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Chapter 18: Problem 7

How does the electron structure of an isolated atom differ from that of a solid material?

Short Answer

Expert verified
Based on the given step by step solution, compare the electron structure of an isolated atom with that of a solid material. The electron structure of an isolated atom consists of electrons organized in discrete energy levels or atomic orbitals (s, p, d, or f), according to the Aufbau Principle. In contrast, the electron structure in a solid material consists of energy bands formed due to the overlap of atomic orbitals between neighboring atoms. The electron distribution in an isolated atom is confined to individual atomic orbitals, while in a solid material, it is delocalized across the entire material, populating continuous energy bands. This difference affects bonding and properties, as isolated atoms have electrons localized around the nucleus with no bonds, while solid materials have various types of bonding (ionic, covalent, or metallic), leading to distinct properties like electrical conductivity, magnetism, or hardness.

Step by step solution

01

Understanding the Electron Structure of an Isolated Atom

An isolated atom has electrons organized in discrete energy levels, known as atomic orbitals. The electrons in an atom fill these orbitals according to the Aufbau Principle, starting with the lowest energy level. The atomic orbitals are designated as s, p, d, or f, corresponding to the different shapes and characteristics of these electron clouds.
02

Understanding the Electron Structure of a Solid Material

In a solid material, atoms are not isolated; they are closely bound together, forming a crystal lattice or a more disordered structure (e.g., amorphous materials). In these materials, the electron structure transforms from atomic orbitals to energy bands. This is a result of the overlap of atomic orbitals between neighboring atoms, creating new energy levels that form a continuous energy band where electrons can occupy.
03

Comparing the Electron Distributions

In an isolated atom, electrons are confined to individual atomic orbitals, while in a solid material, electrons are delocalized across the entire material, populating energy bands made up of closely spaced energy levels. This significant difference affects the electron distribution in the two cases. Specifically, solid materials can have partially filled energy bands, allowing them more freedom to move and contributing to the electrical conductivity of the material. In contrast, isolated atoms have discrete energy levels, and electrons cannot move easily between them.
04

Explaining Differences in Bonding and Properties

The difference between electron structure in isolated atoms and solid materials also explains the variation in their bonding and properties. In an isolated atom, electrons are localized around the nucleus, and no bonds with other atoms are formed. On the other hand, solid materials have various types of bonding such as ionic, covalent, or metallic bonding, which depend on the electron distribution within the energy bands. This difference in bonding leads to various properties in solid materials, such as electrical conductivity, magnetism, or hardness, which cannot be found in isolated atoms.

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