Chapter 1. Chemistry and Measurements

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1 Chapter 1 Chemistry and Measurements

2 Section 1-1

3 Chemistry: the study of matter and the changes it undergoes. macroscopic: relating to large-scale analysis, visible to the naked eye microscopic: not visible to the naked eye

4 Matter: anything that has mass and occupies space. matter as a pure substance element compound

5 Element: substance that cannot be separated into simpler substances by chemical means. Gold Diamond (carbon) 118 elements have been observed (Officially confirmed by I.U.P.A.C.) 98 elements occur naturally on Earth e.g., gold, aluminum, lead, oxygen, carbon 20 elements have been created by scientists e.g., technetium, americium, seaborgium

6 6.2

7 Compound: substance composed of atoms of two or more elements chemically united in fixed proportions. Water, H 2 O Dry Ice, CO 2

8 Measurement: determines the quantity, dimensions, or extent of something, usually in comparison to a specific unit. Unit: a definite quantity adopted as a standard of measurement. Measurement 15.8 g numerical quantity specific unit (grams)

9 Precision vs. Accuracy Precision: relates to the degree of reproducibility or uncertainty of the measurement. Accuracy: refers to how close the measurement is to the true value.

10 Significant Figures (Sig Figs) Significant Figure (sig fig): A digit that is either reliably known or closely estimated. In your math classes, you have always assumed that numerical values are exact. In science, we deal with measured quantities. All measurements are approximations. No measuring device can give perfect measurements without experimental uncertainty.

11 Significant Figures (Sig Figs) Ø Any digit that is not zero is significant kg Ø Zeros between nonzero digits (captive zeros) are significant. 606 m Ø Zeros to the left of the first nonzero digit (leading zeros) are never significant L Ø Zeros at the right end of a number (trailing zeros) are significant only if the number contains a decimal point mg 3200 mg mg

12 How many significant figures are in each of the following measurements? 24 ml 3001 g m molecules 560 kg

13 How many sig figs are in each of the following measurements? 1) 20.6 cm 2) 500 g 3) ml 4) L 5) kg 6) mm

14 Section 1-2

15 Significant Figures (Sig Figs) Addition or Subtraction The answer cannot have more digits to the right of the decimal point than any of the original numbers one decimal place round off to two decimal places round off to 0.79

16 Significant Figures (Sig Figs) Multiplication or Division The number of significant figures in the result is set by the original number that has the smallest number of significant figures = = sig figs round to 3 sig figs = = sig figs round to 2 sig figs

17 Significant Figures (Sig Figs) Exact Numbers Numbers from definitions or numbers of objects are considered to have an infinite number of significant figures The average of three measured lengths: 6.64, 6.68 and = = 6.67 Because 3 is an exact number, it has an infinite number of sig figs. 7

18 Significant Figures (Sig Figs) Carry out the following calculations. Express your answer to the proper number of significant figures or decimal places. 1) ( ) ( ) 2)

19 Percent Error % error: comparison of the experimental value of a measurement to its accepted value, reported as a percent. % error = known value measured value known value 100% *error in textbook, page 22

20 Section 1-3

21 Scientific Notation The number of atoms in g of carbon: 602,200,000,000,000,000,000, The mass of a single carbon atom, in grams:

22 Scientific Notation The number of atoms in g of carbon: 602,200,000,000,000,000,000, The mass of a single carbon atom, in grams:

23 Scientific Notation 4,700,000,000 L L g g

24 Scientific Notation 4,700,000,000 L No credit will be given L g No credit will be given g

25 Section 1-4

26

27 Metric Conversion Mnemonic King (kilo, 1000) Henry (hecto, 100) Died (deca, 10) Unexpectedly (Unit of measurement) Drinking (deci 1/10) Chocolate (cen= 1/100) Milk (milli, 1/1,000)

28

29 Mass vs. Weight Mass: the quantity of matter that a sample contains. 1 kg Weight: the measure of the force due to gravity acting on a sample.

30 Section 1-5

31 Dimensional Analysis (Factor-Label) Method For problems that involve calculations, you must properly show your work in order to get full credit. 1) Always start with what you re given. 2) Set up conversion factors (fraction form), letting the units guide you. 3) Show your steps with units. 4) Express your answer with units, and with the correct number of sig figs.

32 Conversion of Units by Dimensional Analysis Example 1-7, page 35 Convert 129 hours to an equivalent number of days.

33 Conversion of Units by Dimensional Analysis Example 1-10, page 38 How many doughnuts can one purchase for $123 if doughnuts cost $3.25 per dozen?

34 Conversion of Units by Dimensional Analysis Example 1-12, page 39 Convert 55 mi/h to m/min. (1 mi = km)

35 Conversion of Units by Dimensional Analysis Extra problem: How many liters are in 1 m 3?

36 Section 1-6

37 100 C 373 K 0 C 273 K 40 C 233 K T K = T C + 273

38 Converting between Kelvin and degrees Celsius: T K = T C T C = T K 273 *Note: In this class, we DO NOT use the Fahrenheit scale.

39 Showing Work for Free-Response Problems For problems that involve calculations, you must show your work in order to get full credit. If an equation is used, write the equation. Substitute values with units. For conversion problems, show steps with units factor-label method or dimensional analysis. Express your answer with units, and with the correct number of sig figs.

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