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Understanding Covalent Bonds: Nonpolar vs. Polar

Learn about nonpolar and polar covalent bonds, electron sharing, electronegativity differences, molecular polarity, VSEPR theory, and shapes of molecules.

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Understanding Covalent Bonds: Nonpolar vs. Polar

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  1. Polarity

  2. Two types of Covalent Bonds Nonpolar covalent bonds Equal sharing of electron • Polar covalent bonds • Unequal sharing of electron

  3. Nonpolar Covalent Bonds O P O P P Equal Sharing of the shared pair. Little or no difference in electronegativity H H O2 P4 H2

  4. Polar Covalent Bonds H Cl C O S Cl Unequal sharing of electron pair. Measurable difference in electronegativity. H-Cl C-O S-Cl 2.20 3.16 2.55 3.44 2.58 3.16 .96 .89 .58

  5. Type of Bond depends on the difference in electronegativity Electronegativity is a measure of the attraction an atom has for an electron. A difference in electronegativity of less than .4 has essentially equal sharing of the pair of electrons resulting in a nonpolar covalent bond. A difference in electronegativity of more than .4 has an unequal sharing of the pair of electrons resulting in a polar covalent bond.

  6. Covalent Bonds

  7. Compairing Ionic, Polar Covalent and Nonpolar Covalent Electron Clouds Nonpolar Covalent Polar Covalent Ionic

  8. Polar & Non polar Molecules Molecules will be non polar if all of the covalent bonds are symmetrical around the central atom. Molecules will be polar if the molecule contains at least one polar bond that is asymmetrical on the central atom. Molecules will also be polar if the central atom contains an unshared pair of electrons.

  9. Nonpolar molecules

  10. Dipole • A molecule that has two poles is called a dipolar molecule, or dipole.

  11. Summary of Polarity of molecules Nonpolar Molecule Molecules are symmetrical Polar Molecule Molecules are not symmetrical

  12. VSEPR THEORY: How do we determine the shapes of molecules and ions?

  13. VSEPR THEORY • What does VSEPR stand for? • Valence Shell Electron Pair Repulsion

  14. VSEPR THEORY • Why is this important to know? • It explains how molecules and ions behave and the shapes they make

  15. VSEPR charts • Use the Lewis structure to determine the geometry of the molecule • Electron arrangement establishes the bond angles • Molecule takes the shape of that portion of the electron arrangement • Think REGIONS OF ELECTRON DENSITY rather than bonds (for instance, a double bond would only be 1 region)

  16. Geometries • Linear • Trigonal • Tetrahedral

  17. Linear • Number of possible bonds of central Atom • 2 • Number of Lone pairs on central atom • 0 • Angle between bonds • 180

  18. Trigonal Planar • Number of possible bonds of central Atom • 3 • Number of Lone pairs on central atom • 0 • Angle between bonds • 120

  19. Tetrahedral • Number of possible bonds of central Atom • 4 • Number of Lone pairs on central atom • 0 • Angle between bonds • 109.5

  20. Tetrahedral ~ Trigonal Pyramidal • Number of possible bonds of central Atom • 4 • Number of Lone pairs on central atom • 1 • Angle between bonds • 107

  21. Tetrahedral ~ Bent • Number of possible bonds of central Atom • 4 • Number of Lone pairs on central atom • 2 • Angle between bonds • 105

  22. Molecular Shapes Linear Bent Pyrimidal Trigonal Planar Tetrahedral

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