1. Zumdahl’s Chapter 1
Chemical Foundations

2. Chapter Contents Chemistry: “The Science of All that’s Matter”
Theory and Experiment
Systemé Internationale and English Units
Notation and Multipliers
Error Analysis
Dimensional Analysis
Temperature
Extensive Properties
E.g., Ekin = ½ mv 2
Intensive Properties
E.g.,  = m / V
Classification of Matter
Mixtures
Compounds
Elements
Subatomic

3. CHEMISTRY: The Science of All that’s Matter
From subatomic to macroscopic properties
From static to dynamic properties
From shape to functionality
From electronic forces to molar energetics
Synthesis, Analysis, Characterization & Utility
Interactions of Matter with Matter and Light
Understanding Environmental Consequences

4. Experiment and Theory Observations Inferences
Eternal
Reproducible
Importance of Records!
Inferences
Implications leading to new experiments to confirm or deny both inferences and theories
Explanations
Tentative
Consistent with all observations!
Suggest new experiments
Paradigms
Shifted by inconsistencies
Laws of Nature
Impotence postulates
Occam’s Razor

5. Systéme International Units
MASS, the kilogram [ kg ]
LENGTH, the meter [ m ]
TIME, the second [ s ]
COUNT, the mole [ mol ] or NAv = 6.0221023
TEMPERATURE, the Kelvin [ K ]
ENERGY, the Joule [ J ] = 1 kg m2 s-2
FORCE, the Newton [ N ] = 1 J m-1

6. Scientific Notation and Multipliers
Dealing with the very small and the very large
Scientific Notation: ±  10 ±99
Addition & Subtraction need common powers.
Multiplication & Division: exponents add & subtract.
Scale units with Multipliers ( often by 10 ±3n )
10+12 Tera Giga Mega kilo-
10-1 deci centi milli icro-

7. Error Analysis Repeated experimental values differ.
If tightly clustered, they are PRECISE.
If their average falls near the correct value, they are ACCURATE.
Quoted as average value ± uncertainty () with units!
~2/3 fall within  of avg
Exact numbers have zero uncertainty, e.g., 1 cal  J

8. Significant Figures Rules of Thumb:
Multiplication & Division
Use the smaller number of significant figures
Addition & Subtraction
Use the least significant digit of largest magnitude
Zeroes count as significant figures?
Captive & trailing zeroes count; leading don’t.
y = f(x1,x2,…) and y2 =  Xn2 (f / xn)2

9. Dimensional Analysis Add and subtract common units only!
Under multiplication and division, units accumulate with + and – powers, respectively.
Solution sought must have units identical with that accumulation, or it is not correct.
Factor method of unit conversion chains:
[ 102 cm / 1 m ]3  [ 1 L / 103 cm3 ] or 1 m3 = 103 L

10. Temperature SI unit the Kelvin [ K ] Because 0 K is absolute
0°C = K
0 K = – °C
Different origin but the same size units.
TF = 32°F + (9°F/5°C) TC
0 K = – °F
98.6 °F = ? °C

11. Extensive Properties Scale with the AMOUNT or COUNT
Mass and number of moles are obviously extensive.
Volume and energies so scale  extensive.
Temperature is not extensive!
2 hot bricks have twice the energy but not twice the temperature of one

12. Intensive Properties
Remain the same under increases in amount or count. Temperature is intensive.
Density,  = m / V, is the ratio of two extensive variables; so the amount cancels and  is  intensive.

13. Phases of Matter Condensed Phases “incompressible”
SOLID, maximally compacted & immobile
LIQUID, molecules not fixed but fluid yet still adjacent to one another; of fixed density
Rarified Phases “compressible”
GAS, fluid but nonadjacent molecules expand to fill containers completely (by varying density)
PLASMA, hot, ionized gas of charged atoms & electrons

14. Classifications of Matter
MIXTURES
Separable by physical means
E.g., filtration or chromatography
Heterogeneous
Components in different phases or domains
Homogeneous
Components in same phase and domain
COMPOUNDS
Compounded of different elements, but these can be separated chemically
ELEMENTS
Identical building blocks, atoms, react identically.
SUBATOMIC MATTER
Protons, neutrons, and electrons