1) chem 14 syllabus

7/30/2019 1) Chem 14 Syllabus

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General Chemistry I

Junie B. Billones, Ph.D.Department of Physical Sciences and Mathematics

College of Arts and Sciences

University of the Philippines Manila

The Health Sciences CenterEmail:[email protected]
mailto:[email protected]:[email protected]


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SYLLABUS in CHEM 14

Course Description: Fundamentals in General Chemistry I

Credit: 3 units

Prerequisite: Math11/14/17

General Objectives: Know, understand, and apply chemicalconcepts and principles about matter


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COURSE OUTLINE

2. ATOMIC STRUCTURE

1.1 Properties of Matter1. INTRODUCTION

2.1 Development of Atomic Models

1.3 Classification of Matter

1.2 Changes of Matter

2.1.1 Dalton Model

2.1.2 Thomson Model


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3.1 The Periodic Law

2.3 The Quantum Numbers

2.1.3 Rutherford Model

2.1.4 Bohr Model

2.1.5 Schrodinger Model

3. THE PERIODIC TABLE (PT)

3.2 The Different Groups or Families

2.2 The Electronic Configuration

3.2 The Electronic Configuration and the PT


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3.2 Some Trends in the PT

3.2.1 Size

3.2.2 Ionization Energy

3.2.3 Electron Affinity

3.2.4 Electronegativity

3.2.5 Metallic/Non-metallic Property

3.2.6 Oxidizing/Reducing Ability

4. THE CHEMICAL BOND4.1 The Ionic or Electrovalent Bond

4.1.1 The Lewis Dot Symbol/Formula


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4.2 The Covalent Bond

4.2.1 Valence Bond Theory

4.2.2 Properties of Covalent Bond

4.2.1.1 Writing Lewis Structure

4.2.1.2 Molecular Geometry

4.2.2.1 Polar and Nonpolar

4.2.2.2 Order, Length, Energy

4.2.2.3 Hybridization

4.2.3 Molecular Orbital Theory


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4.3 The Metallic Bond

4.3.1 Electron Sea Model

4.3.2 Band Model

4.2.3.1 Homonuclear Diatomic

5. TYPES OF REACTIONS

5.1 Nuclear Change

5.1.1 Differences between nuclear and

chemical reactions

5.1.2 Types of Radiation

1st Departmental Exam:December 15


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5.1.5 Radioactive Disintegration Series

5.1.3 Types of Nuclear Change

5.2.2 Quantitative Relations Involving Formulas

and Equations

5.1.4 Indicators of Nuclear Stability

5.2 Chemical Change

5.2.1 Types of Chemical Reactions

5.2.2.1 Mole Concept

5.2.2.2 Mole-Mass Conversion

5.2.2.3 Mole-Mole Conversion

5.2.2.4 Mass-Mass Conversion


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5.2.2.5 Percent Composition

5.2.2.6 Molecular/Empirical Formula

5.2.2.7 Concept of Limiting Reactant5.2.2.8 Percent Purity

5.2.2.8 Percent Yield

6. PHASES OF MATTER

6.1 Intermolecular Forces of Attraction

6.2 Comparative Description of Gas, Liquid and

Solid

6.3 Phase Changes

6.3.1 Phase Diagram


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6.5 Gases

6.5.1 The Kinetic Molecular Theory

6.5.2 Gas Laws

6.5.2.1 Boyles Law

6.5.2.2 Charles Law6.5.2.3 Avogadros Law

6.5.2.4 Amontons Law

6.5.2.5 Combined Gas Law6.5.2.6 Ideal Gas Equation

6.5.2.7 Daltons Law

6.5.2.8 Gay-Lussacs Law

6.4 Liquid and Solid States


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6.5.2.7 Molecular Speeds

6.5.3 Real Gas Equation (van der Waals)

6.5.2.6 Grahams Law

7. SOLUTIONS

7.1 Solution Process

7.2 Factors Affecting Solubility

7.3 Types of Solutions

7.3.1 Dilute/Concentrated

7.3.2 Saturated/Unsaturated/Supersaturated

7.3.3 Ideal/Non-ideal

2nd Departmental Exam:February 2


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7.4 Concentrations of Solutions

7.4.1 Preparation of Solutions

7.4.2 Dilution

7.5 Properties of Solutions

7.5.1 Electrical Properties

7.5.2 Colligative Properties

8. CHEMICAL THERMODYNAMICS

8.1 First Law of Thermodynamics

8.1.1 Heat, Work, Energy

3rd Departmental Exam:February 23


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8.2 Second and Third Laws of Thermodynamics

8.2.1 Entropy

8.2.2 Gibb's Free Energy

8.1.2 Heat of reaction

9. CHEMICAL KINETICS9.1 Rate Expression

9.2 Theories on Reaction Rates

9.3 Factors Affecting Rates of Reaction

10. CHEMICAL EQUILIBRIUM


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10.1 Molecular Equilibrium

10.1.1 Kinetic Approach to Equilibrium

10.1.2 Thermodynamic Approach toEquilibrium

10.1.3 Factors Affecting Equilibrium

10.2 Ionic Equilibrium

10.2.1 Ionization of Strong and Weak

Electrolytes (acids and bases)10.2.2 pH and pOH

10.2.3 Hydrolysis


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10.2.4 Neutralization and Titration

4th Departmental Exam:March 19

COURSE REQUIREMENTS

Class Standing 2/3Departmental Exams 80%

Nondepartmental 20%

Classroom works 10%

Assignments 5%

Attendance 5%

Final Exam 1/3


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EXEMPTION POLICIES

1.All major exams are taken.

2. No grade lower than 40% in any of the exams.3. A class standing of at least 60%.

POLICY ON ABSENCES

Any student who failed to take a departmental examdue to illness may be excused upon presentation of

a medical certificate issued by the UP Health

Service.

The final exam may then be substituted for the

missed exam. This can be done for only one exam.


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SCHOLASTIC INTEGRITY

All forms of cheating merits a grade of 5.00 for the

course. A student who is found guilty will not beallowed to drop the course to avoid getting a grade

of 5.00.

GRADING SCALE

90 - 100 --------1.00 65 - 69 -------- 2.25

85 - 89 --------1.25 60 - 64 -------- 2.50

80 - 84 --------1.50 55 - 59 -------- 2.7575 - 79 --------1.75 50 - 54 -------- 3.00

70 - 74 --------2.00 40 - 49 -------- 4.00

below 40 -------- 5.00

1) chem 14 syllabus

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