1. Scientific Conventions and Mathematical Procedures
Accuracy, precision, significant figures, scientific notation, conversions, dimensional analysis

2. FRIDAY we talked about – Accuracy and Precision
Closeness to the true value
Requires a tool that is calibrated and used properly
Repeatable measurements
How close do the measurements agree with each other

3. Added and subtracted #s column “mass of Water”
Multiply and divide Density

4. Significant digits
Significant digits are used to convey information about the precision of measurement. When using measured quantities in calculations the following rules should be applied to express significant figures correctly.
In addition or subtraction, express the answer with the same number of decimal places as the quantity having the fewest decimal places.
14.25g g =26.50g g – 10.1g = 5.1g
In multiplication or division calculations express the answer with the same number of significant figures as the quantity having the fewest number of significant figures
20.01 x = cm x 5.10 cm= 66 cm2

5. Significant Digits All non-zero digits are significant
All “captured zeros” are significant
In numbers that DO NOT have a decimal final zeros are not significant
In numbers that have a decimal
Leading zeros are not significant
Final zeros are significant
Special Rules
All digits are significant in correct scientific notation
A decimal can be added to make digits significant

6. Scientific Notation using the powers of ten to express very large and very small numbers
To add and subtract scientific notation you must convert the numbers to the same exponent
To multiply you must add the exponents
To divide you must subtract the exponents

7. TO AVOID ERRORS LEARN TO USE THE CALCULATOR- TODAY
There is a button that says EE, it will save you lots of time, confusion and give us time to focus on higher level chemistry concepts