Which solid has the highest melting point? Why? C(s, diamond), Kr(s), NaCl(s), H₂O(s)

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Step 1: Understand the types of bonding present in each solid.

Step 2: Analyze the structure and bonding of diamond, C(s).

Step 3: Consider the nature of Kr(s) as a solid.

Step 4: Examine the ionic bonding in NaCl(s).

Step 5: Evaluate the hydrogen bonding in H2O(s).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Melting Point

The melting point is the temperature at which a solid becomes a liquid. It is influenced by the strength of the intermolecular or ionic forces holding the solid together. Substances with strong bonds, such as ionic or covalent networks, typically have higher melting points compared to those with weaker van der Waals forces.

Types of Solids

Solids can be categorized into different types, including ionic, covalent, molecular, and metallic solids. Ionic solids, like NaCl, consist of charged ions held together by strong electrostatic forces, while covalent solids, like diamond, have atoms connected by strong covalent bonds. Understanding the type of solid helps predict its melting behavior.

Crystal Structure

The arrangement of atoms in a solid, known as its crystal structure, plays a crucial role in determining its physical properties, including melting point. For example, diamond has a tetrahedral lattice structure that maximizes bond strength, leading to a very high melting point, while molecular solids like H2O have weaker hydrogen bonds, resulting in lower melting points.

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