Download Unit 1 Foundations, Measurement, Safety and Matter

Name: ______Key_____ Block:______ Unit 1 Foundations, Measurement, Safety and Matter Unit 1: Significant Figures and Scientific Notation Scientific Notation Notes To put numbers in scientific notation: 1. Place the decimal after the ______first number moving left to right____. 2. Rewrite the number and multiply it by 10x. 3. Count the number of spaces you moved the decimal. This number is x (the exponent for the ten). 4. If the original number was less than one, the exponent is ___negative___. Practice Problems 5) 0.000 000 000 000 615 g 6.15 x 10‐13 g 98 000 000 000 m 9.8 x 1010 m 0.000 104 s 1.04 x 10‐4 s 407 302 000 000 000 Pa 4.07302 x 1014 Pa 4.38 x 10‐7 km 0.000 000 438 km 1.89 x 104 L 18 900 L 7.4 x 10‐4 g 0.000 74 g 6) 7) 8) 9) 10) 11) 3 Percent Error Notes
Accuracy, Precision, and Error Accuracy – the __closeness____of a measurement to the__true___ value of what is being measured ‐ accuracy can be determined by _one_ measurement ‐ depends on the _quality_of the _____measurement___ Precision – describes the closeness, or ___reproducibility___, of a set of measurements taken under the _same_ conditions ‐ precision is determined by ___more than one _measurement ‐depends on the __skills___of the person measuring Accepted (or theoretical) value – a quantity used by general agreement of the scientific community Experimental (or actual) value – a quantitative value measured during an experiment Error – the __percent error___ between the__actual ___ value and the__experimental__ value Error = Error = E – A E = Experimental value A= Accepted value Percent error = the percent that a measured value differs from an accepted value |
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Example: Peter measured the volume of a 2 liter bottle of soda. The actual volume of the soda was 1.87 Liters. What is the percent error of the volume of soda? %E = │ E — A│ x 100 = A %E = │ 1.87 L — 2.00L│ x 100 = 6.5% 2.00 L 4 Significant Figures The Atlantic/Pacific Rule for Determining Significant Figures
PACIFIC
(Present)
ATLANTIC
(Absent)
1) look for the presence, or not, of a decimal point
- this will tell you which side to start counting from
- Pacific: left
- Atlantic: right
2) if there is a decimal point you start counting from the left side of the number
- starting from the very left side of the number, look for the first non-zero number
- count the first non-zero number and every number (0-9) after that
- example: 0.00010
- because there is a decimal point, we start from the left side of the equation L0.00010, and
look for the first non-zero number
0.00010
- count that number and every number after that regardless of what the number is (0-9)
- in this case there are 2 significant figures
- 0.00010
3) if there is not a decimal point you start counting from the right side of the number
- starting from the very right side of the number, look for the first non-zero number
- count the first non-zero number and every number (0-9) after that
- example: 721000
- because there is a decimal point, we start from the right side of the equation 7210007, and
look for the first non-zero number
721000
- count that number and every number after that regardless of what the number is (0-9)
- in this case there are
5 Significant Figures: All exact digits of a measurement plus one estimated digit. Brief determination of the number of significant digits Rule #1: All non‐zero numbers are significant 732 g Rule #2: Any zero’s between non‐zero numbers are significant 301 cm Rule #3: If there is a decimal point, any zero’s to the right of the last non‐zero are significant a. 320. kg 3 significant figures b. 320 kg 2 significant figures c. 0.70 m 2 significant figures d. 0.070 m 2 significant figures Rule #4: Any number that is used to count things or is a direct conversion has infinite significant figures. a. 45 desks infinite significant figures b. 60 s = 1 minute infinite significant figures c. 10 pennies = 1 dime infinite significant figures d. 4 beakers infinite significant figures Helpful Hint If the value _is written__ with a visible decimal point, then go to the___left__ end of the value. Moving right, find the first non‐zero number; count it and every number to the right. If the decimal point is __Present__you start on the __Pacific___side of the equation. ⟶0.0012040 5 significant figures If the value is not ___written_____ with a visible decimal point, go to the ___right_end of the value. Moving to the left find the first non‐zero number; count it and every number to the left. If the decimal point is __absent__you start on the ___Atlantic__side of the equation. 7201000 ⟵ 4 significant figures Rounding off numbers Rule #1: If the number after the number to be rounded is less than 5, round down. Rule #2: If the number after the number to be rounded is greater than or equal to 5, round up. In a series of calculations, carry extra digits through to the final result and then round off. This means that you should carry all of the digits that show on your calculator (or most of them) until you arrive at your final answer and then round off. Note: Don’t forget significant zeros when writing in scientific notation (ex: 20.0 is 2.00 x 10). Do not write INsignificant zeros when writing in scientific notation (ex: 6 000 000 is 6 x 106, not 6.000 000 x 106 – this number would have 7 sig figs). Addition and Subtraction 6 Rule: Complete the desired calculation and then round off the answer to the number of decimal places as the value from the problem with the ________ NUMBER OF DIGITS _ THE DECIMAL. a) 12.72 370 34.1 + 101.037 + 0.463 1,371.037 47.283 1,371 All numbers are significant to the Left of 47.3 the decimal_ place. all numbers are significant to the tenths place. b) 900 c) 790. 330 + 54.8 1,174.8 1,175 All numbers are significant to the __ left of the decimal__ place. Multiplication and Division Rule: Complete the desired mathematical calculation and then round off the answer to the same number of significant figures as the value from the problem with the __least__ NUMBER OF SIGNIFICANT FIGURES. 34.91 x 0.0053 = 0.185023 Rounds to 0.19 four two two sig figs sig figs sig figs Because 0.0053 has only two significant figures, it limits the answer to two significant figures. 3. 102 ÷ 0.0097 = = 319.7938144 4 sig figs 2 sig figs Rounds to 320 Combination of operations Complete mathematical calculations in correct order and use correct number of significant figures after each step. Example: (5.2 – 0.2) x 7.00 x 1.00 = 35.00 The difference of 5.2 and 0.2 is 5.0 which is precise to the nearest tenth and has 2 sig. figs. Since 7.00 and 1.00 have 3 sig. figs. The least number of sig figs in the multiplication operation is 2 from the 5.0 difference. The final answer has 2 sig figs. Answer = 35 Pacific – Atlantic Rule If the decimal is PRESENT, start on the PACIFIC side or ____left to right___. 14.020 0.00235 1.04 * 105 If the decimal is ABSENT, start on the ATLANTIC side or _____right to left_____. 7300200 1200 839 Significant Figures and Scientific Notation Worksheet 7 Underline the significant figures in the following measurements and put the number in scientific notation: Round the following measurements to the requested number of significant figures and put the number in scientific notation: 1. 0.00325 m 3.25 x 10‐3 m 1.
2. 12500 s 1.25 x 104 s 2.
3. 304.00 g 3.0400 x 102 g 3.
4. 0.00256 kg 2.56 x 10‐3 kg 4.
3.3 x 10‐3 m 5. 0.0030600 J 3.0600 x 10‐3 J 6. 6.0250 Mm 6.0250 x 100 Mm 2. 5620000 g 564025000 g  3 sig. figs. 5.62 x 106 g 5.64 x 108 g 1. 0.000000586 m 5.86 x 10‐7 m 0.003256 m  2 sig. figs. Put the following measurements in scientific notation and put the number in scientific notation: 3. 85000 L 78265 ns  1 sig. fig. 8.5 x 104 L 8 x 104 ns 4. 0.00236 km 0.236578 Pa  4 sig. figs. 2.36 x 10‐3 km 2.366 x 10‐1 Pa 5.
5. 25640000000 Pa 0.008596 ng  3 sig. figs. 2.564 x 1010 Pa 8.60 x 10‐3 ng 6.
6. 0.000001524 s 15.349 mg  4 sig figs. 1.535 x 101 mg 1.524 x 10‐6 s Perform the following calculations and write the answer with the appropriate number of sig figs AND in scientific notation. 1. 6.23 x 106 kL + 5.3 x 106 kL 1.2 x 107 kL 3. 4.8 x 105 km x 2.02 x 103 km 9.7 x 108 km 5. 2.45 x 10‐15 J ÷ 3.4 x 10‐19 J 7.2 x 103 J 8 2. 7.525 x 105 kg ‐ 5.43 x 102 kg 7.52 x 105 kg 4. 8.45 x 102 cm3 ÷ 7.901 x 103 cm3 1.07 x 10‐1 cm3 6. 20.05 x 10343 – 15.9 x 10341 2.0 x 10344 Lab Safety Notes 
__Goggles_______ should be worn at all times when in the lab. 
___Short pants/ dresses / floppy clothes______ can never be worn in the lab. All shoes must have ________closed toes___________________. 
If your lab partner is on fire, you should ________wrap him in the fire blank_______ ____and notify the teacher asap_________________________________. 
If you get chemicals in your eyes you should use the eye wash station for _15/20__ minutes. 
The _______fume hood_____ is used to remove noxious fumes and vapors. 
If you spill a large amount of chemical on you, you should ______________ _______________safety shower______________________. 
When heating a test tube, you should always ______point the mouth (opening) of the testtube away from yourself and others___. 
Wafting is a method of smelling chemicals by _______moving your hand over the chemicals but without directly inhaling the fumes___________. 
You should never __eat__ or ____drink___ in the lab. 
You must complete the ____prelab___ if you want to participate in the lab. You MUST read the __MSDS sheet___ before you enter the lab. 
9 Contact lenses should ___not_____ be worn in the lab area. SI Unit Notes Dimension Length/Distance Mass Temperature Volume Time Energy Speed Frequency Density Pressure Base Unit Symbol Meter kilogram Kelvin Decimeter cubed and Liters second Joule meter per second 1/second = Hertz Gram/centimeter3 Pascal m kg K dm3 and L s J m/s Hz g/cm3 Pa Temperature: Celsius and Kelvin Density: g/mL or g/cm3 Equal Units of Volume: 1 cm3 = 1 mL 1 dm3 = 1 L Theory ‐ Explains a scientific Relationship ‐ Must be testable ‐ Must be falsifiable ‐ Cannot be proven true, can be proven wrong ‐ Can be modified to incorporate new data ‐ Can be used to make accurate predictions Law ‐State a scientific relationship ‐must be verified by data ‐ Modified as conflicting data is gathered ‐Can be used to make accurate predictions ‐Can be expressed mathematically Observation: The act of gathering specific information using the 5 senses.
Inference:
Hypothesis:
Accuracy:
Precision:
10 The act or process of deriving logical conclusions from premises known or
assumed to be true or the act of reasoning from factual knowledge or
evidence.
A tentative explanation for a question, testable through experiments
Accuracy refers to the correctness of a single measurement. Accuracy is
determined by comparing the measurement against the true or accepted
value.
Precision refers to how well experimental data and values agree with each
other in multiple tests.
SI Unit Prefixes Prefix Mega Kilo Deca Base deci centi milli micro nano pico Symbol M k D ‐‐ d c m µ n p Meaning 10 103 101 100 10‐1 10‐2 10‐3 10‐6 10‐9 10‐12 6
You must memorize these prefixes, symbols and meanings! Remember, when you are dividing exponents, you subtract. 103 ÷ 106 = 10‐3 because (3 – 6 = ‐3) Remember, when you are multiplying exponents, you add. 102 x 103 = 105 because (2 + 3 = 5) Steps for SI Conversions 1. Write down the starting measurement 2. Put the units of the starting measurement into the denominator to cancel 3. Put units you want on the top 4. Put a 1 with the larger unit 5. Determine relationship between the two units (MEMORIZE prefix chart) by finding the absolute value of the difference in exponents. 6. Solve. Cancel units. If exponent jumps the line then change the sign (105=1/10‐5) 7. If needed put the number into scientific notation. SI Conversions Example 1: 63 200 centiliters  microliters 63,200 centiliters 104 microliters = 6.32 x 108 microliters 1 centiliters 11 SI Unit Conversions Practice: 1. 89.3 kilometers  nanometers 89.3 kilometers 1012 nanometers = 8.93 x 1013 nanometers 1 kilometers 2. 5.32x108 picograms  milligrams 5.32x108 picograms 1 milligrams = 5.32 x 10‐1 milligrams or 0.532 mg 109 picograms 3. 26.60 millipascals  megapascals 26.60 millipascals 1 megapascals = 2.660 x 10‐8 megapascals 109 millipascals 12 DIMENSIONAL ANALYSIS NOTES: If light from the sun takes 8.11 minutes to get to the Earth, how far away is the sun in km? (speed of light is 3.0x108m/s and there are 1000 m in one km) 1. Identify the values in the problem, include units 8.11 minutes 3.0x108m/s 1000 m in one km 60 s in one minute 2. Start with the value with only one unit 8.11 minutes 3. Put that starting unit into the denominator to cancel units out 8.11 minutes minutes 4. Find the value OR conversion to a given value with the same unit and place it into the problem 8.11 minutes 60 seconds 1 minutes 5. Repeat until you get to the desired units, cross out units which cancel 8.11 minutes 60 seconds 3.0x108 meters 1 Kilometers 1 minutes 1 seconds 1000 meters = 1.46 x 108 km 6. Solve and put into correct scientific notation (multiply numerator and divide denominator) DIMENSIONAL ANALYSIS PRACTICE PROBLEM: If you live 3.2 miles from your best friend and the speed limit is 25 miles/hour, how many seconds will it take you to drive from your house to your friend’s house? = 460.8 seconds 3.2 miles 1 hour 60 minutes 60 seconds 25 miles 1 hour 1 minutes 460 seconds 13 SI Unit Conversions Practice 1. Convert 0.0036 g to mg 0.0036 g 1000 mg = 3.6 mg 1 g 2. Convert 8.9 x 10‐8 s to ps 8.9 x 10‐8 s 1012 ps = 89,000 ps or 8.9 x 10 4 ps 1 s 3. Convert 8200000 nPa to MPa 8200000 nPa 1 MPa = 8.2 x10‐9 MPa 1015 nPa 4. Convert 3.26 L to cm3 3.26 L 1000 cm3 = 3.26 x103 cm3 or 3260 cm3 1 L 5. Convert 0.0012 cm3 to mL 0.0012 cm3 1 mL = 0.0012 mL 1 cm3 6. Convert 0.29 L to cm3 0.29 L 103 cm3 = 290 cm3 1 L 14 Dimensional Analysis Practice Problems:
Remember ‐ The numbers in conversion factors are considered to be exact. Be sure to include units where appropriate, and round your answers according to the number of digits in the original problem. 1. Convert 2.44 L to cm3 2.44 L 103 cm3 = 2440 cm3 1 L 2. Convert 45 654 mg to kg 45 654 mg 1 kg = 0.045654 kg 106 mg 3. Convert 4.7 km/hr to m/s 4. Convert 4.00 g/cm3 to kg/dm3 4.7 km 103 m 1 hr = 1.305556 m/s 4.00 g 1 kg 103 cm3= 4.00 kg/dm3 1 hr 1 km 3600 s 1 cm3 103 g 1 dm3 1.3 m/s 5. Convert 6.72 dm3/s to L/min 6. Convert 0.0598 mg/cm3 to g/cm3 0.0598 mg 1 g = 5.98 x 10‐5 g/cm3 6.72 dm3 1 L 60 s = 403.2 L/min 1 s 1 dm3 1 min 403 L/min 1 cm3 103 mg 7. Convert 2.7 dm3 to mL 8. Convert 0.90 kg/cm3 to mg/ cm3 0.90 kg 106 mg = 0.90 x106 mg/cm3 1 cm3 1 kg 9.0 x 105 mg/cm3 2.7 dm3 103 mL = 2.7 x 103 mL 1 dm3 2,700 mL 15 Dimensional Analysis Word Problems Practice 1. You want to earn $600.00 to buy a new bicycle. You have a job that pays $8.75/hour, but you can work only 3 hours/day. How many days before you will have enough to buy the bike? $600.00 1 hr 1 day = 22.85714 days or 23 days $8.75 3 hr 2. Someone that never learned dimensional analysis went off to work at a fast food restaurant for the past 35 years wrapping hamburgers. Each hour you wrap 184 hamburgers. You work 8 hours per day. You work 5 days a week. You get paid every 2 weeks with a salary of $840.34. How many hamburgers will you have to wrap to make your first one million dollars? $1,000,000 2 weeks 5 days 8 hrs 184 hmbrgrs = 17516719.42 hmbrgrs $840.34 1 week 1 day 1 hr = 17,517,000 hmbrgrs 3. In 1973 the Emergency Highway Energy Conservation Act instituted a National Maximum Speed Law of 55 mph. How many minutes would it take to travel 16 kilometers? (1 mile = 1.6093 km)? 16 km 1 mile 1 hr 60 min = 10.84604825 min 1.6093km 55 mile 1 hr 11 min 16 Conversions and Dimensional Analysis Homework Worksheet Metric Conversions: 6. Convert 2.38 x 102 m to km 2.38 x 102 m 1 km = 2.38 x 10‐1 km 1000 m 7. Convert 40.0 m to mm 2
3.87 m 100 cm = 3.87 x 10 cm 40.0 m 1000 mm = 4.00 x 104 mm 1 m 1 m 3. Convert 25 mm to m 8. Convert 8.0 cm to mm ‐2
25 mm 1 m = 2.5 x 10 m 8.0 cm 10 mm = 80. mm 1000 mm 1 cm 4. Convert 105 m to mm 9. Convert 0.02 mm to cm 3
5
105 m 10 mm = 1.05 x 10 mm 0.02 mm 1 cm = 0.002 cm 1 m 10 mm 5. Convert 1.8 km to m 10.Convert 57.2 mm to km 1.8 km 103 m = 1.8 x 103 m 57.2 mm 1 km = 5.72 x 10‐5 km 1 km 106 mm 1. Convert 2.5 cm to m 2.5 cm 1 m = 2.5 x 10‐2 m 100 cm = 0.025 m 2. Convert 3.87 m to cm 17 Dimensional Analysis Problems: 11. Convert 2.05 x 105 seconds into years. 2.05 x 105 s 1 hr 1 day 1 year = 6.50 x 10‐3 yrs 3600 s 24 hr 365 days 12. Traveling at 65 miles/hour, how many minutes will it take to drive 125 miles to San Diego? 125 miles 1 hr 60 min = 115.3846154 min ≈ 120 min 65 miles 1 hr 13. Convert 50 years into seconds. Express your answer in scientific notation. 50 years 365 days 24 hrs 60 min 60 s = 1.576800000 x 109 s ≈ 2 x 109 s 1years 1 day 1 hr 1 min 14. Traveling at 65 miles/hour, how many feet can you travel in 22 minutes? (1 mile = 5280 feet) 22 min 1 hr 65 miles 5280 ft = 125,840 ft ≈ 130,000 ft = 1.3 x 105 ft 60 min 1 hr 1 mile 15. In Raiders of the Lost Ark, Indiana Jones tried to remove a gold idol from a booby‐trapped pedestal. He replaces the idol with a bag of sand. If the idol has a mass of 2.00 g, how many liters of sand must he place on the pedestal to keep the mass sensitive booby‐trap from activating? (Density of sand is 3.00 g/cm3) 2.00 g 1 cm3 1 L = 6.67 x 10‐4 L 3.00 g 1000 mL 18 Physical/Chemical Properties and Changes Notes 
What is matter? Matter is the term for any type of material. Matter is anything that has mass and takes
up space.
The word is sometimes used to refer to a pure substance. 
Physical Properties: Properties of a substance that can be measured without changing the chemical nature of the substance. o Examples: Color, Smell, Freezing point, Boiling point, Melting point, Magnetism, Opacity, Viscosity, Stability and Density o Intensive Properties: are ___Independent__ of the amount of matter present.  Examples: Temperature, color, hardness, melting point, boiling point, pressure,
molecular weight, and density. Because intensive properties are sometimes
characteristic of a particular material, they can be helpful as clues in
identifying unknown substances. o Extensive Properties: are ____ Dependent ____ on the amount of matter present.  Examples: Mass, volume, length, and total charge. 
Chemical Properties: Properties of a substance that cannot be measured without changing the chemical nature of the substance. o
Examples: Combustion and reactivity with water 
Physical Changes: Changes that do not alter the chemical composition of a substance. o Examples: Physical changes are concerned with energy and states of matter. A
physical change does not produce a new substance. Changes in state or phase
(melting, freezing, vaporization, condensation, sublimation) are physical changes.
Examples of physical changes include crushing a can, melting an ice cube, and
breaking a bottle. 
Chemical Changes: Changes that alter the chemical composition of a substance. o Examples: Chemical changes take place on the molecular level. A chemical change
produces a new substance. Examples of chemical changes include combustion
(burning), cooking an egg, rusting of an iron pan, and mixing hydrochloric acid
and sodium hydroxide to make salt and water. Indications of a chemical change:




 Change in odor
 Change in color
 Energy given off or absorbed
 Formation of a precipitate
 Formation of a gas 19 The Four Aristotelian Elements
Western chemistry grew up around old alchemical ideas of Earth, Air, Fire, and Water – the so
called Aristotelian elements – a concept that originated with the ancient Greeks and others.
Matter Notes Solid Liquid 

Gas Vapor: is not the same as gas. Vapor refers to the gaseous phase of a substance that is a liquid or solid under standard conditions. Alloy: A metallic solid solution composed of two or more elements. 20 Solid 
Liquid Gas Plasma: high temperature, low pressure; electrons separate from nucleus; most common in the universe Elements, Compounds, Mixtures and Solutions  Elements: a pure substance that is made up of only one type of atom and cannot be broken down by physical or chemical means. 


Examples: There are 115 known elements presently, out of which only 91 occur
naturally. The remaining elements have been produced artificially by nuclear
scientists in the laboratory using particle accelerators.
Compounds: a combination of two or more different elements that are combined chemically. o Examples: The smallest unit of a compound, known as a molecule, or a formula unit,
is composed of atoms of the constituent elements. A compound is represented by a
chemical formula which indicates one molecule (formula unit) of the compound
containing atoms of its elements. Mixture: a combination of two or more pure substances in which each pure substance retains its physical properties. Examples: Milk, Salt water o Homogeneous mixture: Mixtures in which the composition is uniform throughout. Also called a SOLUTION.  Examples: 1. Blood
2. Sugar solution when sugar is completely dissolved.
3. Mixture of alcohol & water
4. A glass of orange juice
5.salty water (where the salt is completely dissolved)
6.brewed tea or coffee 21 o Heterogeneous mixture: Mixtures in which the composition is not uniform throughout. You can distinguish the different parts.  Examples: 
1. Oil & water.
2. Soil sample
3.sandy water
4.carbonated beverage or beer (the CO2 gas is mixed with the liquid)
5.orange juice with pulp in it water with ice cubes in it
6.chicken noodle soup
7. sand in a desert Separation of Matter  Elements‐ can only be broken down by nuclear reactions.  Compounds‐ can only be broken down by chemical reactions  Mixtures‐ can be broken down by physical means. Physical Separation Methods  Filtration Chromatography‐ physical separation based on attraction to liquid or solid. Paper Chromatography‐ paper is the stationary phase and liquid is the mobile phase. Column Chromatography‐ beads are the stationary phase and liquid is the mobile phase. http://aphschem.blogspot.com/2009_10_01_archive.html Distillation http://oz.plymouth.edu/~wwf/distillation.htm 22 Chemical and Physical Properties Worksheet 1. Classify the following materials as heterogeneous mixtures (M), homogeneous mixtures/solution (S), compounds (C) or elements (E). h) plutonium E o) orange juice S i) deionized water xS p) carbonated beverage M c) paper M j) ice q) zinc sulfate C d) salt k) shaving cream M r) dirt M e) ethyl alcohol C l) paint M s) river water M f) apple M m) granite M t) milk S g) water C – M ‐ S n) 24 carat gold E a) air M b) ink M C C 2. Classify the following properties as chemical (C) or physical (P). a) color P b) reactivity C c) flammability C b) odor P e) porosity P f) stability C g) ductility P h) solubility P i) expansion P k) rusting C l) reacts with air C m) feel P 3. Classify the following as chemical (C) or physical (P) changes. a) digestion of food C b) boiling water P c) growth of a plant C d) explosion of gasoline C e) cloud formation P f) healing a wound C g) burning of coal C h) kicking a football P i) contracting a muscle P j) distilling water P k) melting silver P l) rusting iron C m) subliming of iodine P 4. Determine the physical process to separate the following mixtures a) ethyl alcohol and water D b) ink in a pen C c) Sand and water d) water and minerals F ‐ D F 23 Classification of Matter Choose words from the list to fill in the blanks in the paragraphs. Word List intensive property extensive property chemical property compound mixture heterogeneous matter element physical property homogeneous matter substance property Matter that has uniform characteristics throughout is called __(1)__. Matter that has parts with different characteristics is called __(2)__. A characteristic by which a variety of matter is recognized is called a(n) __(3)__. A characteristic that depends upon the amount of matter in the sample is called a(n) __(4)__. A characteristic that does not depend upon the amount of matter is called a(n) __(5)__. A characteristic that can be observed without producing new kinds of matter is called a(n) __(6)__. A characteristic that depends on how a kind of matter changes during interactions with other kinds of matter is called a(n) __(7)__. Matter can also be classified according to the basic types of matter it contains. A simple substance that cannot be broken down into other substances by chemical means is called a(n) __(8)__. A chemical combination of different substances that retain their individual properties is called a(n) __(9)__. A physical combination of different substances that retain their individual properties is called a(n) __(10)__. Either an element or a compound may be referred to as a(n) __(11)__. Classify each of the following as an element, compound, heterogeneous mixture, or homogeneous mixture. 1. _homogeneous matter_ 2. _heterogeneous matter 3. _ __property ________ 4. ___extensive property_ 5. ___intensive property_ 6. ___physical property__ 7. __ chemical property __ 8. ___element _________ 9. ___compound________ 10. ___mixture__________ 11. ____substance_______ 12. Water (pure water homogeneous or compound) 12. _ heterogeneous mixture 13. Carbon 13. ___Element___________ 14. Air 14. _ heterogeneous mixture 15. Table salt (pure salt compound) 15. __ heterogeneous __ 16. Sugar dissolved in water 16. ___Homogeneous__ 17. Homogenized milk 17. ____ Homogeneous ____ 18. Granite 18. ____Heterogeneous___ 19. Oxygen 19. ___Element___________ 20. Sand in water 20. ____Heterogeneous____ 24 Properties Recall that physical properties can be observed without producing new substances. Chemical properties describe how a substance interacts (or fails to interact) with other substances to produce new substances. Extensive properties depend upon the amount of matter in the sample; intensive properties do not. Classify each of the properties listed below as extensive physical, intensive physical, or chemical. 1. Color 1. __ intensive physical _ 2. Combustibility 2. ___ chemical _______ 3. Hardness 3. __ intensive physical _ 4. Density 4. __ intensive physical _ 5. Mass 5. __ extensive physical _ 6. Melting point 6. __ intensive physical _ 7. Ductility 7. __ intensive physical _ 8. Volume 8. __ extensive physical _ 9. Failure to react with other substances 9. ___ chemical _______ 10. Odor 10. __ intensive physical _ 11. Weight 11. __ extensive physical _ 12. Malleability 12. __ intensive physical _ 13. Tendency to corrode 13. ___ chemical _______ Some of the measured properties of a given substance are listed below. Write the general name describing each property. Select the names from the properties listed for Exercised 1‐13 above. 14. 15 dm3 14. __ extensive physical _ 15. Can easily be hammered into sheets. 15. __ intensive physical _ 16. 2.8 g/cm3 16. __ intensive physical _ 17. Burns when heated in the presence of O2. 17. ___ chemical _______ 18. Stinks when heated. 18. ___ chemical _______ 19. Can be scratched by a diamond. 19. __ intensive physical _ 20. 500°C 20. __ intensive physical _ 21. Can easily be drawn into a wire. 21. __ intensive physical _ 25 Unit 1 Review Complete the following calculations and report your answer with the correct number of significant figures and with proper units. 1. 1.2 m + 2.35 m = _____________ 6. 1.2 m x 2 m2 = ____________ 2. 2.6538 cm x 2.1 cm = _____________ 7. 859678.2354 cm – 568426.1 cm = ________ 3. 5.681 dm – 2 dm = _____________ 8. 5.3 m x 5.2398 m x 2 m = _____________ 3
9. 45.25252 nm + 45.8563 nm = ____________ 4. 3845.2 m  25.2354 m = ____________ 5. 25 cm + 3 cm = ____________ 10. 68.23 L  38.255 L = ____________ Convert the following measurements; write your answer in standard notation or scientific notation. Conversion (Standard Measurement Notation) Conversion (Scientific Notation) nm nm 155 cm Km Km 155 cm mg mg 2.77 x 10‐7 kg cL cL 867 x 104 µL ds ds 0.000876 Ks Estimate the number of significant figures in each of the following measurements. Write the measurement using Scientific Notation. Measurement How many significant figures? Measurement in Scientific Notation A) 10046 m B) 500 m C) 500. m D) 510 m 26 Round each of the measurements off to 3 significant figures. Write your answer in decimal notation and scientific notation. Measurement Decimal Notation Scientific Notation A) 7534 L B) .002346 mL C) 16.18 cm D) 1504 mL Complete the following Conversions: 1. Convert 16 years to days 2. How many km/hr is 30 m/s? 3.
Sally Leadfoot was pulled over on her way from Syracuse to Ithaca by an officer claiming she was speeding. The speed limit is 65 mi/hr and Sally had traveled 97 km in 102 minutes. How fast was Sally’s average speed? Does she deserve a ticket? Physical or Chemical Properties: Indicate with a P or a C which type of change is taking place. For those labeled with a P, identify them as Intensive (I) or Extensive (E). 1. _____________ Strength 7. _____________ Toxicity 2. _____________ Color 8. _____________ Density 3. _____________ Reacts with Cl 9. _____________ Boiling Point 4. _____________ Volume 10. _____________ Flammability 5. _____________ Corrodes 11. _____________ Boiling Point 6. _____________ Mass 12. _____________ Stability 27 Physical or Chemical Change? 1. ____________ glass breaking 9. ____________ mixing salt and water 2. ____________ hammering wood together 10. ____________ mixing oil and water 3. ____________ a rusting bicycle 11. ____________ water evaporating 4. ____________ melting butter 12. ____________ cutting grass 5. ____________ bleaching your hair 13. ____________ fireworks exploding 6. ____________ frying an egg 14. ____________ cutting your hair 7. ____________ squeeze oranges for juice 15. ____________ crushing a can 8. ____________ melting ice 16. ____________ boiling water Label each process as a physical or chemical change: a. Moth balls gradually vaporize in a closet c. Chlorine gas liquefies at ‐35 °C under normal pressure b. hydrofluoric acid attacks glass (used to etch glassware) d. hydrogen burns in chlorine gas Label the following as an Element (E), Compound (C), Solution (S) or Mixture (M) a. Helium g. Wood b. Brass h. Steel c. Sodium chloride i. Iron d. Air j. Calcium carbonate e. Oily water k. Aluminum Foil f. Dirt l. Glucose (a type of sugar)
Use the best physical means of separation for the following problems. 1. You are given a mixture of acetone and water, acetone has a lower boiling point than water, what method would work best to separate them? 2. Given a mixture of pepper, sand and salt, propose how you would separate the substances. 3. You are given the task of separating ink in a pen, what method would work best to separate the components of ink. Answer the question using the data to support your answer. 4. Which student’s date is both accurate and precise when measuring 1.00 L of sodium chloride solution? Explain your answer. Also include in your answer which student was the most precise. Student: A B C D Trial 1 1150 mL 1030 mL 850 mL 950 mL Trial 2 1140 mL 1090 mL 1020 mL 1140 mL Trial 3 1170 mL 1060 mL 1110 mL 1370
Matching: Match the following terms with the appropriate letter: 1. Solid _____ m. A sample that can be separated only with chemical means 2. Liquid_____ n. Anything that has mass and volume 3. Gas_____ o. An object that has a definite volume but not a definite shape 4. Matter_____ p. An object that has both definite volume and shape 5. Pure Substance_____ q. Made up of 2 or more elements 6. Compound _____ r. An object that has neither a definite shape nor volume 29