Which type (or types) of crystalline solid is characterized by each of the following? (c) high melting point and poor electrical conductivity;

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Identify the types of crystalline solids: molecular, ionic, covalent network, and metallic.

Consider the properties of each type: molecular solids have low melting points and are poor conductors; ionic solids have high melting points and conduct electricity when molten; covalent network solids have high melting points and are poor conductors; metallic solids have variable melting points and are good conductors.

Focus on the given properties: high melting point and poor electrical conductivity.

Match these properties to the type of crystalline solid: covalent network solids are known for having high melting points and being poor conductors of electricity.

Conclude that the type of crystalline solid characterized by a high melting point and poor electrical conductivity is a covalent network solid.

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Key Concepts

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

Types of Crystalline Solids

Crystalline solids can be categorized into several types based on the nature of the bonding and the arrangement of their constituent particles. The main types include ionic, covalent network, metallic, and molecular solids. Each type exhibits distinct physical properties, such as melting points and electrical conductivity, which are influenced by the strength and type of interactions between the particles.

Ionic Solids

Ionic solids are formed from the electrostatic attraction between positively and negatively charged ions. They typically have high melting points due to the strong ionic bonds that require significant energy to break. However, in their solid state, ionic solids do not conduct electricity, as the ions are fixed in place and cannot move freely, making them poor electrical conductors.

Covalent Network Solids

Covalent network solids consist of atoms connected by a network of covalent bonds, forming a rigid structure. Examples include diamond and silicon carbide, which exhibit very high melting points due to the strength of the covalent bonds. Like ionic solids, covalent network solids also lack free-moving charged particles in their solid state, resulting in poor electrical conductivity.

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