What is Chemistry? Chemistry is: the study of matter & the changes it undergoes Composition Structure Properties Energy changes

Taking Measurements

Le Systeme International d’ Unites or SI System The SI System Around 1793, scientists all over the world began to agree upon a single measurement system called Le Systeme International d’ Unites or SI System 7 base units The idea was to create a unifying system of weights and measurements

This is the SI standard unit but the BASE unit is the GRAM Quantity Unit Symbol Mass kilogram kg Length meter m Time second s Amount of Substance mole mol Temperature Kelvin K Electric current Ampere A Luminous intensity candela cd Note: This is the SI standard unit but the BASE unit is the GRAM Crash Course: Units Where’s volume?? What’s missing?

Derived Units Combinations of base units Volume: amount of space taken up by an object Most common unit: cm3 = mL Density: ratio of mass to volume Common units: g/cm3 of g/mL or g/L Does not change for a given substance

Prefix Symbol Meaning Numerical Value Giga- G 109 1,000,000,000 Mega- M 106 1,000,000 Kilo- k 103 1,000 Hecto- h 102 100 Deka da 101 10 BASE g, l, m 1 Deci- d 10-1 .1 Centi- c 10-2 .01 Milli- m 10-3 .001 Micro- 10-6 .000001 Nano- n 10-9 .000000001

5.6 cm to m 56 mg to g 340 mm to cm 1.2 ML to L Practice Problems

Scientific Notation Some numbers are very large or very small, so a short hand notation is needed! Too large: 602,000,000,000,000,000,000,000 6.02 x 1023 Too small: 0.0000000000000000000000199 1.99 x 10-23

General Notation: N x 10n N is a number between 1 and 10 n is a positive or negative integer if n is a negative number, the full number is a small decimal if n is a positive number, the full number is a large number

Practice 3.69 x 10-4 4.382 x 10-2 8.37 x 10-7 1.245 x 105 8.7900 x 108 2.6091 x 102 0.00000568   0.00436 0.00000000002 2460000000 3456965 3400450

Factor-Label Method (Dimensional Analysis) Solve the following mathematical equation: 1 2 x 2 3 x 3 4 x 4 5 x 5 6 x 6 7 x 7 8 x 8 9 = 𝑚𝑖𝑙 ℎ𝑟 x ℎ𝑟 𝑚𝑖𝑛 x 𝑚𝑖𝑛 𝑠𝑒𝑐 x 𝑘𝑚 𝑚𝑖𝑙 x 𝑚 𝑘𝑚 =

Using Factor-Label Method Sample Problems: Converting 9.8 g to kg 9.8 g    x   1 kg        = 0.0098 kg               1000. g   Converting 9.8 kg to g 9.8 kg    x   1000. g        = 9800 g                   1 kg “1” goes in front of larger unit!

Density Practice Density Formula D = m V m D V

Measuring always involves some estimation Certain Digits: A digit that represents a mark on a scale or a non-blinking number on a display. Uncertain (Estimated) Digits: A digit that represents the space between the marks on a scale or a blinking number on a display. 24.62 what is certain? what is uncertain?

Making Measurements

Sig Figs: Using the Pacific/Atlantic Rule Step 1: Ask yourself: is the decimal point Present or Absent? Step 2: Determine which way to start counting If the decimal point is Present, start counting from the LEFT If the decimal point is Absent, start counting from the RIGHT A T L N I C bsent P A C I F resent

Pacific/Atlantic Rule Step 3: Start counting on Pacific or Atlantic side from the first NON-ZERO number. Count all numbers after the first non-zero number including zeros. Examples: 1234 = ________ sig figs 1204 = ________ sig figs 0.00234 = _______ sig figs 1230 = ______ sig figs 1234.0 = ______ sig figs Absent  Absent  Present  Absent  Present 

Using Sig. Figs. In Calculations Addition/Subtraction Rule Answer should contain least # of decimal places Multiplication/Division Rule Answer should contain least sig figs.

Do Now: Precision of Lab Instruments Record the following quantities to the correct number of decimal places. ________ L ________ mL _______ oC Convert your answer in A to milliliters: ________ mL Add your answer from A & B. Record using correct sig. figs. ________ mL

Analyzing Measurements

Accuracy & Precision in Measurements Accuracy: closeness of measurements to correct value Precision: closeness of a set of measurements to each other (assuming they’re made in the same way) When recording a measurement, an instrument that provides the most digits past the decimal is most precise.

Accuracy vs. Precision Example: A student measures the density of a sample of nickel. The density of nickel is 8.9 g.mL -1 Is this accurate or precise? Density Result (g.mL -1) Trial 1 7.8 Trial 2 7.7 Trial 3

% Error = Experimental – Accepted x 100 Percentage Error Accuracy of an individual value (or average) can be compared to the correct/accepted value % Error = Experimental – Accepted x 100 Accepted

Percentage Error What is the percentage error for a mass measurement of 17.7 g, given that the correct value is 21.2 g? A volume is measured experimentally as 4.26 mL. What is the percentage error, given that the accepted value is 4.15 mL?

Scientific Method

logical approach to solving problems SCIENTIFIC METHOD logical approach to solving problems Observation Problem Hypothesis Experiment Data Analysis Conclusion

You have 15 seconds to count how many letter “F”s you see in the following statement.

FEATURE FILMS ARE THE RESULT OF YEARS OF SCIENTIFIC STUDY COMBINED WITH THE EXPERIENCES OF YEARS.

Types of Observations Qualitative (think “quality”): observations using words Example: Quantitative (think “quantity”): observations using numbers and units. Example:

How observant are you?!?

PHYSICAL AND CHEMICAL CHANGES

Physical Properties and Changes physical property: characteristic that can be observed or measured without changing the identity of the substance. melting point, boiling point, density physical change: change in a substance that does not involve a change in the identity of the substance. dissolving, cutting, melting, and boiling

Chemical Properties and Changes chemical property: a substance’s ability to undergo changes that transform it into different substances Example: combustibility, reactivity chemical change: change in which one or more substances are converted into different substance Example: rusting, cooking food

Evidence of a Chemical Change Color change Temperature change Production of a gas Change in odor Formation of a precipitate Precipitate: insoluble solid that separates out of solution

Solubility and Phase changes are PHYSICAL!!!! NOTE: Solubility and Phase changes are PHYSICAL!!!!

In an experiment… System: specific portion of the experiment that has been selected for study Constant: experimental conditions that do not change Control: experimental condition that is used as a standard for comparison Variable: experimental condition that does change

SpongeBob loves to garden and wants to grow lots of pink flowers for his pal Sandy. He bought a special Flower Power fertilizer to see if it will help plants produce more flowers. He plants two plants of the same size in separate containers with the same amount of potting soil. He places one plant in a sunny window and waters it every day with fertilized water. He places the other plant on a shelf in a closet and waters it with plain water every other day. 1. What are Spongebob’s constants in his experiment? 2. What are Spongebob’s variables in his experiment? 3. What did Spongebob do wrong? 4. What should SpongeBob do to test the effectiveness of Flower Power fertilizer? Describe an experiment.

Amount of Fertilizer (g) Plant Growth (cm) 6 5 9 15 17 23 22 Independent Variable Dependent Variable Fertilizer Growth Direct Relationship Title Appropriate scale Axis labeled “Best fit” line

Direct Relationships When 2 quantities divided by each other gives a constant value K (constant value) = Y/X Ex: Density

Inverse Relationships When 2 quantities multiplied by each other gives a constant value K = X Y Ex: Boyle’s Law K = PV