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Week 3; Day 7-9 - Continuing On Ionic and Covalent Compounds.

by: Becca LeBoeuf

Week 3; Day 7-9 - Continuing On Ionic and Covalent Compounds. Chemistry 101

Marketplace > University of Wisconsin - Oshkosh > Chemistry > Chemistry 101 > Week 3 Day 7 9 Continuing On Ionic and Covalent Compounds
Becca LeBoeuf

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Week 3 notes. Continues on covering material about ionic compounds, covalent compounds, melting/freezing point, how to determine if a compound is polar or non polar. We only covered how to determin...
General, Organic, Biological Chemistry
George Vater Olsen
Class Notes
#Chemistry #Chem101 #CovalentCompounds #IonicCompounds #PolarOrNonPolar #MeltingAndFreezingPoint




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This 3 page Class Notes was uploaded by Becca LeBoeuf on Saturday February 20, 2016. The Class Notes belongs to Chemistry 101 at University of Wisconsin - Oshkosh taught by George Vater Olsen in Spring 2016. Since its upload, it has received 19 views. For similar materials see General, Organic, Biological Chemistry in Chemistry at University of Wisconsin - Oshkosh.


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Date Created: 02/20/16
Week 3:    Day 7: Review for exam 1; no notes.    Day 8: Day of exam 1; no notes.    Day 9:    REMEMBER THIS RULES:  ● ate 3 oxygens.  ● it​ 2 oxygens.  ● fate/phat: 4 oxygens.  ● CO ​ 2­ →​o vertical line in letters so 2­.  ● C2H ​O​ 1­ →vertical line in letters so 1­.  ○ Exception: Phosphorus and Ammonium.  ○ Phosphide​ → P.  ○ Phosphate​ → PO4​3­.  ○ Phosphite → PO ​3­.    Dihydrogen Phosphate:  H2PO​4(3­) 1­ → This is now turned into 1­ because you have to add the 3­ charge with the 2+,  which in conclusion equals 1­.    Ammonium Sulfate:      Put In Water:  AQ: Ions are split apart in water.              Iron (III) Oxalate:  Switch method used to balance out.      Colligative Property​: Depend on only the number of particles.  ● Boiling point elevation.  ● Freezing point depression.    Melting Point:  ● NaCl; becomes a solid.  ● Sucrose; becomes a liquid.  ● Ionic compounds stick together at high temperatures. Takes a lot of energy for  molecules to pass each other.    Cl ­ Cl  C ­ O  H ­ O (really polar)  H ­ N (really polar)  H ­ F (really polar)    ● Ionic compounds have a higher melting point.  ● Covalent compounds have a lower melting point.  ● Ionic compounds are ALWAYS polar.  ● Covalent compounds can vary.    LIKE DISSOLVES LIKE:  ● Polar solutes dissolve in polar solutes.  ○ Water is polar.  ● Nonpolar solutes dissolve in nonpolar solutes.    Covalent Compound:  ● Nonpolar: 1 of 2 must occur.  ○ 1:  ■ All bonds must be non polar and no lone pairs of electrons.  ■ No difference in electronegativity for each atom.  ● O = O  ● C ­ H (carbon carbon + hydrogen hydrogen are non polar).      ○ 2:  ■ If you have the same # of identical atoms bonded to the central atom as  there are sites of electrodensity around that central atom.  ● C Cl4:  ○ C has 4 valence electrons.  ○ Cl​has 7 valence electrons.  ■ There are 4 chlorines.  ■ 7 x 4 = 28  ○ 28 + 4 = 32 (total electrons).    32 ­ 8 (4 bonds) = 24 ­ 24 = 0 (ALL SATISFIED).   


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