1. Measurement and Calculation

2. Scientific method
Scientific method is a series of steps followed to solve problems or strategies for drawing conclusion.

3. Scientific Method Experiment may not turn out as expected.
Experiment give much information and observations. Sometime unexpected result leads to new discovery.

4. Scientific Method
Before start investigation, must identify the possible Variables.
A factor that could affect the result of an experiment is called a variable.
A scientist changes variables one at a time to see which variable affects the outcome of the experiment.

5. Accuracy and Precision
The dictionary definitions of these two words do not clearly make the distinction as it is used in the science of measurement.
Accurate means "capable of providing a correct reading or measurement."
Precise means "exact, performance, or repeatable, reliable, getting the same measurement each time."

6. Example High Accuracy High Precision High Accuracy Low Precision
Low Accuracy High Precision

7. Example of Measurement
All measurements are assumed to be approximate with the last digit estimated.
The length in “cm” here is written as:
1.43 cm 1 2
The last digit “3” is estimated as 0.3 of the interval between 3 and 4.

8. Significant Digits and Numbers
All non zero numbers are significant
Zeros between non zero numbers are significant
Leading zeros are never significant
Trailing zeros are not significant if no decimal point
Trailing zeros are significant if decimal point
Rule: cm
2 significant figures cm
5 significant figures cm
4 significant figures
50.0 cm
3 significant figures
3 significant figures
50,600 cm

9. Rule 1. When approximate numbers are multiplied or divided, the number of significant digits in the final answer is the same as the number of significant digits in the least accurate of the factors.
Example:
Least significant factor (45) has only two (2) digits so only two are justified in the answer.
The appropriate way to write the answer is:
P = 7.0 N/m2

10. Rule 2. When approximate numbers are added or subtracted, the number of significant digits should equal the smallest number of decimal places of any term in the sum or difference.
Ex: cm cm – 2.89 cm = cm
Note that the least precise measure is 8.4 cm. Thus, answer must be to nearest tenth of cm even though it requires 3 significant digits.
The appropriate way to write the answer is:
15.2 cm

11. Rules for Rounding Numbers
Rule 1. If the remainder beyond the last digit to be reported is less than 5, drop the last digit.
Rule 2. If the remainder is greater than 5, increase the final digit by 1.
Rule 3. To prevent rounding bias, if the remainder is exactly 5, then round the last digit to the closest even number.

12. Examples
Rule 1. If the remainder beyond the last digit to be reported is less than 5, drop the last digit.
Round the following to 3 significant figures:
becomes
becomes
becomes ,600
95,632
becomes

13. Examples
Rule 2. If the remainder is greater than 5, increase the final digit by 1.
Round the following to 3 significant figures:
2.3452
becomes
becomes
becomes ,700
23,650.01
becomes

14. Rule 3. To prevent rounding bias, if the remainder is exactly 5, then round the last digit to the closest even number.
Round the following to 3 significant figures:
Examples
becomes
becomes
96,6500
becomes ,600
becomes

15. Systems of Units
SI System: The international system of units established by the International Committee on Weights and Measures. Such units are based on strict definitions and are the only official units for physical quantities.
US Customary Units (USCU): Older units still in common use by the United States, but definitions must be based on SI units. 15

16. Seven Fundamental Units

17. SI (System International Unit )
Chapter 1
SI (System International Unit ) 17

18. Units for Chemistry Quantity SI unit USCS unit Mass kilogram (kg)
In Chemistry we use only a few fundamental quantities: mass, volume, and mole etc. An additional quantity, density is derived from some of above units.
Quantity
SI unit
USCS unit
Mass
kilogram (kg)
slug (slug)
Volume
Cubic meter
( )
Cubic foot
Temperature
Celsius ( )
Fahrenheit (F)
Amount of substance
Mole

19. SI system
When working with numbers, be careful to distinguish between a quantity and its unit. Quantity describes something that has magnitude, size, or amount. Unit is a quantity adopted as a standard of measurement. 19

20. Base units can be too large or too small for some measurements, so the base units may be modified by attaching prefixes. 20

21. Procedure for Converting Units
Write down quantity to be converted.
Define each unit in terms of desired unit.
For each definition, form two conversion factors, one being the reciprocal of the other.
Multiply the quantity to be converted by those factors that will cancel all but the desired units. 21

22. Example 1: Convert 12 in. to centimeters given that 1 in. = 2.54 cm.
Step 1: Write down quantity to be converted.
12 in.
Step 2. Define each unit in terms of desired unit.
1 in. = 2.54 cm
Step 3. For each definition, form two conversion factors, one being the reciprocal of the other. 22

23. Example 1 (Cont. ): Convert 12 in. to centimeters given that 1 in. = 2
Example 1 (Cont.): Convert 12 in. to centimeters given that 1 in. = 2.54 cm.
From Step or
Step 4. Multiply by those factors that will cancel all but the desired units. Treat unit symbols algebraically.
Wrong Choice!
Correct Answer! 23

24. Practice problems Let’s do some example problem together
Convert 2.53 mL to Liters
Convert 1258 cm to meters
Convert 15 g to kilograms 24