(NH3)6][Cr(CN)6] and [Cr(NH3)6][Co(CN)6]

Isomers that differ in the connectivity of atoms within the ligand; e.g., [Pt(NH3)2Cl2]

Isomers that differ in the arrangement of ligands around the central atom; e.g., [Fe(CN)6]4- and [Fe(CN)6]3-

Isomers that have the same formula but different physical states; e.g., H2O and ice

What is the main characteristic of geometric isomers?

They differ in the spatial arrangement of ligands around a central atom.

They have different molecular formulas.

They have different functional groups.

They have different numbers of atoms.

Which of the following best describes optical isomers?

Compounds that are non-superimposable mirror images of each other.

Compounds with the same connectivity but different arrangements of atoms.

Compounds with different molecular formulas.

Compounds with different numbers of ligands.

Why is it important to examine specific examples (such as Example 26.5 & 26.6) when studying isomerism?

To understand how theoretical concepts apply to real compounds.

To memorize the names of all isomers.

To ignore the differences between isomers.

To focus only on the chemical formulas.

What is a coordinate covalent bond?

A bond in which both electrons in the shared pair come from the same atom.

A bond formed by the equal sharing of electrons between two atoms.

A bond formed by the transfer of electrons from one atom to another.

A bond that only occurs between nonmetals.

How does coordinate covalent bonding relate to complex ions?

It allows ligands to donate electron pairs to a central metal ion, forming complex ions.

It causes the metal ion to lose electrons and become neutral.

It prevents the formation of any bonds between ligands and metal ions.

It only occurs in organic molecules, not in complex ions.

Which of the following is a possible geometry and respective hybridization for a complex ion?

Octahedral geometry with d2sp3 hybridization.

Linear geometry with sp3d2 hybridization.

Tetrahedral geometry with sp hybridization.

Trigonal planar geometry with sp3d hybridization.

Which of the following best describes crystal field splitting energy in octahedral complexes?

The energy difference between two sets of d orbitals in a metal ion when ligands approach

The energy required to break a crystal lattice

The energy released when a complex ion forms

The energy needed to ionize a metal atom

How do complex ion solutions display brilliant colors?

By absorbing specific wavelengths of visible light due to d-d electron transitions

By emitting light through radioactive decay

By reflecting all wavelengths of visible light equally

By undergoing rapid oxidation-reduction reactions

Ch 26: Transition Metals and Coordination Compounds

Authored by Barbara Will-Henn

Chemistry

University

NGSS covered

Ch 26: Transition Metals and Coordination Compounds

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Transition metals form which type of unique compounds?

Ionic compounds

Coordination compounds

Covalent compounds

Organic compounds

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which of the following is a manmade application of transition metal coordination compounds?

Photosynthesis in plants

Catalysts in industrial processes

Natural mineral formation

Water evaporation

Which theory is used to explain the color development in rubies and emeralds?

Molecular Orbital Theory

Crystal Field Theory

Valence Bond Theory

Band Theory

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Describe how rubies and emeralds obtain their colors spectrophotometrically. (Choose the best answer.)

By reflecting all wavelengths of light

By absorbing specific wavelengths due to transition metal ions

By emitting light through chemical reactions

By being painted with colored dyes

Which of the following best describes the role of transition metals in the color of gemstones?

They act as insulators

They provide structural support only

They cause absorption of certain wavelengths of light

They make the gemstones radioactive

Which of the following is a characteristic of d-block or transition metals?

They often form colored compounds.

They are always gases at room temperature.

They do not conduct electricity.

They are non-reactive with acids.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What chemical property allows transition metals to maintain similar properties to other main group metals?

Variable oxidation states

High melting points

Low density

Poor conductivity

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Ch 26: Transition Metals and Coordination Compounds

Transition metals form which type of unique compounds?

Which of the following is a manmade application of transition metal coordination compounds?

Which theory is used to explain the color development in rubies and emeralds?

Describe how rubies and emeralds obtain their colors spectrophotometrically. (Choose the best answer.)

Which of the following best describes the role of transition metals in the color of gemstones?

Which of the following is a characteristic of d-block or transition metals?

What chemical property allows transition metals to maintain similar properties to other main group metals?

Which of the following is the correct electron configuration for the element Scandium (element 21)?

Which trend is observed for atomic size as you move from left to right across a period on the Periodic Table?

Which trend is observed for atomic size as you move down a group on the Periodic Table?

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