1. Chemistry and Applied Math
We’ll use math quite a lot in this class. Although a good
deal of this class is qualitative in nature, some concepts
(gas laws, molarity, and several others) use math.
Scientific notation. Sometimes we will use incredibly
large or small numbers that necessitate the use of
scientific notation. For example in measuring the
number of atoms in a 10.00 gram sample of iron (Fe) or
when we talk about the mathematical basis for the pH
scale.

2. Scientific Notation...
an example
• The mole 6.02 x 1023
• We celebrate National Mole Day on October 23rd!
• 1.00– 9.99 x 10exponent
• 1000 becomes... 1.00 x 103
• More on calculations later…

3. Units of Measure
• Volume:
ml, l (milliliter/liter)
• Mass/weight:
g, kg (gram/kilogram)
• Length:
mm, cm (millimeter/centimeter)
• Temperature:
oC (degrees Celsius)

4. Density/Specific Gravity
1. Density: Mass (weight) per unit volume
2. D = M/V
3. Measure mass by balance (grams)
4. Measure volume by displacement or length-width-height
5. Specific Gravity= Density Substance A/Density of Water
How would you calculate the density of?
•
Unknown liquid
•
Cube of wood
•
Small rock
•
Air

5. Dimensional Analysis
1. You have probably noticed that the periodic table features an arrangement of
elements with the following information
6
(atomic number)
C
(symbol)
12.01
(atomic weight)
2. The atomic weight is the weight of one mole of carbon atoms (6.02 x 1023).
3. Using a concept called dimensional analysis we can find out how many
atoms there are in 91.00 g.
91.00 g C x 1.00 moles C x 6.02 x 1023 atoms = 4.56 x 1024 atoms
12.01 g C
1.00 moles C

6. Specific Heat
1. Specific Heat: Number of calories or joules of energy required to raise the
temperature 1.0 gram of a substance 1.0oC. The property has wide-reaching
applications in the physical, chemical, and biological world.
2. Remind me about The Blubber Glove activity!
Specific Heat =
Cal
Grams x oC
3. Water has a specific heat of 1.0 Calorie per 1.0 gram per 0C