Chapter 1 Chemistry: Matter and Measurement

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Chapter 1 Chemistry Matter and Measurement
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Classification of Matter

• What are the states of matter?
• Matter can be a gas, a liquid, or a solid.
• Gases have no fixed shape or volume and can be
  compressed to form liquids
• Liquids have no shape, but they do have a volume.
• Solids are rigid and have a definite shape and
  volume.
• This can be understood by taking a look at whats
  happening on the molecular level!

Phases Animation
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Classification of Matter

• Atoms
• Molecules
• One element (H2, O2, Cl2)
• More than one type of atom - a compound (H2O)
• Mixture - more than one type of atom, element, or
  compound are found together

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Classification
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Noble Gases
Alkali Metals
Alkaline Earths
Halogens
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Chemical Properties

• Property a characteristic that can be used to
  describe or identify matter
• i.e. size, odor, color, melting point,
  solubility, etc
• Extensive Property do depend on amount of
  substance
• i.e. length, volume
• Intensive Property do not depend on the amount
  of substance
• i.e. melting point

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Activity Chemical Change

• Draw a representation (a picture) of how you
  think a chemical reaction works. Use the reaction
  between hydrogen and chlorine as an example.
• Your picture should show how you think the
  particles are arranged as reactants and how this
  arrangement changes in order to make the entirely
  new substance known as the product.
• Compare your picture with the picture of three of
  your classmates.

Sodium demo or anim
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Units of Measurement
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Must quickly master the use of common metric
prefixes and scientific notation!
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There are Three Temperature Scales

• Kelvin Scale
• Used in science.
• Same temperature increment as Celsius scale.
• Lowest temperature possible (absolute zero) is
  zero Kelvin.
• Absolute zero 0 K -273.15 oC.

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• Celsius Scale
• Also used in science.
• Water freezes at 0 oC and boils at 100 oC.
• To convert K oC 273.15.
• Fahrenheit Scale
• Not generally used in science.
• Water freezes at 32 oF and boils at 212 oF.
• To convert

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Volume

• Space occupied by solid, liquid or gas
• V (units of length)3
• Base unit Liter (L)
• 1 mL 1 cm3 1 cc

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Why do some things float and And some things
sink?
1kg of cotton balls 1kg of copper metal
Same mass, different?
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Density

• Example If 73.2 mL of a liquid has a mass of
  61.5 g, what is its density in g/mL?

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Is a solid more dense than liquid?
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Measuring Accuracy Precision
Accuracy how close to true value Precision
how well data points agree with one another
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Uncertainty

• To indicate uncertainty in a measurement, the
  value you record should use all the digits you
  are sure of , plus on additional digit that you
  estimate!

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Significant Figures Uncertainty Lets
Practice!! See Handout
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Practice

• What are the number of significant figures in
  each of the following
• 1282 kg
• 0.00296 s
• 8.070 mm
• 0.0105 L
• 3000 yards

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More Practice

• Round each of the following to four significant
  figures and express in scientific notation
• 300.235900
• 0.006543210
• 456,500

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Unit Conversion

• Conversion factor
• a ratio, including units, used as a multiplier
  to change from one system or unit to another
• 1 lb 453.6 g
• Example convert 381 grams to pounds
• Example convert 1.844 gallons to milliliters

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Activity

• Perform the following conversions.
• 1. 0.290 g to mg
• 2. 1.5 km to mm
• 3. 2 qt to ml
• 4. 1500. cm to yards
• 5. -20.2 degrees F to K

Possibly useful 454 g 1.00 lb 946 ml 1.00
qt 2.54 cm 1.00 in