Properties of Matter01

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Properties of Matter 01
Chapter 1

• What is matter?
• anything that has both mass volume.
• What is weight?
• Properties
• describe or identify matter.
• Intensive Properties
• do not depend on amount.
• Extensive Properties
• do depend on amount.

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Properties of Matter 02

• Physical Properties
• can be determined without changing the chemical
  makeup of the sample.
• Some typical physical properties are
• Melting Point, Boiling Point, Density, Mass,
  Temperature, Size, Color, Hardness, Conductivity.
• Some typical physical changes are
• Melting, Freezing, Boiling, Condensation,
  Evaporation, Dissolving, Stretching, Bending.

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Properties of Matter 03

• Chemical Properties
• properties that do change the chemical
  makeup of the sample.
• Some typical chemical properties are
• Burning, Cooking, Rusting, Color change, Souring
  of milk, Ripening of fruit, Browning of apples,
  Taking a photograph, Digesting food.

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Properties of Matter 05

• Homogeneous matter
• has the same appearance, composition, and
  properties throughout.
• Heterogeneous matter
• has visibly different phases which can be seen,
  or properties that vary through the substance.

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Properties of Matter 06

• Pure substances
• have a distinct set of physical and chemical
  properties and cannot be separated by physical
  changes.
• Impure substance or mixture
• two or more pure substances that can be separated
  by physical changes.

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Properties of Matter 07

• An element
• a pure substance with its own set of physical and
  chemical properties that cannot be decomposed
  into simpler chemical substances.
• Compound
• is a pure substance that can be decomposed by a
  chemical change into two or more elements.

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Properties of Matter 09
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Properties of Matter 10

• Which of the following represents a mixture, an
  element, a compound?

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Measurement and Units 01

• Seven Fundamental SI Units of Measurement.

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Measurement and Units 04

• Some Derived Quantities.

g/cm3
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Measurement and Units 02
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Measurement and Units 05

• Density
• relates the mass of an object to its volume.
• Density decreases as a substance is heated
  because the substances volume increases.
• Knowing the density of a substance allows
  measurements of volume to be related to mass or
  measurements of mass to be related to volume.

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Measurement and Units 06
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Measurement and Units 07

• Densities of Some Common Materials.

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Measurement and Units 08

• Density m/V
• density is usually given in g/mL or g /cm3 we
  will treat 1 mL 1 cm3
• What is the density of glass (in grams per cubic
  centimeter) if a sample weighing 26.43 g has a
  volume of 12.40 cm3?
• d 26.43 g/ 12.4 mL 2.131451613 How many
  figures after the decimal should we carry?
• Chloroform, a substance once used as an
  anesthetic, has a density of 1.483 g/mL at 20C.
  How many mL would you use if you needed 9.37 g?
• d 1.483 g/mL 1.483 g.mL 9.37g/x mL
  solving for x
• x 9.37 g/1.483 g/mL 6.318273769 mL
• x 6.31mL

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Scientific Notation

• 2000000 2x106
• 0.0002 2x10-4
• 2x106/2x10-4 1x106x104 1x1010
• 2x104/2x106 1x104x10-6 1x10-2
• 2x106 x 2x10-4 4x102
• 2x106 2x10-4 2000000.0002 2000000.0002

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Temperature 03

• What does temperature measure?
• Temperature measures motion it is a measure of
  the average kinetic energy of molecules 1/2mv2
  where m is the mass of the molecule and v is its
  velocity

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Measurement and Units 09

• Temperature Conversions
• The Kelvin and Celsiusdegree are essentially
  the same because both are one hundredth of
  theinterval between freezing and boiling points
  of water.

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Measurement and Units 10

• Temperature Conversions
• Celsius (C) Kelvin temperature conversion
• Kelvin (K) C 273.15
• Fahrenheit (F) Celsius temperature
  conversions

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What is the freezing point and boiling of water
in C? What is the freezing and boiling point of
water in F?
212 F 32
180
F 1.8 C 32
100
0
100
Centrigrade
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Measurement and Units 11

• Carry out the indicated temperature conversions
• 78C ? K
• 273-78 195 K
• (b) 158C ? F
• F 1.8C32 1.8(158)32 316.4 F
• (c) 375 K ? C
• C 375-273 102
• (d) 98.6F ? C
• C (F -32)/1.8 (98.6-32)/1.8 37.000
• (e) 98.6F ? K
• 98.6F 37.0 C K 27337 310 K

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Measurement and Units 03

• Some Prefixes for Multiples of SI Units.

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Measurement and Units 12

• Dimensional-Analysis
• The use of conversions factors to express the
  relationship between units.

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Measurement and Units 14

• How many meters are there in a marathon race
  (26 miles and 385 yd)?
• 1 mi x 5280 ft/mi x 12 in/ft x 2.54 cm/in x
  1m/100cm 1609.3 m
• 26 mi x(1.6093x103)m/mi 41.84x103 m
• 385 yd x 3 ft/yd x 12 in/ft x 2.54 cm/in x 1
  m/100 cm 352 m
• 41840 m 352 m 42192 m

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Measurement and Units 13

• The volcanic explosion that destroyed Krakatau on
  August 17, 1883, released an estimated 4.3 cubic
  miles (mi3) of debris into the atmosphere. In SI
  units, how many cubic meters (m3) were released?
• 1 mi x 5280 ft/mi x 12 in/ft x 2.54 cm/in x
  1m/100cm 1609.3 m
• 1 mi3 (1609.3)3m3
• 4.3 mi3 4.3(1609.3)3m3 17.92 x 109 m3
• or 4.3(1.6093x103)3 m3

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• How large, in cubic centimeters, is the volume of
  a red blood cell if the cell has a cylindrical
  shape with a diameter of 6.0 x 106 m and a
  height of 2.0 x 106 m?
• The volume of a cylinder is given by V ?r2h
  where r the radius and h is the height of the
  cylinder (? 3.1416), so
• V 3.1416 x (6.0x10-6 m x 100 cm/m)/22 x 2.0 x
  10-6 m x100 cm/m
• V 3.1416 x (3.0x10-4 cm2 x 2.0 x 10-4cm
  5.65 x 10-11cm3

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Accuracy and Precision 03

• What is the difference between accuracy and
  precision? Is there any?

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Accuracy, Precision, and Significant Figures in
Measurement 01

• Accuracy
• how close to the true value a given measurement
  is.
• Precision
• how well a number of independent measurements
  agree with one another.

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Accuracy, Precision, and Significant Figures in
Measurement 02

• Significant Figures
• include the number of digits in the measurement
  in which you have confidence plus an additional
  one which is an estimate.
• The results of calculations are only as reliable
  as the least precise measurement.
• Rules exist to govern the use of significant
  figures after the measurements have been made.

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Accuracy, Precision, and Significant Figures in
Measurement 03

• Rules for Significant Figures
• Zeros in the middle of a number are significant
  eg. 704
• Zeros at the beginning of a number are not
  significant eg. 0.023
• Zeros at the end of a number and following a
  period are significant eq. 230.0
• Zeros at the end of a number and before a period
  may or may not be significant. 230.

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Accuracy, Precision, and Significant Figures in
Measurement 04

• Rules for Calculating Numbers
• During multiplication or division, the answer
  should not have more significant figures than the
  number with the least numbers.
• During addition or subtraction, the answer should
  not have more digits to the right of the decimal
  point than any of the original numbers.

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Accuracy, Precision, and Significant Figures in
Measurement 05

• Rules for Rounding Numbers
• If the last digit is 5 or greater, round to the
  next larger number
• 2.545 2.55
• If the last digit is less than 5 - round down
• 2.544 2.54

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Accuracy, Precision, and Significant Figures in
Measurement 06

• How many significant figures does each of the
  following measurements have?
• 0.036653 m
• 5
• 7.2100 x 103 g
• 3
• (c) 72,100 km
• 3
• (d) 25.03
• 4

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• 12.453/2.3 5.414347826
• 12.453/2.3 5.4
• 12.453
• 2.3
• 14.753
• 14.8

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Chemistry and the Elements
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Properties of Matter 10

• Metals
• Found on left side of periodic table.
• Nonmetals
• Found on the right side of periodic table.
• Semimetals
• Form a zigzag line at the boundary between metals
  and nonmetals.