1. Chapter 1 – Matter and Measurement Why study chemistry?

2. Matter and Measurement Chemistry is the study of matter and how it interacts with other types of matter.

3. Matter and Measurement Matter consists of elements or compounds. Element Compound

4. Matter and Measurement The three states of matter Solid Liquid Gas

5. Matter and Measurement Classification of Matter

6. Matter and Measurement Properties of Matter Physical Properties – characteristics that can be observed without changing the identity of the substance.

7. Matter and Measurement Properties of Matter Chemical Properties – describes how a substance can change by reacting with another substance.

8. Matter and Measurement Units of Measurement Metric System - Adopted in 1960. Derived from the SI system (Systeme International d’Unites).

9. Matter and Measurement Units of Measurement Metric System Base Units

10. Matter and Measurement Measuring Temperature Many units for measuring temperature exist. Lord Kelvin discovered the theoretical coldest temperature of matter. 0 Kelvin (Absolute Zero) 0 Kelvin = -273.15°C

11. Matter and Measurement Measuring Temperature Kelvin temperature = (Celsius temperature) – (273.15°C)

12. Matter and Measurement Metric System Prefixes

13. Matter and Measurement Metric System Conversions Using Dimensional Analysis Dimensional Analysis is the process of multiplying a number by a fraction to cancel units and convert into new units. Convert 45.0 μg into ng. 45.0 μg x ____________ =

14. Matter and Measurement Metric System Conversions Using Dimensional Analysis Convert 2.0 x 10 -3 m into mm. Convert 8.3 x 10 12 nmol into mmol. Convert 2.0 m 2 into cm 2.

15. Matter and Measurement Other Conversions Using Dimensional Analysis Convert 0.35 lbs. into kilograms. Convert 3.0 mmol of O 2 into grams. (1 mole of O 2 = 32.00 g.) Convert 19.0 g/cm 3 into kg/m 3.

16. Matter and Measurement Significant Figures – “You can only be as accurate as your least accurate instrument.” A significant figure is a measured value. All nonzero numbers are significant. Zeros are sometimes significant. Captive zeros are significant. (203 m) 3 s.f. Leading zeros are not significant. (0.002 g) 1 s.f. Trailing zeros are significant if the number contains a decimal point. (450 s) 2 s.f. (1021.00 μmol) 6 s.f

17. Matter and Measurement Significant Figures – “You can only be as accurate as your least accurate instrument.”

18. Matter and Measurement Significant Figures – “You can only be as accurate as your least accurate instrument.”

19. Matter and Measurement Significant Figures – “You can only be as accurate as your least accurate instrument.”

20. Matter and Measurement Significant Figures and Scientific Notation The sig figs of a value is determined by the coefficient. 2.300 x 10 -3 kg = 4 s.f. 6.02 x 10 23 atoms = 3 s.f. 3 x 10 2 students = 1 s.f.

21. Matter and Measurement Significant Figures and Calculations Multiplication and Division – Answer is rounded to the same number of sig figs as the number with the least sig figs in the problem. 45 m x 2.00 m = 9.0 x 10 1 m 2 or 90. m 2 3.500 g / 25.0 g = 0.140

22. Matter and Measurement Significant Figures and Calculations Addition and Subtraction– Answer is rounded to the number with the least number of decimal places. 3.0000 mol – 0.120 mol = 2.880 mol 100. g + 0.1000 g = 100 g