CHEM 208 Lecture Notes - Lecture 1: Pulmonary Fibrosis, Tetracycline Antibiotics, Boiling Point
28 Jun 2018
School
Department
Course
Professor
CHEM 208 Notes
Module 1 – Basics
Lesson 1.1 – Scientific Method
• Five Steps of the Scientific Method
1. Performing experiments
▪ Set of steps under controlled conditions to propose/test hypothesis
2. Making observations:
▪ Quantitative
▪ Qualitative
3. Proposing a Hypothesis
▪ Tentative explanation for observations
4. Confirming the Hypothesis
▪ Validity needs to be confirmed via repeated and controlled experiments
5. Proposing Scientific Law
▪ Repeatedly perform experiments and modify hypothesis
• Significant Figures
o Rules for Determining Sig Figs
▪ All non-zero digits are significant figures
▪ Counting begins from left with first non-zero number (leading 0s not significant)
▪ Zeros between non-zero digits are significant figures
▪ Terminal zeros are always considered significant if number contains decimal
o Rules for Sig Figs in Chemical Calculations
▪ Addition/subtraction: final answer contains same number of decimal places as the
measurement with the least number of decimal places (least precise measurement)
▪ Multiplication/Division: final answer contains same number of significant figures as
the measurement with least number of significant figures
▪ When exact numbers, unit conversions and constants are involved, number of
significant figures are dictated by the measured quantity involved
o Rules for Rounding-Off in Chemical Calculations
▪ For multi-step calculations, all numbers are carried to the final result which is then
rounded off to correct number of significant figures
▪ If digit being rounded is 5, round up if preceding digit is odd and stays same if even
• SI System of Units
o Length → m
o Volume → m3, L, mL
o Mass →kg
o Density → kg/m3, g/L, g/mL
o Prefixes
▪ Giga=109, Mega=106, Kilo-103, Centi=10-2, Milli=10-3, Micro=10-6, Nano=10-9
find more resources at oneclass.com
find more resources at oneclass.com
CHEM 208 Notes
Lesson 1.2 – Matter
• Elements and Compounds
o Elements: one type of atom → metal, non-metal or metalloid
o Compounds: combination of elements
• Atoms
o Protons and neutrons in nucleus
o Electrons surround nucleus
o Electrons = Protons in a neutral atom
• Atomic Number, Mass Number and Atomic Symbol
o Atomic number: number of protons in nucleus, each element has a different number
o Mass number: total number of protons and neutrons
• Molecules and Ions
o Molecules: a combination of atoms → H2O
o Ions: charged species formed by loss or gain of electrons (cation or anion)
o Cation generation: metal in a gaseous state loses electron
o Anion generation: non-metal gains electron
Lesson 1.3 – Periodic Table
• Russian scientist Dmitri Mendeleev proposed periodic table in 1869
• Groups: Vertical columns 1 to 8 and A or B
o Similar chemical properties
o Letter A designation are main-group elements
o Alkali metals, alkaline earth metals, halogens, noble gases
• Period: Horizontal rows 1 to 7
o Different chemical properties
Lesson 1.4 – Naming of Compounds
• Naming of Compounds
o Organic: compounds that contain at least one carbon atom
o Inorganic: compounds that do’t hae aro (eeptios → CO, CO2, CO3 etc.)
▪ Ionic: metal and non-metal
▪ Covalent: two non-metals
• Ionic Compounds
o Electrostatic attraction between positive (cation from metal) and negative ion (anion from
non-metal)
o Have a neutral charge
o In general, metals lose electrons and non-metals gain electrons
• Rules for Naming and Deriving Formulas of Ionic Compounds
1. Metals of group 1A, 2A, 3A → charge = group number
▪ Li=Lithium, Mg=Magnesium etc.
find more resources at oneclass.com
find more resources at oneclass.com
CHEM 208 Notes
2. Non-metals of group 5A, 6A, 7A → charge = group number – 8
▪ Name is root ending with suffix-ide → N=Nitride, O=Oxide, F=Fluoride
3. Many metals can form more than one cation
▪ Sn2+/Sn4+, Pb2+/Pb4+, Cu+/Cu2+, Cr2+/Cr3+
▪ Fe2+ and Fe3+ form FeCl2=iron (II) chloride and FeCl3=iron (III) chloride
4. Ions with a non-neutral charge are referred to as polyatomic ions
▪ Ammonium NH4+ and Carbonate CO32-are examples
▪ Ca2+ and NO3- form Ca(NO3)2
5. Name, formula and charge can be derived from common acids and bases
• Rules for Naming Covalent Compounds
1. Name first element in formula first
2. Name second element as an anion
3. Use prefixes to indicate numbers of atoms of each element
▪ Mono-, Di-, Tri-, Tetra-, Penta-, Hexa-
4. Do not use prefix mono- for first element
Module 2 – Hazards in Work Environment
Lesson 2.1 – Occupational Hazards
• Types of Occupational Hazards
o Safety hazards
▪ Material handling, machine, energy, work practice and confined space
o Health hazards
▪ Physical, chemical, biological and ergonomic
o Causative agent is hazardous in high concentrations or prolonged exposure
• Assessment of Occupational Hazards
o Processes, operations and related activities → emissions
o Equipment → mechanical and electrical safety
o Properties of substances used and produced → eval. of RM and FG in terms of phys/chem.
o Control measures → engineering controls, ventilation system, protective equipment
• Physical Agents
find more resources at oneclass.com
find more resources at oneclass.com
