2. DO NOW…. Which liquid has the highest density? 5 2 3 1 4 Coussement, DeSchepper, et al., Brain Strains Power Puzzles  2002, page 16 least dense 1 < 3 < 5 < 2 < 4 most dense

3. INTENSIVEproperty Density is an INTENSIVE property of matter. - does NOT depend on quantity of matter. -Examples: color, melting point, boiling point, odor, density DIFFERENT THAN EXTENSIVE properties - depends on quantity of matter. - mass, volume, length Styrofoam Brick Gold

4. Density M = DV D = M VM V V = M DM D D M V ensity ass olume

5. The heaviest human brain ever recorded had a mass of 2.3kg. How many micrograms is that? 2.3 kg 1000 g 1 x 10 6 µg = 1 kg 1 g 2.3 x 10 9 µg

6. The density of lead is 11.34 g/cm 3. Find the density of lead in kg/m 3 11.34 g 1 kg 100 cm 100 cm 100 cm = cm 3 1000 g 1 m 1m1m 11,340 kg m 3

7. The average concentration of testosterone in the blood of a male in his twenties is 550 nanograms per deciliter. How many grams per cubic centimeter does this concentration represent? 550 ng 1 g 10 dL 1 L 1 mL = dL 1 x 10 9 ng 1 L 1000 mL 1 cm 3 5.5 x 10 -9 g cm 3

8. Density of Some Common Substances Density of Some Common Substance Substance Density (g / cm 3 ) Air 0.0013* Lithium 0.53 Ice 0.917 Water 1.00 Aluminum 2.70 Iron 7.86 Lead 11.4 Gold 19.3 Density of Some Common Substance Substance Density (g / cm 3 ) Air 0.0013* Lithium 0.53 Ice 0.917 Water 1.00 Aluminum 2.70 Iron 7.86 Lead 11.4 Gold 19.3 *at 0 o C and 1 atm pressure

9. Consider Equal Masses Equal masses… …but unequal volumes. The object with the larger volume (aluminum cube) has the density. aluminum gold Dorin, Demmin, Gabel, Chemistry The Study of Matter, 3 rd Edition, 1990, page 71 smaller Christopherson Scales Made in Normal, Illinois USA

10. Comparing Densities (g/cm 3 ) Jaffe, New World of Chemistry, 1955, page 66 0.9 0.25 water 1.0 ice cork aluminum 2.7

11. Density Practice Problems 1.What is the density of carbon dioxide gas if 0.196 g occupies a volume of 100. mL? 0.196 g 100. mL 1.96 x 10 -3 g/mL D = M VM V

12. Density Practice Problems 2.An irregularly shaped stone has a volume of 5.0 mL. The density of the stone is 1.75 g/mL. What is the mass of this stone? 1.75 g/mL x 5.0 mL 8.8 g M = D x V

13. Density Practice Problems 3.A sample of iron has a mass of 94 g and a density of 7.8 g/cm 3. What is the volume of the iron? 94 g 7.8 g/cm 3 12 cm 3 V = M DM D

14. SI Prefixes mega-1,000,000 kilo-1,000 deci- 1 / 10 centi- 1 / 100 milli- 1 / 1,000 micro- 1 / 1,000,000 Also know… 1 mL = 1 cm 3

15. Practice Measuring 4.5 cm 4.54 cm 3.0 cm Timberlake, Chemistry 7 th Edition, page 7 cm 0 12345 0 12345 0 12345

16. 20 10 15 mL ? 15.0 mL

17. Scientific Notation  Calculating with scientific notation (5.44 × 10 7 g) = ?? (8.1 × 10 4 mol) 5.44 EE ÷ ÷ 78.1 = 671.6049383= 670 g/mol= 6.7 × 10 2 g/mol Type on your calculator: Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem EE = = 4

18. Scientific Notation  Converting into scientific notation:  Move decimal until there’s 1 digit to its left. Places moved = exponent.  Large # (>1)  positive exponent Small # (<1)  negative exponent  Only include sig. figs. 65,000 kg  6.5 × 10 4 kg Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

19. Scientific Notation 2,400,000  g 0.00256 kg 7  10 -5 km 6.2  10 4 mm Practice Problems 2.4  10 6  g 2.56  10 -3 kg 0.00007 km 62,000 mm Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

20. Significant figures: Rules for zeros Leading zeros are not significant. Captive zeros are significant. Trailing zeros are significant, only IF there is a decimal point somewhere in the number. Leading zero Captive zero Trailing zero 0.421 4012 114.20 – three significant figures – four significant figures – five significant figures 11,420 – four significant figures

21. Other Ways of Thinking About Significant Figures…  All digits are significant EXCEPT…  Leading zeros -- 0.0025  Trailing zeros without a decimal point -- 2,500  Pacific Ocean = “Present” and Atlantic Ocean = “Absent” (ask about this one in class ) Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

22. Significant Figures  Calculating with Sig Figs (con’t)  Exact Numbers do not limit the # of sig figs in the answer.  Counting numbers: 12 students  Exact conversions: 1 m = 100 cm Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

23. Significant Figures  Calculating with Sig Figs  Multiply/Divide - The # with the fewest sig figs determines the # of sig figs in the answer. (13.91g/cm 3 )(23.3cm 3 ) = 324.103g 324 g 4 SF 3 SF Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

24. Significant Figures  Calculating with Sig Figs  Add/Subtract - The # with the fewest places after the decimal point determines the # of sig figs in the answer. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem 18.9g - 0.84 g  18.1 g 18.06 g

25. Significant Figures (15.30 g) ÷ (6.4 mL) Practice Problems = 2.390625 g/mL  18.1 g 18.9g - 0.84 g 18.06 g 4 SF2 SF  2.4 g/mL 2 SF Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem