Ionic, Covalent and Metallic Bonding

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Presentation transcript:

Ionic, Covalent and Metallic Bonding Metallic bonding is a special case of covalent bonding were electrons are shared throughout a crystal. More on Metallic bonding another day.

Types of Chemical Bonds The classification of bonds is based on the extent to which electrons are shared or transferred.

C. Bond Polarity Nonpolar Polar Ionic Link to Dog Video .

Link to covalent vs ionic bonds

Ionic Bonds A complete transfer of one or more electrons between two atoms, forming + and – ions. Ionic bonds are typically formed from a metal and a nonmetal.

Ionic Salt Crystal “Lattice ” Lewis Dot Structure:

An equal sharing (“co”) of valence electrons (“valent”). Covalent Bonds An equal sharing (“co”) of valence electrons (“valent”).

Picture:

Polar Covalent Bonds An unequal sharing of valence electrons. Typically forms between 2 nonmetals.

Electronegativity Defn: The pull an atom exerts on electrons in a chemical bond. Pauling Scale: Ranges from 0.0 (no attraction) to 4.0 (Highest Attraction) EN differences are used to predict type of bonds and polarity of bonds.

Electronegativity Values

C. Bond Polarity Electronegativity Trend Increases up and to the right. Largest EN : top right Why?: small atoms attract e- more strongly than larger atoms Smallest EN : bottom left

C. Bond Polarity Most bonds are a blend of ionic and covalent characteristics. Difference in electronegativity determines bond type.

Key idea: It is DIFFERENCE in EN that is important, not EN value of an individual atom

Using Electronegativity Differences to Determine Bond Type If EN difference is between 0.0 = covalent bond 0.1 to less than 1.7 = polar covalent 1.7 or above = Ionic

Using Electronegativity Differences to Determine Bond Type Example: CaCl2 1.9 > 1.7 → IONIC: Example: O2: 3.5 – 3.5 = 0 → COVALENT Example: CO2 0.1 to less than 1.7 = POLAR COVALENT

+ - Polar Covalent Bonds: The MORE EN atom will be “partial” NEGATIVE and have MORE electron density around it. Arrow points toward negative side of molecule Dipole = 2 sides : + side and - side + - More EN atom = δ-