matter, energy, and measurement home work-1.16, 1.17, 1.19, 1.21, 1.25, 1.27,1.33, 1.37, 1.38, 1.39,...
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Matter, Energy, and Measurement
Home Work-1.16, 1.17, 1.19, 1.21, 1.25, 1.27,1.33, 1.37, 1.38, 1.39, 1.41, 1.45, 1.47, 1.48, 1.49,
1.51, 1.57, 1.59, 1.69, 1.73
Chemistry
• Why?
• The universe consists of three things:
Matter, Energy, Empty Space
• Matter- is anything that has mass and takes up space.
Chemistry
• Chemistry- is the science that deals with matter: the structure and properties of matter and the transformations from one form of matter to another.
• Matter can undergo two types of changes
Changes
• Chemical Change: also called a chemical reaction, substances are used up (they disappear) and others are formed to take their place.
• Examples:
Changes
• Physical Change- changes in which the identity of a substance remains unchanged. (usually involves changes in state and/or appearance)
• Examples:
Properties of Matter
• There are two types of properties:
• Chemical properties: the chemical reactions a substance undergoes
• Physical Properties: properties that do not involve chemical reactions such as:
density, color, melting point, physical state
The Scientific Method
• The scientific method establishes a process that provides a foundation of evidence to back up all scientific information!!
• It has four parts!!!
The Scientific Method
• Fact- is a statement based on direct experience. It is a consistent and reproducible observation.
• Hypothesis- is a statement that is proposed without actual proof, to explain the Fact and/or relationships betweens different Facts.
The Scientific Method
• Tests- Designed experiments or observations used to determine the validity of the Hypothesis.
• Theory- the formulation of an apparent relationship of certain observed phenomena, which has been verified to some extent. (A Hypothesis with evidence from the Tests to support it!!)
Serendipity
• Serendipity- is chance observation. Accidental discovery.
Experimental Notation
• This system provides an easy way to express very large and/or very small numbers
• It is based on the power of tens system
• Examples:
Adding and Subtracting in EN
• Appendix 1 page A-1
• Numbers must have the same exponent
• Add/subtract coefficients
• Leave exponent as is
• Examples:
Multiply and Divide in EN
• First multiply/divide Coefficients
• Then Add exponents for multiplication, Subtract exponents for division.
• Examples:
Significant Figures
• Appendix 2 page A-5
• Defined as: The number of digits of a measured number that have uncertainty only in the last digit.
• Examples:
Rules
1) Nonzero digits are Always significant
2) Zeros at the beginning of a number are Never significant
3) Zeros between nonzero digits are Always significant
Rules (cont)
4) Zeros at the end of a number that has a decimal point are Always significant
5) Zeros at the end of a number with no decimal point May or May Not be Significant.
Sig. Figs. In E.N
• In E.N., the EN number must contain the same number of Sig. Figs. as the original number.
Sig. Figs in Functions
• Multiplication/Division- answer must have the same number of sig figs as the one with the Fewest sig figs.
Sig. Figs in Functions (cont)
• Addition/Subtraction- sig fig not relevant. The answer must contain the same number of decimal places as the one with the Fewest.
Rounding
• If the digit to be dropped is 5,6,7,8 or 9, we round up
• Otherwise, we simply drop the digit.
Defined/Counted Numbers
• Numbers that are defined, or counted, are treated as though they have infinite significant figures.
• Example:
Measurements
• A measurement consists of TWO parts: a number and a unit. The units must always be present.
English Units
• Mass- pounds
• Length- miles, inch, feet, etc
• Volume- gallons, pints, quarts, etc
• Time- Seconds
Metric Units
• Mass- gram, kilogram
• Length- meter, kilometer
• Volume- Liter, milliliter
• Time- Seconds
SI Units are typically the same as metric units, just more specific!
Metric System
• Establishes a base unit, and other units are related to that base unit by powers of 10.
Length
• English• 12 inches = 1 foot• 3 feet = 1 yard• 1760 yards = 1 mile
• Metric– Base unit is the meter
• 1 kilometer = 1000 meters• 1 millimeter = 0.001 meters
Metric Prefixes
Prefix Symbol Valuegiga G 109 1 billion
mega M 106 1 million
kilo k 103 1 thousand
BASE UNIT
deci d 10-1 one-tenth
centi c 10-2 one- hundreth
milli m 10-3 one-thousandth
micro 10-6 one-millionth
nano n 10-9 one-billionth
Volume
• Volume is space.
• The volume of a substance is the amount of space it occupies
• Base unit= Liter
Mass
• Mass is the quantity of matter in an object
• Base Unit= Gram
• There is a difference between Mass and Weight!!!!!
Time
• The base unit for time is Seconds.
• This is the same in all 3 systems!!
Temperature• Base unit= Celsius or centigrade (oC)
• English system uses Fahrenheit (oF)
• The following can be used to convert between the two:
oF = (9/5)oC + 32oC = (5/9) x (oF – 32)
The SI temperature unit uses the Kelvin (K)
K= oC + 273
0K = Absolute zero!!!
Comparisons
Length Mass
1 in = 2.54 cm 1 oz = 28.35 g
1 m = 39.37 in 1 lb = 453.6 g
1 mile = 1.609 km 1 kg = 2.205 lb
Comparisons
Volume Temperature
1 qt = 0.946 L 0 K = -459oF = -273oC
1 gal = 3.785 L 233K = -40 oF= -40oC
1 L = 33.81 fl oz 273K = 32oF= 0oC
1 fl oz = 29.57 mL 310K = 98.6oF= 37oC
1L = 1.057 qt 373K = 212oF = 100OC
1 mL = 1 cc = 1 cm3
Unit Conversions
• Factor-Label Method- we multiply and divide units with numbers using conversion factor.
• Using a conversion factor is the same thing as multiply by 1, only the units cancel out!!!!
Examples
• Convert 2,750 L into kL.
• Convert 120 lbs to grams.
More Examples
• Convert 3.5 miles to meters
• Convert 900 g/ml to lbs/qt
States of Matter
• Matter can exist in three states- Solid, Liquid and Gas
• Gases- no definite shape or volume, highly compressible
• Liquids- no definite shape, but do have definite volume, only slightly compressible
• Solids- Definite shape and volume, essentially noncompressible
Density
• Density- the mass of a substance per unit of volume.– All states of matter have a density.– When two liquids are mixed and one does not
dissolve in the other, the one with the lower density floats on top!!
– Density is calculated by dividing the mass of a substance by its volume
d= m/v
Density
• Density is a physical property and always has the same value at a given temperature
• Density usually decreases as temperature increases because the mass remains the same while the volume increases
• EXCEPTION: WATER!!! From 4-100oC density increases, but from 0-4oC it actually decreases!!!
Specific Gravity
• Numerically, it is the same as density, only it has no units.
• It is the density of a substance compared to water.
Energy
• Energy- the capacity to due work
• Kinetic Energy is energy of motion
• KE increases when either an object moves faster or a heavier object is moving.
Energy
• Potential Energy (PE) is stored energy
• The PE possessed by an object arises from its capacity to move or cause motion.
Forms of Energy
• Mechanical, light, heat, and electrical energy– Kinetic energies possessed by all moving
objects
• Chemical energy and Nuclear energy– Potential energies
Chemical Energy
• The energy stored within chemical substances and given off when they take part in a chemical reaction.
• Examples:
Energy
• Various forms of energy can be converted from one to another
• Example
• Law of Conservation of Energy- Energy can neither be created nor destroyed.
Heat
• Heat is the form of energy that most frequently accompanies chemical reactions
• HEAT AND TEMPERATURE ARE DIFFERENT!!!
• Heat is a form of energy, temperature is a measurement.
Heat (cont)
• The Heat unit is usually a calorie
• calorie- the amount of heat necessary to raise the temperature of 1 gram of water by 1oC.
• This is a small unit so kilocalories is typically used (1 kcal = 1000 calories
• Nutritionists use the word Calorie to mean the same thing as kilocalorie, so:
1 Cal = 1000 cal = 1 kcal
• The SI unit is the Joule (J)
1 cal = 4.184 J
Specific Heat• The amount of heat necessary to raise the
temperature of 1 g of any substance by 1oC.
• Each substance has its own specific heat
• Is this a physical property or chemical property?
• Specific Heat can be used to calculate the amount of heat needed or used
Amt of Heat Used = SH x m x (T2-T1)
Aluminum has a SH of .22, Iron has a SH of .11. How much heat is required to raise the temperature of 100 grams of each from 30oC to 100oC?
Fun with SH!!!
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