1. Chapter 1 The Nature of Chemistry

2. Section 1.1 - What is Chemistry?  Is the study of the composition of matter and the changes they undergo.  Matter  Anything that takes up space and has mass.

3. Two types of chemical careers: n Applied Chemistry- use the knowledge of chemistry in their profession. – Nuclear Submarine engineer, Teacher, Pharmacist, etc. n Pure Chemistry- use the knowledge to discover new information on chemistry. – Scientist studying the depletion of ozone, or any scientific unknowns.

4. Section 1.1 n Chemistry is the Central Science. – It overlaps many other sciences, do to the fact that everything is made up of chemicals.

5. Section 1.1 n Five major branches of chemistry: – Organic chemistry n Living or once living material, contain Carbon and Hydrogen. – Inorganic chemistry n Nonliving material, metals, plastic, minerals, etc. – Analytical chemistry n Qualitative and Quantitative study of matter. – Physical chemistry n Energies within the atoms and subatomic particles. – Biochemistry n Chemistry within living organisms.

6. Section 1.1 n Determine which branch of Chemistry is most appropriate to the study: – Study of the respiration in fish. – Amount of mercury levels within fish at in the Allegheny river. – Process of converting crude oil into motor oil. – Determining the energy of a single electron. – Improving the hardness of steel.

7. Section 1.2 n Steps of the Scientific Method – Observation – Hypothesize – Experiment – Conclude (Theory) n Natural Law – helps to describe how nature behaves but does not explain why nature behaves in that particular way. n Theory – statement explaining how things occur in relationship to the natural law. Can still be proven wrong. “superhypothesis”

8. Section 1.3 Safety in Laboratory n Follow teacher’s directions. n Notify teacher of problems. n Know how to use the safety equipment. – Emergency eyewash and shower. n Wear safety goggles. n Tie back long hair and loose clothing. n If it’s hot, let it cool. n Carry chemicals with caution. n Dispose of chemical waste properly. n Clean Up!!!

9. 1.3 Symbols. Safety clothing Safety gloves Safety goggles Heating Poison Corrosive Fumes Fire Electrical Outlet Radioactive Wash hands Explosive Waste Disposal

10. Section 1.6 Working with Numbers n Scientific Notation or Exponential Notation – n. x 10 e – Where n is a digit 1-9. e is the exponent.

11. Section 1.6 Working with Numbers n Converting to scientific notation – Must move the decimal to the ONES position. – Number of spaces needed is the exponent. – Moving the decimal left, is a positive exponent. – Moving the decimal right, is a negative exponent.

12. Section 1.6 Working with Numbers n Convert the following to scientific notation. – 2300. cm.00522 kg1.432m

13. Section 1.6 Working with Numbers n Converting to standard notation. – Positive exponent, move the decimal to the right the number of places as the exponent. – Negative exponent, move the decimal to the left the number of places as the exponent.

14. Section 1.6 Working with Numbers n Convert the following to standard notation. – 4.55 x 10 3 m1.24 x 10 -4 kg

15. Section 1.4 Units of Measurement n Metric System – The International System of Units Standard – Based upon tens or decimal places. – Used throughout the world.

16. Section 1.4 Units of Measurement n International System of Units (S.I.) – Le Systeme International d`Unites.

17. Section 1.4 Units of Measurement Standard S.I. Units – Length – meter (m) – Mass – kilogram (kg) n Derived Units: – Area – length x width = (m 2 ) – Volume – length x width x height = (m 3 ) Liquid Volume – (mL)

18. Section 1.4 Units of Measurement n Other common S.I. Units used in chemistry. – Pressure – pascals (Pa) – Temperature – kelvins (K)

19. Section 1.4 Units of Measurement n Converting metric units using prefixes – Prefix and Value n Large Prefixes: – Tera (T) = 10 12 – Giga (G) = 10 9 – Mega (M) = 10 6 – Kilo (k) = 10 3 – Hecto (h) = 10 2 – Deca (da) = 10 1 n Base – no prefix (m, g, L, Hz or K ….) n Small Prefixes: – deci (d) = 10 -1 – centi (c) = 10 -2 – milli (m) = 10 -3 – micro (μ) = 10 -6 – nano (n) = 10 -9 – pico (p) = 10 -12

20. Section 1.5 Uncertainty in Measurement n Precision – Repeatable measurement. n Accuracy – Closeness to the correct value. – Describe the following lists of measure by accurate or precise: (+/-.5 error) n 4.55g, 4.60g, 4.58g ; The true value is 4.60g n 1.2m, 2.0m, 2.5 m ; The true value is 1.0m

21. Section 1.6 Working with Numbers n Significant Digits – The certain digits and the estimated digits are together called the significant digits.

22. Rules for significant digits: – All non-zero digits are significant. n 1234 5663121112 – Zeroes in between two non-zero digits are always significant. n 1031004102003 – Zeroes after a non-zero digits are only significant if the number has a decimal. n 200.3450.10. – Zeroes after non-zero digits are not significant if the number has no decimal. n 200400204230 – Zeroes in front of non-zero digits are never significant. n.000040.0343.00430

23. Section 1.6 Working with Numbers n Significant Digits in Calculations – Round all answers to the fewest significant digits that is shown in the given. – Standard rule is to round all to 3 sig figs. – Scientific Notation is the easiest way of writing the correct number of significant digits. n Every number in scientific notation before the (x10 e ) will always be a significant digit. n Example – 4000 g has 1 significant digit – 4.00 x 10 3 g has 3 significant digits.

24. Section 1.6 Working with Numbers n Practice, answer the following problems and round to 3 significant figures: 1) 303 cm + 900 cm + 23 cm = 2) 4.5 x 10 5 g + 1.2 x 10 3 g = 3) 60.7 cm  205 cm  4 cm = 4) 22.2 g / 75 cm 3 =

25. Using dimensional analysis with prefixes. n Dimensional Analysis – Technique of converting units and solving problems. – Uses Conversion Factors: n Units of equality. n Set prefix value equal to unit of the base value. n Ex. mm to m: 1 mm = 1x10 -3 m – Always start with the known value and express it as a fraction over 1. – Setup the conversion so that the unit of the known cancels out the unit in the conversion.

26. Section 1.4 Units of Measurement n Convert 30 cm to m. n Convert 50 kg to g.

27. Section 1.4 Units of Measurement n Convert 4 m to cm. n Convert 400 g to kg.

28. Section 1.4 Units of Measurement n Multiple prefix conversions use two conversion factors. – Example: Converting 400 cm to km. n 400 cm = ____ km n c = 10 -2 and k = 10 3 n 1x10 -2 m = 1cm and 1x10 3 km = 1m n 4 x 10 -3 km

29. Section 1.4 n Practice 1. 8.2 x 10 -23 cm = ? nm 2. 1.3 x 10 -2 mm = ? km 3. 5.2 x 10 8 pm = ? m 4. 2.6 x 10 19 Mm = ? mm

30. Conversion of Cubic Units of Volume n Ideal method of converting cubic or squared units, is by using the basic units. – 1 cm 3 = 1 mL – 1 m 3 = 1000 L – 1 x 10 6 cm 3 = 1 m 3, How? n Note the basic metric equality between the units: n 100 cm = 1 m or (1 x 10 2 cm = 1 m) n Cube both sides, (1x10 2 cm) 3 =(1 m) 3

31. Conversion of Cubic Units of Volume n 350 mm 3 = ? cm 3 n 1 mm = 1x10 -3 m n Cube both units and values. n 1 mm 3 = 1x10 -9 m 3 and n 1cm = 1x10 -2 m n Cubed : 1cm 3 = 1x10 -6 m 3

32. Conversion of Cubic Units of Volume n Practice – 1.2 x 10 -3 nm 3 = ? mL – 1.4 x 10 -2 m 3 = ? mm 3

33. Section 1.5 Uncertainty in Measurement n Recording a Measurement – All known digits of a measurement and an estimated digit should always be recorded. n Example: Using a graduated cylinder, you can record known digits to the ones and estimate the tenths.

34. Section 1.7 Problem Solving n Dimensional Analysis – Technique of converting units and solving problems. – Uses Conversion Factors: n Units of equality. n 1ft = 12in – Always start with the known value and express it as a fraction over 1. – Setup the conversion so that the unit of the known cancels out the unit in the conversion.

35. Section 1.7 Problem Solving n Example Problem: – How many feet are in 400. inches? n Conversion 1 ft = 12 in n Known 400 in

36. Section 1.7 Problem Solving n Multiple step problem. – How many cm are in 2 miles?

37. Section 1.7 Problem Solving n Complex Problems – How many mi/hr are equivalent to 60 ft/s?

38. Section 1.7 Problem Solving n Four-Step Problem-Solving Strategy – Analyze – Plan – Solve – Evaluate

39. Section 1.7 Problem Solving n Determine the number of seconds in 2009 years. Not counting leap years.

40. p.p#37 n If 1500 white blood cells (WBC) are lined up side by side they would form a row 1.0 in long. What is the average diameter in micrometers of a single WBC? (1in = 2.54cm)

41. p.p. #38 n A radio wave travels 186000 miles per second. How many kilometers will the wave travel in one microsecond? (1 mi = 1.61 km)

42. p.p. #40 n Eggs are shipped from a poultry farm in trucks. The eggs are packed in cartons of one dozen eggs each; the cartons are placed in crates that hold 20 cartons each. The crates are stacked in the trucks, 5 crates across, 25 crates deep, and 25 crates high. How many eggs are in 5 truckloads?

43. p.p. #41 n Iodine is an essential nutrient in our diet that prevents goiter. To obtain enough iodine, we can use iodized salt, which is.01%NaI by mass. How many kilograms of NaI should be added to 1000kg of table salt to achieve this percentage of NaI?

44. p.p. #42 n The antlers of a deer are 50% Ca by mass. The calcium comes from leaves that the deer eat. The leaves are.07%Ca by mass. How many kilograms of leaves would a deer need to eat in order to provide enough calcium to grow antlers weighing 3 kilograms?

45. Section 1.6 Working with Numbers n Percent Error – A percent value, showing the amount error in an experiment.

46. Example: n Allison and Todd had completed an experiment together and found the density of water to be.839 g/mL. Knowing the true density of water to be 1g/mL, what was their percent error?

47. Section 1.6 Working with Numbers n Conversions or Ratios – Equalities expressed as fractions. n Speed = distance / time n Density = mass / volume – Knowing the density of water = 1 g/cm 3 n What is the mass of 200 cm 3 of water? n What is the volume of 34g of water?

48. Section 1.6 Density n What is the mass of 200 cm 3 of water? n Knowing the density of water is 1g/cm 3 – Answer :  What is the volume of 34 g of water?  Answer :