BIO 111 Lecture Notes - Lecture 3: Boiling Point, No Charge, Ammonia

102 views4 pages
15 Sep 2016
Department
Course
Professor

Document Summary

3 types of bonds: covalent, polar or nonpolar, hydrogen. Helps fill the outer shell (octet rule!) Example: hydrogen fluoride ( h f or hf ) Covalent bonds often the strongest of all bonds. Shared electrons behave as if they belong to each atom. 1 pair of electrons single bond h-f. 2 pairs of electrons double bond o=o. 3 pairs of electrons triple bond n n. Distribution of electrons creates a polarity, or difference in electric charge, across the molecule. One atom is more electronegative than the other(s), so electrons are. Polar= puller ;one holds the electrons closer. Between atoms with similar electronegativities (attraction to electrons) Partially positive hydrogen is attracted to an electronegative atom nearby. So the result is that cl becomes cl- and na becomes na+ due to the lose of its electron. Ion: atom or molecule that lost/gained electrons. Anions: gain of an electron; negative charge. Water is vital to life on earth.

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