Chp5 - Chapter 5: The Covalent Bond Theory of Covalent Bond...

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Unformatted text preview: Chapter 5: The Covalent Bond Theory of Covalent Bond Bond Polarity Naming Lewis Structures Resonance Formal Charge and Ox States The Covalent Bond REMEMBER : Ionic bond is formed by TRANSFER of electron(s) to unfilled orbital of lower energy Electrons can also be stabilized by interacting with another positive charge (nucleus is a great source of positive charge) Atoms can acquire a noble gas configuration (stable) by sharing electrons with another atom COVALENT BOND bond formed by sharing of electrons; usually between nonmetals ( is small) Interaction of 2 H Atoms + + + + + + + + Bond Energy (kJ/mol) 0.74 (bond length) + +-436 Covalent Bond Length and Energy + + Bond Length (r): 0.74 - 2.7 ( = 100 pm) Bond Energy: 100-1000 kJ/mol Bond Length Bond Energy H 2 0.74 436 kJ/mol I 2 2.7 151 kJ/mol Bond Polarity Bond polarity is best described by = 0 ; covalent bond (e- shared equally, H 2 , N 2 , Cl 2 ) small ; polar covalent bond (atom with larger becomes e- rich, results in bond dipole, HCl, H 2 O, CH 4 , NH 3 ) large ; ionic bond (e- transferred to atom with larger , NaCl, Al(NO 3 ) 3 , NH 4 Cl) Bond Dipole In HCl, Cl has a higher electronegativity (pull) so the electrons are located closer to the Cl nucleus....
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This note was uploaded on 10/30/2009 for the course CH Ch101 taught by Professor Bigham during the Fall '08 term at N.C. State.

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Chp5 - Chapter 5: The Covalent Bond Theory of Covalent Bond...

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