Question

What is a hydrated compound? Use an example to illustrate your answer.

Short answer

A hydrated compound is a chemical compound that contains water molecules within its crystal lattice, forming coordination bonds with other atoms or ions. For example, copper(II) sulfate pentahydrate (CuSO4·5H2O) is a hydrated compound where each copper(II) sulfate ion is bound to five water molecules. The blue color of this compound is due to the presence of water molecules, and when these water molecules are removed, the white anhydrous copper(II) sulfate (CuSO4) is obtained.

Step-by-step solution

Define hydrated compound

A hydrated compound is a chemical compound that contains water molecules within its crystal lattice. The water molecules are bound to the other atoms or ions present in the compound, forming coordination bonds. These water molecules can be removed by heating or chemical reactions, leaving behind the anhydrous (or water-free) form of the compound.

Provide an example with an explanation

A common example of a hydrated compound is copper(II) sulfate pentahydrate, CuSO4·5H2O. In this compound, each copper(II) sulfate ion is surrounded by five water molecules. The blue color of copper(II) sulfate pentahydrate is due to the presence of these water molecules in its structure. When the water molecules are removed through heating or a chemical reaction, the anhydrous form is obtained, which is a white powder called anhydrous copper(II) sulfate, with the formula CuSO4.

Key concepts

Understanding Crystal Lattice in Hydrated Compounds

In chemistry, a crystal lattice is a three-dimensional arrangement of particles—these could be atoms, ions, or molecules—structured in a repeating pattern.
This pattern is the foundation that holds a solid together and determines how it looks and behaves. Hydrated compounds, which contain water molecules within this crystal lattice, illustrate this concept beautifully.
The water molecules are not randomly scattered but are systematically organized within the lattice framework.
For example, in copper(II) sulfate pentahydrate, the water molecules occupy specific positions in the lattice, ensuring the stability and unique properties of the compound.

• The organized structure ensures geometric stability.
• The lattice influences physical properties like color.
• This orderly pattern can be altered to remove water.

Understanding this concept is vital because, without the crystal lattice, the water molecules in hydrated compounds could not form stable arrangements essential for the compound's unique characteristics.

Exploring Coordination Bonds in Hydrated Compounds

Coordination bonds form when water molecules connect with the ions in a compound within the crystal lattice. These are a type of chemical bond that's particularly crucial in hydrates.
Typically, a metal ion serves as a center, coordinated with water molecules acting as ligands - which are molecules that donate electrons. For instance, in copper(II) sulfate pentahydrate, water molecules form coordination bonds with the copper ions. This interaction results in the metal being enveloped by these water molecules, creating a stable structure.

• Coordination bonds are more common in transition metal complexes.
• These bonds are directional, contributing to the geometric shape of the compound.
• They are pivotal for the physical attributes such as color changes.

This strong interaction between metal ions and water molecules in hydrated compounds is what defines their unique chemistry, differentiating them from compounds without such interactions.

Anhydrous Compounds: The Dehydrated Relatives

Anhydrous compounds are the dehydrated forms of hydrated compounds.
The term 'anhydrous' refers to substances that do not contain water molecules.
You can often produce an anhydrous form by heating a hydrated compound, a process that removes the water molecules embedded in the crystal lattice by breaking the coordination bonds.
Taking copper(II) sulfate as an example, the hydrated form is blue due to the water molecules embedded in it. Once heated, the water leaves, resulting in an anhydrous copper(II) sulfate—white in color.

• Heating or a chemical reaction can remove the water molecules.
• The process is often reversible, where rehydration restores the original water content.
• Anhydrous forms can possess different physical properties, such as color.

Anhydrous compounds serve various industrial and laboratory purposes, where the water-free form might be essential for reactions or for use as drying agents.