Chemistry 12/1/14
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Fill out Valence Electron Practice on the notes
sheet.
HW:
◦ Finish pg. 1, Bonding Practice
◦ pg. 3 #15-22
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IWBAT
◦ Create and name a structure for ionic compounds
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Drill
Ionic Bonding Notes
Ionic Bonding Practice
Closure
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Paired valence
electrons
◦
◦
◦
◦
Relatively stable
Resistant to change
Don’t form
chemical bonds
Called nonbonding pairs or
lone pairs.
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Unpaired valence
electrons
◦
Have a strong
tendency to
participate in
chemical bonding
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Atoms gain or lose valence electrons until the
valence shell is filled or empty;
Since valence shells are made of “s” and “p”
sublevels, they can hold a maximum of 8
electrons (or 2 electrons for the 1st energy
level)
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occurs when the less electronegative element
(metal) transfers one or more valence
electrons to the more electronegative element
(nonmetal)
the metal loses electrons to become a cation
(a positively charged ion) while the nonmetal
gains an electron to become an anion ( a
negatively charged ion)
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Transfer of valence
electrons
Formed by a Metal
& Nonmetal ion
◦ ex. NaCl
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The smallest unit of
the compound is a
formula unit.
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Properties of ionic compounds:
◦ Crystalline solids at room temperature
◦ Conduct electric current in molten state, but not
solid state (ions not free to move)
◦ High melting and boiling points
◦ Usually water-soluble. Mobile ions in solution
conduct electricity -- electrolytes
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Use Lewis Structures to show ionic bonding:
◦ Ms. Bloedorn will demonstrate with pg. 1 – Bonding
Practice
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The charge of any compound MUST be ZERO!!
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Criss-Cross Basics
◦ Cross the numbers and drop the charges
◦ Don’t write “1”
◦ Reduce the ratio – 2:2  1:1, 2:4  1:2
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Naming basics – Name the CATION, then ANION
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Mg and F form a compound.
◦ What is the formula?
◦ Draw the Lewis structure.
◦ Name it!