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2: Atomic Structure

Last updated

Mar 19, 2021
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- 1.5: Practice problems
- 2.1: Historical Development of Atomic Theory

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2.1: Historical Development of Atomic Theory
- 2.1.1: The Periodic Table
- 2.1.2: Discovery of Subatomic Particles and the Bohr Atom
2.2: The Schrödinger equation, particle in a box, and atomic wavefunctions
This page discusses the development of quantum mechanics by Erwin Schr??dinger and Werner Heisenberg, focusing on the dual nature of electrons exhibiting both wave and particle properties. The Schr??dinger Equation is introduced as a fundamental equation describing electron behavior, incorporating terms for kinetic and potential energy through the Hamiltonian operator.
2.3: Periodic Properties of Atoms
General periodic trends on the periodic table include patterns in properties like electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. These trends help chemists predict an element's properties due to similar atomic structures within element group families or periods. Ionization energy, for instance, is the energy needed to remove an electron from a gaseous atom or cation, and is a key trend described.
2.4: Problems
The page provides a series of exercises that test understanding of periodic table trends such as ionization energy, atomic radius, electronegativity, and electron affinity. It includes specific questions asking to identify elements with the highest ionization energy, larger atomic radius, and more electronegativity between given elements. Additionally, it explores concepts like noble gas stability and orders elements by electron affinity.

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