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Chapter 23: Problem 38

Give the coordination number of the transition element in each of the following complexes. a. \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]\left(\mathrm{ClO}_{3}\right)_{2}\) b. \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) c. \(\left[\mathrm{Cr}(\mathrm{en})_{3}\right] \mathrm{Cl}_{3}\) d. \(\mathrm{K}_{2}\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]\)

Short Answer

Expert verified
Coordination numbers: a) 6, b) 4, c) 6, d) 4.

Step by step solution

01

Understand Coordination Number

The coordination number is the number of ligand donor atoms directly bonded to the central metal atom in a complex. Each ligand in a complex can donate one or more pairs of electrons to form coordinate bonds.
02

Determine for Complex a

For \[\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]\left(\mathrm{ClO}_{3}\right)_{2},\]Nickel (Ni) is coordinated with six ammonia (NH鈧�) molecules. Each NH鈧� provides one nitrogen atom that coordinates with the nickel, making the coordination number 6.
03

Determine for Complex b

For \[\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4},\]Copper (Cu) is coordinated with four ammonia (NH鈧�) molecules. Each NH鈧� provides one nitrogen atom coordinated to the copper, giving a coordination number of 4.
04

Determine for Complex c

For \[\left[\mathrm{Cr}(\mathrm{en})_{3}\right] \mathrm{Cl}_{3},\]Chromium (Cr) is coordinated with three ethylenediamine (en) ligands. Each en provides two nitrogen donor atoms per ligand, so the coordination number is 3 脳 2 = 6.
05

Determine for Complex d

For \[\mathrm{K}_{2}\left[\mathrm{Ni}(\mathrm{CN})_{4}\right],\]Nickel (Ni) is coordinated with four cyanide (CN) ions. Each CN is a monodentate ligand providing one donor atom, resulting in a coordination number of 4.

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Key Concepts

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

Coordination Number
The coordination number is a foundational concept in coordination chemistry, crucial for understanding the structure and reactivity of metal complexes. It refers to the number of ligand donor atoms that are directly bonded to the central metal ion in a coordination complex. Simply put, it is the count of connections each metal ion makes with ligand atoms via coordinate bonding.
  • For example, if a metal ion is surrounded by six ammonia molecules, its coordination number is six, because each ammonia donates one pair of electrons to the metal.
  • The coordination number is not fixed and can range from 2 to 12, with 4 and 6 being the most common in these complexes.
  • Understanding coordination number helps predict geometrical structure, which influences the properties and function of the complex.
In complexes like \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]\left(\mathrm{ClO}_{3}\right)_{2}\), the nickel has a coordination number of six due to six ligands coordinating with the metal ion.
Transition Metals
Transition metals are the elements found in the d-block of the periodic table. They include familiar metals such as iron, copper, and nickel, which play a key role in forming coordination complexes. These metals have unique properties:
  • They have partially filled d-orbitals, enabling them to form complex structures with various ligands.
  • Transition metals can exhibit multiple oxidation states, making them versatile in chemical reactions.
  • They often display beautiful colors in their compounds due to d-d electron transitions.
In coordination chemistry, transition metals have the ability to bind to ligands via their d-orbitals, allowing for diverse and stable complex geometries. Their ability to easily donate and accept electrons makes them invaluable in biological systems and industrial catalysts.
Ligands
Ligands are molecules or ions that bind to the central metal in a coordination complex via coordinate bonds. These entities donate a lone pair of electrons to the metal atom, forming a coordinate covalent bond. Here are some important points about ligands:
  • Ligands can vary in size and charge, from small molecules like water and ammonia to larger entities like ethylenediamine (\(\mathrm{en}\)).
  • Ligands are classified based on the number of donor atoms: monodentate (one donor atom) and bidentate (two donor atoms), as seen in \(\left[\mathrm{Cr}(\mathrm{en})_{3}\right] \mathrm{Cl}_{3}\) where ethylenediamine acts as a bidentate ligand.
  • Bidentate and polydentate ligands form chelates with the metal, resulting in more stable complexes due to the chelate effect.
The arrangement and type of ligands strongly influence the properties and functions of the coordination complex.
Coordinate Bonding
Coordinate bonding is a type of chemical bond where one atom provides both electrons to form the bond, as opposed to a regular covalent bond where each atom supplies an electron. In coordination chemistry, ligands form coordinate bonds with the central metal ion. This interaction is fundamental to the stability and characteristics of coordination compounds.
  • Coordinate bonds are formed when ligands, like ammonia or cyanide, donate a pair of electrons to a metal ion.
  • These bonds are just as strong as covalent bonds and can create complex geometrical arrangements around the metal.
  • This type of bonding is responsible for the formation of stable structures like \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{SO}_{4}\) and \(\mathrm{K}_{2}\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]\).
The nature of coordinate bonds allows transition metals to expand their coordination sphere, making them versatile and crucial for biological and synthetic processes.

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Most popular questions from this chapter

Define the terms complex ion, ligand, and coordination number. Use an example to illustrate the use of these terms.

Palladium and platinum are very similar to one another. Both are unreactive toward most acids. However, nickel, which is in the same column of the periodic table, is an active metal. Explain why this difference exists.

Find the concentrations of \(\mathrm{Ag}^{+}(a q), \mathrm{NH}_{3}(a q)\), and \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q)\) at equilibrium when \(0.10 \mathrm{~mol} \mathrm{Ag}^{+}(a q)\) and \(0.10 \mathrm{~mol} \mathrm{NH}_{3}(a q)\) are made up to \(1.00 \mathrm{~L}\) of solution. The dissociation constant, \(K_{d}\), for the complex \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\) is \(5.9 \times 10^{-8}\)

Draw cis-trans structures of any of the following square planar or octahedral complexes that exhibit geometric isomerism. Label the drawings cis or trans. a. \(\left[\mathrm{Pd}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]\) b. \(\mathrm{Pd}\left(\mathrm{NH}_{3}\right){ }_{3} \mathrm{Cl}^{+}\) c. \(\mathrm{Pd}\left(\mathrm{NH}_{3}\right)_{4}^{2}+\) d. \(\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}^{+}\)

Describe step by step how the name potassium hexacyanoferrate(II) leads to the structural formula \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\)
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