CHEMISTRY COURSE
Academic Year: Fall 2015
Subject: Inorganic Chemistry
Classroom: E2
Hour: 15:00
Instructor: Miss Damylen Ruiz Robles, Chem. Eng.
STUDENTS COMMON CORES
To become familiar with the scope, methodology, and application of
modern chemistry and to learn to appreciate its ability to explain the
physical world.
.
To understand that all matter consists of atoms, and that the limitless
variety observed around us stems from the ways that these atoms bond with
one another.
.
To become adept at problem solving by learning to interpret data, to
employ valid and efficient methods of analysis, and to assess whether or
not the results of calculations are reasonable.
.
COURSE MAIN GOALS
The progression of the course will have emphasis on core chemistry theorical and
practical classes, including basic themes as:
♠ Learning the principles of chemical kinetics, chemical equilibrium, thermodynamics,
and nuclear chemistry.
♠ Modules on organic, inorganic and physical chemistry.
♠ Atomic structure, constitution and shape of organic compounds
♠ Thermodynamics of fluids.
♠ Spectroscopy and inorganic reaction mechanisms.
♠ Lab work builds confidence and developing good technical skills.
♠ Full time mathematic study cases.
♠ Taking another science course related, such as Physics, or other subject outside of
science and engineering.
♠ Preparing presentations and problem-solving exercises.
♠ Being involved in scientific research projects.
CHEMISTRY
TYPICAL
STUDY CASES:
Achieving a sustainable environment is a major
scientific challenge in which Chemistry plays a
fundamental role:
Creating a greener future through green
chemistry: increased industrial efficiencies
and provide us a better future
Developing new synthetic routes for medicines
Developing new molecules and new materials
Understanding reaction pathways
Use of advanced detection and analysis techniques
Obtetion of new crystalline structures
Improving efficiency equipments: solar cells and waste streams
Catalysts for fuel cells.
Waste reduction and remediation protocols
Chemistry substances at extreme conditions
Modelling of smart materials - molecular machines.
Pollution monitoring, simulation and modelling.
Carbon dioxide -CO2 utilisation
THE PERIODIC TABLE OF ELEMENTS
OVERVIEW
This course provides a systematic
presentation of the chemical
applications of group theory with
emphasis on the formal
development of the subject and its
applications to the physical
methods of inorganic chemical
compounds.
1.
Names of the elements
TOPICS
2.
The periodic table
3.
Melting points and boiling points of the elements
4.
First ionization energy, electron affinity and electronegativity of the elements
5.
Atomic and ionic radio of the elements
6.
Covalent bond lengths
7.
Bond enthalpies and average bond enthalpies at Organic compounds—
thermodynamic
8.
Enthalpies of combustion (experimental and theoretical values). Strengths of
organic acids and bases
9.
Acid–base indicators Infrared data
10. Structural formulas of some medicines and drugs
11. Structural formulas of some biological molecules
12. Structural formulas of some food chemistry molecules
REQUIREMENTS
The required materials for laboratory activities in this course are:
 Manual: “Chemistry in the Laboratory” by Scaife, Beachley, and
Allendoerfer, University at Buffalo, 11th Ed.” Harcourt Brace
Custom Publishers 2009. (Photocopies will not be accepted.)
 Lab Materials: laboratory apron, mono goggle safety glasses, and
a padlock for lab drawer are required
 Proper protective clothing is required, including: long sleeve
shirts, pants that reach the ankle, and intact footwear covering the
entire upper portion of the foot. You will not be able to work in
the laboratory without proper clothing. Protective clothing is also
detailed in the Laboratory Notes Document.
SUGGESTED BIBLIOGRAPHY
Another solicited materials are:
 Textbook - Chemistry: The Molecular Nature of Matter and Change, 7th Ed., by Martin S. Silberberg.
 Scientific Calculator - Your calculator must be capable of evaluating logarithms, performing
exponentiation, and calculating trigonometric functions.
ASSIGMENTS FOR THE ENTIRE PROGRAM
Chemistry Homework: Completed online at www.damylen.wordpress.com
Assignments are due at 6 am on the designated day
The Introduction assignment is highly recommended for first time users.
The Math skills & Introduction to Mastering Chemistry assignments are optional, designed to prepare you to succeed in the course
There are 7 graded assignments:
A. Pre-lab assignment: o Read entire experiment & any information located in the Lab Notes
B. Laboratory Experiments: Digital Media o Hand-write a flow chart outlining the experimental section and any safety
precautions.
C. Answer pre-lab questions located in the lab manual (specific questions are indicated in the Lab Notes).
D. The flowchart & pre-lab questions are handed in to the instructor at the beginning of recitation on the day the experiment is
conducted.
E. B. Lab Report: due at the beginning of the next recitation meeting o Hand in the following pages from the lab manual;
measurements, data, sample calculations and post-lab questions (specific questions are indicated on the Lab Notes).
F. Quizzes: There are 4 quizzes, administered in recitation, the content is based on lecture and homework material.
G. A copy of a previous exams will be made available on the course web site, the day of the test.
ASSESMENT FOR EXPERIMENT REPORTS
This is assessed by means of a single extended practical experiment, which the students carry out and write
reports on. The new assessment model uses five criteria to assess the final report of the individual
investigation with the following raw marks and weightings assigned:
The exam report is assessed according to the following criteria:
• Personal engagement - (8%)
• Exploration - (25%)
• Analysis - (25%)
• Evaluation - (25%)
• Communication - (17%)
Total - (100%)
Levels of performance are described using multiple indicators per level. In many cases the indicators occur
together in a specific level, but not always. Also, not all indicators are always present. This means that a
candidate can demonstrate performances that fit into different levels
GRADING SUMARY PLOT
The final course grade (A-F including +/–'s) is determined strictly on the basis of the total number of
points accumulated. Individual exams, quizzes, etc., are not assigned letter grades.
Students should keep all examinations, quizzes, laboratory reports and homework assignments until they
have received their course grade. These are the only materials which will be accepted as evidence of
clerical error in determining a course grade.
CONSIDERATIONS
 Late homework will not be accepted.
 Medical excuses for missed recitations do not cover homework. If you miss a recitation, turn in your homework at the
next meeting.
 Numerical answers to the homework problems will be posted on the course webpage shortly before the due date.
 All documentation MUST include your name and the dates.
 If you are ill on an exam day (or have been ill prior to it and have not been able to prepare adequately) talk with me
before the exam - I visit every exam room before the exam begins.
 A matter of conduct: When I catch a student cheating they receive an automatic F for the course and they are reported
to the dean of their school. Cheating includes carrying any unauthorized written material during a quiz or exam,
storing any information in your calculator (which we will check for), talking to anyone other than an instructor during
a quiz or exam, copying work from another student (or allowing another student to copy from you), changing an
answer on a quiz or exam after it has been graded, and anything else that would give you an unfair advantage over
other members of the class. If your cell phone rings during an exam, you lose 10 points. (so … turn it off before the
exam!).
EXAMPLE OF A REGULAR TASK
PICK AN ELEMENT, ANY ELEMENT
Name: _______________________________________
Choose an element on the periodic table and answer the questions that follow.
1.) What is the name of the element?
2.) What is the atomic symbol of the element?
3.) What is the atomic number?
4.) What is the atomic weight (including units)?
5.) What period and what group is this element found?
a. Period:_______ b. Group:________
6.) Name two facts/properties that you learned about this element?
7.) What is this element used for? Application
TEACHING LESSON PLAN UNIT 1