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Chapter 9: Problem 23

Which one of the following is a correct representation of tetraamminecopper(II) hexacyanoferrate(II)? (a) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{2}\) (b) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{2}\) (c) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (d) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\)

Short Answer

Expert verified
\(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{2}\) is the correct representation of tetraamminecopper(II) hexacyanoferrate(II).

Step by step solution

01

Understand the Components

Tetraamminecopper(II) refers to a copper ion with a charge of +2 that is coordinated to four ammonia (NH3) molecules. Hexacyanoferrate(II) refers to an iron ion with a charge of +2 that is coordinated to six cyanide (CN) ions.
02

Determine the Correct Charge Balance

To determine the correct formula, we must ensure that the charges are balanced. Since tetraamminecopper(II) has a charge of +2, and hexacyanoferrate(II) has a charge of -4, we need three tetraamminecopper(2+) ions to balance the charge of two hexacyanoferrate(2–) ions.
03

Identify the Correct Formula

The correct representation of tetraamminecopper(II) hexacyanoferrate(II) must have a 3:2 ratio between the copper and iron complexes to achieve charge balance. The only formula with this ratio is \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{2}\).

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Key Concepts

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

Complex Ion Charge Balance
Understanding the charge balance within complex ions is crucial for chemistry students. Complex ions are species formed from a central metal ion surrounded by ligands, which are molecules or ions that donate a pair of electrons to the metal ion. The charge of the complex ion is the sum of the charge of the metal ion and the charges on its ligands.
Coordination Compounds
Coordination compounds feature a unique combination of molecules or ions bound to a central metal ion. These compounds are pervasive in nature and technology—offering varied applications from vibrant pigments to biological enzymes. The nature of the bond between the metal and its ligands is coordinate covalent, where both electrons in the bond originate from the same atom or molecule—specifically the ligand.
Chemical Nomenclature
Chemical nomenclature is like the language of chemistry, and it follows a set of rules to ensure that each compound has a unique, globally recognized name. The International Union of Pure and Applied Chemistry (IUPAC) creates the nomenclature standards that provide systematic ways to name chemical substances. These rules encompass all types of chemicals, including coordination compounds.
NEET Chemistry Preparation
The National Eligibility cum Entrance Test (NEET) is a preeminent exam for students in India aiming to pursue medical sciences. Chemistry, one of the key subjects in NEET, demands a deep understanding of principles, formulas, and their applications. Preparing for this subject involves a structured approach focusing on Physical, Organic, and Inorganic chemistry.

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Most popular questions from this chapter

In which of the following pairs, the EAN of the central metal atom is not the same? (a) \(\left[\mathrm{FeF}_{6}\right]^{3+}\) and \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) (b) \(\left[\mathrm{Fe}\left(\mathrm{CN}_{6}\right)\right]^{3-}\) and \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}\) (c) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) and \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{3-}\) (d) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) and \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

The complex with spin-only magnetic moment of \(\sim\) \(4.9\) B.M. is (a) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3+}\) (b) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) (d) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\)

The value of 'spin only' magnetic moment for one of the following configurations is \(2.84 \mathrm{BM}\). The correct one is: (a) \(\mathrm{d}^{4}\) (in strong ligand field) (b) \(\mathrm{d}^{4}\) (in weak ligand field) (c) \(\mathrm{d}^{3}\) (in weak as well as in strong fields) (d) \(\mathrm{d}^{5}\) (in strong ligand field)

The correct order of magnetic moments (spin only values in B.M.) among the following is: (Atomic number of \(\mathrm{Mn}=25, \mathrm{Fe}=26, \mathrm{Co}=27\) ) (a) \(\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) (b) \(\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}>\left[\mathrm{CoCl}_{4}\right]^{2-}\) (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}>\left[\mathrm{MnCl}_{4}\right]^{2-}>\left[\mathrm{CoCl}_{4}\right]^{2-}\) (d) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}>\left[\mathrm{CoCl}_{4}\right]^{2-}>\left[\mathrm{MnCl}_{4}\right]^{2-}\)

Which of the following will exhibit geometrical isomerism? (M stands for a metal, and a and \(b\) are achiral ligands, (1) \(\mathrm{Ma}_{2} \mathrm{~b}_{2}\) (2) \(\mathrm{Ma}_{4} \mathrm{~b}_{2}\) (3) \(\mathrm{Ma}_{5} \mathrm{~b}\) (4) \(\mathrm{Ma}_{6}\) (a) 1 and 2 (b) 2 and 3 (c) 1 and 3 (d) 2 and 4
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