tutorial

Chapter 7: ORGANIC CHEMISTRY

Sun, 24 Jun 2012 02:14:37 +0100

Chapter 7: Organic Chemistry

At the end of the lesson the students should be able to :

List the elements that made up organic compounds C, H, O, N, P, S and halogens.
State the ability of carbon to form 4 covalent bonds with other carbons or elements.
Differentiate between saturated and unsaturated organic compounds.
Give examples of organic compounds used in medicine, engineering, biotechnology and agriculture.
Define functional group.
Name functional groups and classify organic compounds according to their functional groups.
Define homologous series and explain general characteristics of its members.
Define isomerism.
Explain constitutional isomerism.

chain isomer
positional isomers
functional group isomer

At the end of the lesson the students should be able to explain the main types of organic reactions:

State the relative stabilities of primary, secondary and tertiary free radicals, carbocations and carbanions.
Explain the inductive effect of alkyl group towards the stability of carbocations and carbanions.
Define electrophile and nucleophile.
addition: electrophilic and nucleophilic
substitution: electrophilic, nucleophilic and free radical elimination

Chapter 6: ACIDS AND BASES

Sun, 24 Jun 2012 02:15:16 +0100

Chapter 6: Acids and bases

Learning outcomes:

At the end of this lesson, students should be able to:

Define acid and base according to Arrhenius, Bronsted- Lowry and Lewis theories.
Define and identify conjugate acid and conjugate base according to Bronsted- Lowry theory.

Chapter 5: CHEMICAL EQUILIBRIUM

Sun, 24 Jun 2012 02:17:16 +0100

Chapter 5: CHEMICAL EQUILIBRIUM

5.1 Dynamic Equilibrium

At the end of the lesson, students should be able to:

Explain a reversible reaction, dynamic equilibrium and law of mass action
State the characteristics of a system in equilibrium
Explain the features of a graph of concentration against time for a reversible reaction

5.2 Equilibrium Constants

At the end of the lesson, students should be able to:

Define homogeneous and heterogeneous equilibria.
Deduce and write expressions for equilibrium constants in terms of concentration, K_c and partial pressure, K_p for homogeneous and heterogeneous systems.
Derive and use the equation, K_p = K_c (RT)^ⁿ.

5.3 Le Chatelier’s Principle

At the end of the lesson, students should be able to:

State Le Chatelier’s principle
Explain the effect of the following factors on a system at equilibrium by using Le Chatelier’s principle:

Concentration of reacting species
Pressure and volume (include the addition of inert gas at constant pressure and at constant volume)
Temperature
catalyst

Chapter 4: CHEMICAL BONDING

Sun, 24 Jun 2012 02:19:32 +0100

CHAPTER 4 :CHEMICAL BONDING

Lecture 1

a) Describe the formation of the following bonds using Lewis dot symbol.

i. Ionic or electrovalent bond

ii. Covalent bond

iii. Dative or coordinate bond

(b) Draw Lewis structure of covalent species with single, double and triple bonds.

(d) Determine the formal charge and the most plausible Lewis structure.

(e) Explain the exception to the octet rule: incomplete octet, expanded octet and odd number electrons.

(h) Explain the concept of resonance using appropriate examples.

Lecture 2

(a) Explain Valence Shell Electron Pair Repulsion theory (VSEPR)

(b) Draw the basic molecular shapes: linear, trigonal planar, tetrahedral, trigonal bipyramidal and octahedral.

Lecture 3

At the end of the lesson the students should be able to:

Describe a hybridization process.
Draw and explain hybrid orbital sp³.
Use hybrid orbitals to explain bond formation in selected molecules.

Chapter 3: PERIODIC TABLE

Sun, 24 Jun 2012 02:19:58 +0100

Periodicity

Lecture 1 :
At the end of the lesson the students should be able to :
(a)     Indicate period, group and block (s, p, d, f).
(b)     Specify the position of metals, metalloids and non-metals in the periodic table.
(c)     Deduce the position of elements in the periodic table from its electronic configuration

Lecture 2:
At the end of the lesson the students should be able to :
(a)       Explain the variation in atomic and ionic radii
i.     across periods 2 and 3
ii.     across the first row of transition elements.
iii.     down a group.
(b)   Explain the variation in the radius of isoelectronic

Lecture 3:
At the end of the lesson the students should be able to :

Define the first and second ionisation energies.
Explain the increase in the successive ionisation energies of an element.
Explain the variations in the first ionisation energy

        i.    across periods 2 and 3.
        ii. down groups 1 and 2.

Lecture 4:
At the end of the lesson the students should be able to :

    (a) Deduce the electronic     configuration     of an element     and its      position     in the     periodic table based on     successive ionisation energy data.

Lecture 5:
At the end of the lesson the students should be able to :

Define electron affinity and electronegativity.
Explain the variation in electronegativity of elements

i. across periods 2 and 3
ii. down a group.

Chapter 2: ATOMIC STRUCTURE

Sun, 24 Jun 2012 02:20:31 +0100

2.1 Bohr’s Atomic Model
2.2 Quantum Mechanical Model
2.3 Electronic Configuration

Bohr’s Atomic Model

At the end of this topic students should be able to:-Describe the Bohr’s atomic postulates.

Explain the existence of electron energy levels in an atom and calculate the energy of electron
Differentiate between line spectrum and continuous spectrum.
Perform calculation involving the Rydberg equation for Lyman, Balmer, Paschen, Brackett and Pfund series
Calculate the ionisation energy from Lyman series
Outline the weaknesses of Bohr’s atomic model.
State the de Broglie’s postulate and Heisenberg’s uncertainty principle

Quantum Mechanical Mode

At the end of this topic students should be able to:-

Define the term orbital.
State the four quantum numbers.
Sketch the shape of s, p and d orbitals.

Electronic Configuration

At the end of this topic students should
be able to:-

Write the electronic configuration of an atom using spdf notation and orbital diagram
State and use Aufbou principle, Hund’s rule and Pauli exclusion principle in filling of orbitals.
Write the electronic configuration of atom or monatomic ion based on its proton number.
Explain the anomalous electronic configurations of chromium and copper.

Chapter 1 : MATTER

Sat, 23 Jun 2012 12:29:59 +0100

Chapter 1 : MATTER
1.1    Atoms and Molecules
1.2     Mole Concept

Learning Outcome
   At the end of this topic, students should be able :

   (a) Identify and describe proton, electron and
        neutron as subatomic particle.

   (b) Define proton number, Z, nucleon number, A
         and isotope. Write isotope notation.
   (c) Define relative atomic mass, Ar and
       relative molecular mass, Mr based on
       the C-12 scale.

   (d) Sketch and explain the following main
       components of a simple mass
       spectrometer.

   (e) Analyse mass spectrum of an element.
        Calculate the average atomic mass of
        an element given the relative
        abundance of isotopes or a mass
        spectrum.