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 ---> 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 @ 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%