BIO 101 Lecture Notes - Lecture 4: Ionic Bonding, Chemical Polarity, Surface Tension

16 views2 pages

Document Summary

Water is a polar molecule because of electronegaivity so electrons are not shared equally because o is more electronegaivity than h so parial charges exist on the o and h atoms. Polar molecules are soluble in water because the opposites atract and the charges of the polar molecules interact with the charges in water. Polar molecules and ions dissolve readily in water. Non-polar molecules are neutral and not soluble in water because there are no charges to interact with the polar water. There are single bonds, double bonds, and even triple bonds. Single bonds are examples like h2o, ch4, and nh3 (ammonia) Add nacl to water since its an ionic bond the na and cl breaks up and the na+ goes toward the negaive oxygen and the cl- goes toward the posiive hydrogen. See a coninuum between covalent non-polar, covalent polar, and ionically bonded. Hydrogen bonds- a bond between a hydrogen and nearby oxygen, nitrogen, or luorine.

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers

Related textbook solutions

Related Documents

Related Questions