Transition and Inner Transition Elements

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Questions and Answers

Which electronic configuration is generally associated with transition elements, accommodating exceptions like Palladium (Pd)?

  • $(n-1)d^{1-10}ns^{0-2}$ (correct)
  • $(n-1)s^{2}p^{6}$
  • $(n-1)d^{5}ns^{2}$
  • $(n-1)d^{1-5}ns^{1-2}$

Why are elements like Zinc (Zn), Cadmium (Cd), and Mercury (Hg) not considered transition metals despite being located in the d-block?

  • They are poor conductors of electricity.
  • They have completely filled _d_ orbitals in their common oxidation states. (correct)
  • They do not exhibit variable oxidation states.
  • They primarily form ionic compounds.

How does the enthalpy of atomization generally relate to the strength of interatomic interaction in transition metals?

  • Lower enthalpy of atomization indicates stronger interatomic interaction.
  • Enthalpy of atomization is unrelated to interatomic interaction.
  • Greater enthalpy of atomization indicates stronger interatomic interaction. (correct)
  • Enthalpy of atomization only affects boiling points.

What is the primary cause for the general decrease in ionic radii across a series of transition metal ions with the same charge?

<p>Poor shielding effect of d electrons and increasing effective nuclear charge. (B)</p>
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Which statement accurately describes the trend in standard electrode potentials ($E^\circ$) across the first transition series?

<p>There is a general trend towards less negative values, indicating a decreasing tendency to form divalent cations. (C)</p>
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Why do transition metals exhibit variable oxidation states?

<p>Due to the similar energies of the <em>ns</em> and $(n-1)d$ orbitals. (D)</p>
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In the context of transition metal chemistry, what is responsible for the color of many transition metal compounds?

<p>d-d transitions. (B)</p>
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What is a key factor contributing to the catalytic activity of transition metals and their compounds?

<p>Their ability to adopt multiple oxidation states and form complexes. (D)</p>
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Which of the following is a characteristic of interstitial compounds formed by transition metals?

<p>Metallic conductivity. (A)</p>
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What is the 'lanthanoid contraction,' and how does it affect the properties of elements in the periodic table?

<p>It is the cumulative decrease in atomic and ionic radii across the lanthanoid series, leading to similar properties in subsequent elements. (D)</p>
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Why is Cerium(IV) ($Ce^{4+}$) known as a good analytical reagent?

<p>It is a strong oxidizing agent with a slow reaction rate. (C)</p>
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What is a common use for lanthanoids?

<p>In the production of steel alloys. (C)</p>
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What accounts for the more complex chemistry observed in actinoids compared to lanthanoids?

<p>Actinoids have a wider range of oxidation states and are radioactive. (A)</p>
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What is a key difference in the behavior of electrons in actinoids versus lanthanoids?

<p>Actinoids' 5f electrons participate more readily in bonding. (A)</p>
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Which of the following describes how potassium dichromate ($K_2Cr_2O_7$) acts as an oxidizing agent in an acidic solution?

<p>It gains electrons to oxidize other substances. (C)</p>
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When acidified, potassium permanganate ($KMnO_4$) is reacted with hydrogen sulfide ($H_2S$). What is formed in this reaction?

<p>Sulfur (S) (B)</p>
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What property makes silver (Ag) a transition element, even though it has a completely filled d orbital ($4d^{10}$) in its ground state?

<p>Its ability to exhibit +2 oxidation state. (B)</p>
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Why is manganese capable of exhibiting the largest number of oxidation states among the 3d series?

<p>It has an electronic configuration that allows the most varying degrees of electron loss or sharing. (D)</p>
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Why are Mo(VI) and W(VI) more stable than Cr(VI)?

<p>The greater ease of d-orbital participation in bonding. (B)</p>
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Why exhibit copper a positive $E^\circ$?

<p>High 1st and 2nd ionization enthalpy and low hydration enthalpy. (B)</p>
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What is the main condition for alloys to form?

<p>Alloys are formed by metal atoms that have metallic radii that are within about 15 % of each other. (D)</p>
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What special property leads to the application of $AgBr$ in film photography?

<p>Specific light-sensitive properties. (D)</p>
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Which of the following statements is NOT associated to transition metals and their properties?

<p>Successive ionization enthalpies increase as steeply as in the main group elements because there are not any electrons to remove from <em>d</em> orbitals. (D)</p>
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What is the general characteristics of the actinoids series?

<p>The actinoids have the structural variability is obtained due to irregularities in metallic radii which are far greater than in lanthanoids, they are radioactive elements, and show great range of oxidation states due to comparable energies. (D)</p>
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The f-block elements or inner transition elements have a general electronic configuration:

<p>(n-2)$f^{1-14}$(n-1)$d^{0-1}ns^2$ (C)</p>
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Which is a general reaction for the lanthanoids?

<p>$Ln + H_2O \longrightarrow Ln(OH)_3 + H_2$ (C)</p>
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Flashcards

d-block elements

Elements in groups 3-12 where d orbitals are progressively filled.

f-block elements

Elements where 4f and 5f orbitals are progressively filled; placed at the bottom of the periodic table.

Transition metals

Metals with incomplete d subshells.

Transition metal series

The four series of transition metals are 3d series (Sc to Zn), 4d series (Y to Cd), 5d series (La and Hf to Hg), and 6d series (Ac and Rf to Cn).

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Lanthanoids

4f series (Ce to Lu).

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Actinoids

5f series (Th to Lr).

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d-block electronic configuration

Electronic configuration of outer orbitals is generally (n-1)d¹⁻¹⁰ns¹⁻².

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Orbital stability

Half and completely filled sets of orbitals are relatively more stable.

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Location of d-block

The middle section of the periodic table occupied by the d-block elements

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Metallic properties

3d metals usually have high tensile strength, ductility, malleability, thermal and electrical conductivity, and metallic luster.

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High melting points

High b/c greater number of electrons from (n-1)d & ns involve the interatomic metallic bonding.

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Ionic/atomic size trend

Decrease in radius with increasing atomic number

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Lanthanide contraction

Second and third series have similar radii

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Ionization Enthalpies

Irregular increase across transition series is due to the alteration of relative energies of 4s and 3d orbitals when electrons are removed.

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Factors affecting Ionization Enthalpy

Attraction, Repulsion, and Exchange energy.

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Exchange energy

The stabilisation of energy states

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Oxidation states

Elements can exhibit great variety of these

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Oxidation states trend

Elements giving greatest # of oxidation states occur in the middle of the series.

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Oxidation state variability

Elements with incomplete filling of d orbitals have oxidation states that differ by unity.

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Chemical reactivity

Transition metals exhibit varying amounts of this

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E° value trend

E° values indicate potential to form divalent cations

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Magnetic properties

Attraction or repulsion by magnetic field.

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Paramagnetism

Arises from presence of unpaired electrons

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Spin-only formula

µ = √n(n+2)

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Formation of colored ions

From lower to higher d orbital excites via visible light.

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Complex compounds

Metal ions bind anions or neutral molecules.

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Catalytic properties

Adopt multiple oxidation states and form complexes

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Interstitial compounds

Form when small atoms are trapped in metal lattices.

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Alloy formation

Blend of metals, homogeneous solid solutions.

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Potassium Permanganate

Undergo catalytic hydrogenation and produce alkali metals

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Study Notes

  • Iron, copper, silver, and gold are transition elements significant in the development of human civilization.
  • Thorium, protactinium, and uranium, are inner transition elements, serving as nuclear energy sources.

d-Block Elements

  • Consist of Groups 3-12 in the periodic table
  • d orbitals are progressively filled in the four long periods.
  • Located in the large middle section of the periodic table, between the s- and p-blocks

f-Block Elements

  • Consist of elements with progressively filled 4f and 5f orbitals
  • Often referred to as inner transition metals
  • They are placed in a separate panel at the bottom of the periodic table.

Transition Metal Series

  • Four main series exist
  • 3d series (Sc to Zn)
  • 4d series (Y to Cd)
  • 5d series (La and Hf to Hg)
  • 6d series (Ac and Rf to Cn)

Inner Transition Metal Series

  • Two series exist
  • 4f (Ce to Lu), known as lanthanoids
  • 5f (Th to Lr), known as actinoids.

IUPAC Definition of Transition Metals

  • Metals with an incomplete d subshell in neutral atoms or their ions
  • Zinc, cadmium, and mercury are not considered transition metals because they have a complete d¹⁰ configuration in their ground state and common oxidation states.

Properties of Transition Elements

  • Partially filled d or f orbitals make transition elements different from non-transition elements.
  • Transition elements and their compounds are studied separately.

Electronic Configuration

  • General configuration of outer orbitals: (n-1)d¹⁻¹⁰ns¹⁻²
  • Palladium (Pd) is an exception with an electronic configuration of 4d¹⁰5s⁰.
  • (n-1) represents the inner d orbitals
  • The outermost ns orbital can have one or two electrons
  • Half-filled and completely filled sets of orbitals contribute to stability, influencing configurations like those of Cr (3d⁵4s¹) and Cu (3d¹⁰4s¹).

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