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Matter and Measurements. Matter and Energy - Vocabulary. Chemistry Matter Energy Natural Law-(scientific law) Observation, Hypothesis, Theory, Law. States of Matter. Solids. States of Matter. Solids Liquids. States of Matter. Solids Liquids Gases. States of Matter. Change States

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matter and energy vocabulary
Matter and Energy - Vocabulary
  • Chemistry
  • Matter
  • Energy
  • Natural Law-(scientific law)
    • Observation, Hypothesis, Theory, Law
states of matter1
States of Matter
  • Solids
  • Liquids
states of matter2
States of Matter
  • Solids
  • Liquids
  • Gases
states of matter3
States of Matter
  • Change States
    • heating
    • cooling
states of matter4
States of Matter
  • Illustration of changes in state
    • requires energy
substances compounds elements and mixtures
Substances, Compounds, Elements and Mixtures
  • Substance
    • matter that all samples have identical composition and properties
  • Elements
    • Pure substances that cannot be decomposed into simpler substances via chemical reactions
    • Special elemental forms of atoms (diatomic)

Elemental symbols

    • found on periodic chart
substances compounds elements and mixtures2
Substances, Compounds, Elements and Mixtures
  • Compounds
    • Pure substances composed of two or more elements in a definite ratio by mass
    • can be decomposed into the constituent elements

REVIEW

    • Element cannot be broken down
    • Compound can be broken down into its elements!
substances compounds elements and mixtures3
Substances, Compounds, Elements and Mixtures
  • Mixtures
    • composed of two or more substances
    • homogeneous mixtures
      • Uniform throughout
      • Example: solutions
    • heterogeneous mixtures
      • Not uniform
      • Example: rocks
slide12
Classify the following substances as an element, compound or a mixture (homogeneous or heterogeneous). Which are pure substances?
  • Lightly scrambled egg
  • Water
  • Lava lamp
  • Seawater
  • Chicken noodle soup
  • Root beer
  • Sucrose (C12H22O11)
separating mixtures1
Separating Mixtures
  • Chromatography

paper

chemical and physical properties
Chemical and Physical Properties
  • Extensive Properties - depend on quantity of material

Ex. mass

  • Intensive Properties - do not depend on quantity of material

Ex. boiling point

chemical and physical properties1
Chemical and Physical Properties
  • Chemical Properties - chemical changes
    • Observed during change of material to new material
      • Iron rusting
  • Physical Properties - physical changes
    • No change to the identity of the substance
      • changes of state
      • density
      • color
      • solubility
physical properties
Physical Properties
  • Density
    • mass / volume intensive property
    • Mass and volume extensive properties
  • Solubility
    • Amount of substance dissolved in the solvent at a given temperature
      • Saturated solution
      • Unsaturated solution
      • Supersaturated solution
identify the following as either a chemical or physical change
Identify the following as either a chemical or physical change.
  • Combination of sodium and chlorine to give sodium chloride.
  • Liquefaction of gaseous nitrogen.
  • Separation of carbon monoxide into carbon and oxygen.
  • Freezing of water.
measurements in chemistry
Measurements in Chemistry
  • length meter m
  • volume liter l
  • mass gram g
  • time second s
  • current ampere A
  • temperature Kelvin K
  • amt. substance mole mol
measurements in chemistry1
Measurements in Chemistry
  • mega M 106
  • kilo k 103
  • deka da 10
  • deci d 10-1
  • centi c 10-2
  • milli m 10-3
  • micro m 10-6
  • nano n 10-9
  • pico p 10-12
  • femto f 10-15
units of measurement
Units of Measurement
  • Mass
    • measure of the quantity of matter in a body
  • Weight
    • measure of the gravitational attraction for a body
  • Length

1 m = 39.37 inches

2.54 cm = 1 inch

  • Volume

1 liter = 1.06 qt

1 qt = 0.946 liter

the use of numbers
The Use of Numbers
  • Exact numbers 1 dozen = 12 things
  • Accuracy
    • how closely measured values agree with the correct value
  • Precision
    • how closely individual measurements agree with each other
the use of numbers2
The Use of Numbers
  • Exact numbers 1 dozen = 12 things
    • Counted numbers ex. 3 beakers
  • Significant figures
    • digits believed to be correct by the person making the measurement
  • Scientific notation
    • Way of signifying the significant digits in a number
significant figures rules
Significant Figures - rules
  • leading zeroes - never significant

0.000357 has three sig fig

  • trailing zeroes - may be significant

must specify (after decimal – significant

before decimal - ambiguous)

1300 nails - counted or weighed?

Express 26800 in scientific notation with

4 sig figs 3 sig figs 2 sig figs

significant figures rules1
Significant Figures - rules
  • imbedded zeroes are always significant

3.0604 has five sig fig

How many significant figures are in the following numbers?

0.0124

0.124

1.240

1240

significant figures rules2
Significant Figures - rules

multiply & divide rule - easy

product has the smallest number of sig. fig. of multipliers

significant figures rules3
Significant Figures - rules
  • multiply & divide rule - easy

product has the smallest number of sig. fig. of multipliers

significant figures rules4
Significant Figures - rules
  • multiply & divide rule - easy

product has the smallest number of sig. fig. of multipliers

practice
Practice
  • 142 x 2 =
  • 4.180 x 2.0 =
  • 0.00482 / 0.080 =
  • 3.15x10-2 / 2.00x105 =
  • 24.8x106 / 6.200x10-2 =
practice1
Practice
  • 142 x 2 = 300
  • 4.180 x 2.0 =
  • 0.00482 / 0.080 =
  • 3.15x10-2 / 2.00x105 =
  • 24.8x106 / 6.200x10-2 =
practice2
Practice
  • 142 x 2 = 300
  • 4.180 x 2.0 = 8.4
  • 0.00482 / 0.080 =
  • 3.15x10-2 / 2.00x105 =
  • 24.8x106 / 6.200x10-2 =
practice3
Practice
  • 142 x 2 = 300
  • 4.180 x 2.0 = 8.4
  • 0.00482 / 0.080 = 0.060
  • 3.15x10-2 / 2.00x105 =
  • 24.8x106 / 6.200x10-2 =
practice4
Practice
  • 142 x 2 = 300
  • 4.180 x 2.0 = 8.4
  • 0.00482 / 0.080 = 0.060
  • 3.15x10-2 / 2.00x105 = 1.58x10-7
  • 24.8x106 / 6.200x10-2 =
practice5
Practice
  • 142 x 2 = 300
  • 4.180 x 2.0 = 8.4
  • 0.00482 / 0.080 = 0.060
  • 3.15x10-2 / 2.00x105 = 1.58x10-7
  • 24.8x106 / 6.200x10-2 = 4.00x108
significant figures rules5
Significant Figures - rules
  • add & subtract rule - subtle

answer contains smallest decimal place of the addends

significant figures rules6
Significant Figures - rules
  • add & subtract rule - subtle

answer contains smallest decimal place of the addends

significant figures rules7
Significant Figures - rules
  • add & subtract rule - subtle

answer contains smallest decimal place of the addends

practice6
Practice
  • 416.2 – 10.18 =
  • 16.78 + 10. =
  • 422.501 – 420.4 =
  • 25.5 + 21.1 + 3.201 =
  • 42.00x10-4 + 1.8x10-6 =
practice7
Practice
  • 416.2 – 10.18 = 406.0
  • 16.78 + 10. =
  • 422.501 – 420.4 =
  • 25.5 + 21.1 + 3.201 =
  • 42.00x10-4 + 1.8x10-6 =
practice8
Practice
  • 416.2 – 10.18 = 406.0
  • 16.78 + 10. = 27
  • 422.501 – 420.4 =
  • 25.5 + 21.1 + 3.201 =
  • 42.00x10-4 + 1.8x10-6 =
practice9
Practice
  • 416.2 – 10.18 = 406.0
  • 16.78 + 10. = 27
  • 422.501 – 420.4 = 2.1
  • 25.5 + 21.1 + 3.201 =
  • 42.00x10-4 + 1.8x10-6 =
practice10
Practice
  • 416.2 – 10.18 = 406.0
  • 16.78 + 10. = 27
  • 422.501 – 420.4 = 2.1
  • 25.5 + 21.1 + 3.201 = 49.8
  • 42.00x10-4 + 1.8x10-6 =
practice11
Practice
  • 416.2 – 10.18 = 406.0
  • 16.78 + 10. = 27
  • 422.501 – 420.4 = 2.1
  • 25.5 + 21.1 + 3.201 = 49.8
  • 42.00x10-4 + 1.8x10-6 = 4.2 x 10-3
more practice
More Practice

4.18 – 58.16 x (3.38 – 3.01) =

more practice1
More Practice

4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =

more practice2
More Practice

4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =

4.18 – 21.5192 =

more practice3
More Practice

4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =

4.18 – 21.5192 =

-17.3392

Round off correctly

more practice4
More Practice

4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =

4.18 – 21.5192 =

-17.3392

Round off correctly to 2 sig. figs

-17

unit factor method dimensional analysis
Unit Factor MethodDimensional Analysis
  • simple but important way to always get right answer
  • way to change from one unit to another
  • make unit factors from statements

1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft

3 ft = 1 yd becomes 3ft/1yd or 1yd/3ft

unit factor method dimensional analysis1
Unit Factor MethodDimensional Analysis
  • simple but important way to always get right answer
  • way to change from one unit to another
  • make unit factors from statements

1 ft = 12 in becomes 1 ft/12 in or 12in/1 ft

  • Example: Express 12.32 yards in millimeters.
unit factor method2
Unit Factor Method
  • Example: Express 323. milliliters in gallons
unit factor method3
Unit Factor Method
  • Express 323. milliliters in gallons.
unit factor method4
Unit Factor Method
  • Example: Express 5.50 metric tons in pounds. 1 metric ton = 1 Megagram
unit factor method5
Unit Factor Method
  • Example: Express 5.50 metric tons in pounds.
unit factor method6
Unit Factor Method
  • area is two dimensional
  • Example: Express 4.21 x 106 square centimeters in square feet
unit factor method7
Unit Factor Method
  • area is two dimensional

express 4.21 x 106 square centimeters in square feet

unit factor method8
Unit Factor Method
  • area is two dimensional

express 4.21 x 106 square centimeters in square feet

unit factor method9
Unit Factor Method
  • area is two dimensional

express 4.21 x 106 square centimeters in square feet

unit factor method10
Unit Factor Method
  • volume is three dimensional
  • Example: Express 3.61 cubic feet in cubic centimeters.
unit factor method11
Unit Factor Method
  • volume is three dimensional
  • Example: Express 3.61 cubic feet in cubic centimeters.
percentage
Percentage
  • Percentage is the parts per hundred of a sample.
  • Example: A 500. g sample of ore yields 27.9 g of sulfur. What is the percent of sulfur in the ore?
percentage1
Percentage
  • Percentage is the parts per hundred of a sample.
  • Example: A 500. g sample of ore yields 27.9 g of sulfur. What is the percent of sulfur in the ore?
derived units density
Derived Units - Density
  • density = mass/volume
  • What is density?
  • Example: Calculate the density of a substance if 123. grams of it occupies 57.6 cubic centimeters.
derived units density1
Derived Units - Density
  • density = mass/volume
  • What is density?
  • Example: Calculate the density of a substance if 123. grams of it occupies 57.6 cubic centimeters.
derived units density2
Derived Units - Density
  • density = mass/volume
  • What is density?
  • Example: Calculate the density of a substance if 123. grams of it occupies 57.6 cubic centimeters.
derived units density3
Derived Units - Density
  • Example: Suppose you need 175. g of a corrosive liquid for a reaction. What volume do you need?
    • liquid’s density = 1.02 g/mL
derived units density4
Derived Units - Density
  • Example: Suppose you need 175. g of a corrosive liquid for a reaction. What volume do you need?
    • liquid’s density = 1.02 g/mL
derived units density5
Derived Units - Density
  • Example: Suppose you need 175. g of a corrosive liquid for a reaction. What volume do you need?
    • liquid’s density = 1.02 g/mL
heat temperature
Heat & Temperature
  • heat and T are not the same thing

T is a measure of the intensity of heat in a body

  • 3 common T scales - all use water as a reference
heat temperature1
Heat & Temperature

MPBP

  • Fahrenheit 32oF 212oF
  • Celsius 0oC 100cC
  • Kelvin 273 K 373 K
heat and temperature
Heat and Temperature
  • Example: Convert 111.oF to degrees Celsius.
heat and temperature1
Heat and Temperature
  • Example: Convert 111.oF to degrees Celsius.
heat and temperature2
Heat and Temperature
  • Example: Express 757. K in Celsius degrees.
heat and temperature3
Heat and Temperature
  • Example: Express 757. K in Celsius degrees.
the measurement of heat
The Measurement of Heat
  • SI unit J (Joule)
  • calorie

1 calorie = 4.184 J

  • English unit = BTU
synthesis question
Synthesis Question
  • It has been estimated that 1.0 g of seawater contains 4.0 pg of Au. The total mass of seawater in the oceans is 1.6x1012 Tg, If all of the gold in the oceans were extracted and spread evenly across the state of Georgia, which has a land area of 58,910 mile2, how tall, in feet, would the pile of Au be?

Density of Au is 19.3 g/cm3. 1.0 Tg = 1012g.

group activity
Group Activity
  • On a typical day, a hurricane expends the energy equivalent to the explosion of two thermonuclear weapons. A thermonuclear weapon has the explosive power of 1.0 Mton of nitroglycerin. Nitroglycerin generates 7.3 kJ of explosive power per gram of nitroglycerin. The hurricane’s energy comes from the evaporation of water that requires 2.3 kJ per gram of water evaporated. How many gallons of water does a hurricane evaporate per day?
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