8: Chemistry of the Main Group Elements
- Page ID
- 151407
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 8.1: General Trends in Main Group Chemistry
- 8.1.1: The Periodic Table is an Organizing Concept in Main Group Chemistry
- 8.1.1.1: The metal-nonmetal-metalloid distinction and the metal-nonmetal "line" are useful for thinking about trends in elements' physical properties
- 8.1.1.2: There are qualitative differences between the chemistry of the elements in the first two rows and those in the rest of the periodic table
- 8.1.2: Electronegativity increases and radius decreases towards the upper left of the periodic table, with electron withdrawing substituents, and with oxidation state
- 8.1.3: Ionization energy roughly increases towards the upper left of the periodic table but is also influenced by orbital energy and pairing energy effects
- 8.1.4: 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
- 8.1.4.1: Latimer Diagrams summarize elements' redox properties on a single line
- 8.1.4.2: Frost Diagrams show how stable element's redox states are relative to the free element
- 8.1.4.3: Pourbaix Diagrams are Redox Phase Diagrams that Summarize the most stable form of an element at a given pH and solution potential
- 8.7: Group 14
- 8.7.1: The Group 14 Elements and the Many Allotropes of Carbon
- 8.7.2: Inorganic Compounds of the Group 14 Elements
- 8.7.3: Chemistry of Carbon (Z=6)
- 8.7.4: Chemistry of Silicon (Z=14)
- 8.7.4.1: Silicates
- 8.7.4.2: Silicon and Group 14 Elements
- 8.7.5: Chemistry of Germanium (Z=32)
- 8.7.6: Chemistry of Tin (Z=50)
- 8.7.7: Chemistry of Lead (Z=82)
- 8.7.7.1: Lead Acetate
- 8.7.7.2: Lead Plumbate
- 8.9: The Nitrogen Family
- The nitrogen family includes the following compounds: nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). All Group 15 elements have the electron configuration ns2np3 in their outer shell, where n is the principal quantum number.
- 8.11: The Oxygen Family (The Chalcogens)
- The oxygen family, also called the chalcogens, consists of the elements found in Group 16 of the periodic table and is considered among the main group elements. It consists of the elements oxygen, sulfur, selenium, tellurium and polonium. These can be found in nature in both free and combined states.
- 8.11.1: General Properties and Reactions
- 8.11.1.1: Oxygen Group (Group VIA) Trends
- 8.11.2: Chemistry of Oxygen (Z=8)
- 8.11.2.1: Ozone
- 8.11.2.1.1: Important properties of ozone
- 8.11.2.1.2: Ozone Layer and Ozone Hole
- 8.11.3: Chemistry of Sulfur (Z=16)
- 8.11.4: Chemistry of Selenium (Z=34)
- 8.11.5: Chemistry of Tellurium (Z=52)
- 8.11.6: Chemistry of Polonium (Z=84)
- 8.11.7: Chemistry of Livermorium (Z=116)
- 8.13: The Halogens
- The halogens are located on the left of the noble gases on the periodic table. These five toxic, non-metallic elements make up Group 17 and consist of: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). Although astatine is radioactive and only has short-lived isotopes, it behaves similarly to iodine and is often included in the halogen group. Because the halogen elements have seven valence electrons, they only require one additional electron to form a full octet.
- 8.13.1: Physical Properties of the Halogens
- 8.13.1.1: Atomic and Physical Properties of Halogens
- 8.13.1.2: General Properties of Halogens
- 8.13.1.3: Halogen Group (Group 17) Trends
- 8.13.1.4: Physical Properties of the Group 17 Elements
- 8.13.2: Chemical Properties of the Halogens
- 8.13.2.1: Halide Ions as Reducing Agents
- 8.13.2.2: Halogens as Oxidizing Agents
- 8.13.2.3: Interhalogens
- 8.13.2.4: More Reactions of Halogens
- 8.13.2.5: Oxidizing Ability of the Group 17 Elements
- 8.13.2.6: Testing for Halide Ions
- 8.13.2.7: The Acidity of the Hydrogen Halides
- 8.13.3: Chemistry of Fluorine (Z=9)
- 8.13.4: Chemistry of Chlorine (Z=17)
- 8.13.4.1: The Manufacture of Chlorine
- 8.13.5: Chemistry of Bromine (Z=35)
- 8.13.6: Chemistry of Iodine (Z=53)
- 8.13.7: Chemistry of Astatine (Z=85)
- 8.14: The Noble Gases
- The noble gases (Group 18) are located in the far right of the periodic table and were previously referred to as the "inert gases" due to the fact that their filled valence shells (octets) make them extremely nonreactive. The noble gases were characterized relatively late compared to other element groups.
- 8.14.1: History, usage, properties, and distribution of the elements
- 8.14.2: Properties of Nobel Gases
- 8.14.2.1: Noble Gas (Group 18) Trends
- 8.14.3: Chemistry of the Group 18 (Noble Gas) Elements
- 8.14.4: Reactions of Nobel Gases
- 8.14.5: Chemistry of Helium (Z=2)
- 8.14.6: Chemistry of Neon (Z=10)
- 8.14.7: Chemistry of Argon (Z=18)
- 8.14.8: Chemistry of Krypton (Z=36)
- 8.14.9: Chemistry of Radon (Z=86)
- 8.14.10: Chemistry of Xenon (Z=54)