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An Introduction to Chemistry
• Important biological elements
– Carbon
– Oxygen
– Nitrogen
– Hydrogen
– Sulfur
– Na
–K
II. Atomic Structure
• A. Definition
• B. Analogy of
structure
• C. Subatomic
particles
– 1.
– 2.
– 3.
Protons
Neutrons
Electrons
III. Electron orbitals
• A. Location
• B. Maximum number
of electrons in an
orbital
• C. Orbital filling
• D. Examples
–
–
–
–
1.
2.
3.
4.
H
C
Na
Si
III. Electron orbitals
• E. Valence electrons
– 1.
– 2.
– 3.
– 4.
Definition
Involved in chemical bond formation
Determines chemical properties of the
atom
Elements with the same number of
valence electrons have similar
chemical properties
III. Electron orbitals
• E. Valence electrons
– 5.
gaining and
losing energy
IV. Periodic table
An atom with an atomic number of
13 and a mass of 22 possesses
____ electrons.
79%
21%
Th
e
an
sw
er
ca
nn
o
tb
...
3
0% 0%
9
0%
22
13
22
9
3
The answer
cannot be
determined
13
1.
2.
3.
4.
5.
An atom with an atomic number of
13 and a mass of 22 possesses
____ valence electrons.
68%
2
3
8
13
16%
11%
13
8
3
5%
2
1.
2.
3.
4.
V.
Chemical Bonding
• A. Octet Rule
– 1.
– 2.
Definition
Noble Gases
V. Chemical Bonding
• B. Ionic Bonding
– 1.
Example
•
11Na
•
17Cl
V. Chemical Bonding
• B. Ionic Bonding
– 2. Definition
Ionic bonding
What is the equation of the compound formed
when 20Ca and 17Cl combine by ionic bonding?
Ca2Cl
CaCl
CaCl2
The answer
cannot be
determined
63%
19% 19%
Th
e
an
sw
er
ca
nn
o
C
tb
...
aC
l2
aC
l
C
a2
Cl
0%
C
1.
2.
3.
4.
V. Chemical Bonding
• C. Covalent bonding
– 1.
– 2.
– 3.
Definition
Example of nonpolar covalent
Example of polar covalent bonding
Nonpolar Covalent
Polar Covalent Bond