Term
Pure Substance
and example |
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Definition
Matter composed of one type of particle
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Definition
| composed of two or more different substances in which each retains its own chemical identity |
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Definition
Homogeneous same example salt water
heterogeneous different ex. sand water |
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Term
Properties of matter
2 types? |
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Definition
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| Intensive Properties of matter |
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Definition
Independent of the amount of substance present.
Example Density, boiling point
Remember the IN for INdependnt and INtensive |
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| Extensive Properties of matter |
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Definition
Dependent on the amount of substance present.
example Mass, volume. |
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| Physical Changes of matter |
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Definition
| Changes in matter that do not change the composition of a substance. |
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Definition
| Changes that result in new substances. |
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Term
Problem 1.
Physical (P) or Chemical (C) change?
A. dissolution of a penny in nitric acid
B. crushing of stone
C. the formation of polyethylene from
ethylene
D. rusting of iron
E. melting of lead |
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Definition
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Term
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Definition
Separates solid substances from liquids and solutions
Example sand from water |
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Definition
Separates a homogeneous mixture based on differences in boiling points.
Example salt and water and alcohol and water
complicated looking boiling things |
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Definition
Separates substances on the basis of differences in solubility in a solvent
example different shades of colors in an ink pen, they run different on the paper because of their varably solubilty |
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Term
| 3 types of ways to separate mixtures |
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Definition
Filtration
Distillation
Chromatography |
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Term
A combination of sand, salt, and water is an example of a __________.
homogeneous mixture
heterogeneous mixture
compound
pure substance |
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Definition
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Term
| SI Unit for amount of substance |
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Definition
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Term
| SI Unit for electric current |
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Definition
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Term
| Celsius scale is based on the properties of ? |
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Definition
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| Kelvin scale is based on the properties of ? |
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Definition
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Term
| Converting F to C and visa versa |
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Definition
C = 5/9(F - 32) or
F = 9/5(C) + 32 |
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Definition
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Definition
| refers to how well measured quantities agree with the “true value |
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Term
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Definition
| refers to how well measured quantities agree with one another |
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Term
| Significant Figures Rules |
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Definition
All nonzero digits are significant
Zeros between nonzero digits are always significant.
Zeros at the beginning of a number are never significant.
Zeros at the end of a number are significant if a
decimal point is written in the number |
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Term
| Sig Fig rules in subtraction and addition |
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Definition
| the result has the same number of decimal places as the measurement with the fewest decimal places. |
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| Sig Fig Rules in multiplication or division |
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Definition
| the result has the same number of significant figures as the measurement with the fewest significant figures. |
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Term
WORK
A certain amount of ethanol has a mass of 4.1 g and occupies
a volume of 5.25 mL. What is the density (g/mL)? |
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Definition
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WORK
Determine the length in meters of a 500.0-mi
automobile race.
Use the conversion factors from the back inside
cover of the textbook: 1 km = 0.62137 mi. |
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Definition
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WORK
Convert the length of a 16.0 m rod to inches.
1 in. = 2.54 cm |
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WORK
If the volume of an object is reported as 22.0 ft3,
what is the volume in cubic meters.
1 mi = 1.6093 km 1 mi = 5280 ft |
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Definition
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Term
WORK
If an automobile is able to travel 125 miles on
7.4 gallons of gasoline, what is the gas mileage in
km/L.
1 mi = 1.6093 km 1 gal = 3.7854 L |
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Definition
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