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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


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 mixtures
Separating Mixtures a mixture (homogeneous or heterogeneous). Which are pure substances?

  • Distillation


Separating mixtures1
Separating Mixtures a mixture (homogeneous or heterogeneous). Which are pure substances?

  • Chromatography

    paper


Chemical and physical properties
Chemical and Physical Properties a mixture (homogeneous or heterogeneous). Which are pure substances?

  • 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 a mixture (homogeneous or heterogeneous). Which are pure substances?

  • 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 a mixture (homogeneous or heterogeneous). Which are pure substances?

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

multiply & divide rule - easy

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


Significant figures rules3
Significant Figures - rules change.

  • multiply & divide rule - easy

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


Significant figures rules4
Significant Figures - rules change.

  • multiply & divide rule - easy

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


Practice
Practice change.

  • 142 x 2 =

  • 4.180 x 2.0 =

  • 0.00482 / 0.080 =

  • 3.15x10-2 / 2.00x105 =

  • 24.8x106 / 6.200x10-2 =


Practice1
Practice change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • add & subtract rule - subtle

    answer contains smallest decimal place of the addends


Significant figures rules6
Significant Figures - rules change.

  • add & subtract rule - subtle

    answer contains smallest decimal place of the addends


Significant figures rules7
Significant Figures - rules change.

  • add & subtract rule - subtle

    answer contains smallest decimal place of the addends


Practice6
Practice change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

4.18 – 58.16 x (3.38 – 3.01) =


More practice1
More Practice change.

4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =


More practice2
More Practice change.

4.18 – 58.16 x (3.38 – 3.01) =

4.18 – 58.16 x (0.37) =

4.18 – 21.5192 =


More practice3
More Practice change.

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 change.

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 Method change.Dimensional 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 Method change.Dimensional 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 change.

  • Example: Express 323. milliliters in gallons


Unit factor method3
Unit Factor Method change.

  • Express 323. milliliters in gallons.


Unit factor method4
Unit Factor Method change.

  • Example: Express 5.50 metric tons in pounds. 1 metric ton = 1 Megagram


Unit factor method5
Unit Factor Method change.

  • Example: Express 5.50 metric tons in pounds.


Unit factor method6
Unit Factor Method change.

  • area is two dimensional

  • Example: Express 4.21 x 106 square centimeters in square feet


Unit factor method7
Unit Factor Method change.

  • area is two dimensional

    express 4.21 x 106 square centimeters in square feet


Unit factor method8
Unit Factor Method change.

  • area is two dimensional

    express 4.21 x 106 square centimeters in square feet


Unit factor method9
Unit Factor Method change.

  • area is two dimensional

    express 4.21 x 106 square centimeters in square feet


Unit factor method10
Unit Factor Method change.

  • volume is three dimensional

  • Example: Express 3.61 cubic feet in cubic centimeters.


Unit factor method11
Unit Factor Method change.

  • volume is three dimensional

  • Example: Express 3.61 cubic feet in cubic centimeters.


Percentage
Percentage change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

  • 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 change.

MPBP

  • Fahrenheit 32oF 212oF

  • Celsius 0oC 100cC

  • Kelvin 273 K 373 K





Heat and temperature
Heat and Temperature change.

  • Example: Convert 111.oF to degrees Celsius.


Heat and temperature1
Heat and Temperature change.

  • Example: Convert 111.oF to degrees Celsius.


Heat and temperature2
Heat and Temperature change.

  • Example: Express 757. K in Celsius degrees.


Heat and temperature3
Heat and Temperature change.

  • Example: Express 757. K in Celsius degrees.


The measurement of heat
The Measurement of Heat change.

  • SI unit J (Joule)

  • calorie

    1 calorie = 4.184 J

  • English unit = BTU


Synthesis question
Synthesis Question change.

  • 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 change.

  • 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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