Electronic Configuration of 3d Series Elements

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?

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

On what ground is Scandium classified as a transition element?

It has partially filled d-orbitals. Signup and view all the answers

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

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

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

Presence of unfilled and partially filled d-orbitals. Signup and view all the answers

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

Zinc (Zn) Signup and view all the answers

What causes the color of transition metal ions?

The presence of d-d transitions and unpaired electrons Signup and view all the answers

Why are Cu(I) salts colorless?

They contain no d-electrons at all Signup and view all the answers

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

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

What makes transition metals effective catalysts?

Variable oxidation states and large surface areas Signup and view all the answers

Why are zinc salts colorless?

They have fully paired d-electrons Signup and view all the answers

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

Smaller size and higher ionic charges Signup and view all the answers

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

They have unpaired d-electrons Signup and view all the answers

Which of the following statements about transition metals is correct?

Transition metals typically have unpaired electrons Signup and view all the answers

Why is Cu+ considered diamagnetic?

It contains no unpaired electrons. Signup and view all the answers

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

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

What is the magnetic moment of Sc3+?

0 BM Signup and view all the answers

Which statement is true regarding Cu2+?

It contains unpaired d-electrons. Signup and view all the answers

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

Its electronic configuration of d⁵ Signup and view all the answers

Using the formula, what is n for Mn2+?

5 Signup and view all the answers

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

Stability is inversely proportional to E° value Signup and view all the answers

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

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

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

1 Signup and view all the answers

Why is Cr²⁺ considered a strong reducing agent?

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

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

10 - n Signup and view all the answers

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

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

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

Cannot be determined without oxidation state. Signup and view all the answers

Why are Sc3+ salts considered diamagnetic?

They contain no unpaired d-electrons. Signup and view all the answers

Which of the following elements are considered diamagnetic?

Zn²⁺ and Co³⁺ Signup and view all the answers

What is the cause of paramagnetism in transition metals?

Presence of unpaired electrons in d-orbitals Signup and view all the answers

Which of the following correctly describes d-block elements?

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

What characteristic defines transition elements?

They possess partially filled d-subshells. Signup and view all the answers

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

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

Which group numbers do d-block elements occupy?

Groups 3-12. Signup and view all the answers

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

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

How many series of d-block elements are known?

Four series. Signup and view all the answers

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

3d¹-¹⁰ 4s¹-². Signup and view all the answers

Which series belongs to the second transition series?

4d series. 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?

Increased number of unpaired electrons Signup and view all the answers

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

Mercury (Hg) Signup and view all the answers

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

They have a stable half-filled d5 configuration Signup and view all the answers

Regarding the enthalpy of atomization, which statement is correct?

4d and 5d series have higher enthalpy than 3d series Signup and view all the answers

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

Atomic radius decreases, but less after midway Signup and view all the answers

How do ionization enthalpies change across a transition series?

They increase due to increased effective nuclear charge Signup and view all the answers

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

Both decrease with increase in atomic number Signup and view all the answers

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

Decrease in metallic radius due to effective nuclear charge Signup and view all the answers

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

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

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

Second ionization enthalpy. Signup and view all the answers

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

Manganese Signup and view all the answers

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

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

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

It is lower than iron's. 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?

It increases. Signup and view all the answers

What configuration does copper achieve after the first ionization?

d^9 Signup and view all the answers

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

Copper and zinc Signup and view all the answers

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

Manganese (Mn) Signup and view all the answers

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

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

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

Cr²⁺ Signup and view all the answers

Which compound is expected to show more covalent character?

Mn₂O₇ Signup and view all the answers

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

CrO₃ Signup and view all the answers

Which transition element does not exhibit variable oxidation states?

Zinc (Zn) Signup and view all the answers

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

Copper has high energy of atomization and low hydration energy. Signup and view all the answers

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

Manganese (Mn) Signup and view all the answers

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

Ionic and basic Signup and view all the answers

Which of the following oxides is classified as amphoteric?

V2O5 Signup and view all the answers

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

Chromite ore Signup and view all the answers

What does the reaction of V2O5 with acids produce?

VO43- Signup and view all the answers

Which of these is NOT a use of potassium dichromate?

In pharmaceuticals Signup and view all the answers

Which of the following statements about amphoteric oxides is true?

They can react with both acids and bases 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.

Properties Trends Among Transition Metals

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.