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Chemistry Bonding Types of Bonds

Chemistry Bonding Types of Bonds. Do Now: What does the term “chemical bond” mean to you? CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED. A chemical bond is when atoms attract each other’s electrons in such a way that the atoms stick together. Three main types

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Chemistry Bonding Types of Bonds

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  1. ChemistryBondingTypes of Bonds Do Now: What does the term “chemical bond” mean to you? CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED

  2. A chemical bond is when atoms attract each other’s electrons in such a way that the atoms stick together. Three main types Ionic – electrical attraction of opposite ions Covalent – “sharing” of electrons between two atoms Metallic– sharing of electrons between multiple atoms These two bond types are based off of the polarity of the bond: how much “sharing” of electrons happens? What is a bond?

  3. IONIC Metal-Nonmetal High melting points and boiling points. Make crystal networks (molecules have no distinct shape) Electrolytes in solution (do not conduct electricity as solids) Ex: NaClCaSO4 COVALENT Nonmetal-Nonmetal Lower mp and bp Molecules can stand alone (not in a crystal, and have distinct shapes such as linear, bent, etc.) Do not conduct electricity Ex. NH3, H2O Ionic vs. Covalent

  4. METALLIC Metal-Metal Not “bonding” in the sense that new substances are created A sea of valence electrons that no one atom particularly wants, binding a metal together. This gives metals its malleability and ductility. Examples: Au, Ag, brass, bronze, steel CRYSTALS ALL SOLIDS ARE CRYSTALS Ionic crystals:Made from positive and negative ions, brittle. Also known as salts. Covalent crystals: Exist as single molecules, or networksH2O (ice): single moleculesC (diamond)C (graphite): network Metallic crystals:positive ions in a sea of electrons. Metallic Bonding & Crystals

  5. Electronegativity determines bond polarity. Polar – uneven distribution of charge Two atoms, X and Y, bond together Take the difference in electronegativities of X and Y 0.0: nonpolar (covalent) H-H 0.1-0.3: slightly polar (covalent) 0.4-1.7: moderately polar (covalent) O-H 1.8 and up: extremely polar (ionic) Na-Cl The larger the electronegativity difference, the more ionic the bond. (and vice versa) The atom with the larger electronegativity value will be the one that the electrons gravitate toward (most negative) Predicting Bond Type

  6. Bond Type Triangle • Combining the difference in electronegativity (ΔEN) with the average electronegativity (EN) tells us whether or not a substance is metallic, covalent, or ionic. • This is called the bond type triangle.

  7. Lewis Dot Diagrams • In order to draw bonds, we need a system for drawing valence electrons. • The Lewis dot diagram allows us to draw atoms with their proper number of valence electrons. • These valence electrons surround the element’s symbol. • One VE goes on each side before doubling up.

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