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Chapter 16: Problem 61

Write equations for the stepwise formation of each of the following complex ions. a. \(\mathrm{Ni}(\mathrm{CN})_{4}^{2-}\) $$ \text { b. } \mathrm{V}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}{ }^{3-} $$

Short Answer

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Short Answer: The stepwise formation equations for the complex ions are as follows: a. Ni(CN)鈧劼测伝 : 1. Ni虏鈦 + CN鈦 鈫 NiCN虏鈦 2. NiCN虏鈦 + CN鈦 鈫 Ni(CN)鈧偮斥伝 3. Ni(CN)鈧偮斥伝 + CN鈦 鈫 Ni(CN)鈧冣伌鈦 4. Ni(CN)鈧冣伌鈦 + CN鈦 鈫 Ni(CN)鈧劼测伝 b. V(C鈧侽鈧)鈧兟斥伝 : 1. V鲁鈦 + C鈧侽鈧劼测伝 鈫 VC鈧侽鈧勨伜 2. VC鈧侽鈧勨伜 + C鈧侽鈧劼测伝 鈫 V(C鈧侽鈧)鈧傗伝 3. V(C鈧侽鈧)鈧傗伝 + C鈧侽鈧劼测伝 鈫 V(C鈧侽鈧)鈧兟斥伝

Step by step solution

01

Identify the central metal ion and ligands

In this complex ion, the central metal ion is Ni虏鈦 (nickel ion) and the ligand is the CN鈦 ion (cyanide ion). There are 4 CN鈦 ions surrounding the Ni虏鈦 ion.
02

Write the stepwise formation equations for the complex ion

Now we will write the equations for the formation of the Ni(CN)鈧劼测伝 complex ion as the CN鈦 ions progressively bind to the Ni虏鈦 ion. 1. Ni虏鈦 + CN鈦 鈫 NiCN虏鈦 2. NiCN虏鈦 + CN鈦 鈫 Ni(CN)鈧偮斥伝 3. Ni(CN)鈧偮斥伝 + CN鈦 鈫 Ni(CN)鈧冣伌鈦 4. Ni(CN)鈧冣伌鈦 + CN鈦 鈫 Ni(CN)鈧劼测伝 b. V(C鈧侽鈧)鈧兟斥伝
03

Identify the central metal ion and ligands

In this complex ion, the central metal ion is V鲁鈦 (vanadium ion) and the ligand is the C鈧侽鈧劼测伝 ion (oxalate ion). There are 3 C鈧侽鈧劼测伝 ions surrounding the V鲁鈦 ion.
04

Write the stepwise formation equations for the complex ion

Now we will write the equations for the formation of the V(C鈧侽鈧)鈧兟斥伝 complex ion as the C鈧侽鈧劼测伝 ions progressively bind to the V鲁鈦 ion. 1. V鲁鈦 + C鈧侽鈧劼测伝 鈫 VC鈧侽鈧勨伜 2. VC鈧侽鈧勨伜 + C鈧侽鈧劼测伝 鈫 V(C鈧侽鈧)鈧傗伝 3. V(C鈧侽鈧)鈧傗伝 + C鈧侽鈧劼测伝 鈫 V(C鈧侽鈧)鈧兟斥伝 These are the stepwise formation equations for the given complex ions.

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Key Concepts

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

Stepwise Formation
Stepwise formation is an important concept in chemistry, particularly when studying the creation of complex ions. To understand it, let's imagine we are assembling a complex ion piece by piece. Each piece represents a ligand attaching to a central metal ion. With stepwise formation, each ligand joins in a separate and distinct step.
This process is simple when broken down:
  • The first step involves the combination of a central metal ion with one ligand.
  • In subsequent steps, additional ligands attach to this initial metal-ligand assembly.
Think of it as attaching more pieces to a central core until the complete ion is formed. This methodical process allows chemists to understand how complex ions are built and how each part contributes to the ion's overall stability and characteristics.
Ligands
Ligands are fundamental in the formation of complex ions, serving as the attachments or 'arms' that bind to central metal ions. They are atoms or molecules that donate electrons to form a coordinate bond with the metal ion.
Ligands can vary greatly:
  • They range from simple ions like CN鈦 (cyanide) to larger molecules like C鈧侽鈧劼测伝 (oxalate).
  • Each ligand has a specific number of sites to attach or bind, determining its classification as unidentate (bonding at one site), bidentate (two sites), or polydentate (multiple sites).
This ability to bind gives ligands their role in stabilizing metal ions and affecting properties like color and reactivity of the complexes they form. In complex ion formation, selecting the right ligand is crucial for determining the characteristics of the final compound.
Coordination Chemistry
Coordination chemistry studies compounds made from a central metal atom or ion surrounded by molecules or ions called ligands. The field examines how these bonds form and the properties that result.
Key concepts include:
  • Coordinate bonds, also known as dative covalent bonds, are formed when a ligand donates a pair of electrons to the metal ion.
  • The coordination number is the number of ligand donor atoms attached to the central metal ion, influencing the structure and shape of the complex.
This branch of chemistry plays a crucial role in understanding biochemical processes and industrial applications, providing insights into the behavior and stability of various metal complexes.
Metal Ions
Metal ions are at the heart of complex ion formation, serving as the central entity to which ligands attach. These ions usually come from transition metals, known for their ability to form stable complexes.
Metal ions possess distinct properties:
  • These properties include variable oxidation states and the ability to form colored compounds.
  • They can accept electrons from ligands to establish bonds, making them versatile in forming diverse structures.
Understanding metal ions' behavior is vital for predicting how they will interact with ligands, influencing the resulting compound's stability and functionality.

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Most popular questions from this chapter

\(\mathrm{Ag}_{2} \mathrm{~S}(s)\) has a larger molar solubility than CuS even though \(\mathrm{Ag}_{2} \mathrm{~S}\) has the smaller \(K_{\mathrm{sp}}\) value. Explain how this is possible.

Calculate the solubility (in moles per liter) of \(\mathrm{Fe}(\mathrm{OH})_{3}\) \(\left(K_{\mathbb{\infty}}=4 \times 10^{-3 \mathrm{~s}}\right)\) in each of the following. a. water b. a solution buffered at \(\mathrm{pH}=5.0\) c. a solution buffered at \(\mathrm{pH}=11.0\)

Describe how you could separate the ions in each of the following groups by selective precipitation. a. \(\mathrm{Ag}^{+}, \mathrm{Mg}^{2+}, \mathrm{Cu}^{2+}\) c. \(\mathrm{Pb}^{2+}, \mathrm{Bi}^{3+}\) b. \(\mathrm{Pb}^{2+}, \mathrm{Ca}^{2+}, \mathrm{Fe}^{2+}\)

A solution is prepared by mixing \(100.0 \mathrm{~mL}\) of \(1.0 \times 10^{-2} M\) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) and \(100.0 \mathrm{~mL}\) of \(1.0 \times 10^{-3} M \mathrm{NaF}\). Will \(\mathrm{PbF}_{2}(s)\) \(\left(K_{\text {sp }}=4 \times 10^{-8}\right)\) precipitate?

Calculate the equilibrium concentrations of \(\mathrm{NH}_{3}, \mathrm{Cu}^{2+}\), \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)^{2+}, \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{2}^{2+}, \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{3}^{2+}\), and \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}{ }^{2+}\) in a solution prepared by mixing \(500.0 \mathrm{~mL}\) of \(3.00 \mathrm{M} \mathrm{NH}_{3}\) with \(500.0 \mathrm{~mL}\) of \(2.00 \times 10^{-3} M \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\). The stepwise equilib- ria are \(\mathrm{Cu}^{2+}(a q)+\mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{CuNH}_{3}^{2+}(a q)\) \(K_{1}=1.86 \times 10^{4}\) \(\mathrm{CuNH}_{3}{ }^{2+}(a q)+\mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{2}^{2+}(a q)\) \(K_{2}=3.88 \times 10^{3}\) \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{2}{ }^{2+}(a q)+\mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{3}^{2+}(a q)\) \(K_{3}=1.00 \times 10^{3}\) \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{3}{ }^{2+}(a q)+\mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}{ }^{2+}(a q)\) \(K_{4}=1.55 \times 10^{2}\)
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