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Chapter 23: Problem 35

Describe the makeup of a complex ion, including the nature of the ligands and their interaction with the central metal ion. Explain how a complex ion can be positive or negative and how it occurs as part of a neutral coordination compound.

Short Answer

Expert verified
A complex ion consists of a central metal ion bonded to ligands via coordinate bonds. The overall charge of the complex ion is the sum of the charges of the metal ion and the ligands. Complex ions form neutral compounds by combining with counter ions.

Step by step solution

01

Identifying the Central Metal Ion

A complex ion consists of a central metal ion. Identify this metal ion by noting the element symbol and its charge. This metal is usually a transition metal.
02

Choosing the Ligands

Ligands are ions or molecules that donate electrons to the metal ion to form coordinate bonds. Recognize the ligands in your complex ion, noting their type (neutral or anionic) and how many bond sites they have (e.g., monodentate, bidentate).
03

Forming Coordinate Bonds

Each ligand donates at least one pair of electrons to the central metal ion to form a coordinate bond. Describe the nature of these coordinate bonds and how electron donation from ligands stabilizes the metal ion.
04

Determining the Charge of the Complex Ion

Sum the charges of the central metal ion and all the ligands to find the overall charge of the complex ion. This charge can be positive, negative, or zero.
05

Neutral Coordination Compounds

Complex ions can combine with counter ions so that the entire molecule is electrically neutral. Explain how adding counter ions with opposite charges to the complex ion results in a neutral coordination compound.

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Key Concepts

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

central metal ion
In complex ion chemistry, the central metal ion serves as the core around which the rest of the structure is built. It is typically a transition metal like iron (Fe), copper (Cu), or nickel (Ni). Transition metals are commonly used because they have empty orbitals that can accept electron pairs.
The central metal ion can have various oxidation states, which are indicated by its charge. This charge is key in determining the stability and reactivity of the resulting complex ion. Understanding the central metal ion is the first step in analyzing any complex ion as it dictates the bonding and interaction with ligands.
ligands
Ligands are ions or molecules that donate electron pairs to the central metal ion, forming coordinate bonds. They act as Lewis bases, which means they are electron pair donors. Some common ligands include water \((H_2O)\), ammonia \((NH_3)\), chloride \((Cl^-)\), and cyanide \((CN^-)\).
Ligands can be classified based on how many donor sites they have. For example:
  • Monodentate ligands: These donate one pair of electrons. Examples are \((H_2O)\) and \((NH_3)\).
  • Bidentate ligands: These donate two pairs of electrons from two different atoms. An example is ethylenediamine \((en)\).
  • Polydentate ligands: These donate electron pairs from multiple sites. An example is ethylenediaminetetraacetate (EDTA).
Understanding ligands and their interactions is crucial for interpreting the structure and behavior of complex ions.
coordinate bonds
Coordinate bonds, also known as dative covalent bonds, are formed when a ligand donates a pair of electrons to the central metal ion. This type of bonding is special because both electrons in the bond come from the ligand, not one from each partner as in typical covalent bonds.
These bonds are crucial for the stability of the complex ion. The strength and number of coordinate bonds influence both the geometry and the overall stability of the complex. For example:
  • Six coordinate bonds typically form octahedral structures.
  • Four coordinate bonds can create either tetrahedral or square planar structures.
Understanding how coordinate bonds work helps in predicting the shape and properties of a complex ion.
charge determination
Determining the overall charge of a complex ion is a necessary step to fully understand its properties. This is achieved by summing the charges of the central metal ion and all the ligands attached to it.
For example, if the central metal ion has a charge of +3 and it is bonded to three chloride ligands \((Cl^-)\), the total charge of the complex ion would be \(+3 + (-1 \times 3) = 0\). Thus, the complex ion is neutral. The charge can be positive, negative, or zero based on this calculation.
neutral coordination compounds
A neutral coordination compound is formed when a complex ion associates with counter ions of opposite charge to balance out the overall charge. The resulting molecule is electrically neutral.
For example, consider the complex ion \[Cu(NH_3)_4^{2+}\]. To neutralize this, you could add two sulfate ions \[(SO_4^{2-})\], resulting in the compound \[Cu(NH_3)_4SO_4\], which is neutral.
Understanding the concept of neutral coordination compounds is essential for balancing equations and predicting the solubility and reactivity of these molecules in different environments.

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Most popular questions from this chapter

For any of the following that can exist as isomers, state the type of isomerism and draw the structures: (a) \(\left[\mathrm{Zn}(\mathrm{en}) \mathrm{F}_{2}\right]\) (b) \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)\left(\mathrm{NH}_{3}\right) \mathrm{FCl}\right]\) (c) \(\left[\mathrm{Pd}(\mathrm{CN})_{2}(\mathrm{OH})_{2}\right]^{2-}\)

Criticize and correct the following statement: strong-field ligands always give rise to low-spin complexes.

Give formulas corresponding to the following names: (a) Tetraamminezinc sulfate (b) Pentaamminechlorochromium(III) chloride (c) Sodium bis(thiosulfato)argentate(I)

The actinides \(\mathrm{Pa}, \mathrm{U},\) and \(\mathrm{Np}\) form a series of complex ions, such as the anion in the compound \(\mathrm{Na}_{3}\left[\mathrm{UF}_{8}\right],\) in which the central metal ion has an unusual geometry and oxidation state. In the crystal structure, the complex ion can be pictured as resulting from interpenetration of simple cubic arrays of uranium and fluoride ions. (a) What is the coordination number of the metal ion in the complex ion? (b) What is the oxidation state of uranium in the compound? (c) Sketch the complex ion.

A shortcut to finding optical isomers is to see if the complex has a plane of symmetry-a plane passing through the metal atom such that every atom on one side of the plane is matched by an identical one at the same distance from the plane on the other side. Any planar complex has a plane of symmetry, since all atoms lie in one plane. Use this approach to determine whether these exist as optical isomers: (a) \(\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}\right]\) (tetrahedral); (b) \(\left[\mathrm{Pt}(\mathrm{en})_{2}\right]^{2+} ;\) (c) trans-[PtBr \(\left.\left._{4} \mathrm{Cl}_{2}\right]^{2-} ;\) (d) trans-[Co(en) \(\left._{2} \mathrm{~F}_{2}\right]^{+}\) (e) \(c i s-\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{~F}_{2}\right]^{+}\)
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