Electronic Configuration of 3d Series Elements
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Questions and Answers

What is the electronic configuration of Chromium?

  • [Ar]3d⁵4s¹ (correct)
  • [Ar]3d⁶4s²
  • [Ar]3d¹⁰4s¹
  • [Ar]3d⁴4s²

    • Why is Copper not considered to have the same electronic configuration as other d-block elements?

  • It has a configuration of [Ar]3d⁹4s².
  • It does not exhibit oxidation states.
  • It has a configuration of [Ar]3d¹⁰4s¹. (correct)
  • It has a completely filled 4s orbital.

    • Which statement accurately describes why Zn is not classified as a transition metal?

  • It does not exhibit variable oxidation states.
  • It has completely filled d-orbitals in its oxidation states. (correct)
  • It belongs to the f-block elements.
  • It has partially filled d-orbitals.

    • What characteristic do Ag and Au share that qualifies them as transition metals?

    <p>They exhibit variable oxidation states with partially filled d-orbitals.</p> Signup and view all the answers

    On what ground is Scandium classified as a transition element?

    <p>It has partially filled d-orbitals.</p> Signup and view all the answers

    Which of the following is true regarding the exceptional electronic configurations of d-block elements?

    <p>They show stability in half-filled and fully filled d-orbitals.</p> Signup and view all the answers

    What property allows transition metals to exhibit a range of oxidation states?

    <p>Presence of unfilled and partially filled d-orbitals.</p> Signup and view all the answers

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

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

    What causes the color of transition metal ions?

    <p>The presence of d-d transitions and unpaired electrons</p> Signup and view all the answers

    Why are Cu(I) salts colorless?

    <p>They contain no d-electrons at all</p> Signup and view all the answers

    Which ion is colored among Sc3+, Zn2+, and Cr3+?

    <p>Cr3+ due to the presence of unpaired d-electrons</p> Signup and view all the answers

    What makes transition metals effective catalysts?

    <p>Variable oxidation states and large surface areas</p> Signup and view all the answers

    Why are zinc salts colorless?

    <p>They have fully paired d-electrons</p> Signup and view all the answers

    Which feature primarily contributes to the formation of complex compounds by transition metals?

    <p>Smaller size and higher ionic charges</p> Signup and view all the answers

    What characteristic of Cu(II) salts contributes to their color?

    <p>They have unpaired d-electrons</p> Signup and view all the answers

    Which of the following statements about transition metals is correct?

    <p>Transition metals typically have unpaired electrons</p> Signup and view all the answers

    Why is Cu+ considered diamagnetic?

    <p>It contains no unpaired electrons.</p> Signup and view all the answers

    Why does Vanadium have a relatively low E°(M³⁺ / M²⁺) value?

    <p>Due to the extra stability of V²⁺ from half filled t₂g orbital</p> Signup and view all the answers

    What is the magnetic moment of Sc3+?

    <p>0 BM</p> Signup and view all the answers

    Which statement is true regarding Cu2+?

    <p>It contains unpaired d-electrons.</p> Signup and view all the answers

    What accounts for the high stability of Mn²⁺ compared to other ions?

    <p>Its electronic configuration of d⁵</p> Signup and view all the answers

    Using the formula, what is n for Mn2+?

    <p>5</p> Signup and view all the answers

    How can the stability of cations be related to their standard electrode potential?

    <p>Stability is inversely proportional to E° value</p> Signup and view all the answers

    Which factor contributes to the increasing oxidizing power in VO₂⁺ < Cr₂O₇²⁻ < MnO₄⁻?

    <p>Increasing stability of lower species to which they are reduced</p> Signup and view all the answers

    What is the calculation for the number of unpaired electrons in Ti3+?

    <p>1</p> Signup and view all the answers

    Why is Cr²⁺ considered a strong reducing agent?

    <p>Because of its lower standard reduction potential than Fe²⁺</p> Signup and view all the answers

    If n > 5, how do you calculate the number of unpaired electrons?

    <p>10 - n</p> Signup and view all the answers

    What makes copper (I) compounds unstable in aqueous solutions?

    <p>The lower enthalpy of hydration of Cu⁺ compared to Cu²⁺</p> Signup and view all the answers

    What is the magnetic moment of a divalent ion with atomic number 25?

    <p>Cannot be determined without oxidation state.</p> Signup and view all the answers

    Why are Sc3+ salts considered diamagnetic?

    <p>They contain no unpaired d-electrons.</p> Signup and view all the answers

    Which of the following elements are considered diamagnetic?

    <p>Zn²⁺ and Co³⁺</p> Signup and view all the answers

    What is the cause of paramagnetism in transition metals?

    <p>Presence of unpaired electrons in d-orbitals</p> Signup and view all the answers

    Which of the following correctly describes d-block elements?

    <p>They have electrons entering the (n - 1)d orbitals.</p> Signup and view all the answers

    What characteristic defines transition elements?

    <p>They possess partially filled d-subshells.</p> Signup and view all the answers

    Where are d-block elements located in the periodic table?

    <p>In between the s- and p-block elements.</p> Signup and view all the answers

    Which group numbers do d-block elements occupy?

    <p>Groups 3-12.</p> Signup and view all the answers

    What is the general electronic configuration for d-block elements?

    <p>[Noble gas] (n - 1)d¹-¹⁰ ns¹-².</p> Signup and view all the answers

    How many series of d-block elements are known?

    <p>Four series.</p> Signup and view all the answers

    What is the valence shell electronic configuration of the 3d series of elements?

    <p>3d¹-¹⁰ 4s¹-².</p> Signup and view all the answers

    Which series belongs to the second transition series?

    <p>4d series.</p> Signup and view all the answers

    What is the primary reason for the maximum melting and boiling points of transition metals found at the middle of each series?

    <p>Increased number of unpaired electrons</p> Signup and view all the answers

    Which element has the lowest melting point among the transition metals?

    <p>Mercury (Hg)</p> Signup and view all the answers

    Why do Mn, Tc, and Re have lower melting points despite having more unpaired electrons?

    <p>They have a stable half-filled d5 configuration</p> Signup and view all the answers

    Regarding the enthalpy of atomization, which statement is correct?

    <p>4d and 5d series have higher enthalpy than 3d series</p> Signup and view all the answers

    What trend is observed in atomic radius across a transition series?

    <p>Atomic radius decreases, but less after midway</p> Signup and view all the answers

    How do ionization enthalpies change across a transition series?

    <p>They increase due to increased effective nuclear charge</p> Signup and view all the answers

    Which of the following pairs correctly identifies the relationship between atomic and ionic radii in transition metals?

    <p>Both decrease with increase in atomic number</p> Signup and view all the answers

    What explains the increase of density in transition metals along a period?

    <p>Decrease in metallic radius due to effective nuclear charge</p> Signup and view all the answers

    What is the reason for the higher second ionization enthalpy of copper compared to zinc?

    <p>Removal of a second electron from copper results in a less stable d configuration.</p> Signup and view all the answers

    During which process does manganese form a half-filled d configuration?

    <p>Second ionization enthalpy.</p> Signup and view all the answers

    Which of the following elements shows the maximum oxidation state of +7 in the 3d series?

    <p>Manganese</p> Signup and view all the answers

    Which statement best describes the variable oxidation states of transition metals?

    <p>They arise from the loss of both (n - 1)d and ns electrons.</p> Signup and view all the answers

    How does the second ionization enthalpy of manganese compare to that of iron?

    <p>It is lower than iron's.</p> Signup and view all the answers

    What happens to the oxidation state of transition elements as the atomic number increases up to manganese in the 3d series?

    <p>It increases.</p> Signup and view all the answers

    What configuration does copper achieve after the first ionization?

    <p>d^9</p> Signup and view all the answers

    Which two elements have a third ionization enthalpy that is considered very high?

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

    Which element in the 3d series exhibits the highest oxidation state?

    <p>Manganese (Mn)</p> Signup and view all the answers

    What is the reason that +2 oxidation state is the most common for 3d series transition metals?

    <p>It results from the loss of two 4s electrons.</p> Signup and view all the answers

    Which of the following is known to be a stronger reducing agent?

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

    Which compound is expected to show more covalent character?

    <p>Mn₂O₇</p> Signup and view all the answers

    In which oxidation state is chromium more acidic, CrO or CrO₃?

    <p>CrO₃</p> Signup and view all the answers

    Which transition element does not exhibit variable oxidation states?

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

    What is the significance of the E°(M²⁺/M) value for copper being positive?

    <p>Copper has high energy of atomization and low hydration energy.</p> Signup and view all the answers

    Which 3d series transition metal has the largest number of oxidation states?

    <p>Manganese (Mn)</p> Signup and view all the answers

    What is the nature of oxides formed by all transition metals except scandium?

    <p>Ionic and basic</p> Signup and view all the answers

    Which of the following oxides is classified as amphoteric?

    <p>V2O5</p> Signup and view all the answers

    What is the primary ore from which potassium dichromate is manufactured?

    <p>Chromite ore</p> Signup and view all the answers

    What does the reaction of V2O5 with acids produce?

    <p>VO43-</p> Signup and view all the answers

    Which of these is NOT a use of potassium dichromate?

    <p>In pharmaceuticals</p> Signup and view all the answers

    Which of the following statements about amphoteric oxides is true?

    <p>They can react with both acids and bases</p> Signup and view all the answers

    Study Notes

    Electronic Configuration of 3d Series Elements

    • Scandium (Sc): Atomic number 21, electronic configuration [Ar]3d¹4s².
    • Titanium (Ti): Atomic number 22, electronic configuration [Ar]3d²4s².
    • Vanadium (V): Atomic number 23, electronic configuration [Ar]3d³4s².
    • Chromium (Cr): Atomic number 24, unique configuration [Ar]3d⁵4s¹ due to stability of half-filled orbitals.
    • Manganese (Mn): Atomic number 25, electronic configuration [Ar]3d⁵4s².
    • Iron (Fe): Atomic number 26, electronic configuration [Ar]3d⁶4s².
    • Cobalt (Co): Atomic number 27, electronic configuration [Ar]3d⁷4s².
    • Nickel (Ni): Atomic number 28, electronic configuration [Ar]3d⁸4s².
    • Copper (Cu): Atomic number 29, unique configuration [Ar]3d¹⁰4s¹ due to stability of fully filled orbitals.
    • Zinc (Zn): Atomic number 30, electronic configuration [Ar]3d¹⁰4s².

    Exceptional Electronic Configurations

    • Some d-block elements show exceptions due to the energy difference between ns and (n-1)d orbitals.
    • Half-filled (d⁵) and completely filled (d¹⁰) configurations provide extra stability.
    • Cu and Cr have unique configurations to exploit this stability.

    Transition Elements

    • Zn, Cd, and Hg are not transition elements because they have completely filled d-orbitals in their common oxidation states.
    • Cu, Ag, and Au are considered transition elements since they possess partially filled d-orbitals in oxidation states.
    • Scandium (Sc) is a transition element due to partially filled d-orbitals, while Zn is not, as it has a completely filled d-orbital.

    Magnetic Properties

    • Transition metals are often paramagnetic, possessing unpaired electrons in d-orbitals.
    • Diamagnetic substances lack unpaired electrons and are not attracted to magnets.
    • Magnetic moment can be calculated using the formula (μ = \sqrt{n(n+2)}) where (n) is the number of unpaired electrons.

    Coloration of Transition Metal Ions

    • Color arises from unpaired d-electrons undergoing d-d transitions, absorbing visible light.
    • Cu²⁺ ions absorb red and emit blue, showcasing complementary colors.
    • Zn²⁺ salts are colorless due to lacking unpaired electrons.

    Catalytic Properties

    • Transition metals and their compounds act as catalysts due to multiple oxidation states, large surface area, and the presence of unpaired d-orbitals.
    • Example: Vanadium pentoxide is used as a catalyst in the manufacturing of sulfuric acid.

    Oxidation States of Transition Elements

    • Variable oxidation states result from the loss of inner (n-1)d and outer ns electrons.
    • Manganese exhibits the highest oxidation state (+7), while zinc typically shows +2.
    • The stability of oxidation states can be explained through standard electrode potentials.

    Characteristics of Transition Metal Compounds

    • Transition metals form a variety of complex compounds due to their small ionic size and high polarizing power.
    • The presence of vacant d-orbitals allows for effective bond formation.
    • Melting and boiling points are generally highest in the middle of transition series due to optimal metallic bonding from unpaired electrons.
    • Ionization enthalpies generally increase across the period, influenced by effective nuclear charge and electron configurations.
    • Atomic and ionic radii decrease with increasing atomic number, although patterns may vary slightly among specific elements.

    Summary of Oxides and Oxoanions

    • Transition metals mainly form ionic and basic oxides, while higher oxidation states exhibit covalent and acidic properties.
    • Certain oxides show amphoteric characteristics and can react both as acids and bases.

    Notable Transition Element Compounds

    • Potassium dichromate (K₂Cr₂O₇) is used widely, especially in the leather industry, and is obtained from chromite ore.

    General Observations

    • Transition metals generally display a wide range of oxidation states and complex formation abilities, maintaining unique properties that differentiate them from main group elements.

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    Description

    Test your knowledge on the electronic configurations of 3d series elements including Scandium, Titanium, and more. Explore both standard configurations and exceptions, focusing on the stability of half-filled and fully filled orbitals. This quiz will help reinforce your understanding of d-block elements.

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