CHE111 - MODULE 1

1
CHE111 - MODULE 1
0
CHAPTER 1 Lecture Outline
2
Types of Matter
0

• ATOM - The smallest particle of an element that
  retains the chemical properties of that element.
• COMPOUND - Matter that is composed of 2 or more
  elements combined in definite proportions.
• ELEMENT - Matter that is composed of only one
  type of atom.

3
Types of Matter (cont.)
0

• MOLECULE - A definite group of atoms that are
  chemically bonded, i.e. tightly connected by
  attractive forces.
• MATTER - Anything that has mass and occupies
  space.
• SUBSTANCE - Matter that can not be separated by
  physical techniques, and that has a unique set of
  properties.

4
Scientific Method
0

• EXPERIMENT - An observation of natural phenomena
  carried out in a controlled manner so that the
  results can be recorded, duplicated, and rational
  conclusions obtained.
• HYPOTHESIS - A tentative explanation of or
  prediction derived from experimental
  observations.
• LAW - A concise verbal or mathematical statement
  that is always the same under the same
  conditions.
• THEORY - A tested explanation of basic natural
  phenomena.

5
Law of Conservation of Mass
0

• Total mass remains constant throughout a chemical
  reaction
• ex. 2Hg O2 ---gt 2HgO, where the mass of the Hg
  2.53g and the mass of the HgO 2.73g, the mass
  of the O2 has to equal 0.20g.

6
Physical States of Matter
0

• Solid - Relatively incompressible, has a fixed
  shape and fixed volume.
• Liquid - Has a fixed volume and takes the shape
  of its container, fluid, and incompressible.
• Gas (Vapor)- Takes the shape of its container,
  fluid, and is compressible.

7
Physical vs. Chemical Change
0

• Physical Change Change that takes place in the
  form or phase of matter, but not in its chemical
  identity.
• Chemical Change Change that involves the
  combination, recombination, or separation of
  atoms with each other.

8
Types of Mixtures
0

• HOMOGENEOUS - Completely uniform at the
  macroscopic level, no visual or optical
  magnification can distinguish the components of
  the mixture.  (It looks the same!)
• HETEROGENEOUS - A mixture that is composed of
  visually distinctive components. (Looks
  different!)
• Mixtures can be separated by the differences
  in the physical properties of each component.

9
Physical Properties
0

• Color
• State of Matter
• Melting Point
• Boiling Point
• Heat of Vaporization
• Heat of Fusion
• Density - where density mass/volume
• Solubility
• Metallic Characteristics
• Conductivity
• Magnetic Properties
• Geometric Shape
• Viscosity

10
Classic Methods of Separation
0

• DISTILLATION - Components of a mixture are
  separated by the differences in boiling points. 
  Many industrial chemical processes utilize
  distillation for the isolation and purification
  of chemicals.  Refer to the diagram shown in
  class.
• EVAPORATION - A simple but effective means of
  isolating chemicals from solution, for example,
  salt from water.
• CHROMATOGRAPHY - Separation of different
  chemicals by utilizing competing attractive
  forces between a stationary phase and a mobile
  phase.  We will discuss paper, TLC, column, HPLC
  and GC in class.  

11
SI Units
0

• Mass kilograms (kg)
• Length meters (m)
• Time seconds (s)
• Amount of Substance mole (mol)
• Electric Current ampere (A)
• Temperature kelvin (K), where 0?C 273.15K and
  100?C 373.15K

12
Common Metric Prefixes
0

• 1 giga (G) 1X109 basic unit
• 1 mega (M) 1X106
• 1 kilo (k) 1X103
• 1 deci (d) 1X10-1
• 1 centi (c) 1X10-2
• 1 milli (m) 1X10-3
• 1 micro(?) 1X10-6
• 1 nano (n) 1X10-9
• 1 pico (p) 1X10-12
• 1 fenta (f) 1X10-15

13
Primary Units of Metric Measurement
0

• Volume - liter (L), where 1L 1000cm3
• Mass - gram (g) or (gm)
• Length - meter (m)
• In pure water _at_ 4?C, the density of the pure
  water is 1.000g/cm3, and 1g 1cm3 1ml

14
Review of Scientific Notation   -.--- x 10?
0

• One digit . all other significant figures X 10 to
  some power
• Addition and subtraction - the powers of 10 must
  be the same           ex. 2.03 x104 4.56 x104
  6.59 x104
• Multiplication - the powers are additive, the
  constants are multiplied    ex. (2.0 x105)(4.5
  x10-2) 9.0 x103
• Division - the powers are subtracted (denominator
  from numerator), the constants are divided  
•          ex. (6.0 x104)/(3.0 x106)
  2.0 x10-2

15
Rules for Significant Figures
0

• Significant figures are used to describe the
  digits in a measurement that are valid to be used
  based on the acceptable limits of the tool being
  used for measurement.
• When adding or subtracting numbers, the answer is
  rounded to the place value equal to the number
  with the largest place value.
• When multiplying or dividing numbers, the answer
  is rounded to the number of digits equal to that
  of the factor with the least number of digits.
• See guidelines on page 33.

16
Precision and Accuracy
0

• PRECISION - a measurement that indicates how well
  the same data agrees among repetitive testing
  often expressed by the average deviation (Did you
  hit the same mark each time?)
• ACCURACY - a measurement that meets or matches
  the accepted or true value (Did you hit the
  bull's eye?)
• PERCENT ERROR (Error in Measurement/Accepted
  Value)X100