CHM136H1 Lecture Notes - Lecture 3: Covalent Bond, Yorkshire Carnegie, Euclidean Vector

• School: UTSG
• Department: Chemistry
• Course: CHM136H1
• Professor: Clive Scott Browning, Kristine Quinlan

Document Summary

Condensed (chemical formula with groupings, ie. ch3ch2och2ch3) Skeletal structure (h"s and c"s are not shown) Explaining the shapes and the types of bonds formed. Non-polar covalent bond = equal sharing of electrons. Polar covalent bond = one atom has stronger hold on electrons. Based on electronegativity; how strong an atom attracts electrons. Have dipoles that form partial positive/negative charges (arrow points to area of higher electron density) Electronegativity: the ability of an atom in a molecule to attract electrons toward itself. Increases up and to the right of the periodic table. Dipole moment: describes a separation of charge in a molecule. The vector sum of all bond dipoles to determine a net dipole. = # valence - # bonds - # lone electrons. Sum of all fcs must equal overall charge of molecule. Delocalized pi bond: sharing of 2 electrons amount more than 2 atoms. Real life molecule exists as a hybrid of all resonance form.