Chapter 1 Chemical Foundations

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Chapter 1Chemical Foundations

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SI Base Units

• Quantity Unit Symbol
• Length meter m
• Mass kilogram kg
• Time second s
• Electric current ampere A
• Temperature Kelvin K
• Amount of substance mole mol
• Luminous intensity candela cd

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How do we get from one unit to another unit?

• Dimensional Analysis- converting from one unit to
  another
• Use a conversion factor? Ratio
• 1m 100cm 1000mm

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Using Scientific Measurements

• Significant Figures- those digits known with
  certainty plus one estimated digit
• Rules for Determining Sig. Figs.
• a. All nonzero digits are significant
• b. Zeros between nonzero digits are sig.
• c. Zeros appearing in front of all nonzero
  digits are not significant
• d. Zeros at the end of a number and to the
  right of a decimal point are significant
• e. Zeros at the end of a number may or may not
  be significant. Depends if there is a decimal.

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Cont.

• Rounding Rules
• greater than 5, increase by 1
• less than 5, stay the same
• 5 followed by nonzero digit(s), increase by 1
• 5, not followed by nonzero digit(s), and
  preceded by an odd digit, increase by 1
• 5, not followed by nonzero digit(s), and the
  preceding s.f. is even, stay the same

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Cont.

• Addition or subtraction
• the answer must have the same of digits to the
  right of the decimal point as there are in the
  measurement having the fewest digits to the right
  of the decimal point
• Multiplication and division
• the answer will have the same number of
  significant figures as the measurement with the
  fewest number of sig. figs.

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Cont.

• Scientific Notation
• uses the form, M x 10n
• M is a number greater than or equal to one but
  less that 10
• n is a whole number
• 1. Determine M by moving the decimal pt. to the
  left/right so that only 1 nonzero digit remains
  to the left of the decimal pt.
• 2. Determine n by counting the number of places
  you moved the decimal pt. If you moved it left,
  n is positive. If you moved it right, n is
  negative.

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Temperature

• TK TC 273.15
• TC TK - 273.15
• TF TC 9/5 32
• TC (TF 32) 5/9

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Density

• D m/v
• States Of Matter
• 1. Solid? fixed volume and shape
• 2. Liquid ? fixed volume, variable shape
• 3. Gas ? variable volume and shape
• 4. Plasma ?high temperature physical state in
  which atoms lose their electrons

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Classification of Matter

• Pure Substances
• - made of only one kind of atom or molecule
• a. Elements- contains only one kind of atom or
  molecules
• examples of molecules are N2, O2
• b. Compounds- 2 or more elements chemically
  combined
• examples NaCl, CO

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Classification cont.

• Mixtures
• - a blend of 2 or more pure substances
  physically mixed together
• a. Homogeneous Mixture- uniform in composition
• also known as a Solution(small particles)
• Colloid-contains intermediate sized particles
• b. Heterogeneous Mixture- not uniform
  throughout
• Suspension-separates into layers over time

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Separation of Mixtures

• Magnetism
• Filter
• Evaporation
• Centrifuge
• Decant
• Chromatography
• Distillation
• Density

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Lesson Plans

• Day 1
• Intro. To class guidelines,books, etc.
• Individual notes
• PHEOC
• SI base units(7)
• Dimensional analysis
• Density

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continued

• States of matter
• Classification of matter- find handout, define on
  sheet
• Separation of mixtures methods
• Day 2 and 3
• Show slides 5-9
• HW. P. 33-36 24,26,28,30,36,48,54,60,68,80

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Cont.

• Day 4
• Lab
• Day 5
• Ch. 1 Test