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Ch.1 - Chemical Tools: Experimentation & Measurement

Ch.2 - Atoms, Molecules & Ions

Ch.3 - Mass Relationships in Chemical Reactions

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BONUS: Mathematical Operations and Functions

Ch.4 - Reactions in Aqueous Solution

Ch.5 - Periodicity & Electronic Structure of Atoms

Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory

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Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure

Ch.9 - Thermochemistry: Chemical Energy

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Ch.11 - Liquids & Phase Changes

Ch.12 - Solids and Solid-State Materials

Ch.13 - Solutions & Their Properties

Ch.14 - Chemical Kinetics

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Ch.16 - Aqueous Equilibria: Acids & Bases

Ch.17 - Applications of Aqueous Equilibria

Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium

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Chapter 5, Problem 124

Orbital energies in single-electron atoms or ions, such as He+, can be described with an equation similar to the Balmer–Rydberg equation:
where Z is the atomic number. What wavelength of light in nanometers is emitted when the electron in He+ falls from n = 3 to n = 2?

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Chapter 5, Problem 124

Orbital energies in single-electron atoms or ions, such as He+, can be described with an equation similar to the Balmer–Rydberg equation: where Z is the atomic number. What wavelength of light in nanometers is emitted when the electron in He+ falls from n = 3 to n = 2?

Orbital energies in single-electron atoms or ions, such as He+, can be described with an equation similar to the Balmer–Rydberg equation:
where Z is the atomic number. What wavelength of light in nanometers is emitted when the electron in He+ falls from n = 3 to n = 2?