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Chapter 14: Problem 236

Among the following, the coloured compound is: (a) \(\mathrm{CuCl}\) (b) \(\mathrm{K}_{3}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]\) (c) \(\mathrm{CuF}_{2}\) (d) \(\left[\mathrm{Cu}\left(\mathrm{CH}_{3} \mathrm{CN}\right)_{4}\right] \mathrm{BF}_{4}\)

Short Answer

Expert verified
The colored compound is (c) \(\mathrm{CuF}_{2}\).

Step by step solution

01

Understanding Color in Compounds

The color of a compound typically arises from the presence of transition metals with unpaired electrons. These electrons can absorb visible light, promoting transitions that result in color.
02

Analyzing Each Option

- (a) \(\mathrm{CuCl}\) : Copper in CuCl is in the Cu鈦� state, which has a completely filled d subshell, leading to a colorless compound.- (b) \(\mathrm{K}_{3}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]\) : Copper here is also in the Cu鈦� state and similarly lacks unpaired electrons, making it colorless.- (c) \(\mathrm{CuF}_{2}\) : Copper is in the Cu虏鈦� state which has an unfilled d subshell, enabling it to exhibit color.- (d) \(\left[\mathrm{Cu}\left(\mathrm{CH}_{3} \mathrm{CN}\right)_{4}\right]\mathrm{BF}_{4}\) : Copper in this complex is in the Cu鈦� state, essentially colorless due to filled d levels.
03

Conclusion

From the analysis of the electronic configuration of copper in each compound, (c) \(\mathrm{CuF}_{2}\), with Cu虏鈦�, has unpaired d-electrons and is therefore colored.

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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 group of elements found in the d-block of the periodic table. They include elements such as iron, copper, and nickel. One of the fascinating features of transition metals is their ability to form colored compounds. This characteristic is prominently due to their electronic structure.
Transition metals often have incomplete d sub-levels, allowing them to form various oxidation states and coordination complexes. This property of having variable oxidation states is crucial for their function in many chemical reactions and determines how they interact with light. The ability to display different colors is mostly due to these unique electronic transitions.
Electron Configuration
Electron configuration refers to the arrangement of electrons in an atom or a molecule. For transition metals, electron configuration can play a significant role in their color properties. The electrons occupy orbitals in a specific sequence following the Aufbau principle, filling from lower to higher energy levels.
In the case of transition metals, the d-orbital can hold up to 10 electrons. The electron configuration can vary depending on the compound and the oxidation state of the metal. When transition metals form ions, they often lose electrons from the s and d orbitals, which can lead to configurations that allow electron transitions responsible for colors in compounds.
Unpaired Electrons
Unpaired electrons are electrons that do not have a partner with opposite spin in an orbital. These electrons are crucial in determining the magnetic and optical properties of compounds, particularly in transition metals.
The presence of unpaired electrons allows for electron transitions, often between d-orbitals, which result in the absorption of specific wavelengths of light. This absorption imparts color to the compound. For instance, if a transition metal ion has more unpaired electrons, it tends to exhibit a more intense color. The specific wavelength of light absorbed and thus the color observed depends on the energy gap between the electron levels.
CuF2
CuF鈧�, or copper(II) fluoride, is a compound where copper exists in the Cu虏鈦� oxidation state. This state of copper is characterized by incomplete d orbitals, specifically where the d sub-level is not filled.
In CuF鈧�, copper has a 3d鈦� electron configuration, meaning there is one unpaired electron. These unpaired electrons make it possible for CuF鈧� to absorb visible light and display color. This ability to exhibit color distinguishes CuF鈧� from other copper compounds, like those containing Cu鈦� ions, which typically are colorless due to filled d-orbitals.
Color Properties of Compounds
The color properties of compounds, especially those involving transition metals, can be strongly influenced by the metal's electron configuration and the ligand field created by surrounding atoms or molecules.
When a transition metal compound absorbs light, it often involves electron transitions between different energy levels, particularly within the d orbitals. The specific color of the compound corresponds to the light wavelengths not absorbed but reflected.
  • The nature of the ligands attached to the metal can significantly alter these energy gaps, influencing the color observed.
  • Compounds with large energy gaps typically absorb higher-energy light (such as blue), appearing more towards the red end of the spectrum, while those with smaller gaps may absorb red and appear green or blue.
  • The oxidation state of the metal also plays a crucial role, as seen with CuF鈧�, where the Cu虏鈦� state leads to unpaired electrons and color development.
Understanding these aspects helps predict and explain the rich variety of colors exhibited by metal compounds.

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Most popular questions from this chapter

Which of the following is the lunar caustic? (a) \(\mathrm{AgNO}_{3}\) (b) \(\mathrm{Cu}_{2} \mathrm{Cl}_{2}\) (c) \(\mathrm{CuCl}_{2}\) (d) \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\)

Percentage of gold in 14 carat gold is: (a) 58 \(\square\) (b) 80 (c) 40 (d) 14

The formula of the product formed, when sodium thiosulphate solution (hypo solution) is added to silver bromide is: \(\quad\) (a) \(\mathrm{Ag}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) (b) \(\mathrm{Ag}_{2} \mathrm{~S}\) (c) \(\mathrm{Ag}_{3}\left[\mathrm{Na}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}\right]\) (d) \(\mathrm{Na}_{3}\left[\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}\right]\)

The matte obtained by smelting copper pyrites with coke and \(\begin{array}{ll}\text { sand contains mainly : } & \text}\end{array}\) (a) \(\mathrm{FeS}+\mathrm{ZnS}\) (b) \(\mathrm{Cu}_{2} \mathrm{~S}+\mathrm{FeS}\) (c) \(\mathrm{CuS}+\mathrm{FeS}_{2}\) (d) \(\mathrm{ZnS}+\mathrm{CuS}\)

Which metallurgy involves leaching? (a) Au [ (b) Ag (c) both (a) and (b) \(\square\) (d) none of these
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