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Chapter 26: Problem 3

Give the highest oxidation states for \(\mathrm{Sc}, \mathrm{Ti}, \mathrm{V}\), Cr, and \(\mathrm{Mn}\).

Short Answer

Expert verified
Sc: +3, Ti: +4, V: +5, Cr: +6, Mn: +7.

Step by step solution

01

Determine the Electron Configuration

Identify the electron configuration of each element to determine how many electrons can be lost to attain the highest oxidation state. - **Scandium (Sc):** [Ar] 3d鹿 4s虏 - **Titanium (Ti):** [Ar] 3d虏 4s虏 - **Vanadium (V):** [Ar] 3d鲁 4s虏 - **Chromium (Cr):** [Ar] 3d鈦� 4s鹿 - **Manganese (Mn):** [Ar] 3d鈦� 4s虏.
02

Calculate Highest Oxidation State

The highest oxidation state of a transition element corresponds to the total number of d and s electrons available for bonding. - **Scandium (Sc):** Can lose 3 electrons (3d鹿 and 4s虏) resulting in an oxidation state of +3. - **Titanium (Ti):** Can lose 4 electrons (3d虏 and 4s虏) resulting in an oxidation state of +4. - **Vanadium (V):** Can lose 5 electrons (3d鲁 and 4s虏) resulting in an oxidation state of +5. - **Chromium (Cr):** Can lose 6 electrons (3d鈦� and 4s鹿) resulting in an oxidation state of +6. - **Manganese (Mn):** Can lose 7 electrons (3d鈦� and 4s虏) resulting in an oxidation state of +7.
03

Check for Stability

Verify whether the calculated oxidation states are common and stable in typical compounds: - **Sc:** +3 is stable and common (e.g., Sc鈧侽鈧�). - **Ti:** +4 is stable and common (e.g., TiO鈧�). - **V:** +5 is stable and common (e.g., VO鈧�). - **Cr:** +6 is stable and common (e.g., CrO鈧�). - **Mn:** +7 is stable and common (e.g., KMnO鈧�).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Transition Metals
Transition metals are a fascinating group of elements found in the d-block of the periodic table. They are known for their unique properties, including the ability to form various oxidation states. This is due to the participation of d electrons in bonding. Transition metals often exhibit:
  • High melting and boiling points
  • Variable oxidation states
  • Ability to form colored compounds
Their varied oxidation states and complex chemistry make them essential in many industrial and biological processes. They play a vital role in catalysis and are integral to structural materials.
Electron Configuration
Understanding electron configuration is key to predicting the behavior of transition metals. Electron configuration denotes the distribution of electrons across available shells and subshells in an atom. For instance:
  • Scandium (Sc): [Ar] 3d鹿 4s虏
  • Titanium (Ti): [Ar] 3d虏 4s虏
  • Vanadium (V): [Ar] 3d鲁 4s虏
  • Chromium (Cr): [Ar] 3d鈦� 4s鹿
  • Manganese (Mn): [Ar] 3d鈦� 4s虏
The electron configuration helps in determining how many electrons can be lost to form a positive oxidation state, thus catalyzing reactions or bonding with other elements.
Oxidation State Calculation
Calculating oxidation states is crucial in understanding the chemistry of transition metals. The highest oxidation state generally refers to the total electrons that can be removed from both d and s orbitals.
  • Scandium: Can lose 3 electrons resulting in a +3 state.
  • Titanium: Can lose 4 electrons resulting in a +4 state.
  • Vanadium: Can lose 5 electrons resulting in a +5 state.
  • Chromium: Can lose 6 electrons resulting in a +6 state.
  • Manganese: Can lose 7 electrons resulting in a +7 state.
Calculating these states aids in predicting how a transition metal will behave in reactions.
Chemical Stability
Chemical stability describes how likely a compound is to maintain its form and structure over time. In transition metals, the stability of an oxidation state is important in predicting reactivity and compound formation.
  • Scandium's +3 state is common and stable in Sc鈧侽鈧�.
  • Titanium's +4 state remains stable in TiO鈧�.
  • Vanadium's +5 oxidation level is stable in VO鈧�.
  • Chromium often forms stable compounds like CrO鈧� in the +6 state.
  • Manganese's +7 state is stable as seen in KMnO鈧�.
Understanding the chemical stability of oxidation states allows scientists and engineers to gauge their practical uses.
Scandium
Scandium is the first element in the d-block of transition metals. Its unique electron configuration \[\text{[Ar]} 3d^1 4s^2\]allows it to form a +3 oxidation state easily. Found in compounds such as scandium oxide \(\text{Sc}_2\text{O}_3\), it is known for its lightweight and durable nature. Scandium is also used in aerospace materials due to these properties.
Titanium
Titanium possesses an electron configuration of \[\text{[Ar]} 3d^2 4s^2\]which allows it to lose four electrons and reach a +4 oxidation state. Well-known for forming stable compounds like \(\text{TiO}_2\), titanium is celebrated for its strength and corrosion resistance. Because of these characteristics, it is widely used in the manufacture of aircraft, medical devices, and jewelry.
Vanadium
Vanadium features an electron configuration of \[\text{[Ar]} 3d^3 4s^2\]allowing the element to exhibit a +5 oxidation state by losing up to 5 electrons. Vanadium pentoxide \(\text{VO}_5\) is a common and stable compound of vanadium. This element finds application in steel production, catalysis, and as an alloying agent due to its ability to confer toughness and wear resistance.
Chromium
Chromium's electron configuration \[\text{[Ar]} 3d^5 4s^1\]gives it access to a +6 oxidation state. Chromium compounds like \(\text{CrO}_3\) are recognized for their stable high oxidation states. Known for its hard, silvery appearance and high corrosion resistance, chromium is used in stainless steel production, plating, and pigment manufacturing.
Manganese
Manganese boasts an electron configuration of \[\text{[Ar]} 3d^5 4s^2\]which supports the removal of up to seven electrons, achieving a +7 oxidation state. A typical example of this is potassium permanganate \(\text{KMnO}_4\), a stable compound exhibiting this highest state. Manganese is vital in steelmaking for deoxidizing and sulfur-fixing, and serves as a component in batteries and chemical reactions due to its diverse oxidation states.

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Most popular questions from this chapter

Give the oxidation state of the metal in (a) \(\left[\left.\operatorname{Ir}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right|^{3+}\right.\) (b) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}(\mathrm{CO})_{3}\right]^{3+}\) (c) \(\left[\mathrm{CuCl}_{4}\right]^{2-}\) (d) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

Give the systematic name for: $$ \left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{Pt} \mathrm{I}_{4}\right] $$

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Alloys are usually mixtures of metals. Give the elemental compositions of the common alloys: brass, bronze, common solder, and white gold. You may have to do an Internet search or consult a handbook of chemistry in the library for the necessary information.

Ores containing as little as \(0.25 \%\) copper are sometimes used to obtain copper metal. What mass of such an ore is needed to produce 91 metric tons of copper, the amount used in the Statue of Liberty?
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