7: Chemistry of the Main Group Elements
- Page ID
- 551809
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 7.1: General Trends in Main Group Chemistry
- This page outlines key principles for understanding the chemical properties and trends of main group elements, focusing on the Periodic Law and the organization of the Periodic Table. It emphasizes periodic trends in atomic properties, including atomic radii, ionization energy, electron affinity, and electronegativity, while noting diagonal relationships.
- 7.1.1: The Periodic Table is an Organizing Concept in Main Group Chemistry
- 7.1.1.1: The metal-nonmetal-metalloid distinction and the metal-nonmetal "line" are useful for thinking about trends in elements' physical properties
- 7.1.1.2: There are qualitative differences between the chemistry of the elements in the first two rows and those in the rest of the periodic table
- 7.1.2: Electronegativity increases and radius decreases towards the upper left of the periodic table, with electron withdrawing substituents, and with oxidation state
- 7.1.3: Ionization energy roughly increases towards the upper left of the periodic table but is also influenced by orbital energy and pairing energy effects
- 7.1.4: As may be seen from considering an element's redox diagrams, main group elements (aside from the noble gases) generally are more oxidizing towards the upper left of the periodic table and more reducing towards the lower right of the periodic table
- 7.1.4.1: Latimer Diagrams summarize elements' redox properties on a single line
- 7.1.4.2: Frost Diagrams show how stable element's redox states are relative to the free element
- 7.1.4.3: Pourbaix Diagrams are Redox Phase Diagrams that Summarize the most stable form of an element at a given pH and solution potential
- 7.2: What are the main group elements and why should anyone care about them?
- This page discusses the significance of main group elements in the s and p blocks of the periodic table, emphasizing their role in chemistry and industry. It aims to highlight their key characteristics and bonding behavior, which can sometimes challenge conventional rules. The chapter also reviews concepts that help clarify periodic trends in the chemistry of these elements.
- 7.3: Group 1, The Alkali Metals
- This page discusses the alkali metals in group 1 of the periodic table, ranging from lithium to francium. These highly reactive metals exist mainly as +1 cations and are primarily obtained through electrolytic reduction of their salts. They are soft, silvery solids with low melting and boiling points, characterized by weaker metallic bonds, lower ionization energies, and larger atomic radii. Their extreme reactivity necessitates careful storage to prevent oxidation.
- 7.4: Hydrogen
- This page provides an overview of hydrogen isotopes: protium (hydrogen-1), deuterium (hydrogen-2), and tritium (hydrogen-3). It covers their atomic properties, including symbols, neutron counts, atomic masses, abundance, half-lives, melting and boiling points, and notable aspects like NMR activity. Protium is the most prevalent isotope, whereas tritium is radioactive with a half-life of 12.32 years. A table summarizes the information for easy reference.
- 7.5: Group 2, The Alkaline Earth Metals
- This page discusses the alkaline earth metals, which range from beryllium to radium and are found in group 2 of the periodic table. It highlights their similar properties and behaviors attributed to comparable electron configurations, emphasizing the importance of understanding their placement and characteristics for studying their chemical properties and reactions.
- 7.6: Group 13 (and a note on the post-transition metals)
- This page discusses Group 13 elements, from Boron to Nihonium, emphasizing their chemical diversity. Boron is a nonmetal or metalloid, while Aluminum is either a metalloid or metal. Gallium, Indium, Thallium, and Nihonium are post-transition metals exhibiting the inert pair effect. These post-transition metals are typically electron-rich and electronegative, leading to lower melting points and higher covalency.
- 7.7: Group 14
- This page provides an overview of Group 14 elements in the periodic table, spanning from carbon (C) to flerovium (Fl), acknowledging that the modern periodic table currently identifies element 115 as Flerovium (Fl). It emphasizes the evolution of the periodic table and its approach to classifying elements, with the content adapted from a general chemistry source.
- 7.7.1: The Group 14 Elements and the Many Allotropes of Carbon
- 7.7.2: Inorganic Compounds of the Group 14 Elements
- 7.7.3: Chemistry of Carbon (Z=6)
- 7.7.4: Chemistry of Silicon (Z=14)
- 7.7.4.1: Silicates
- 7.7.4.2: Silicon and Group 14 Elements
- 7.7.5: Chemistry of Germanium (Z=32)
- 7.7.6: Chemistry of Tin (Z=50)
- 7.7.7: Chemistry of Lead (Z=82)
- 7.7.7.1: Lead Plumbate
- 7.8: The Nitrogen Family
- This page covers the nitrogen family (Group 15), which includes nitrogen, phosphorus, arsenic, antimony, and bismuth, all sharing the electron configuration ns2np3. Nitrogen is essential for life and industry, while phosphorus is crucial for biological molecules. Arsenic and antimony have historical significance, and bismuth is noted for its low melting point. It also mentions the synthesis of the synthetic element moscovium.
- 7.9: The Oxygen Family (The Chalcogens)
- This page discusses the oxygen family (chalcogens) in Group 16, detailing key elements like oxygen, sulfur, selenium, tellurium, polonium, and Livermorium. Oxygen is essential for respiration, while sulfur is common in Earth's crust. Selenium and tellurium, though less abundant, are still significant. Polonium is a rare radioactive element created in labs, and Livermorium is a synthetic element named after a research lab. Each element plays a vital role in nature and various chemical processes.
- 7.9.1: General Properties and Reactions
- 7.9.1.1: Oxygen Group (Group VIA) Trends
- 7.9.2: Chemistry of Oxygen (Z=8)
- 7.9.2.1: Ozone
- 7.9.2.1.1: Ozone Layer and Ozone Hole
- 7.9.3: Chemistry of Sulfur (Z=16)
- 7.9.4: Chemistry of Selenium (Z=34)
- 7.9.5: Chemistry of Tellurium (Z=52)
- 7.9.6: Chemistry of Polonium (Z=84)
- 7.9.7: Chemistry of Livermorium (Z=116)
- 7.10: The Halogens
- This page details the five halogens found in Group 17 of the periodic table: fluorine, chlorine, bromine, iodine, and astatine. It explains their shared feature of seven valence electrons, which makes them highly reactive. The page notes trends in physical properties—melting and boiling points increase down the group while ionization energy decreases. It further discusses their chemical properties, redox behavior, and highlights the distinct characteristics and applications of each halogen.
- 7.10.1: Physical Properties of the Halogens
- 7.10.1.1: Atomic and Physical Properties of Halogens
- 7.10.1.2: General Properties of Halogens
- 7.10.1.3: Halogen Group (Group 17) Trends
- 7.10.1.4: Physical Properties of the Group 17 Elements
- 7.10.2: Chemical Properties of the Halogens
- 7.10.2.1: Halide Ions as Reducing Agents
- 7.10.2.2: Halogens as Oxidizing Agents
- 7.10.2.3: Interhalogens
- 7.10.2.4: More Reactions of Halogens
- 7.10.2.5: Oxidizing Ability of the Group 17 Elements
- 7.10.2.6: Testing for Halide Ions
- 7.10.2.7: The Acidity of the Hydrogen Halides
- 7.10.3: Chemistry of Fluorine (Z=9)
- 7.10.4: Chemistry of Chlorine (Z=17)
- 7.10.4.1: The Manufacture of Chlorine
- 7.10.5: Chemistry of Bromine (Z=35)
- 7.10.6: Chemistry of Iodine (Z=53)
- 7.10.7: Chemistry of Astatine (Z=85)
- 7.11: The Noble Gases
- This page discusses noble gases in Group 18 of the periodic table, originally termed "inert gases" due to their low reactivity from filled valence shells. It notes their later identification compared to other elements, underlining their unique stability and properties.
- 7.11.1: Properties of Nobel Gases
- 7.11.1.1: Noble Gas (Group 18) Trends
- 7.11.2: Reactions of Nobel Gases
- 7.11.3: Chemistry of Helium (Z=2)
- 7.11.4: Chemistry of Neon (Z=10)
- 7.11.5: Chemistry of Argon (Z=18)
- 7.11.6: Chemistry of Krypton (Z=36)
- 7.11.7: Chemistry of Xenon (Z=54)
- 7.11.8: Chemistry of Radon (Z=86)