Cellular Chemistry &
Macromolecules
Biology
T. Meyer 2006
October 9, 2006
I. Atomic Structure
A. Protons
1. Positive (+) particles in the nucleus
of the atom.
2. Attracted to the electrons in the
orbit of the atom
B. Neutrons
1. Neutral (no charge)
2. Gives the atom its mass
C. Electrons
1. Negative (-) particles in the orbit of
the atom
2. Attracted to the protons in the
nucleus
Atomic Structure
Orbit
Proton
Electron
Neutron
Nucleus
II. Atomic Vocabulary
A. Atomic Number: the exact number
of protons in the nucleus.
Fun Fact
B. Atomic Mass: the number of
protons and neutrons in the nucleus.
C. Isotope: atoms of the same element
with different numbers of neutrons.
Vocabulary Examples
Carbon
Atomic Number : 6
Atomic Mass:
12.011
Isotopes: C12,13,14
http://www.mse.uiuc.edu/info/mse182/PeriodicTable.gif
III.
Types of Atomic Bonds
A. Covalent:
Atomic bond where
electrons are shared evenly.
H:H
B. Polar-Covalent: Atomic bond
Ex:
where electrons are shared unevenly
giving a slight charge to the molecule.
Ex: H2O
C. Ionic Bonding:
Atomic
bond where electrons are not shared
evenly. Results in a charged molecule.
Ex: NaCl- (Sodium Chloride)
http://images.google.com/imgres?imgurl=http://library.thinkquest.org/27819/media/ionic.gif&imgrefurl=http://library.thinkquest.org/27819/ch2_2.shtml&h=234&w=216&sz=5&tbnid=D5DLYg3udsJ:&tbnh=104&tbnw=96&hl=en&start=18&prev=/images%3Fq%3Dionic%2Bbond%26svnum%3D10%26hl%3Den%26lr%3D%26safe%3Dactive
Covalent Bonds
Ionic Bonds
IV.
Types of Mixtures
A. Mixtures: individual substances retain
their own property.
EX: Sand (SiO2) and H2O
B. Solutions: individual substance
(solute) is distributed evenly in
another (solvent).
EX: Salt (NaCl) and H2O
C. Suspension: a combination of
molecules in which some distribute
evenly and some retain their own
properties. (Mixture + Solution)
EX: Blood
V.
Acids vs. Bases
A. Acid: substance that forms Hydrogen
ions (H+) in water.
B. Base: substance that forms Hydroxide ions
(OH-) in water.
C. pH Scale: scale used to determine acids
and bases. Numbers 1-14.
Neutral = 7
Acidic (+) = 1 - 6
Basic (-) = 8 - 14
Chemical Equations
Balancing Chemical Equations
Law of Conservation of Matter:
Matter cannot be created or destroyed, but can
be rearranged.
Example Problems:
H2 + O2 
H2O
H2 + O 2 
≠
2 Atoms of Hydrogen
H2O
2 Atoms of
Hydrogen
1 Atom
of Oxygen
2 Atoms of Oxygen
Balanced
2H2
+
O2

2H2O
Chemical Bonds Video