matter properties and changes - mr. acosta's...
TRANSCRIPT
Matter: Properties and Changes
Properties of Matter
A pure substance is matter that has ____________________ and ____________________
composition. Examples: ____________________ and ____________________
A physical property is a characteristic that can be ____________________ or
____________________ without changing the sample’s ____________________.
Examples: ____________________, ____________________, ____________________,
____________________, ____________________
Physical properties can fall under two categories: extensive properties or intensive
properties.
Extensive properties are dependent upon ________________________________________________.
Examples: ___________________, ___________________, ___________________, ___________________
Intensive properties are dependent upon ______________________________________________.
Example: ___________________, ___________________, ___________________, ___________________,
A chemical property is ___________________________________________________________________
_________________________________________________________________________________________
Examples: ___________________, ______________________, ______________________
States of Matter: List the properties for each state of matter.
Solids
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Liquids
Gases
Changes in Matter
A physical change is a type of change that alter the ___________________ properties of a
substance but does not change its ______________________.
Examples:
___________________
___________________
___________________
___________________
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A chemical change is a process involving one or more substances changing into ___________
___________________. This process is also called a ______________________________________.
Evidence of a Chemical Change (make list)
Conservation of Mass
Mass is neither ___________________ nor ___________________ in a chemical reaction – it is
___________________.
Mass products = Mass reactants
Example
10.00 g of red mercury (II) oxide powder is placed in an open flask and heated until it is
converted to liquid mercury and oxygen gas. The liquid mercury has a mass of 9.26 g. What
is the mass of oxygen formed by the reaction?
Mixtures of Matter
A mixture is a _____________________________________________________________________
__________________________________________________________________________________
__________________________________________________________________________________.
A heterogeneous mixture is one that does not ___________________ ___________________ and
the individual substances remain ___________________.
Examples: __________________, ____________________
A homogeneous mixture has ___________________ ___________________ throughout. These
mixtures are also referred to as ___________________.
Examples: _________________, _____________________3
Separating Mixtures
Filtration is a technique that uses a ___________________ ___________________ to separate a
___________________ from a ___________________.
Distillation is a technique that is used to separate ___________________ mixtures based on
differences in the ___________________ ___________________ of the substances involved.
Elements vs. Compounds
An element is ___________________________________________________________________
________________________________________________________________________________.
Examples: __________________, __________________ .
A compound is a combination of two or more ___________________ ___________________
that are combined ___________________. They are combined in a___________________
___________________.
Examples: __________________, __________________ .
Compounds cannot be separated by ___________________ means. A ___________________
___________________ must occur in order for the substance to separated.
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Name______________________________________________Date_____________________________Period______
Matter – Substances vs. Mixtures
All matter can be classified as either a substance (element or compound) or a mixture
(heterogeneous or homogeneous).
Directions: Classify each of the following as to whether it is a substance or a mixture. If it is a
substance, write element or compound in the Substance column. If it is a mixture, write
heterogeneous or homogeneous in the Mixture column.
Type of Matter Substance Mixture
1. chlorine
2. water
3. soil
4. sugar water
5. oxygen
6. carbon dioxide
7. rocky road ice cream
8. alcohol
9. pure air
10. iron
Matter
Substancecan write chemical
formula; homogeneous
Elementone type of atom
Compound2 or more different atoms chemically
bonded
Mixturesvariable ratio
Homogeneous
solutions
Heterogeneous
colloids & suspensions
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Name____________________________________________Date______________________________Period_______
Physical vs. Chemical Changes
In a physical change, the original substance still exists, it has only changed form. In a
chemical change, a new substance is produced. Energy changes always accompany
chemical changes.
Directions: Classify the following as being a physical or chemical change.
Type of Change
1. Sodium hydroxide dissolves in water
2. Hydrochloric acid reacts with potassium hydroxide to
produce a salt, water, and heat
3. A pellet of sodium is sliced in two
4. Water is heated and changed to steam
5. Potassium chlorate decomposes to potassium chloride
and oxygen gas.
6. Iron rusts.
7. When placed in H2O, a sodium pellet catches on fire as
hydrogen gas is liberated and sodium hydroxide forms
8. Evaporation
9. Ice melting
10. Milk sours
11. Sugar dissolved in water
12. Wood rotting
13. Pancakes cooking on a griddle
14. Grass growing in a lawn
15. A tire is inflated with air
16. Food is digested in the stomach
17. Water is absorbed by a paper towel
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Name________________________________________________Date___________________________Period______
Physical & Chemical Properties A physical property is observed with the sense and can be determined without destroying
the object. For example, color, shape, mass, length, and odor are all examples of physical
properties.
A chemical property indicates how a substance reacts with something else. The original
substance is fundamentally changed in observing the chemical property. For example, the
ability of iron to rust is a chemical property. The iron has reacted with oxygen, and the
original iron metal has changed. It now exists as iron oxide, a different substance.
Directions: Classify the following properties as either chemical or physical by putting a check
in the appropriate column.
Physical
Property
Chemical
Property
1. blue color
2. density
3. flammability
4. solubility
5. reacts with acid to form hydrogen gas (H2)
6. supports combustion
7. sour taste
8. melting point
9. reacts with water to form a gas
10. reacts with a base to form water
11. hardness
12. boiling point
13. can neutralize a base
14. luster
15. odor
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Science, Measurement, and Uncertainty: Accuracy and Precision
ACCURACY AND PRECISION Definitions: Accuracy – how close a measurement is to ______________________________
Precision – how close a measurement is to _______________________________
Precision versus Accuracy: Look at each target and decide whether the “hits” are accurate, precise, both accurate and precise, or neither accurate nor precise: (Note: An accurate “hit” is a bulls eye!)
Accurate?: Yes / No Precise?: Yes / No
Accurate?: Yes / No Precise?: Yes / No
Accurate?: Yes / No Precise?: Yes / No
Precision Problems: A group of students worked in separate teams to measure the length of an object. Here are their data:
Team 1 Team 2 Team 3 Team 4 Team 5 Team 6 Team 7 2.65 cm 2.75 cm 2.80 cm 2.77 cm 2.60 cm 2.65 cm 2.68 cm
• The average length is ________ cm.This is the mean or average.
• Subtract the highest value from the lowest value: _________ cm.This is the range or spread.
• Divide this number by 2: _______ cm.This is the approximate ± range from the average.
• The precision of the measurement can be shown as average ± range.The precision of the measurement was ________±_____ cm.
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Science, Measurement, and Uncertainty: Accuracy and Precision
A second group of students obtained the following data:
Team 8 Team 9 Team 10 Team 11 Team 12 Team 13 Team 14 2.60 cm 2.70 cm 2.80 cm 2.75 cm 2.65 cm 2.62 cm 2.78 cm
• The average length is ________ cm.
• The precision of the measurement was ________±_____ cm.
In comparing groups, the first or the second, which group was more precise or was the precision the same? Justify your answer.
Expressing Errors in Measurement: Scientists often express their uncertainty and error in measurement by giving a percent error. The percent error is defined as:
% error = valueactual
valuemeasuredvalueactual − x 100
Answer the following four questions. Pay attention to significant figures, and show your work!
1. While doing a lab, a student found the density of a piece of pure aluminum to be 2.85g/cm3. The accepted value for the density of aluminum is 2.70 g/cm3. What was thestudent's percent error?
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Science, Measurement, and Uncertainty: Accuracy and Precision
2. A student measured the specific heat of water to be 4.29 J/g · Co. The literaturevalue of the specific heat of water is 4.18 J/g · Co. What was the student’spercent error?
3. A student took a calibrated 200.0 gram mass, weighed it on a laboratory balance, andfound it read 196.5 g. What was the student’s percent error?
4. Accuracy is often expressed as an average of severalmeasurements. Look at the target to the right. In your opinion,how well do the measurements on the target represent:(Justify your opinion.)
a. Accuracy?
b. Precision?
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A. Express the following numbers in correct scientific notation:
_______________1. 8 720 000
_______________2. 0.00 000 628
B. Rewrite the following numbers so they are in correct scientific notation:
_______________3. 652.9 x 105
_______________4. 0.00 598 x 10-15
_______________5. 0.0 259 x 108
C. Carry out the indicated operations and express your answer in correct scientific notation:
_______________6. (3.04 x 1022) + (3.04 x 1023)
_______________7. (6.54 x 105) - (2.0 x 103)
_______________8. (2.5 x 103) (3.62 x 105)
_______________9. (9.12 x 101) ( 6.55 x 10-2)
_______________10. (3.2 x 102) (2.0 x 10-5) (3 x 104)
_______________11. (3.80 x 104) ÷ (1.25 x 10-3)
_______________12. (2.5 x 10-7) ( 5.0 x 10-8)
(9.5 x 10-14) (6.0 x 108)
_______________13. (389 000 000) (0. 000 75)
_______________14. (0.000 686 8) ÷ (87 000)
_______________15. (3.5 x 1018) (1.47 x 106) (3.442 x 10-3) (9.97 x 105)
(9 x 1031) (6.634 x 108) (2.7 x 104) (6.02 x 1023)
CHEMISTRY Scientific Notation Practice
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http://www.chemfiesta.com
Significant Figures Practice Worksheet
How many significant figures do the following numbers have?
1) 1234 _____
2) 0.023 _____
3) 890 _____
4) 91010 _____
5) 9010.0 _____
6) 1090.0010 _____
7) 0.00120 _____
8) 3.4 x 104 _____
9) 9.0 x 10-3 _____
10) 9.010 x 10-2 _____
11) 0.00030 _____
12) 1020010 _____
13) 780. _____
14) 1000 _____
15) 918.010 _____
16) 0.0001 _____
17) 0.00390 _____
18) 8120 _____
19) 7.991 x 10-10_____
20) 72 _____
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Write the number of significant figures in the
following measurements.
1._____ 2.708
2._____ 16.3050
3._____ 50.007
4._____ 3000010
5._____ 0.00045
6._____ 0.00458
7._____ 589000
8._____ 6.38 x 109
9._____ 50800
10._____ 4.678 x 1022
11. _____. 789.006
12._____ 3.67 x 10-4
13._____ 507.7800
14._____0.000000875
15._____ 0.00480
16._____ 3322.008
17._____ 540300
18._____ 4506.003
19._____ 287.345
20._____ 56.000
21. Round off the following numbers to threesignificant figures.
(a) 4325
(b) 6.873 x 103
(c) 0.17354
(d) 7.8939
(e) 9.237 x 10-3
(f) 0.0299817
22. How many significant figures does eachof the numbers contain?
(a) 0.0278 meter
(b) 1.3 centimeters
(c) 1.00 foot
(d) 8 021 yards
(e) 7.98 x 10-3 pound
(f) 0 2003 ton
(g) 4.69 x 104 tons
(h) 1 x 1012 atoms
(i) 1.73 x 1024 atoms
23. Express the following numbers inscientific notation with the indicated number of significant figures.
(a) 1000 (2 sig. fig. )
(b) 43,927 (3 sig. fig.)
(c) 0.000286 (3 sig. fig.)
(d) 0.000098765 (5 sig. fig.)
CHEMISTRY SIGNIFICANT FIGURE PRACTICE IV
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Do the following calculations and write your answer with the correct number of significant figures.
1. 2.345 + 6.487 =
2. 68.439 - 54.1 =
3. 2.7 x 104 + 3.67 x 104 =
4. 7.8 x 106 - 2.4 x 105 =
5. 8.4 x 10-4 + 6.89 x 10-4 =
6. 2.7 x 10-4 - 3.67 x 10-5 =
7. 456 x 21 =
8. 3200 x 460 =
9. 12407 ÷ 5 3=
10. 6.74034 x 105 ÷ 4.302 10-3
CHEMISTRY SIGNIFICANT FIGURE PRACTICE V
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Unit 1 – Math & Measurement
Rulers, graduated cylinders, and thermometers on “Practice With Reading Measuring Devices Worksheet” are from math-aids.com
READING MEASURING DEVICES NOTES Here are a couple of examples of graduated cylinders:
An important part of Chemistry is measurement. It is very important that you read the measuring devices we use in lab as accurately as possible. Here is how to determine how accurately a measuring device can be read: Look at the graduation marks on the piece of equipment. (Those are the lines or marks that are not numbered.) Decide what each mark is worth using the numbers given as a guide. You should read the instrument to one more decimal place to the right than the smallest graduation mark. This last number
will be an estimate on your part. This will lead us into our next topic in measurement – significant figures. A: Each of the smaller lines represents 1 mL. That means that our reading should be to one place to the right of the decimal point. To me, it looks like the bottom of the curve is about halfway between the 16 and the 17, so I would say that the reading on this graduated cylinder would be 16.5 mL. B: Each line represents 0.1 mL. That means that our reading should be to two places to the right of the decimal point. The bottom of the curve looks to me like it is exactly on the line that would represent 3.8. My reading, however, needs to be to two places to the right of the decimal. Because it is exactly on the line, my reading will be 3.80 mL. =======================================================
PRACTICE WITH READING MEASURING DEVICES WORKSHEET
Part 1 - What are the readings on these metric rulers? Be sure to include units with your answers.
1.)
2.)
3.)
4.)
5.)
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Unit 1 – Math & Measurement
Notes and Worksheets
Part 2 – What are the readings on these graduated cylinders? Be sure to include units with your
answers.
6.) 7.) 8.) 9.)
10.) 11.) 12.) 13.)
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Unit 1 – Math & Measurement
Notes and Worksheets
Part 3 – What are the readings on these thermometers? Be sure to include units with your answers.
14.) 15.) 16.) 17.)
Part 4 – What are the readings on these triple beam balances? Be sure to include units with your
answers.
18.)
19.)
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1. The distance from the thumb to the little finger on Jacob Grill's hand is 9 inches. Convert this tocentimeters.
2. According to the Guinness Book of Records the heaviest baby ever born weighed 29 lbs 4 oz. (29.25 lbs).What was the baby's mass in kg? (Historical Note: The birth occurred in Effingham IL in 1939 and due torespiratory problems the baby died two hours later. The heaviest babies to survive weighed 22.5 lbs and were born in 1955 and 1982.)
3. Regan's cross country skis are 210 cm long. What is their length in inches?
4. A condor has a wing span of 3.05 m. What is the wing span in feet?
5. In Europe gasoline is sold by the liter. Assume that it takes 14 gallons of gasoline to fill the tank of a compactcar. How many liters of gasoline will it take?
6. You have just received a French cookbook from the exchange student. You want to make 3 quarts of punchfor a party. Will a recipe of 2.5 L be enough?
CHEMISTRY : DIMENSIONAL ANALYSIS PRACTICE
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7. One 1.6 oz. of package of cinnamon and spice instant oatmeal contains 34 g of carbohydrates. If you hadinstant oatmeal 6 days a week, how many ounces of carbohydrate would you consume in a week? (16 oz =1 lb = 454 g = 256 Drams = 7000 Grains)
8. Many candybars have 9 g of fat per bar. If during a "chocolate attack" you ate one pack of candy (0.6dekabars), how many ounces of fat would you have eaten? There are approximately 9 Calories per gram of fat, how many Calories is this?
9. If the RDA for vitamin C is 60 mg per day and there are 70 mg of vitamin C per 100 g of orange, how many 3oz. oranges would you have to eat each week to meet this requirement?
10. Because you never learned dimensional analysis, you have been working at a fast food restaurant for thepast 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?
11. Mark McGuire hit 70 home runs in the 1998 season. Given that there are 4 bases with 90 feet between eachbase, how many miles did he run last season just from home runs?
12. A high School senior was applying to college and wondered how many applications she needed to send.Her counselor explained that with the excellent grade she received in chemistry she would probably be accepted to one school out of every three to which she applied. [3 applications = 1 acceptance] She immediately realized that for each application she would have to write 3 essays, [1 application = 3 essays] and each essay would require 2 hours work [1 essay = 2 hours]. Of course writing essays is no simple matter. For each hour of serious essay writing, she would need to expend 500 calories [1 hour = 500 calories] which she could derive from her mother's apple pies [1 pie = 1000 calories]. How many pies would she have to eat in order to gain acceptance to 10 colleges?
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1. Calculate the number of kilometers (km) there are in 105 meters (m).
2. How many millimeters are there in 5.97 x 10-6 meters (m)?
3. Calculate the number of kilometers (km) there are in 1.549 micrometers (mm).
4. Calculate the number of centimeters (cm) there are in 6.245101 kilometers (km).
5. A very small object is found to have a length of 3.44 x 10-4 meter (m). Express this lengthin micrometers (mm).
6. How many decigrams (dg) are there in 0.822 microgram (mg)?
7. How many kilograms (kg) are there in 2.023 x 103 milligram (mg)?
8. Calculate the number of milligrams (mg) in 6.2 x 104 micrograms (mg).
9. How many cubic decimeters (dm3) are there in 1.733 x 105 cubic meters (m3)?
10. The volume of a sample of water is found to be 86.3 cubic centimeters (cm3). What is
the volume of the sample in cubic millimeters (mm3)?
CHEMISTRY METRIC DIMENSIONAL ANALYSIS
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Name ___________________________ Period _________
Density Worksheet
In order to receive full credit, you must show ALL work and circle your final answer.
1. 100 grams of a liquid completely fill a 200 mL bottle. What is the density of the liquid?
2. A solution has a density of 1.50 g/mL. How many grams are needed to obtain 10.0 mL ofsolution?
3. If a block of copper measures 2.00 cm x 4.00 cm x 5.00 cm and weighs 356 grams, whatis its density?
4. The density of mercury is 13.6 g/mL.
a. what is the mass of 8.20 mL of mercury?
b. what volume would 120 grams of mercury occupy?
5. A piece of silver has a mass of 2800 grams and occupies a volume of 266 cm3. What isthe density of silver?
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6. A bottle has a capacity of 1.2 liters. If the density of ether is 0.74 g/mL, what mass of
ether can the bottle hold?
7. A student pipets 5.00 mL of ethanol into a flask weighing 15.25 grams. She finds that the
mass of the flask plus ethanol = 19.17 grams. Calculate the density of ethyl alcohol.
8. Peanut oil has a density of 0.92 g/mL. If a recipe calls for ¼ cup of peanut oil, what mass
of peanut oil is required? (Hint: 1 cup = 237 mL).
9. A chemist needs 2.00 g of a liquid compound, which has a density of 0.718 g/mL. If thecompound costs $5.67 per mL, how much will a 2.0 gram sample cost?
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