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Covalent Bonding

Covalent Bonding. What’s going on? Molecule – formed when 2 or more atoms bond covalently. Sharing of electrons. Two Types of Covalent Bonds. i) nonpolar covalent – equal sharing of e - ii) polar covalent – UN equal sharing of e -. Nonpolar vs. Polar. NONPOLAR. POLAR.

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Covalent Bonding

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  1. Covalent Bonding • What’s going on? • Molecule – formed when 2 or more atoms bond covalently Sharing of electrons

  2. Two Types of Covalent Bonds i) nonpolar covalent – equal sharing of e- ii) polar covalent – UNequal sharing of e-

  3. Nonpolar vs. Polar NONPOLAR POLAR

  4. Nonpolar vs. Polar

  5. Nonpolar vs. Polar

  6. Predict these shapes NH3 H2O CO2 • • • • H N H • • • • H O H • • O C O • • • • H trigonal pyramidal bent linear

  7. Using electronegativity to determine bond type • Recall electronegativity: how much an atom wants electrons • Each atom is assigned a number between 0-4.0 to determine electronegativity strength

  8. Using electronegativity to determine bond type • We know 3 types of bonds: - nonpolar covalent - polar covalent - ionic • To determine bond type, subtract electronegativity values and see scale

  9. Scale nonpolar covalent polar covalent ionic 0.3 1.7 0 4.0

  10. 2.2 – 2.2 = 0 H-H nonpolar polar 3.44 – 2.2 = 1.24 H-O polar 2.55 – 2.2 = 0.35 H-C ionic 3.98 – 0.82 = 3.16 K-F

  11. Dipole Moment • defn – imbalance of electron density in a covalent bond • Due to electronegativity of atoms - (partial negative) = signifies more EN atom +(partial positive)= signifies less EN atom = shows direction of dipole moment

  12. Examples + - - + H O Cl C H = 2.2 C = 2.6 N = 3.0 Cl = 3.2 O = 3.4 F = 4.0 + - - + C F N H

  13. Intermolecular Forces • Defn – attractive forces between 2 molecules; weak compared to bonds

  14. Intermolecular Forces • London Dispersion Forces – very weak, exist in all molecules due to temporary shifts in the electron cloud

  15. Electrons evenly distributed London force Temporary dipole

  16. Intermolecular Forces • Dipole-Dipole – attraction between oppositely charged regions of polar molecules - - + + - +

  17. Intermolecular Forces • Hydrogen Bonding – special type of dipole-dipole occurring btwn molecules that have a H bonded to either a N,O, or F of another molecule; strongest force - Water is prime example - O O H H + +

  18. - O O O O H H H + + H - O hydrogen bond O H H + + O O O O H H H H

  19. Strength Ranking Hydrogen > dipole-dipole > London

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