Transition Metals Quiz
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Questions and Answers

Which transition metal ion is typically colored blue in aqueous solution?

  • Cu2+ (correct)
  • Fe2+
  • Cr3+
  • Ni2+

What factor contributes to the formation of complexes by d-block metals?

  • High effective nuclear charge (Zeff) (correct)
  • Low melting point
  • Inability to form ions
  • Presence of d10 electrons

Which of the following transition metal halides does not exist due to steric crowding?

  • CuF
  • TiF2
  • MnF7 (correct)
  • CrF6

Which oxides correspond with a transition metal oxidation state of +7?

<p>Mn2O7 (B)</p> Signup and view all the answers

Which combination of elements is commonly used to form brass as an alloy?

<p>Copper and zinc (A)</p> Signup and view all the answers

What happens to the atomic size of transition metals when moving from Sc to Cr?

<p>Atomic size decreases (D)</p> Signup and view all the answers

Which transition metal has the lowest melting point among the following?

<p>Zn (A)</p> Signup and view all the answers

How does the density of transition metals generally change from left to right across a period?

<p>Density increases continuously (A)</p> Signup and view all the answers

Which of the following metals is closest in atomic radius to Ag?

<p>Au (B)</p> Signup and view all the answers

What trend is observed for ionization energy across the transition metals from Sc to Zn?

<p>Ionization energy increases (D)</p> Signup and view all the answers

What is the primary reason for the increase in melting point in transition metals when moving down a group?

<p>Increase in mass and effective nuclear charge (C)</p> Signup and view all the answers

How does the number of unpaired electrons affect the melting point of transition metals?

<p>More unpaired electrons result in higher melting point (D)</p> Signup and view all the answers

What phenomenon is observed when comparing ionization energies among transition metals?

<p>Unusual trends can occur due to electron configuration shifts (D)</p> Signup and view all the answers

Which element usually does not show variable oxidation states?

<p>Sc (B)</p> Signup and view all the answers

Which of the following ions does not liberate hydrogen gas when reacting with dilute acids?

<p>Cr2+ (C)</p> Signup and view all the answers

In the context of standard electrode potentials, which trend is observed from left to right in a period?

<p>Eo values decrease (A)</p> Signup and view all the answers

What is the expected magnetic behavior of a d5 system?

<p>Lower than expected magnetic moment (C)</p> Signup and view all the answers

What condition leads to the stability of M2+ over M3+ in standard oxidation potential?

<p>IE &gt; HE (B)</p> Signup and view all the answers

Which statement about transition metals and their catalytic properties is true?

<p>Their variable oxidation states contribute to their catalytic properties. (C)</p> Signup and view all the answers

Which ion has a higher ionization energy based on its standard oxidation potential?

<p>Mn2+ (D)</p> Signup and view all the answers

What does the formula for calculating the spin only magnetic moment (in Bohr Magneton, BM) incorporate?

<p>√n(n+2) (D)</p> Signup and view all the answers

What is the defining criterion for transition elements in the new definition?

<p>D-block elements with unpaired electrons (C)</p> Signup and view all the answers

Which of the following elements is NOT considered a transition element?

<p>Zinc (B)</p> Signup and view all the answers

What is the atomic number for the last element in the first transition series?

<p>30 (D)</p> Signup and view all the answers

According to the general electronic configuration, what does it mean when an element has the configuration (n - 1)d 1-10 ns0-2?

<p>It signifies variable oxidation states. (B)</p> Signup and view all the answers

What is an exception to the electron configuration rule mentioned in the content?

<p>Gold having an interrupted d-electron count (B)</p> Signup and view all the answers

Which of the following elements belongs to the second transition series?

<p>Yttrium (B)</p> Signup and view all the answers

In terms of atomic size, what trend is observed within the transition series from scandium to zinc?

<p>Atomic size uniformly decreases (D)</p> Signup and view all the answers

How many elements are present in the second transition series?

<p>10 (D)</p> Signup and view all the answers

What color is the permanganate ion (KMnO4)?

<p>Purple (B)</p> Signup and view all the answers

Which of the following reagents will produce Cl2 gas when reacting with KMnO4?

<p>HCl (C)</p> Signup and view all the answers

What is the general electronic configuration of lanthanides?

<p>[Xe]4f1-14 6s2 (A)</p> Signup and view all the answers

Which of the following ions is expected to show color due to f-d transitions?

<p>Sm3+ (D)</p> Signup and view all the answers

Which decomposition product is obtained from KMnO4 under heating conditions?

<p>MnO2 (A)</p> Signup and view all the answers

Which of the following reactions will produce hydrogen gas?

<p>Zn metal + HCl (A)</p> Signup and view all the answers

What type of structure does potassium dichromate (K2Cr2O7) have?

<p>Bridged Tetrahedral (A)</p> Signup and view all the answers

Which oxidation state of manganese is present in manganate ion?

<p>+6 (B)</p> Signup and view all the answers

Which of the following properties is common to lanthanides?

<p>Common oxidation state of +3 (A)</p> Signup and view all the answers

What is the primary use of lanthanide oxides?

<p>As catalysts in petroleum cracking (B)</p> Signup and view all the answers

Which reaction correctly represents lanthanides reacting with oxygen?

<p>Ln + O2 ⟶ Ln2O3 (C)</p> Signup and view all the answers

Which lanthanide oxide property leads to its use in television screens?

<p>Phosphorescence (A)</p> Signup and view all the answers

What is the expected oxidation state for most actinides?

<p>+3 (D)</p> Signup and view all the answers

Which of the following statements correctly describes actinide contraction?

<p>It is due to the poor shielding of 5f electrons. (B)</p> Signup and view all the answers

Which lanthanide does not exhibit a +4 oxidation state?

<p>Eu (B)</p> Signup and view all the answers

Mischmetal is primarily an alloy composed of which types of metals?

<p>Lanthanoid metals (D)</p> Signup and view all the answers

Flashcards

Atomic Size Trend (3d)

Atomic size generally decreases across the 3d transition series (Sc to Zn) due to increasing effective nuclear charge. However, there are irregularities. Sc to Cr shows a decrease, while Mn to Ni is roughly constant, and then Ni to Zn increases.

Metallic Radius

Half the distance between the nuclei of two adjacent metal atoms in a metallic crystal.

Melting Point Trend (3d)

Melting points of 3d transition metals increase with increasing number of unpaired electrons (stronger M-M bonds) .However, there are irregularities depending on the number of unpaired electrons. Lower melting point may indicate a weaker metallic bonding forces.

3d Transition Metals Melting Point Trend

Melting points of 3d transition metals generally increase up to the elements with the maximum number of unpaired electrons, then decrease.

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Density Trend (3d)

Density generally increases across the 3d transition series due to increasing mass and decreasing atomic size. There's a slight irregularity in the middle of the series.

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Ionization Energy Trend (3d)

Ionization energy of 3d transition metals generally increases from left to right. However, there are exceptions related to electron configurations and stability.

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Electron Configuration Irregularity (Iron)

The electron configuration of iron(Fe) and its ions, particularly the +1 state, show deviations from the expected patterns due to energy stabilization from electron pairing.

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3d Transition Metals Density

Density is influenced mostly by mass and atomic size. It rises left to right due to mass increase while the trend in size is irregular, hence the uneven density curve.

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Variable Oxidation State

Transition metals often exhibit multiple oxidation states (different charges) in their compounds.

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Colour of Transition Metals

Transition metal compounds often have colour due to d-d electron transitions in their d-orbitals. Some are colourless, others are various colours.

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Standard Oxidation Potential

Measure of tendency of a species to lose electrons, forming ions.

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Colourless Transition Metals

Metals with d0 or d10 electron configurations in their aqueous ions are colourless.

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Complex Formation in d-block

d-block metals readily form complexes due to vacant (n-1)d orbitals and high effective nuclear charge (Zeff).

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Standard Electrode Potential (E°)

Measure of a half-reaction to get oxidized or reduced related to a standard hydrogen electrode.

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Alloy Formation

Metals with similar atomic sizes (<15% difference) make good alloys. d-block metals are often used in alloys

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Magnetic Moment

Measure of the strength of a substance's magnetic field related to un-paired electrons.

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Transition Metal Catalyst

Transition metals are frequently used in reactions as catalysts due to their variable oxidation states and active surface area.

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3d Transition Metal Halides

3d transition metal halides often limit their oxidation states and halides due to factors like steric crowding and redox reactions, particularly with fluorine.

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Oxidation State Max.

Maximum oxidation state is related to highest charge it can have. (n=number of valence electrons=number of electrons lost, d=inner electrons.)

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Reactivity Trend (3d)

Reactivity generally decreases across 3d transition series in terms of losing/gaining electrons.

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Hydrogen Gas Liberation

Certain metal ions react with acid to produce hydrogen gas; this is an indication in the position of an element in a series of elements.

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Transition Elements (New Def)

D-block elements with unpaired electrons or partially filled d-orbitals in any oxidation state.

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3d Transition Series

The group of elements from Scandium (Sc) to Zinc (Zn), where 3d orbitals fill.

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General Electronic Configuration (Transition Elements)

(n-1)d1-10 ns0-2 (Where n represents the principal quantum level).

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Exceptions to Electronic Configuration Rule

Elements like Chromium (Cr), copper (Cu), and others deviate from the expected n+l rule.

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Transition metals vs d-block elements

Not all d-block elements are considered as transition metals. Some elements like Zn, Cd, & Hg are excluded from the transition metal classification

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First Transition Series

The 10 elements (Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, and Zn) in the 3d transition series

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Second Transition Series Elements

The set of 10 elements beginning with Yttrium (Y) and ending with Cadmium (Cd)

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Atomic Size Trend

Atomic size in the 3d transition series generally decreases, then slightly increases, affected by the effective nuclear charge.

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Potassium Dichromate Reactions

Potassium dichromate (K₂Cr₂O₇) reacts with HCl, HBr, HI to produce Cl₂, Br₂, I₂, respectively. It also reacts with reducing agents like Fe²⁺ and Sn²⁺, oxidizing them to Fe³⁺ and Sn⁴⁺, respectively.

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KMnO₄ Oxidizing Reactions

Potassium permanganate (KMnO₄) is a strong oxidizing agent. It reacts with various reducing agents and itself can gain electrons.

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Lanthanides (Ln)

The 4f series of transition metals, with atomic numbers 58 to 71.

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Lanthanide Contraction

A steady decrease in the atomic radii of lanthanide elements across the series.

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Potassium Dichromate Structure

Potassium dichromate has a bridged tetrahedral structure with all angles of slightly under 109 degrees.

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Manganese Compounds

Manganese forms various compounds like manganate (green) and permanganate (purple), each differing in their oxidation states and electronic configuration.

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KMnO₄ Decomposition

Potassium permanganate decomposes at high temperatures to form manganese dioxide and other products.

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Oxidizing Agents in Reactions

Oxidizing agents accept electrons from other species during chemical reactions.

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Lanthanide Reactivity

Lanthanides are more reactive than hydrogen and react with water to produce lanthanum hydroxide.

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Lanthanide Common Oxidation State

The most common oxidation state for lanthanides is +3, but they can also exhibit +2 and +4.

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Lanthanides' Color

Aqueous solutions of lanthanides are often colored due to electron transitions involving f-orbitals.

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Mischmetal Composition

Mischmetal alloy consists mainly of lanthanide metals, with a small percentage usually of iron.

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Actinoid Radioactive Nature

All actinoids are radioactive elements, starting from element 90.

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Actinoid Contraction

Actinoid contraction is the decrease in atomic radii due to poor shielding of 5f electrons.

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Actinoid Variable Oxidation States

Actinides show a range of oxidation states (+3 to +7) due to the closeness in energy levels of 5f, 6d, and 7s orbitals.

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Lanthanide without +4 OS

Europium is the lanthanide that doesn't exhibit a +4 oxidation state.

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Study Notes

D & F Block Elements

  • D & F block elements are transition metals
  • Transition metals are elements that have partially filled d-orbitals in their ground state or any of their oxidation states.
  • The old definition of transition elements was all elements in the d-block.
  • The new definition of transition metals are d-block elements that have unpaired electrons, or partially filled d-orbitals in any oxidation state.
  • Elements Zn, Cd, and Hg are d-block elements but not considered transition metals.

The First Transition Series

  • The 3d series includes elements from scandium (Z=21) to zinc (Z=30).
  • There are 10 elements in the first transition series.
  • The filling of 3d orbitals is involved in elements from scandium to zinc.

The Second Transition Series

  • The 4d series includes elements from yttrium (Z=39) to cadmium (Z=48).
  • There are 10 elements in the second transition series.
  • The filling of 4d orbitals is involved in elements from yttrium to cadmium.

General Electronic Configuration

  • (n-1)d1–10ns2 is the general electronic configuration
  • Exceptions are common among the transition metals.
  • Elements such as Cu, Cr, Nb, Mo, Ru, Rh, Pd, Ag, Pt have exceptions to the previous rule

Physical Properties

  • Atomic size: Decreases across a period (left to right) due to increase in effective nuclear charge but increases slightly down a group.
  • Metallic radius: The radius of the atom in a metallic crystal.
  • Melting point :Generally increases across a period then decreases very slightly. Then it increases again.
  • Density : Increases generally across a period but decreases slightly down a group.
  • Ionization energy: Generally increases across a period and decreases down a group.

Catalytic Properties

  • Transition elements often used as catalysts due to variable oxidation states and high surface area.

Colour of Transition Metal Compounds

  • The colour of a compound depends on the $d – d$ transitions that occur when electrons move between d orbitals of different energies.
  • d0, d10 are typically colourless.
  • Colourless compounds usually have no partially filled d-orbitals.
  • Other coloured compounds are due to the promotion of electrons within the d orbitals

Complex Formation Tendency

  • d-block metals can act as Lewis acids due to the presence of empty (n-1) d-orbitals.
  • They form complexes when they attract ligands.

Halides of 3d Series

  • Oxidation state often correlates to the number of halides (F-, Cl-, Br-, and I-) each element can form
  • The higher the oxidation state, more halides it forms
  • Some halides from transition metals do not exist due to the nature of the oxidising and reducing agents present.

Oxides of 3d series

  • Most transition metals exhibit a variety of oxidation states.
  • Different transition metal oxides can form various compounds.

Oxidation nature of KMnO4

-In a mild basic environment, KMnO4 can act as a strong oxidising agent
-The oxidation state of manganese in KMnO4 is +7
-In acidic solution, KMnO4 can be reduced to Mn2+

Reactions of KMnO4

-HCl, HBr, HI can be oxidised by KMnO4

  • HNO2 / H2SO3/H2C2O4, CO2/H2SO4
  • Fe2+/ Sn2+, H2S/S can be oxidised by KMnO4

Decomposition of KMnO4

-Decomposition of KMnO4 yields K2MnO4, MnO2 and O2

Properties of Lanthanides

  • All are silvery-white metals
  • Found in earth's crust (rare earth metals)
  • High reactivity with halogens and sulfur -Their reactivity is generally more than that of alkaline earth metals.
  • Aqueous solutions are often colored due to f-f transitions.

Reactions of Lanthanides

  • Lanthanides react with halogens, air, nitrogen and hydrogen.

Uses of Lanthanides

  • Used in TV screens, and
  • Also used in alloys

f-Block Elements

  • 4f series: Lanthanides (atomic numbers 58-71).
  • 5f series: Actinides (atomic numbers 90-103).
  • All are radioactive and unstable
  • All are man-made.

Oxidation States of Actinides

  • Actinides display a greater range of oxidation states compared to lanthanides

Mischmetal

  • Mischmetal is an alloy of mostly lanthanide metals and iron.
  • The alloy is used to manufacture various pyro-technical products.

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Test your knowledge on transition metals with this quiz that covers their properties, colors in solution, and complex formation. Explore questions about metal halides, oxidation states, and alloy compositions. Perfect for chemistry enthusiasts and students alike.

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