BIOA11H3 Lecture Notes - Lecture 1: Sodium Chloride, Lewis Structure, Hydrogen Bond

39 views6 pages
23 Aug 2019
School
Course

Document Summary

Electronegativity is the measure of the tendency of an atom to attract to a bonding pair of electrons. The trend follows nonmetallic character in the trends to the right. Covalent: one metallic and one non- metallic element, transfer of electrons. En >1. 6: bond energy: 3-7 kcal/mol, two non-metallic elements. Sharing of electrons: can have double and triple bonds as well, bond energy: 50-100 kcal/mol (strongest bond type) 0< en <2. 0: 0 pure covalence, 0< en < 0. 5 non polar covalence, 0. 5< en <2 polar covalence. In the range of 1. 6< en <2. 0 , check the types of elements that you"re bonding and use the first rule: that"s the type of bond that you have: example: sodium chloride (ki, example: carbon dioxide (co2) Bonds that aren"t actually bonds: (van der walls: hydrogen bonds (h-o, h-n, h-fl) (3-7 kcal/mol, hydrophobic interactions (1-2 kcal/mol) london dispersion and dipole dipole.

Get access

Grade+
$40 USD/m
Billed monthly
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
10 Verified Answers
Class+
$30 USD/m
Billed monthly
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
7 Verified Answers

Related Documents

Related Questions