Chem 101 course outline
Course Name
Fundamentals in Chemistry
Course Code:
CHEM 101
Course Provider:
The Division of Arts, Sciences and General Studies
Level
1
Semester in which course is offered:
1
No. of Credits:
4
Total Study Hours:
56
Course Description:
This course introduces students to the fundamental concepts in chemistry. It explores the structure of the atom, bonding between atoms/particles, the concept of the mole, redox reactions, kinetic theory and energetics. A laboratory component will be used to aid in the understanding of these topics.
Course Rationale:
CHEM 101 seeks to enlighten students about the historical development of the structure of the atom and the forces that keep subatomic particles together. It also looks at the importance of intramolecular and intermolecular forces of attraction and how these are linked with the kinetic theory of matter. It further deepens students’ knowledge of the mole concept and introduces the concept of energetics.
General Objectives:
At the end of this course, participants will be able to: Content:
1. Understand the theory of atoms
2. Appreciate that the forces of attraction between particles influence the properties and behavior of matter
3. Understand the mole concept
4. Understand redox reactions
5. Understand the kinetic theory
6. Understand concepts associated with energy changes
Unit Objectives
Understanding the theory of atoms
At the end of this unit, students should be able to:-
1. Discuss the process of theoretical change with respect to Dalton’s atomic theory
2. Describe the structure of the atom
3. Define the terms: mass number, isotopes, relative atomic and isotopic masses and use them in calculations
4. Explain the phenomenon of radioactivity and cite the use of radioisotopes
5. Explain how data from the emission spectra provide evidence for discrete energy levels within the atom
6. Describe the atomic orbitals, with emphasis on the shapes of the s and p orbitals
7. Determine the electronic configurations of atoms and ions in terms of s, p, and d orbitals
8. State the factors which influence the 1st ionization energy of elements
9. Explain how ionization energy data provide evidence for sub-shells
10. Derive the electronic configuration of an element from data on successive ionization energies
Appreciating that the forces of attraction between particles influence the properties and behavior of matter
At the end of this unit, students should be able to:-
1. State the various forces of attraction between particles and how they relate to the states of matter
2. Relate physical properties of matter to differences in strength of forces of attraction
3. Explain the formation of: ionic, covalent and metallic bonds
4. Illustrate the properties of ionic and covalent compounds
5. Describe co-ordinate (dative covalent) bonding
6. Describe the origin of intermolecular forces
7. Predict the shapes of and bond angles in simple molecules and ions
8. Explain the shapes and bond angles of simple organic compounds (ethane, ethene and benzene and their derivatives)
9. Describe qualitatively the lattice structure of crystalline solids and their relation to physical properties
Understanding the mole concept
At the end of this unit, students should be able to:-
1. Apply Avogadro’s law
2. Define the terms: mole and molar mass
3. Write balanced molecular and ionic equations
4. Perform calculations based on the mole concept
5. Apply the mole concept to molecular and ionic equations
6. Calculate empirical and molecular formulae
7. Perform titrimetric analyses and use their results to calculate: mole ratios, molar concentrations and mass concentration
Understanding redox reactions
At the end of this unit, students should be able to:-
1. Explain redox reactions in terms of electron transfer and changes in oxidation state/number
2. Deduce balanced equations for redox reactions from relevant half equations
3. Perform simple displacement reactions to order elements in terms of oxidizing or reducing
Understanding the kinetic theory
At the end of this unit, students should be able to:-
1. State the basic assumptions of the kinetic theory with reference to an ideal gas
2. Explain the difference between real and ideal gases
3. Perform calculations using: Boyle’s law, Charles’ law and the ideal gas equation
4. Explain the following terms: liquid state, melting, vaporization
Understanding the concepts associated with energy changes
At the end of this unit, students should be able to:-
1. State that chemical reactions take place through energy changes(usually in the form of heat) associated with bond breaking and bond forming
2. Explain the differences between exothermic and endothermic reactions using energy profile diagrams
3. Explain the term bond energy and how it may be used to show the relationship between strength of covalent bonds and reactivity of covalent molecules
4. Apply concepts associated with enthalpy changes
5. Explain the effect of ionic charge and radius on the magnitude of lattice energy
6. State Hess’ law of constant heat summation
7. Calculate enthalpy changes from appropriate experimental data.
Assessment:
Incourse exams/assignments 10%
Labs 15%
Final exam 75%
Course Evaluation
Formative
Summative
Required texts
Recommended texts
Ratcliff, B. Eccles, H. Raffan, J., Nicholson, J. and Johnson, D. 2004. AS Level and A Level Chemistry. Cambridge University Press.
Norris, R., Barrett, L., Maynard-Alleyne, A. and Murray, J. CAPE unit 1 Chemistry Study Guide. Nelson Thornes Limited.
Clarke, J. 2000. Calculations in AS/A Level Chemistry. Pearson Education limited.
Norris, R. Ryan, L and Acaster, David. 2011. Cambridge International AS and A Level Chemistry Coursebook.
Lister,T. and Renshaw, J. 2000. Understanding Chemistry for Advanced Level. Cheltenham. Trans-Atlantic Publications
Reference text
Ramsden,E. 2000. A-Level Chemistry. Cheltenham. Nelson Thorne Limited
Clugston,M and Flemming, R. 2000. Advanced Chemistry. London. Oxford University Press
Useful websites http://www.chemguide.co.uk/ http://www.a-levelchemistry.co.uk/
Pre-requisite none Academic staff member who may be contacted for more information
Name: Veronica Luke
Title: Lecturer
Division: Arts Sciences and General Studies.
Fundamentals in Chemistry
Course Code:
CHEM 101
Course Provider:
The Division of Arts, Sciences and General Studies
Level
1
Semester in which course is offered:
1
No. of Credits:
4
Total Study Hours:
56
Course Description:
This course introduces students to the fundamental concepts in chemistry. It explores the structure of the atom, bonding between atoms/particles, the concept of the mole, redox reactions, kinetic theory and energetics. A laboratory component will be used to aid in the understanding of these topics.
Course Rationale:
CHEM 101 seeks to enlighten students about the historical development of the structure of the atom and the forces that keep subatomic particles together. It also looks at the importance of intramolecular and intermolecular forces of attraction and how these are linked with the kinetic theory of matter. It further deepens students’ knowledge of the mole concept and introduces the concept of energetics.
General Objectives:
At the end of this course, participants will be able to: Content:
1. Understand the theory of atoms
2. Appreciate that the forces of attraction between particles influence the properties and behavior of matter
3. Understand the mole concept
4. Understand redox reactions
5. Understand the kinetic theory
6. Understand concepts associated with energy changes
Unit Objectives
Understanding the theory of atoms
At the end of this unit, students should be able to:-
1. Discuss the process of theoretical change with respect to Dalton’s atomic theory
2. Describe the structure of the atom
3. Define the terms: mass number, isotopes, relative atomic and isotopic masses and use them in calculations
4. Explain the phenomenon of radioactivity and cite the use of radioisotopes
5. Explain how data from the emission spectra provide evidence for discrete energy levels within the atom
6. Describe the atomic orbitals, with emphasis on the shapes of the s and p orbitals
7. Determine the electronic configurations of atoms and ions in terms of s, p, and d orbitals
8. State the factors which influence the 1st ionization energy of elements
9. Explain how ionization energy data provide evidence for sub-shells
10. Derive the electronic configuration of an element from data on successive ionization energies
Appreciating that the forces of attraction between particles influence the properties and behavior of matter
At the end of this unit, students should be able to:-
1. State the various forces of attraction between particles and how they relate to the states of matter
2. Relate physical properties of matter to differences in strength of forces of attraction
3. Explain the formation of: ionic, covalent and metallic bonds
4. Illustrate the properties of ionic and covalent compounds
5. Describe co-ordinate (dative covalent) bonding
6. Describe the origin of intermolecular forces
7. Predict the shapes of and bond angles in simple molecules and ions
8. Explain the shapes and bond angles of simple organic compounds (ethane, ethene and benzene and their derivatives)
9. Describe qualitatively the lattice structure of crystalline solids and their relation to physical properties
Understanding the mole concept
At the end of this unit, students should be able to:-
1. Apply Avogadro’s law
2. Define the terms: mole and molar mass
3. Write balanced molecular and ionic equations
4. Perform calculations based on the mole concept
5. Apply the mole concept to molecular and ionic equations
6. Calculate empirical and molecular formulae
7. Perform titrimetric analyses and use their results to calculate: mole ratios, molar concentrations and mass concentration
Understanding redox reactions
At the end of this unit, students should be able to:-
1. Explain redox reactions in terms of electron transfer and changes in oxidation state/number
2. Deduce balanced equations for redox reactions from relevant half equations
3. Perform simple displacement reactions to order elements in terms of oxidizing or reducing
Understanding the kinetic theory
At the end of this unit, students should be able to:-
1. State the basic assumptions of the kinetic theory with reference to an ideal gas
2. Explain the difference between real and ideal gases
3. Perform calculations using: Boyle’s law, Charles’ law and the ideal gas equation
4. Explain the following terms: liquid state, melting, vaporization
Understanding the concepts associated with energy changes
At the end of this unit, students should be able to:-
1. State that chemical reactions take place through energy changes(usually in the form of heat) associated with bond breaking and bond forming
2. Explain the differences between exothermic and endothermic reactions using energy profile diagrams
3. Explain the term bond energy and how it may be used to show the relationship between strength of covalent bonds and reactivity of covalent molecules
4. Apply concepts associated with enthalpy changes
5. Explain the effect of ionic charge and radius on the magnitude of lattice energy
6. State Hess’ law of constant heat summation
7. Calculate enthalpy changes from appropriate experimental data.
Assessment:
Incourse exams/assignments 10%
Labs 15%
Final exam 75%
Course Evaluation
Formative
Summative
Required texts
Recommended texts
Ratcliff, B. Eccles, H. Raffan, J., Nicholson, J. and Johnson, D. 2004. AS Level and A Level Chemistry. Cambridge University Press.
Norris, R., Barrett, L., Maynard-Alleyne, A. and Murray, J. CAPE unit 1 Chemistry Study Guide. Nelson Thornes Limited.
Clarke, J. 2000. Calculations in AS/A Level Chemistry. Pearson Education limited.
Norris, R. Ryan, L and Acaster, David. 2011. Cambridge International AS and A Level Chemistry Coursebook.
Lister,T. and Renshaw, J. 2000. Understanding Chemistry for Advanced Level. Cheltenham. Trans-Atlantic Publications
Reference text
Ramsden,E. 2000. A-Level Chemistry. Cheltenham. Nelson Thorne Limited
Clugston,M and Flemming, R. 2000. Advanced Chemistry. London. Oxford University Press
Useful websites http://www.chemguide.co.uk/ http://www.a-levelchemistry.co.uk/
Pre-requisite none Academic staff member who may be contacted for more information
Name: Veronica Luke
Title: Lecturer
Division: Arts Sciences and General Studies.