What is Chemistry1

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REVIEW CHAPTERS 1 and 2
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What is Chemistry 1

• Chapter Overview
•   An understanding of the history of chemical
  investigation.
• The history of experimentation and scientific
  inquiry.
• 1.1 Science and Technology
• 1.2 Matter
• What Is Matter?
• A. Occupies space and has mass
• B. Atom smallest unit of matter
• C. Molecule atoms joined together
• See next slide for classification of matter into
  Pure substances and mixtures
• Classifying Matter According to Its State Solid,
  Liquid, and Gas
• A. Solid (fixed volume, incompressible)
• 1. Crystalline
• 2. Amorphous
• B. Liquid
• 1. Fixed volume
• 2. Fluid

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Classifying Matter Section 1.2
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• 1.3, 1.4 and Inserts section 3.5 and 3.6
• How We Tell Matter Apart Physical and Chemical
  Properties
• A. Physical property
• 1. Observable without changing the identity
• 2. Melting point, odor, color
• B. Chemical property
• 1. Observable only by changing the
  identity-Chemical reactions
• 2. Flammability
• How Matter Changes Physical and Chemical Changes
• A. Physical change
• 1. Appearance and properties can change
• 2. Composition does not change
• B. Chemical change
• 1. Appearance and properties can change
• 2. Composition changes
• C. Separation of mixtures through physical
  changes
• 1. Decanting

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Numerical Side of Chemistry 2
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Chapter Overview   A cornerstone of the chemical
sciences, the manipulation of numbers and their
associated units. Measurement accuracies,
significant figures, rounding and scientific
notation.

• 2.1 and 2.2 Numbers in chemistryUnits and
  precision and accuracy in reporting it

• 2.3 Significant Figures Writing Numbers to
  Reflect Position
• A. How many digits can I report? How many should
  I report?
• B. Certain digits and estimated digits
• C. Counting significant figures
• 1. All nonzero digits are significant 1234 4
  Sig fig
• 2. Interior zeros are
  significant 505 3 sig fig
• 3. Trailing zeros after a decimal are
  significant 55.00 4 sig fig
• 4. Leading zeros are not significant 0.012 2
  sig fig
• 5. Zeros at the end of a number, without a
  decimal point, are ambiguous 150 ambiguous
• D. Exact numbers
• 2.4 Scientific Notation Writing Big and Small
  Numbers
• A. Shorthand notation for numbers
• B. Two main pieces decimal and power-of-10
  exponent
• C. Measured value does not change, just how you
  report it (550.6 to 1 sig fig?)

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• 2.5 Significant Figures in Calculations
• Multiplication and division
• Result carries as many significant digits as the
  factor with the fewest significant digits
• B. Rounding
• 1. If leftmost dropped digit is 4 or less,
  round down (leave it same)
• 2. If leftmost dropped digit is 5 or higher,
  round up (increment it by 1)
• C. Addition and Subtraction
• Result carries as many decimal places as the
  quantity with the fewest decimal places
• D. Calculations Involving Both
  Multiplication/Division and Addition/Subtraction
• Do steps in parentheses first
• Determine the number of significant figures in
  intermediate answer
• Do remaining steps
• 2.6 The Basic Units of Measurement
• A. English, metric, SI
• B. SI Units (Mass kg Length m Time sec)
• C. Prefix Multipliers
• milli (m) 0.001
• centi (c) 0.01

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Common Prefixes in the SI System MEMORIZE
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2.8 Converting from One Unit to Another (UNIT
1 to UNIT 2) A. Units are important, most
numbers get one B. Include units in all
calculations C. Conversion factors (Unit you
have comes in the bottom, unit you want comes in
the TOP) Unit 1 X Unit 2 UNIT 2
Unit 1 D. Significant figure of the final
answer depends on UNIT 1 given in problem NOT the
sig. fig of the conversion factor Solving
Multistep Conversion Problems A. Understand
where you are going first B. Not all
calculations can be done in one step 2.8
Units Raised to a Power A. 1 inch 2.54 cm so 1
inch3 2.54 cm3 16.4 cm3 2.7 Density (D
Mass/Volume) A. Mass per unit volume (D
Mass/Volume) B. Derived unit (Volume
Mass/Density) (Mass Density X Volume) C. Can
be used as a conversion factor between mass and
volume Numerical Problem Solving Strategies
and the Solution Map A. Come up with a plan
before you pull out your calculator B. Use the
units to guide your plan
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2.10 Energy A. Energy cannot be created or
destroyed B. Units of energy 1. Joule (J)
2. calorie (cal) (1 cal 4.184J) 3. Calorie
(Cal) (1Cal 1000cal 1kcal) 4. Kilowatt-hour
(kWh)- - Will not be used in CH19 Temperature
Random Molecular and Atomic Motion A. Fahrenheit
(?F) B. Celsius (?C) C. Kelvin (K) Conversions
And
Calorimetry Measuring Quantities of Heat NO
MATH PROBLEMS ON THIS SECTION Read
definitions of Specific heat (cal/gºC) meaning of
it Specific of heat of water 1cal/g ºC
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EXAM 1- 100 POINTS Feb. 27, 2008, 6.00 730
pm, Room T-109
Section I - Multiple Choice 25 of the total
points Section II Fill in the Blanks
scientific notation, chemical change, physical
change, chemical and physical properties, Pure
substances and mixtures 20 of the total points
Section II - Show calculations for partial/full
credit 55 of total points Simple Conversions
show all work round to correct to correct Sig.
Fig, scientific notation when
indicated Density, calories, temperature Show
all calculations/work No Calorimetry problems
for the first test We will decide about them
after the Calorimentry Lab