Question

What does a low fusion enthalpy for a solid tell you about the solid (its bonding or type)?

Short answer

A low fusion enthalpy suggests weak bonding, typically in molecular or low-lattice-energy ionic solids.

Step-by-step solution

Understanding Fusion Enthalpy

Fusion enthalpy, also known as the enthalpy of fusion, is the amount of energy needed to change a substance from a solid to a liquid at its melting point. It is usually measured in kilojoules per mole (kJ/mol). A low fusion enthalpy indicates that less energy is required to change the solid into a liquid.

Relating Fusion Enthalpy to Bonding

The amount of energy required for fusion depends on the strength of the bonds between the atoms or molecules in the solid. A low fusion enthalpy suggests that the bonds holding the solid together are not very strong, making it easier for the solid to melt.

Identifying the Type of Bonding

Solids with low fusion enthalpy often have weaker intermolecular forces or ionic bonds. These might include molecular solids with van der Waals forces or ionic compounds with low lattice energy. In contrast, solids with strong covalent or metallic bonds generally have higher fusion enthalpies.

Key concepts

Bonding in Solids

When discussing solids, bonding plays a crucial role in determining their properties. Solids are structures where atoms or molecules are closely packed, and the type of bonding present affects characteristics such as melting point, hardness, and more. The bonding can be broadly classified into several types:

• Ionic Bonds: Formed between metals and non-metals, involving the transfer of electrons. They create a lattice structure that can have variable strength depending on the lattice energy.
• Covalent Bonds: Found within molecular solids, where atoms share electron pairs. These can form strong networks, such as in diamond or silicon.
• Metallic Bonds: Consist of a 'sea of electrons' that are free to move, which explains the conductivity of metals.
• Van der Waals Forces: Weak attractions present in molecular solids, significant in molecules like iodine or noble gases.

Bonding type influences the fusion enthalpy, with weaker bonds like van der Waals often resulting in lower fusion enthalpies.

Intermolecular Forces

Intermolecular forces are the attractions that occur between molecules, influencing the physical properties of substances. These forces, while generally weaker than chemical bonds, play a critical role in determining the behavior of materials at different states, especially solids.

• Van der Waals Forces: These are weak forces that result from instantaneous dipole moments in molecules. They are critical in non-polar compounds and influence properties like boiling and melting points.
• Dipole-Dipole Interactions: Occur between molecules with permanent dipole moments, contributing to higher fusion enthalpies compared to nonpolar molecules.
• Hydrogen Bonding: A strong form of dipole interaction, significantly impacting the melting points of compounds like ice.

Intermolecular forces, especially in molecular solids, are primarily responsible for dictating the fusion enthalpy, with weaker forces correlating with lower values.

Ionic and Molecular Solids

Ionic and molecular solids differ significantly in their structures and bonding, which in turn affects their fusion enthalpy.

• Ionic Solids: Comprised of positive and negative ions held by strong electrostatic forces, like table salt. They often have high melting points due to significant lattice energy but can show low fusion enthalpy if the lattice energy is distributed over many atoms.
• Molecular Solids: Made up of neutral molecules held together by intermolecular forces. Common examples include sugar or dry ice. These solids have lower melting points and fusion enthalpies due to weaker van der Waals forces.

Understanding these differences aids in predicting and explaining the physical properties of materials, with ionic solids generally showing more robust structuring compared to molecular solids.