9: Electrons in Atoms and the Periodic Table
- Page ID
- 47423
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 9.2: Light- Electromagnetic Radiation
- This page explores the concepts of wavelength and frequency in the context of wave energy and electromagnetic radiation. It defines wavelength as the distance between points on a wave and frequency as the number of waves per unit time, highlighting their inverse relationship. Examples, including harmful UV B wavelengths from the sun, illustrate the significance of the speed of light in their connection, represented by the equation \(c = \lambda \nu\).
- 9.3: The Electromagnetic Spectrum
- This page covers the electromagnetic spectrum, detailing types of radiation from gamma rays to radio waves. It highlights the dangers of high-energy radiation like gamma rays, X-rays, and UV rays, while discussing the visible light spectrum relevant to human perception. The page explains color perception based on how different wavelengths are absorbed or reflected, and emphasizes the interplay between energy, frequency, and color in electromagnetic waves.
- 9.4: The Bohr Model - Atoms with Orbits
- This page explains the Bohr model of the atom, which details how electrons occupy defined energy levels around the nucleus and produce atomic spectra through energy absorption and emission. It connects these principles to real-world applications like light bulbs and neon signs, and concludes that while the atomic spectra support Bohr's model, it is mainly applicable for calculating energy levels in hydrogen.
- 9.5: The Quantum-Mechanical Model- Atoms with Orbitals
- This page discusses quantum mechanics, focusing on atomic and subatomic particles, their wave-particle duality, and the uncertainty in electron positioning. It highlights the shift from classical mechanics to a framework where energy changes in quanta and orbitals represent probability zones for electrons. This modern perspective, influenced by scientists such as Niels Bohr and Richard Feynman, challenges traditional concepts of physics.
- 9.6: Quantum-Mechanical Orbitals and Electron Configurations
- This page covers electron configurations and orbital diagrams, illustrating how electrons fill orbitals (s, p, d, f) following the Aufbau principle, Pauli Exclusion Principle, and Hund's Rule. It highlights the filling order of atomic sublevels based on energy, including examples from the first two periods of the periodic table, and explains concepts such as quantum numbers and orbital shapes.
- 9.7: Electron Configurations and the Periodic Table
- This page explains how electron configurations relate to the structure of the periodic table, where elements are organized by atomic number and grouped by similar properties. It describes the arrangement of elements into distinct blocks (s, p, d, f) determined by subshell filling. Valence electrons, which significantly influence chemical behavior, correspond to the highest shell and unfilled subshells.
- 9.8: The Explanatory Power of the Quantum-Mechanical Model
- This page explains the organization of the periodic table into groups and periods, highlighting that elements in the same group have similar chemical properties due to their valence electron configurations. Key groups discussed include alkali metals, alkaline earth metals, halogens, and noble gases. It also covers an alternate numbering system for groups and the significance of periods in indicating the energy levels of valence electrons, while defining relevant vocabulary terms.
- 9.9: Periodic Trends - Atomic Size, Ionization Energy, and Metallic Character
- This page explores periodic trends of atomic properties, including atomic radius, ionization energy, and electron affinity, based on element positioning in the periodic table. It highlights that atomic radius increases down columns and decreases across rows, ionization energy decreases down columns and rises across, and electron affinity varies.
- 9.E: Electrons in Atoms and the Periodic Table (Exercises)
- This page covers the properties of light, including wavelength, frequency, energy, and the Bohr model, explaining electron orbits and their relation to light emission. It introduces the quantum-mechanical model and discusses electron configurations in relation to the periodic table, including energy levels and valence electrons.