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4: Chemical Bonds

Last updated

Jun 13, 2023
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- 3.E: Atoms and the Periodic Table (Exercises)
- 4.1: The Art of Deduction- Stable Electron Configurations

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4.1: The Art of Deduction- Stable Electron Configurations
4.2: Lewis (Electron-Dot) Symbols
4.3: The Reaction of Sodium with Chlorine
4.4: Using Lewis Symbols for Ionic Compounds
4.5: Formulas and Names of Binary Ionic Compounds
4.6: Free Radicals and the Environment
The majority of molecules or complex ions discussed in general chemistry courses are demonstrated to have pairs of electrons. However, there are a few stable molecules which contain an odd number of electrons. These molecules, called "free radicals", contain at least one unpaired electron, a clear violation of the octet rule. Free radicals play many important roles a wide range of applied chemistry fields, including biology, medicine, and environmental chemistry.
4.7: Free Radicals and Health
Free radicals can be generated by a number of processes. For example, combustion of any material will produce OH (not hydroxide) free radicals. Once inhaled, OH can enter the body and affect cells. Free radical exposure has been linked to cancer, aging, and a number of autoimmune diseases.
4.8: Covalent Bonds- Shared Electron Pairs
Ionic bonding typically occurs when it is easy for one atom to lose one or more electrons and another atom to gain one or more electrons. However, some atoms won’t give up or gain electrons easily. Yet they still participate in compound formation. How? There is another mechanism for obtaining a complete valence shell: sharing electrons. When electrons are shared between two atoms, they make a bond called a covalent bond.
4.9: Unequal Sharing- Polar Covalent Bonds
4.10: Polyatomic Molecules- Water, Ammonia, and Methane
4.11: Polyatomic Ions
4.12: Rules for Writing Lewis Formulas
4.13: Molecular Shapes- The VSEPR Theory
4.14: Shapes and Properties- Polar and Nonpolar Molecules
4.15: Metallic Bonding
- 4.15.1: Crystal Structure of Metals
4.16: Network Covalent Atomic Solids
Covalent solids are formed by networks or chains of atoms or molecules held together by covalent bonds. A perfect single crystal of a covalent solid is therefore a single giant molecule.

Thumbnail: Non-polar covalent bonds in methane ( $\ce{CH4}$ ). The Lewis structure shows electrons shared between C and H atoms. (CC BY-sa 2.5; via ).

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