CHEM 1406
(revised08/24/07)
Study Guide #4: Ions, Formulas, Small Molecules and the Mole
www.delmar.edu/nsci/cgambill/sg0604.pdf
Textbook
Chapter 4: pages 111 - 148.
Know: Figure 4.2 (page 120), Table 4.5 (page 120), Table 4.7 (page 124),
Table 4.11 (page 130),Table 4.12 (page 131), Figure 4.4 (page 133)
Know Key Terms: page 144
Problems: all in chapter 4
Chapter 7: pages 227 – 232.
Know terms: solute, solvent, electrolyte, nonelectrolyte, acid, base
Problems: 7.1 – 14
Chapter 10: pages 332 – 339; pages 350 – 355
Know: Table 10.8 (page 350), Table 10.9 (page 353),
Concept Map (page 355)
Know Key Terms: page 356
Problems: 10.1, 2, 8, 31, 32, 33, 34, 36, 39, 40, 49, 50, 51, 52, 53, and 54
Recognize tetrathedral atoms, Draw line-angle drawings
Chapter 11: pages 362 – 369, 375 – 378.
Know terms and STRUCTURES alkane, alkene, alkyne, arene, phenyl ring,
benzene ring, cis/trans orientation, rotational about bonds
Problem 11.29 plus handouts
Organic Structural Units: alcohols, pg 385; aldehydes and ketones, pgs 399 – 404;
carboxylic acids, pgs 427 – 430; esters, pgs 435 – 437;
Problems: handout sheets
Chapter 15, Lipids: pages 496 – 531
Know terms and structures: fatty acid, unsaturated fatty acids, steroids
prostaglandins, triglycerides
Problems: Handouts
Dosage Calculations Textbook
Chapters: 10, and 11
Laboratory Textbook: www.delmar.edu/nsci/cgambill/labsch06071.pdf
Experiments #7 (pages 72 – 73), #15 (pages 147 – 154), #21 (pages 209 – 210),
#24 (page 231), and #25 (page 239)
Turn in problems and exercises from lab textbook as directed in lab class
No Computer Problem Set for Structure and Bonding
CHEM 1406
Study Guide #4
page 2
Student Study Guide (optional):
Chapter 4: pages 48 - 63. practice exam questions 1- 43;
Chapter 7: pages 106 -107. sections 7.2A and 7.2B
Chapter 10: pages 151 – 152, 158 – 159; practice exam questions 1 – 8,
25 – 38 (pages 160 – 161)
WEB Resources:
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Writing Chemical Formulas; see:
http://newtraditions.chem.wisc.edu/FPTS/fbform/newformf.htm
Tutorials and quizzes for writing chemical formulas, naming chemical
compounds and the mole; see:
http://www.fcps.k12.va.us/AnnandaleHS/Sadananda/chemformula.htm
Lipids and Friends; see: http://old.jccc.net/~pdecell/biochemistry/lipids.html
Lipid Health; see: http://www.lipidhealth.org/default.asp?src=54
Glossary of Standard Terms in Lipid Management; see:
http://www.lipidhealth.org/default.asp?src=54
Hyperlipidemia Hub; see: http://www.knowdeep.org/hyperlipidemia/
Evidence-based Medicine and the Statins: Applying the Highest Standards to
Clinical Practice; see: http://www.mednet.ca/html/ph02-513.htm
Basic Lipid Protocol; see:
http://www.cholesterolclinic.com/Basic%20Lipid%20Protocol.htm
All About Mole Calculations; see: http://misterguch.brinkster.net/molecalculations.html
Mole Calculations; see
http://www.css.edu/USERS/lmcgahey/web/CHM102/Stoichiometry/mole.html
Iron Use and Storage in the Body: Ferritin and Molecular Representations; see
http://wunmr.wustl.edu/EduDev/LabTutorials/Ferritin/Ferritin.html
Table of Common Polyatomic Ions; see:
http://wunmr.wustl.edu/EduDev/LabTutorials/PeriodicProperties/Ions/ions.html
From Explosives to the Gas That Heals: Nitric Oxide in Biology and Medicine; see:
http://www.beyonddiscovery.org/content/view.page.asp?I=981
Nitric Oxide; see: http://www.diabetesselfmanagement.com/article.cfm?aid=16&sid=6
Statins and ACE-I: Effects on the Endothelium via Nitric Oxide; see:
http://www.google.com/search?hl=en&lr=&ie=ISO-8859-1&q=%22nitric+oxide%22+statins
Biomolecules, Chemistry of Lipids; see:
http://web.indstate.edu/thcme/mwking/lipids.html
Ionic Bonding; see: http://www.chemguide.co.uk/atoms/bonding/ionic.html
CHEM 1406
Study Guide #4
page 3
Ionic and Covalent Bonding
From: http://neon.chem.uidaho.edu/~honors/electneg.html
Pure Covalent, Polar Covalent, and Ionic Bonds
It's not unusual for covalent bonds and ionic bonds to be presented to introductory
students as two clearly distinct categories. In the usual definition, covalent bonds involve
electron sharing and ionic bonds involve electron transfer to form ions. These definitions
are correct, but they miss the reality that pure covalent and ionic bonds sit on a
continuum dictated by the difference in electronegativity. The bigger this difference, the
more polar the bond. At some point we would expect the bond to have become so polar
that it constitutes a transfer of an electron from one atom to the other. The chart below
gives an idea of how this trend works.
Using some simple calculations of % ionic and % covalent character, it is possible to
show that a difference of electronegativity of about 1.7 is the point where a bond may be
thought of as ionic. There are a few exceptions to this rule such as HF, in which the
electronegativity difference is 1.9, but the molecular properties are decidedly covalent.
CHEM 1406
Study Guide #4
page 4
Again, in many introductory courses, students are presented with a thumb rule:
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•
Covalent bond = non-metal + non-metal
Ionic bond = metal + non-metal
It's easy to see that this rule is only a rough approximation and works well for compounds
of the Group 1 or 2 metals with the halides of Group 17, but doesn't reflect reality when
we consider bonds between carbon and most metals. Carbon is certainly a non-metal, but
it forms covalent bonds (sometimes highly polar, but covalent none the less) with almost
all of the elements on the periodic table.
Also,
http://www.chem.umass.edu/people/botch/Chem121F05/Chapters/Ch3/PercentIonic.jpg
CHEM 1406
Study Guide #4
page 5
See also: http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/FG11_07.JPG