Match each characteristic property of transition metals on the left with its fundamental a… — JAMB UTME

Match each characteristic property of transition metals on the left with its fundamental atomic or electronic explanation on the right.

Formation of colored ionsExcitation of electrons between split $d$ -orbital energy levels by absorption of visible light
Variable oxidation statesSmall energy difference between the $(n-1)d$ and $ns$ subshells allowing electrons from both to participate in bonding
ParamagnetismPresence of one or more unpaired electrons in the $d$ -subshell
High catalytic efficiencyAbility to adopt multiple oxidation states and provide active surface sites using vacant $d$ -orbitals

Answer

Formation of colored ions matches excitation of electrons between split d-orbital energy levels; Variable oxidation states matches small energy difference between (n-1)d and ns subshells; Paramagnetism matches presence of unpaired d-electrons; High catalytic efficiency matches ability to adopt multiple oxidation states and provide active surface sites.

Transition elements owe their distinct properties to incompletely filled

d

-subshells. Colored compounds are created by

d

d

electron transitions when visible light is absorbed. Variable oxidation states arise because

3d

and

4s

energy levels are very close, so electrons from both subshells participate in reaction pathways. Paramagnetism originates from unpaired

d

-electrons, while catalytic behavior is driven by vacant/partially filled

d

-orbitals that adsorb reactants and facilitate intermediate oxidation states.

Step-by-Step Solution

Analyze the cause of color in transition metal complexes.

Ligands split the degenerate

d

-orbitals into different energy levels. Absorption of visible light promotes an electron (

d

d

transition), imparting color.

Relates the macroscopic color property to internal crystal field splitting.

Analyze why transition metals exhibit multiple oxidation states.

The energy gap between

(n-1)d

and

ns

subshells (such as

3d

and

4s

) is minimal, enabling electrons from both subshells to participate in bonding.

Explains why metals like Iron can exist as

Fe^{2+}

and

Fe^{3+}

Determine the electronic basis of paramagnetism.

Unpaired electrons possess a net magnetic spin moment, causing the ion or atom to be attracted into an external magnetic field.

Distinguishes paramagnetism (unpaired electrons) from diamagnetism (all paired electrons).

Examine how transition elements act as catalysts.

Partially filled

d

-orbitals adsorb reactants onto active sites, and variable oxidation states allow the metal to lower activation energy by forming intermediate species.

Connects surface adsorption and redox cycles to catalytic mechanism.

Key Concept

Electronic Configurations and Characteristic Properties of Transition Elements

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