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3: Chemical Bonding

Last updated

Aug 20, 2021
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- 2.5: Periodic Trends- Atomic Size, Ionization Energy, Electron Affinity, and Metallic Character
- 3.1: Valence Electrons

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3.1: Valence Electrons
Valence electrons are the electrons in the highest occupied principal energy level of an atom. In the second period elements, the two electrons in the 1s sublevel are called inner-shell electrons and are not involved directly in the element's reactivity or in the formation of compounds.
3.2: Ions
Ions can be positively charged or negatively charged. A Lewis diagram is used to show how electrons are transferred to make ions and ionic compounds.
3.3: Formulas for Ionic Compounds
Proper chemical formulas for ionic compounds balance the total positive charge with the total negative charge. Groups of atoms with an overall charge, called polyatomic ions, also exist.
3.4: Ionic Nomenclature
Each ionic compound has its own unique name that comes from the names of the ions. After learning a few more details about the names of individual ions, you will be a step away from knowing how to name ionic compounds. This section begins the formal study of nomenclature, the systematic naming of chemical compounds.
3.5: Covalent Bonds
Covalent bonds are formed when atoms share electrons. Lewis electron dot diagrams can be drawn to illustrate covalent bond formation. Double bonds or triple bonds between atoms may be necessary to properly illustrate the bonding in some molecules.
3.6: The Covalent structure of Polyatomic Ions
Polyatomic ions, common in any lab, contain several atoms covalently bonded together. Often, these ions are charged and combine with metals to form ionic bonds.
3.7: Covalent Compounds - Formulas and Names
The chemical formula of a simple covalent compound can be determined from its name. The name of a simple covalent compound can be determined from its chemical formula.

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