Chapter 5 Study
Guide
Chemical
Bonding
Review Notes, Labs,
Homework, and the Textbook.
1.
Using the Periodic Table,
you should be able to draw the electron dot diagram for all of the elements
covered in class.
2.
Ionic Bonds
A.
Know that an ion is a
charged atom or group of atoms
B.
A polyatomic ion is what we
call a charged group of atoms
C.
Atoms become charged when
the gain or lose electrons.
D.
Atoms have positive charges
when the lose electrons (mostly metals) and negative charges when they gain
electrons (mostly nonmetals).
E.
Ionic Bonds form when
electrons are transferred from one atom to another resulting in ions. The opposite charges of the ions
attract each other. This is a very
strong bond.
F.
You should know how to write
chemical formulas using ion charges.
You should know how to name compounds using the chemical formula. I will give you an ion list to use on
the test.
G.
You should know the
characteristics of ionic compounds:
1)
Ionic compounds form
crystals because of the regular repeating pattern of ions.
2)
Conduct electricity when
dissolved in water.
3)
High melting points
4)
Not flammable
5)
Almost all ionic compounds
(salts) are formed from
a metal and a nonmetal bonding.
3.
Covalent Bonds
A.
Know that covalent bonds
form when atoms share electrons.
B.
Usually form when nonmetals
bond to other nonmetals.
C.
Sometimes atoms have to
share lots of electrons when they bond (example: Nitrogen forms a triple bond).
D.
Covalent molecules often
have low melting points and burn easily (more flammable).
E.
Most covalent compounds do
not conduct electricity in water like ionic compounds do.
F.
If electrons are not shared
equally between all atoms, the molecule is said to be polar. A polar bond makes one part of the
molecule more positive and another part of the molecule more negative. An example is water where the Hydrogen
atoms are more positive and the oxygen is more negative because the electrons
like the oxygen better.
