5 Major Areas of Chemistry

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1 Chapter 1

2 What is Chemistry? Chemistry is the study of the composition of matter (matter is anything with mass and occupies space), its composition, properties, and the changes it undergoes. Has a definite affect on everyday life - taste of foods, grades of gasoline, etc.

3 5 Major Areas of Chemistry 1) Analytical Chemistry- concerned with the composition of substances. 2) Inorganic Chemistry- primarily deals with substances without carbon 3) Organic Chemistry- essentially all substances containing carbon 4) Biochemistry- Chemistry of living things 5) Physical Chemistry- describes the behavior of chemicals (ex. stretching); involves lots of math! Boundaries not firm they overlap and interact

4 The Scientific Method A logical approach to solving problems or answering questions. Starts with observation- noting and recording information and facts hypothesis- a proposed explanation for the observation; must be tested by an experiment

5 Steps in the Scientific Method 1. Observations (uses your senses) a) quantitative involves numbers = 95 o F b) qualitative is word description = hot 2. Formulating hypotheses (ideas) - possible explanation for the observation, or educated guess 3. Performing experiments (the test) - gathers new information to help decide whether the hypothesis is valid 4. Analyze Data 5. Draw Conclusions

6 Parts of an experiment A controlled experiment- designed to test the hypothesis. You can only test one thing. only two possible answers: 1) hypothesis is right 2) hypothesis is wrong We gather data and observations by doing the experiment Modify hypothesis - repeat the cycle

7 Scientific Method We deal with variables, or factors that can change. Two types: 1) Manipulated variable (or independent variable) is the one that we change 2) Responding variable (or dependent variable) is the one observed during the experiment For results to be accepted, the experiment needs to always produce the same result

8 Outcomes over the long term Theory (Model) - A set of well-tested hypotheses that give an overall explanation of some natural phenomenon not able to be proved Natural Law (or Scientific Law) - The same observation applies to many different systems; summarizes results - an example would be: the Law of Conservation of Mass

9 Law vs. Theory A law summarizes what has happened. A theory (model) is an attempt to explain why it happened this changes as new information is gathered.

10 - Page 22 Using your senses to obtain information The procedure that is used to test the hypothesis Hypothesis is a proposed explanation; should be based on previous knowledge; an educated guess Tells what happened A well-tested explanation for the observations; cannot be proven due to new discoveries

11 Measurements in Chemistry Chapter 2

12 Measurements Qualitative measurements are words, such as heavy or hot Quantitative measurements involve numbers (quantities), and depend on: 1) Remember the tool determines the number of significant digits a measurement will have.

13 Accuracy, Precision, and Error It is necessary to make good, reliable measurements in the lab Accuracy how close a measurement is to the true value Precision how close the measurements are to each other (reproducibility)

14 Precision and Accuracy Neither accurate nor precise Precise, but not accurate Precise AND accurate

15 Accuracy, Precision, and Error Accepted value = the correct value based on reliable references Experimental value = the value measured in the lab

16 Accuracy, Precision, and Error Error = accepted value exp. value Can be positive or negative Percent error = the absolute value of the error divided by the accepted value, then multiplied by 100% error % error = accepted value x 100%

17 The Fundamental SI Units

18 Significant Figures in Measurements Significant figures in a measurement include all of the digits that are known, plus one more digit that is estimated. Measurements must be reported to the correct number of significant figures.

19 Figure 3.5 Significant Figures - Page 67 Which measurement is the best? What is the measured value? What is the measured value? What is the measured value?

20 Sig Fig Practice #1 How many significant figures in the following? m 5 sig figs kg 4 sig figs 100,890 L 5 sig figs 3.29 x 10 3 s 3 sig figs These all come from some measurements cm 2 sig figs 3,200,000 ml 2 sig figs 5 dogs unlimited This is a counted value

21 Rounding Calculated Answers Addition and Subtraction The answer should be rounded to the same number of decimal places as the least number of decimal places in the problem.

22 Rules for Significant Figures in Mathematical Operations Addition and Subtraction: The number of decimal places in the result equals the number of decimal places in the least precise measurement = (3 sig figs)

23 - Page 70

24 Rounding Calculated Answers Multiplication and Division Round the answer to the same number of significant figures as the least number of significant figures in the problem.

25 - Page 71

26 Rules for Significant Figures in Mathematical Operations Multiplication and Division: # sig figs in the result equals the number in the least precise measurement used in the calculation x 2.0 = (2 sig figs)

27 Sig Fig Practice #2 Calculation Calculator says: Answer 3.24 m x 7.0 m m 2 23 m g 23.7 cm g/cm g/cm cm x cm cm cm m 3.0 s m/s 240 m/s lb x 3.23 ft lb ft 5870 lb ft g x 2.87 ml g/ml 2.96 g/ml

28 Scientific Notation Coefficient raised to power of 10 (ex. 1.3 x 10 7 ) Review: Textbook pages R56 & R57

29 Density The formula for density is: mass Density = volume Common units are: g/ml, or possibly g/cm 3, (or g/l for gas) Density is a physical property, and does not depend upon sample size

30 Density and Temperature What happens to the density as the temperature of an object increases? Mass remains the same Most substances increase in volume as temperature increases Thus, density generally decreases as the temperature increases

31 Density and Water Water is an important exception to the previous statement. Over certain temperatures, the volume of water increases as the temperature decreases (Do you want your water pipes to freeze in the winter?) Does ice float in liquid water?

32 Sink or Float The Density of water is 1g/ml Sink: the density of the object must be greater than the density of water(1g/ml) Float: the density of the object must be less than the density of water(1g/ml)

33 - Page 91

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