Fundamentals of Chemistry 1A
The order of topics presented here is essentially the order of presentation in the lecture course, although individual lecturers may make some variations from this. Some topics span more than one week.
Jump to week <1> <2> <3> <4> <5> <6> <7> <8> <9> <10> <11> <12> <13>
Week |
Topics covered |
Introduction
- admin. matters
- overview of course
Elements and Atoms
- elements, compounds and mixtures
- physical and chemical change
- chemical symbols
- allotropes |
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Elements and Atoms (continued)
- atomic structure
- protons
- electrons
- neutrons
- atomic number
- isotopes
- radioactivity
- shell structure
Molecules and Ions - formation of ions
- ionic compounds: formation, formulas, naming
- covalent bonding, valence, bonding/nonbonding pairs |
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Molecules and Ions (continued)
- double and triple bonds
- naming covalent compounds
- polyatomic ions
- empirical, molecular, and structural formulas
- types of bonding in solids
Chemical Equations
- reaction types: combination, precipitation, decomposition, replacement, acid/base
- molecular/ionic equations
- specification of phase
- balancing equations for neutral and charged species
- reactions involving acids |
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Stoichiometry
- atomic, formula and molecular weights
- the Avogadro constant, the mole and molar mass
- % composition, empirical and molecular formulas
- calculations involving balanced equations
- limiting reagents and percentage yield
- molarity and calculations on solutions |
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The Periodic Table
- chemical basis of the periodic table using main group element
Atomic Energy Levels - sub-shells available for each shell and filling these subshells
- electron configurations for atoms and atomic ions
Lewis Model of Bonding
- Lewis structure
- pi bonding
- resonance
- bonding in O3, CO32-, NO3-, benzene, etc |
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VSEPR
- molecular shape
- application to larger molecules including organic molecules
- shape and bonding of common functional groups |
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Gas Laws
- effects of temperature and pressure on volume
- ideal gas law
Thermochemistry - heat and temperature
- greenhouse effect
- kinetic and potential energy
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First Law of Thermodynamics
- heat capacity
- enthalpy
- enthalpy change in a reaction (endo- and exothermic)
- enthalpy as a state function
- Hess's Law
- heat of formation
- CO2 /energy release from fuels
- use of H2 as an alternative fuel
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Types of Intermolecular Forces
- dipole, induced dipole, dispersion, hydrogen bonding
- effects on boiling points
Oxidation Numbers Nitrogen Chemistry & Compounds - high explosives
- nitrogen biocycle, nitrification and denitrification
- hydrides, halides, oxides, oxoacids
Nitrogen in the Atmosphere
- NO/NO2 cycle
- formation of pollutants |
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Chemical Equilibrium - equilibrium as a dynamic process
- the equilibrium constant
- the reaction quotient
- predicting direction of chemical change
- equilibrium calculations
- introduce particular equilibrium constants
- Kp and partial pressures
- Kc and units of concentration
- Ksp
- equilibrium calculations
- Ka and Kb; pKa and pKb
- Le Chatelier’s principle
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| Equilibrium and Thermochemistry in Industrial Processes Mining
- general principles
- example: Mining of copper
- example: The Steel Story
Top 10 chemicals produced in the world:
- special example, sulfuric acid, ammonia
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| Introduction to Electrochemistry -oxidation states
-redox reactions
-cell potential
-half-reactions
-voltaic Cells
Electrochemistry -voltaic or galvanic cells
-using half-reactions
-table of standard reduction potentials
- effect of concentration
-Nernst Equation
-link between E and K
-concentration cells |
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| Electrochemistry (Batteries & Corrosion) - difference between primary and secondary batteries
- how common batteries work
- fuel cells and how they work
- corrosion and corrosion protection
Electrolytic Cells
- how does electrolysis work?
- concept of overpotential
- chlor-alkali process (H2, NaOH, Cl2 from seawater) |
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TextbookEither of the following: |