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Nature of Chemistry- Qualitative Relationships

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Presentation on theme: "Nature of Chemistry- Qualitative Relationships"— Presentation transcript:

1 Nature of Chemistry- Qualitative Relationships

2 Must repeat several times.
Scientific Method Observation State the Problem Gather Information If hypothesis is proven false, propose new hypothesis and experiment. Hypothesis Experiment Must repeat several times. Theory Law

3 Laws & Theories theory: explanation based on supported hypothesis -broad principle of nature supported over many years -can be modified -can lead to new conclusions law: describes something known to happen without error -doesn’t explain why it happens -there are no exceptions -several scientists come to the same conclusion

4 Experiemental Data When we perform experiments, data is separated into 2 types: 1. qualitative-uses the 5 senses -physical characteristics 2. quantitative-numerical data -measurable

5 Experimental Variables
There are 2 types of variables when doing an experiment: 1. independent: variable you change 2. dependent: variable that changes due to a change in the independent variable. It is also important to have controls, or standards for comparison.

6 SI Units and Derived Units
The SI base unit is the unit in a system of measurements that is based on an object or event in the physical world.     Unit Quantity Symbol Abbrev. length l meter m mass kilogram kg time t second s temperature T Kelvin K amount of substance n mole mol electric current I ampere A luminous intensity Iv candela cd

7 Temperature There are three possible temperature scales:
Celsius-based on metric system -based on temp when water freezes and boils Kelvin-SI Unit -based on the idea of absolute zero, the lowest possible theoretical temperature -will discuss more in Ch 14 (Gas Laws) 3. Farenheit-what we are used to using

8 Converting Temperature
Celsius to Kelvin / Kelvin to Celcius TK = TC TC = TK 2. Celsius to Farenheit / Farenheit to Celsius TC = (TF -32oF)5oC 9oF TF = TC 9oF oF 5oC

9 SI Units and Derived Units
derived unit: unit that is defined by a combination of base units -volume: space occupied by an object; unit is the liter, L, for liquids and gases, or cubic centimeter, cm3, for solids V = l x l x l -density: ratio of the mass of an object to its volume; unit is g/mL or g/cm3 since 1 mL = 1cm3 D = m/V

10 Prefixes Prefix Symbol Meaning Multiple of Base Unit 10n yotta- Y
septillion 1,000,000,000,000,000,000,000,000 1024 zetta- Z sextillion 1,000,000,000,000,000,000,000 1021 exa- E quintillion 1,000,000,000,000,000,000 1018 peta- P quadrillion 1,000,000,000,000,000 1015 tera- T trillion 1,000,000,000,000 1012 giga- G billion 1,000,000,000 109 mega- M million 1,000,000 106 kilo- k thousand 1000 103 hecto- h hundred 100 102 deca- da ten 10 101 base deci- d tenth 0.1 10-1 centi- c hundredth 0.01 10-2 milli- m thousandth 0.001 10-3 micro- millionth 10-6 nano- n billionth 10-9 pico- p trillionth 10-12 femto- f quadrillionth 10-15 atto- a quintillionth 10-18 zepto- z sextillionth 10-21 yokto- y septillionth 10-24

11 Converting Between Prefixes
Dimensional analysis is a method of problem-solving that focuses on the units used to describe matter. A conversion factor is a ratio of equivalent values used to express the same quantity in different units. -they change the units of a quantity without changing its value -ratio of units, such as 1 km 1000m -set up so the units you don’t need cancel out 48 m x 1 km = km 1000 m

12 Dimensional Analysis It is common in scientific problems to use dimensional analysis to convert more than one unit at a time. What is the speed of 550 m/s in km/min? Convert m to km Convert s to min

13 Dimensional Analysis Sometimes we need to convert from metric to standard (and vice versa). -some of these common conversions you will need to know are: 1 cm3 = 1 mL s = 1 min 1 in = 2.54 cm 60 min = 1 hr 1 ft = 12 in Practice: 152 cm = ____ m in = ____ ft

14 Significant Figures significant figures: number of all known digits in a measurement plus one estimated digit. -allows more precision in measurement -not all measuring devices show the same precision Example: In the following measurement, what are the known values and what is the estimated value? 16.25 mL known = 162 estimated = 5

15 Significant Figures-Rules
The easiest way to determine significant figures of a given number is by using the Pacific/Atlantic rules. 1. Decimal point PRESENT, start from the PACIFIC. -Begin counting on the left hand (Pacific) side of the number. Move toward the right and start with the first nonzero number. has 7 significant figures has 2 significant figures

16 Significant Figures-Rules
2. Decimal point ABSENT, start from the ATLANTIC. -Begin counting on the right hand (Atlantic) side of the number. Move toward the left and start with the first nonzero digit. 1200 has 2 significant figures 1207 has 4 significant figures Zeros that act as placeholders are not significant: and 1200

17 Significant Figures Practice 1
Copy the following questions and answer. Determine the number of significant figures in the following numbers. 1) ) ) 2) ) ) 3) )

18 Significant Figures and Rounding
Suppose you are asked to find the density of an object with a m=of g and whose V=14.2 cm3. Using a calculator, you get , which has 8 significant figures. Does this answer make sense? No. The mass only has 4 sig figs and the volume has 3. Your answer would be more precise than the starting information.

19 Significant Figures and Rounding
How would you correctly round this? By using the starting data with the fewest sig figs (when multiplying/dividing), which is 3: g/cm3 -when adding/subtracting, your answer will have the smallest number of decimal places based on the starting information. 3.12 m m = 6.32 m = 6.3 m

20 Significant Figures Practice 2
Perform the following operations expressing the answer in the correct number of significant figures. 1) m x m 2) m2 ÷ 42 m 3) mL mL + 6 mL Round to four significant figures. 6) kg 7) g

21 Accuracy and Precision
Density collected by Three Students. A B C T1 (g/cm3) 1.54 1.40 1.70 T2 (g/cm3) 1.60 1.68 1.69 T3 (g/cm3) 1.57 1.45 1.71 Avg. (g/cm3) 1.51 accuracy: how close a measured value is to an accepted value. precision: how close a series of measurements are to one another. -may not be accurate Example: For the following data, the actual density value is 1.59 g/cm3.

22 Percent Error percent error: ratio of the difference in the measured value and accepted value divided by the accepted value multiplied by 100 % error = │measured value – accepted value│ x 100 accepted value Ex: Calculate the % error of Student A’s Average Data. % error = │1.57 g/cm3 – 1.59 g/cm3 │ x 100 1.59 g/cm3 = │-0.02 g/cm3 │ x 100 = 0.02 g/cm3 x 100 = 1 %

23 Accuracy & Precision Practice
Density collected by Three Students. A B C T1 (g/cm3) 1.54 1.40 1.70 T2 (g/cm3) 1.60 1.68 1.69 T3 (g/cm3) 1.57 1.45 1.71 Avg. (g/cm3) 1.51 Calculate the percent error for each of the three students (A, B, C). The accepted value is 1.59 g/cm3)

24 Graphing In chemistry, we mainly deal with line graphs.
A graph is used to reveal patterns by giving a visual representation of data. a. must know the independent (x axis) and dependent variable (y axis) b. determine the range of data that needs to be plotted for each axis: try to take up at least ¾ of the paper -use a pencil and ruler c. number and label each axis: don’t forget the units d. plot the points and draw a line of best fit -curved or straight e. title the graph

25 Graphing-You Try Graph the data set A for T1, T2, and T3 using the rules you know. Density collected by Three Students. A B C T1 (g/cm3) 1.54 1.40 1.70 T2 (g/cm3) 1.60 1.68 1.69 T3 (g/cm3) 1.57 1.45 1.71 Avg. (g/cm3) 1.51


27 Graphing Practice Problem Solving Lab (p 44)
Answer the Analysis and Thinking Critically questions on the back of the graph. Data: Analysis: What does the graph tell you about the relationship between speed and stopping distance? Explain using complete sentences. Predict whether reaction distance or braking distance will increase more rapidly as the speed increases. Explain using complete sentences. Speed (m/s) 11 16 20 25 29 Stopping Distance (m) 18 32 49 68 92


29 Scientific Notation Values in science are often very large or very small, requiring a lot of zeros. Scientists use scientific notation, a short hand method of writing extremely large or small numbers, to make calculations easier. -scientific notation is a value written as a simple number multiplied by a power of 10.

30 Power of 10 equivalents: = 10,000 = 1000 = 100 = 10 = 1 = 0.1 = = =

31 Writing Scientific Notation
1. Write the first 2 or 3 digits as a simple number with only one digit to the left of the decimal point. 2. Count the number of decimal places you move the decimal. This will give you your power of 10. -If you move the decimal to the left the power of ten will be positive. -If you move the decimal to the right the power of ten will be negative. If you must adjust the decimal: -if moved to the left, add to the exponent -if moved to the right, subtract from the exponent

32 Dividing with Scientific Nototation Example
Lets calculate the time it takes for light to travel from Neptune to Earth. The speed of light is 3.0x108m/s and the distance from Neptune to Earth is 4.6x1012m. -Use the formula v = d/t -Rearrange to solve for t: t = d/v -d = 4.6x1012m, v = 3.0x108m/s, t = ? - t = 4.6x1012m = 1.5x104s (no adjustment) 3.0x108m/s

33 Dividing with Scientific Notation Practice
Convert the following into scientific notation. Convert the following into common form. x x104 Solve the following: x105 ÷ 3.0x102 2.0x104 ÷ 5x102 Don’t forget about significant figures!!!

34 Multiplying with Scientific Notation
Example If it takes 2.7 x 1023 seconds for light to travel from one planet to another, how far apart are the planets? Remember light travels at a speed of 3.0 x 108 m/s. -Use the formula v = d/t. -Rearrange to solve for d: d = vt -d = ?, v = 3.0 x 108 m/s d = vt = (2.7 x1023 s) (3.0 x 108 m/s) = 8.1 x 1031 m (no adjustment necessry)

35 Multiplying with Scientific Notation Practice
Don’t forget significant figures when doing the calculations. (1.2x103)(2.4x104) 2. (4.6x10-3)(2.3x10-5) 3. (6.02x105)(2.0x102) 4. (2.70x105)(3.0x10-2)

36 Combined Measurement Practice
Show all work, including units!! Metrics: Convert the following: 1) 35 mL = ____ L 2) kg = ____ g Dimensional Analysis: Convert the following: 3) 3500 s = ____ hr 4) 4.2 L =_____ cm3 Scientific Notation: Convert to scientific notation: 5) ) ) Scientific Notation: Convert to standard notation: 8) 1.5x ) 3.35x10-6 Calculations: using Scientific Notation 10) (1.5 x 103)(3.5x105) 11) (3.45x10-3)/(1.2x 10-2) 12) (7.6x10-3)(8.2x107) 13) (6.8x107)/(2.2x10-5)

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