/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 175 The puir of which salrs is cxpcc... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 7: Problem 175

The puir of which salrs is cxpccted ro have same: colour in rheir froshly prcparcd aqucous solurions? (a) \(\mathrm{VOCl}_{2}, \mathrm{C} . \mathrm{uCl}_{2}\) (b) \(\mathrm{C} \mathrm{u} \mathrm{C} \mathrm{l}_{2}, \mathrm{FeCl}_{2}\) (c) \(\mathrm{FeCl}_{2}, \mathrm{VOCl}_{2}\) (d) \(\mathrm{MnCl}_{2}, \mathrm{FeCl}_{2}\)

Short Answer

Expert verified
Option (a): Both \\ \( \text{VOCl}_2 \\ \) and \\ \( \text{CuCl}_2 \\ \) form blue solutions.

Step by step solution

01

Understanding the Problem

We need to determine which pair of salts from the given options will have aqueous solutions of the same color. Each salt dissociates into its constituent ions when dissolved in water, influencing the color of the solution due to the presence of certain transition metal ions.
02

Analyze Colors of Aqueous Solutions

Transition metals often form colored solutions due to their electron configurations. For example:- \ \( \text{Cu}^{2+} \ \) typically forms blue or blue-green solutions.- \ \( \text{Fe}^{2+} \ \) solutions are generally pale green.- \ \( \text{VO}^{2+} \ \) solutions are often blue.- \ \( \text{MnCl}_2 \ \) typically forms very pale pink solutions.
03

Evaluate Each Option for Similar Colors

(a) \ \( \text{VOCl}_2, \text{CuCl}_2 \ \): Both \ \( \text{VO}^{2+} \ \) and \ \( \text{Cu}^{2+} \ \) form blue solutions.(b) \ \( \text{CuCl}_2, \text{FeCl}_2 \ \): Blue vs. green solutions.(c) \ \( \text{FeCl}_2, \text{VOCl}_2 \ \): Green vs. blue solutions.(d) \ \( \text{MnCl}_2, \text{FeCl}_2 \ \): Pale pink vs. pale green solutions.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Aqueous Solution Color
The color of aqueous solutions is a fascinating aspect of chemistry, especially when examining transition metal ions. In many cases, the vibrant hues that we observe are due to specific electron transitions within the metal ions. When transition metal salts dissolve in water, they dissociate to form ions. These ions can absorb certain wavelengths of light, and the light that they do not absorb is reflected into our eyes, giving the solution its noticeable color.
  • Blue and Blue-Green Colors: Copper(II) ions ( \( ext{Cu}^{2+} \) ) usually impart a blue or blue-green tint to the solution.
  • Pale Green Colors: Iron(II) ions ( \( ext{Fe}^{2+} \) ) typically produce a pale green color.
  • Blue Colors: Vanadium(II) ions ( \( ext{VO}^{2+} \) ) can result in blue solutions as well.
  • Very Pale Pink Colors: Manganese(II) ions ( \( ext{Mn}^{2+} \) ) yield a very pale pink color.
The various possible colors of solutions are not only beautiful but are also used as a rich source of information about the chemistry and structure of the hydrated ions.
Transition Metal Ions
Transition metal ions are at the heart of why some solutions appear colored and are an important topic in inorganic chemistry. These metals, which include elements such as copper, iron, and vanadium, are characterized by d electrons that aren't filled in their atomic structure.
  • D-Electron Configurations: The d-electron configuration plays a crucial role. It affects how light interacts with and is absorbed by these ions.
  • Formation of Complexes: In aqueous solutions, transition metals often form complex ions. The specific structure and electronic configuration of these complexes are instrumental in determining the color.
  • Metal-Ligand Interaction: The interaction between metal ions and water molecules or other ligands can cause differences in color due to changes in energy levels. This is called ligand field splitting.
The presence of partially filled d-orbitals is what gives transition metal ions the flexibility to form a variety of strongly-colored ions. Understanding these principles can help predict the outcomes and interactions in chemical reactions.
Electronic Configurations
Electronic configuration is a fundamental concept in understanding the behavior of atoms and ions, especially transition metals, in inorganic chemistry. It refers to the distribution of electrons among the atomic or molecular orbitals. The configuration has a direct impact on the color we observe in solutions.
  • The D-Block: Transition metals are distinguished from others by their d-block electron configurations. The d-orbital electrons play a significant role in determining the chemical properties, including color.
  • Electron Excitation: When light hits the solution, electrons may be excited to a higher energy level within the d-orbitals. This process is what creates an observable color, as different wavelengths of light are absorbed and reflected.
  • Energy Level Differences: Slight differences in energy levels of the d-orbitals caused by external factors like ligand type and arrangement lead to varying colors.
By mastering electronic configurations, one can predict and explain many properties of transition metal compounds, including why some are brightly colored while others remain subdued.
Inorganic Chemistry
Inorganic chemistry investigates the properties and behavior of inorganic compounds, including metals, minerals, and organometallics. Transition metals, with their complex structures and vivid colors, are a key area of study within this field.
  • Ligand Field Theory: A crucial theory in inorganic chemistry, it helps explain the colors and magnetic properties of inorganic compounds by focusing on the effect of ligands on metal ion d-orbitals.
  • Complex Ion Formation: Transition metal ions can form complex ions by coordinating with multiple ligands. The chemistry and symmetry of these complexes are central themes in inorganic chemistry.
  • Color and Coordination Compounds: The color of coordination compounds, a major study topic, is influenced by the transition metal鈥檚 electronic configuration and the ligand's properties.
  • Reactivity and Applications: These aspects explore how inorganic compounds react under various conditions, providing insights into their practical applications in industries such as electronics and materials manufacturing.
Through inorganic chemistry, the principles of transition metal ions, solution color, electronic configuration, and complex formation come together to explain a wide range of natural phenomena and industrial processes.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of these pair does not represent any type of constitutional isomerism here? (a) \(\left[\mathrm{Co}\left(\mathrm{N} 1 \mathrm{I}_{3}\right), \mathrm{Br}\right] \mathrm{SO}_{1}\) and \(\left[\mathrm{Co}\left(\mathrm{N} 1 \mathrm{l}_{3}\right)_{5} \mathrm{SO}_{1}\right] \mathrm{Br}\) (b) \(\left[\mathrm{CrCl}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}\right] \mathrm{Cl}_{2} \cdot \mathrm{H}_{2} \mathrm{O}\) and \(\left[\mathrm{CrCl}_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right]\) \(\mathrm{Cl}_{2} \mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{Cis}-\left[\mathrm{CrCl}_{2}(\mathrm{Ox})\right]^{3}\) and rrans-[CrCl \(_{2}\) \(\left.(\mathrm{Ox})_{2}\right]^{3}\) (d) \(\left[\operatorname{Pr}\left(\mathrm{NII}_{3}\right)_{4}\right](\mathrm{PtCl})\) and \(\left[\operatorname{Pr}\left(\mathrm{N} 1 \mathrm{I}_{3}\right)_{4} \mathrm{Cl}_{2}\right]\) \(\left(\operatorname{PrCl}_{4}\right)\)

The numbcr of ions procluces from onc molccule of \(\left[\mathrm{Pr}\left(\mathrm{N} \mathrm{I} \mathrm{I}_{3}\right)_{5} \mathrm{Br}\right] \mathrm{Br}_{3}\) in the aqucous solution will he (a) 4 (b) 5 (c) 6 (d) 7

Which of rhe following can show gcomerrical isomerism? (a) \(\left[\mathrm{Cr}(\mathrm{O} \mathrm{x})_{3}\right]^{3-}\) (b) \(\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (c) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{CI}_{2}\right] \mathrm{I}\) (d) \(\left[\mathrm{NiCl}_{4}\right]^{--}\) 0

Which of the following srarcment is/arc corrocr? (a) In \(\mathrm{K}_{3}\left[\mathrm{~F} \mathrm{C}(\mathrm{CN})_{e}\right]\), the ligand has sar isficd borh primary and sccondary valcncies of ferric ion. (b) In \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) the ligand has satisfied only the secondary valency of fertic ion. (c) In \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) the ligand has satisfied both primary and secondary valencies of ferrous ion. (d) In [Cu(NH \(\left.y_{4}\right] \mathrm{SO}_{4}\), the ligatid has satisfied only the secotidary valency of copper.

Column I \(\quad\) Column II A. Coloured ion (p) \(\mathrm{Cu}\) B. \(\mu=1.73 \mathrm{~B} . \mathrm{M}\). (c) \(\mathrm{Cu}^{2+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.