Unit I - The Basic Principles of Organic Chemistry and Alkanes
Introduction and Rational:
The purpose of this unit is to review the basic
concepts of chemistry used in the study of
organic chemistry, apply these concepts to the
unique structure and properties of alkanes, and
introduce the nomencalture of simple alkanes to
the students. Since this unit introduces the
students to the basic principles of organic
chemistry that are invlved in organic reactions,
the mastery of these concepts by the students will
facilitate their mastery of the concepts involved in
the study of organic reactions and their mechnism
studed in subsequest units.
Topics
Topic Number Topic
1 Bonding
2 Hybridization of Atomic Orbitals
3 Structure and Nomenclature of Alkanes & Cycloalkanes
4 Structural Isomerism
5 Functional Groups
6 Polarity of Molecules
7 Resonance
8 The Physical Properties of Alkanes and Cycloalkanes
9 Conformations of Alkanes and Cycloalkanes
10 Stereoismerism in Cycloalkanes
11 Acids and Bases
Objectives
Objective Number Objective
Distinguish between ionic, non-polar covalent and polar
covalent bonds in terms of the electronegativities of the
1
elements in the compound and electrostatic attractions in
the compound.
Indicate the positive and negative poles in polar covalent
bonds and the direction of electron flow in non-polar
2
covalent bonds, if any given the electronegativities of the
atoms in the bonds
Write Lewis electron formulas for polar covalently and
3 non-polar covalently bonded compounds knowing the
electron structure of the atoms in the compound.
Determine the formal charge on each atom in a molecule,
4 given the molecule's Lewis electron dot or structural
formula.
Distinguish between polar and nonpolar molecules given
5
their shape and individual bond polarities.
Explain the bonding structure of organic molecules in
6
terms of atomic orbital hybridization, covalent bonding,
bonding angles and molecular orbital formation.
Predict the shapes of molecules and bond angles about
7
each atom in a compound given their Lewis structural
formula and atomic orbital hybridization of the atoms.
Draw Lewis electron dot formulas for different functional
8 groups of organic molecules given the functional group
formula.
Define the terms: resonance, resonance hydrid,
9
resonance structure and contributing structure.
Given the structural formula of a molecule or ion, draw all
10 the resonance structures and hybrids of the molecule or
ion where resonance occurs.
Indicate equivalent and nonequivalent resonance
11 structures and indicate the stability of the different
resonance structures, given the resonance structures.
Name alkanes and cycloalkanes by the IUPAC system of
12
nomenclature given their structural formula.
Write the structural formulas for alkanes and
13
cyclosalkanes given their IUPAC name.
14 Define the term structural or constitutional isomerism.
Determine the number of structural isomers a molecular
15 formula can have, given the molecular formula and draw
all the isomers.
Explain the boiling points and melting points of alkanes in
16 terms of their bonding, type of intermolecular attractions
and compactness.
Define the terms: conformation, dihedral angle, torsional
17 strain, angle strain, steric strain, Van der Wall's radius,
configuration and stereoisomerism.
Draw the different conformations of alkanes using the
18
sawhorse and Newman projection methods.
19 Explain the stability of the various alkane conformations
in terms of torsional and/or steric strain.
20 Explain the stability of the various alkane conformations
in terms of torsional and/or steric strain.
Draw the different conformations of cycloalkanes in terms
21 of the size of the ring, molecular orbital structure and
angle strain.
Determine the stability of the different conformations of
22 cycloalkanes in terms of torsional strain, angle strain and
steric strain.
23
Define axial and equitorial bonds in chair cyclohexanes.
24
Distinguish between configurations and conformations.
Distinguish between cis and trans isomers in
25
cycloalkanes.
Distinguish between Bronsted-Lowry acids and bases,
26
Arrhenius acids and bases, Lewis acids and bases,
strong acids or bases and weak acids or bases.
Write Bronsted-Lowry acid-base reaction equations given
27 the starting reagents and indicate the conjugate acid-
base pairs in the equations.
Predict the position of equilibrium in a Bronsted-Lowry
28 equilibrium reaction given the starting reagents and the
Ka or pKa of the acids.
Write the chemical equations for Lewis acid-base pair
29 reactions given the starting reagents and then identify the
Lewis acid and Lewis base in the equation.
Section Pages in Brown & Foote Done
1.1-1.2 1-16
1.4,1.7-1.8 20-23, 31-42
2.1,2.2, 2.4A, 2.5 51-53, 56-61, 63-66
1.3, 2.2 16-20, 53-55
1.3 16-20
1.5 24-25
1.6 26-31
2.8 85-88
2.6 66-79
2.7A 80-83
4.1-4.5 134-152
Done