Teaching

Teaching process involves four basic steps and they are;

Preparation
Presentation
Application
Review and Evaluation

The Subject materials taught by me during my service period (from December, 2004) at Faculty of Agricultural Sciences of Sulaimani University;

A- Graduate Students,(M Sc. Students): Instrumental Analysis; Plant Ecology and Environment impacts on soil.

B-Undergraduate Students:

First Year (Freshman Grade): General Chemistry; Analytical Chemistry.
Second Year (Sophomore Grade): No lectures have been given by me for the stage.
Third Year (Junior Grade): Quantitative Chemical Analysis ; EIA (Environmental Impact Assessment).
Fourth Year (Senior Grade): Soil, Water and Plant Analysis; Atmospheric Chemistry and Air Pollution.

Currently, at the Faculty of Agricultural Sciences, I am teaching several courses namely:

General Chemistry (1st stage students of Field Crops and Food Science Departments )
Analytical Chemistry (1st stage students of Field Crops and Food Science Departments ) )
Atmospheric Chemistry and Air Pollution(4th stage students of Soil and Water Sciences Department)

Some Quotes about Teaching;

“I never teach my pupils, I only attempt to provide the conditions in which they can learn.” (Albert Einstein)
“It would seem that you have no useful skill or talent whatsoever," he said. "Have you thought of going into teaching?” (Terry Pratchett, Mort).
“The mediocre teacher tells. The good teacher explains. The superior teacher demonstrates. The great teacher inspires.” (William Arthur Ward).
“True teachers are those who use themselves as bridges over which they invite their students to cross; then, having facilitated their crossing, joyfully collapse, encouraging them to create their own.” (Nikos Kazantzakis).
“Real learning comes about when the competitive spirit has ceased.” ( Jiddu Krishnamurti)
“Share your knowledge. It is a way to achieve immortality.” ( Dalai Lama XIV).
“The whole art of teaching is only the art of awakening the natural curiosity of the mind for the purpose of satisfying it afterwards.” ( Anatole France ).
“If you want to teach people a new way of thinking, don't bother trying to teach them. Instead, give them a tool, the use of which will lead to new ways of thinking.” ( R. Buckminster Fuller)
“One child, one teacher, one book, one pen can change the world.” (Malala Yousafzai )
“They may forget what you said but they will not forge how you made them feel.”(Carl W Buechner).

My Philosophy in Teaching;

I can resume the main theme of my teaching philosophy during more than 23 years experience in teaching process as follows;

1- Teaching is an empowering force that can be used to facilitate and spark passion, productivity, and civic responsibility in today’s youth. The goal of education should be to encourage seeking answers, as it is in this way that we advance. Therefore we have to seek for facilitating this advancement of knowledge.

2- Another important theme of my teaching is building a relationship with the students but it’s crucial to create parameters to conversations without consequently promoting division. Relationship building with the students is one of my favorite aspects of teaching. I love hearing about the students 'thoughts, their cultural, lifestyle and their hobbies, since these issues are helpful for a successful teaching. It is important for students and teachers to realize that teaching and education are allies rather than enemies in the academic enterprise.

3- Another important element of my teaching philosophy is encouraging reasoned seminar and critical thinking, especially in developing logical arguments. A major factor of this is spending my time making suggestions, as students can only learn to present their ideas and constructive suggestions more effectively if someone shows them how and why modifications could be made to their natural style to make it clearer.

4- As a science lecturer, I aim to develop students’ understanding of scientific inquiry, helping them visualize science as a process of asking questions about phenomena, conducting investigations to answer those questions, and building explanations based on evidence.

5- The best lecturers or teachers are those that never stop learning and continue striving to improve. It is important to realize that teaching is full of surprises and new situations and one must be ready to adapt, react and discover new strategies.

6- What remains true, it is the necessity to create a meaningful learning environment and to understand how to relate one’s knowledge to students. In order to produce a meaningful environment and acquire a significant learning outcome, it is important to create real world connections, to incorporate student -centered learning, to utilize technology, to generate remaining approachable. If students do not believe they will use classroom material in their future, they see lessons as insignificant, pointless and not worth their time.

7- Finally, as it has been pointed out by Carl W. Buechner, “Students may forget what you said but they will not forge how you made them feel.”Therefore, it is important that students feel comfortable asking questions and that they see a teacher as an adult that cares and one that they can trust. It is necessary to maintain the role of an authority figure while communicating respect to students and relating to them. If a teacher is respected, students are more likely to adhere to one’s rules and take class seriously.

General Chemistry Course Book for the Academic Year 2015-2016

First Part

First year students

Lecturer (Instructor): Dr. Salih N. Majid

Contents

1- Course coordinator and list of lecturers on this course.

2- Course overview

3- Course objectives.

4- Course contents and syllabus

5- Laboratory experiments

6- Course grading

7- Cheating

8- Some general policies

9- References or Texts (Required Materials)

10- Samples of the exam and questions

1- Course coordinator and list of instructors on this course:

Course coordinator: Shno Osman Sofi

E-mail Address of the Course Coordinator: Shna.sofy@yahoo.com

Mobile No>: 07701424743

Lecturers on this course.

1- Dr. Salih N. Majid: (Lecturer)

E-mail: salih.majeed@univsul.edu.iq; salihnm@yahoo.de

Mobile No.: 07701589206

2- Didar Abdulkarim

E-mail: dedar_85@hotmail.com

Mobile No.: 07701595132

3- Zana Gafor Ahmad

E-mail: zana.cann@yahoo.com

Mobile No.: 07701489009

2-Course overview:

Chemistry’ is a subject that delivers a central platform to study other disciplines like agricultural, biology, geology, material science, physics, medicine, and many branches of engineering. It is extremely relevant for businesses as chemistry plays an important role in our economy (we consume a large variety of chemicals every day).

General chemistry course is targeted for first year graduate students and will require students to become familiar with the important principles of chemistry theories, concepts, equations, reactions. General Chemistry is designed for students who have aspirations of obtaining careers in biochemistry, chemistry, agricultural and environmental sciences, biology, medicine, dentistry, pharmacy, and similar areas.

This course examines the fundamental law of chemistry and atomic structure, with an emphasis on intermolecular forces, properties of solutions, bonding, chemical stoichiometry (quantitative relationships) and calculations, states of matter, chemical thermodynamics, reaction rates, electrochemistry, aqueous equilibria and chemical equilibrium. Also includes problem solving skills and descriptive contents for these topics. Furthermore, studying of general chemistry is a basic and integration part for understanding the other related chemistry branches.

3-Course objectives:

Chemistry is the study of properties and transformations of matter. In this course we will study the properties and interactions of matter from a molecular viewpoint. The main objective of general chemistry is to help you in developing a picture of matter and their properties at the atomic and molecular levels. Topics of this course include mathematics in chemistry, structure of atoms, atomic properties, periodic trends, the bonding and molecular structure, the physical states of matter, chemical reactions types, chemical equations, and stoichiometry.

Upon successful completion of this course, the student will demonstrate knowledge and/or skill in the following:

General familiarity with the following areas in chemistry: environmental chemistry, agricultural chemistry, analytical, biochemistry, food chemistry, , organic and physical.
The ability to work effectively and safely in a laboratory environment.
Learned how to think critically and analyze chemical problems.
The ability to separate and precipitate metal in the laboratory using published reactions, protocols, standard laboratory equipment.
The ability to prepare chemical solutions and reagents.
Solve problems involving the principles of chemical kinetics
Solve problems involving the principles of thermodynamics
Solve problems involving the principles of chemical equilibrium and stoichiometry.

4-Course contents and syllabus: Outline and schedule of the topics

Weeks

1

2

Topics

Introductions and Basic Concepts definitions

Atoms, Molecules, & Ions

A Brief Description of the Topics

Chemistry is the science of change; chemistry beings with the description of matter and change. Chemistry classifies materials as elements, compounds, or mixtures. Substances are defined as pure elements or pure compounds. Mixtures contain more than one substance. Sample may be homogenous or heterogeneous.

The atomic theory and nature of matter/ A historical perspective: Aristotle Early Greek Theories; John Dalton, Ernest Rutherford, Bohr’s model, Atomic numbers, Mass numbers, Bohr -Rutherford diagrams, Isotopes and Radioisotopes. Molecular nature of matter and change; Intermolecular Forces/Colligative Properties. Ions; An atom or group of atoms with one or more positive or negative electric charge. Ions is an atom that has either lost or gained one or more electron Positively charged ions are cations, negatively charged ones anions.

A solution is a homogenous mixture of 2 or more substances. Solutions consist of solute and solvent. The solute is (are) the substance(s) present in the smaller amount(s), while the solvent is the substance present in the larger amount. Molarity, Normality, Molality

, Percent, Parts per million (ppm), Parts per billion and P-function are units of concentration.

In chemistry, colligative properties are properties of solution that depend upon the ratio of the number of solute particles to the number of solvent molecules in a solution.^[1] They are independent of the nature of the solute particles, and are due essentially to the dilution of the solvent by the solute.

Colligative properties include: (1) relative lowering of vapor presssure; (2) elevation of boiling point; (3) depression of freezing point and (4) osmotic pressure. The word colligative is derived from the Latin colligatus meaning bound together, since these properties are bound together by the fact that they all depend on the number of solute particles and not on the type of chemical species present

----------------------

Stoichiometry: Calculations with chemical formulas and equations. Stoichiometry explains quantitative information from balanced equations. Balanced chemical equation gives number of molecules that react to form products. Interpretation: ratio of number of moles of reactant required to give the ratio of number of moles of product. These ratios are called stoichiometric ratios.

Real ratios of reactants and products in the laboratory need to be measured (in grams and converted to moles).

Basic Concepts of Chemical Bonding/ Chemical Bonds, Lewis Symbols, and the Octet Rule;

Chemical bond: attractive force holding two or more atoms together.

Covalent bond results from sharing electrons between the atoms. Usually found between nonmetals.

Ionic bond results from the transfer of electrons from a metal to a nonmetal.

Metallic bond: attractive force holding pure metals together.

A branch of physical chemistry concerned with the mechanisms and rates of chemical reactions.

Chemical kinetics, also known as reaction kinetics, is the study of rates of chemical processes. Chemical kinetics includes investigations of how different experimental conditions can influence the speed of a chemical reaction and yield information about the reaction’s mechanism and transition states, as well as the construction of mathematical models that can describe the characteristics of a chemical reaction.

---------------------------------

Energy Changes in Chemical Reactions: Chemical thermodynamics studies the role of entropy in chemical reactions. Entropy is a measure of a system's energy that is unavailable for work, or of the degree of a system's disorder. When heat is added to a system held at constant temperature, the change in entropy is related to the change in energy, the pressure, the temperature, and the change in volume.

Enthalpy is a measure of the total energy of a thermodynamic system. The total enthalpy, H, of a system cannot be measured directly. Thus, change in enthalpy, ΔH, is a more useful quantity than its absolute value. The change ΔH is positive in endothermic reactions, and negative in exothermic processes.

---------------------------------

3

4 & 5

Exam 1

6 & 7

8 & 9

10 & 11

Exam 2

12 & 13

Final exam

Solutions and concentrations units

Colligative Properties of Solution

---------

Stoichiometric Calculations

Chemical Bonding

Chemical kinetics

a. Rates

b. order

c. mechanism

Thermodynamics

a. enthalpy

b. entropy

c. free energy

----------------

5-Laboratory Experiments

The laboratory is an important part of the general chemistry course and will count 30% toward your course grade. All students are encouraged to go through the assigned lab material before the lab. There will be a brief pre-lab quiz based on the material to be covered. Most experiments will be performed in pairs or groups, however, some in-lab practical exercises will be performed individually. Points will be awarded based on their overall performances in the lab that will include pre-lab quiz, completion of required lab activities, post-lab assignments and in-lab practical exercises.

All labs start out with a half-hour discussion period followed by a two and half-hour lab. There will be 10 inorganic qualitative analysis experiments of separation and characterization of group cations throughout the semester.

Inorganic qualitative analysis is the unambiguous identification of cations (and/or anions) present in solution. Unique tests for all ions in the possible presence of all others are virtually impossible to devise. Many tests give similar results with different cations. However, if a solution is treated to separate ions into smaller groups, identification is simplified. The most common way to subdivide cations into smaller groups is by selective precipitation, in which a small group of cations is precipitated chemically. The precipitate can then be physically separated from the remaining cations in solution by centrifuging. The precipitate (insoluble solid) settles out and the solution (supernatant liquid) is decanted into another container. In this way the initial large group can be separated into smaller groups until a definitive test can be performed to verify the presence or absence of each specific cation.

It is important to realize that many chemical reactions do not go to completion. The extent to which a reaction occurs depends on the magnitude of the equilibrium constant, Ksp for the reaction and the concentrations of reagents present. Equilibria can be shifted by adding or removing reagents and by altering the physical conditions in accordance with Le Châtelier's principle. In this analysis scheme, you will use various reagents to force precipitation to occur, dissolve sparingly soluble compounds or complex particular ions so they will not interfere with tests for other ions.

There are several ways to classify metal ions according to the solubility of the compounds they form with various anions. The experiments included the following metal group analysis:

Exp.1: Analysis of silver group (Group 1).

Exp.2: Analysis of the copper group (Group IIA)

Exp.3: Analysis of the arsenic group (Group IIB)

Exp.4: Analysis of the iron group (Group IIIA)

Exp.5: Analysis of the zinc group (Group IIIB)

Exp.6: Analysis of the calcium group (Group IV)

Exp.7: Analysis of the alkali group (Group V)

Exp.8: Separation of cations into groups

Exp.9: Preliminary examination for acid radicals with hydrochloric acid (HCl)

Exp.8: Preliminary examination for acid radicals with sulfuric acid (H₂SO₄)

Once you finish the laboratory experiment, you must follow all the lab directions and safety rules for cleaning your bench work, all the used glassware and keeping the chemical reagents. Then after you must complete and write your results and personal notes.

6- Course Grading:

The grade in this course is similar to others courses and will be based on the student performance on 3 examinations (2 monthly exams and the final). The lecture portion will constitute 75% of the final grade and the laboratory 25% of the final grade. Sometime quizzes will also cover theoretical material presented in lecture and studied through homework problems.

The hundredth grading scale for this class is as follows:

7- Cheating:

According to University policy and regulations, there is zero tolerance for cheating in any of student's test or examination. If you are caught cheating in any way, you will fail the course. In addition, any student caught cheating will be subject to disciplinary action that could result in expulsion from the faculty. Plagiarism of another student’s work or from any other source, talking during an exam, looking at another student’s work during an exam, using a calculator as a memory device, opening a book, using notes, or changing an answer on an exam once it’s been returned are some examples of cheating. In these cases, the student will be immediately dismissed from the room and given a zero score, because it may be assumed that he/she intended to use such materials unlawfully, and he/she may be penalized accordingly. Such behavior will result in disciplinary sanctions resulting in suspension, dismissal or expulsion from the University.

Copying pre-lab, lab write-up, or post-lab answers from other students is also cheating and will not be tolerated.

8- Some general policies:

No cell phones or texting in lecture or lab. No food, drinks, or gum in lab although you can go outside to eat or drink during lab. No food in lecture although drinks are permitted. During lecture, remain in your seats for the duration. No earphones in either lecture or lab. Don't hurt yourself or others by doing something stupid. Let’s say you are doing a lab that you use highly toxic and flammable chemicals and if misused could kill you. Regular class attendance should be kept. A student who persists in being absent from class will be reported to the student’s affairs section. If you miss an exam because of illness or other extenuating circumstance (travel for family matters is not considered to be an emergency circumstance), you must contact the instructor to discuss your situation prior to the absence.

9- References or Texts:

Brady, J. E. (1982). General Chemistry: Principles and Structure. Fifth Edition. John Wiley & Sons. New York Wiley. Oxtoby, D. W., Freeman, W. A. and Block, T. F. (2003). Chemistry Science of Chance. Fourth Edition. THOMSON, BROOKS/COLE. Australia. Canada. United Kingdom. United States. Whitten, K. W., Davis, R. E., Larry Peck, M. and Stanley, G. G. (2004). General Chemistry. Seventh Edition. THOMSON, BROOKS/COLE. Australia. Canada. United Kingdom. United States.

Pauling, L. (1988). General Chemistry. Third Edition. Dover Publications. USA. الكيمياء العامة، د. ابراهيم صادق الخطيب و د. مصطفى تركى اعبيد. اسس و مبادى الكيمياء. د. محمد بشير حسن، د. محمد الامين صابر و د. عثمان ابراهيم عثمان. مبادى الكيمياء العامة. دز محمد مجدى واصل

11- Samples (1) of the exam and questions

University of Sulaimani

Faculty of Agriculture Sciences

Soil and Water Sciences Dept.

General Chemistry Exam for First Years Class

Theoretical Part

Q- 1/ Match the statement under column B with the most appropriate statement written in column A. (10 Mark)

No.

1

2

3

4

5

6

7

8

9

10

Column A

No.

1

2

3

4

5

6

7

8

9

10

Column B

due to the presence of nonvolatile, non ionizing solute is summarized by Raoult’s Law.

naturally lie close to those of the pure solvent.

or allowing the passage of more solvent molecules from a dilute solution to a more concentrated one.

atoms exhibit a tendency for their valence shells either to be empty or to have a full complement of eight electrons (octet rule).

that are directly proportional to the number of solute particles present.

It is always associated with a chemical formula and represents Avogadro’s number of particles represented by that formula and expressed in gram.

that dissolves in a given volume of solvent at a given temperature.

and is the most powerful and the widest used tool for separation and measuring of a complex mixture.

but having more neutrons (therefore, have greater mass).

then it is a heterogeneous mixture.

Osmotic pressure ( ) is the pressure required to stop osmosis,

The lowering of the vapor pressure of a solvent

Isotope is an atom with the same number (#) of protons

Chromatography means "color writing"

For dilute solutions, the numerical values of physical properties

Solubility is the amount of a substance (

If matter is not uniform throughout,

A concept of chemical bonding theory based on the assumption that in the formation of compounds,

There are four important colligative properties of a solution

The mole (mol) is the SI unit for the amount of a chemical species.

Q-2/ Choose only the most appropriate answer given for the following expressions:

1- ……………….. take the shape and volume of their container.

(a-Solid substances, b- Liquid substances, c- Gas substances)

2- If homogeneous matter cannot be separated by physical means, then the matter is a ……………

(a-pure substance, b- heterogeneous mixture, c- homogenous mixture)

3- …………………….. is an intensive physical property of a matter.

(a-Volume, b- Pressure, c- Density)

4- The proportions of elements in ………………….are the same irrespective of how it was formed. That is considered as a Law of Constant Composition.

(a-mixtures, b- compounds, c- atoms)

5- …………. are measurements that are close to the “correct” value.

(a-Accurate, b-Precise, c-error)

6- ……………… bond results from the transfer of electrons from a metal to a nonmetal.

(a-Ionic, b-Hydrogen, c-Covalent)

7- The closest shell to the nucleus is called the "1 shell" and it is also called ……………

(a-M shell, b-N shell, c-K shell,)

8- A ……………. molecule or portion of a molecule is one that has a tendency to interact with or be dissolved by water and other polar substances.

(a-Hydrophobic, b-Hydrophilic, c-Diatomic)

9- There are some covalent bonds in which the electrons are located closer to one atom than the other, and these results in ………………. bonds.

(a-polar, b-non-polar, c-double)

10- Semi-quantitative expressions of concentration can be described as ……………… or …………………….

(a-dilute, b-concentrated, c-saturated, d-unsaturated, e-molarities , f-molality ).

11- …………liter is a prefix of 10^-3 liter, whereas…………meter is a prefix of 10^-9meter, but …………..gram is a prefix of 10⁹gram.

(a-micro, b- mega, c-femto, d- pico, e- giga, f- nano, g- milli, h-kilo, i- deci

12- Protium is an isotope of hydrogen which has the symbol of …………………

(a- ₁H¹; b-₁H²; c-₁H³ ) (15 Mark)

Q-3/ A solution was made by dissolving 60 g of glucose C₆H₁₂O₆, (M.wt = 180 g/mol) in 180 g of water (M.wt = 18 g/mol). Find the vapor pressure lowering of the solution if the vapor pressure of pure water at 25 C^o is 23.8 torr. (7 Marks)

Q-4/ A 0.2 mol of each fructose (C₆H₁₂O₆) (non-electrolyte) and calcium chloride CaCl₂ (electrolyte) were dissolved in one liter of a solution separately. Calculate the van’t Hoff factor (i) for each solute, if Avogadro's number is 6.022 x 10²³. Then indicate which solute cause greater change (Δ) in the physical properties of the solutions and why? (6 Marks)

Q-5/ What is the freezing point of a solution containing 478 g of ethylene glycol (antifreeze) in 3202 g of water? The molar mass (M. wt) of ethylene glycol is 62.01 g. If K_f the molal freezing-point depression constant of water (K_f) = 1.86 ⁰C/m. (7 Marks)

Q-6/ Gallium is a metal that can melt in your hand at 29.93 °C. What is the temperature in °F?

Practical Part:

Q-1/ A slight excess of dilute HCl solution will be added in separation of silver group (Group I). Explain why? (3 Marks)

Q-2/ Complete the following chemical reaction; (2 Marks)

PbCl₂+K₂CrO₄

Q-3/ Fill in the blanks with the most suitable word(s) or terms;

(silver group, ammonium chloride, iron group, four, five, qualitative analysis) (5 Marks)

1-Anions are divided into --------------groups, while cations are divided into --------------groups.

2- ---------------- forms soluble complex with group IV of cations.

3--------------------is mainly focused on detecting of ions in an aqueous solution.

4- The group (I) of cations is called ………….. , while group (III) is called------------------.

Samples (2) of the exam and questions

University of Sulaimani

Faculty of Agriculture Sciences

Soil and Water Sciences Dept.

General Chemistry Exam for First Years Class

Answer only (4) questions of the following;

Q- 1/ Verify the sentences below with True (T) or False (F).

1- Some nonmetals like sodium (Na) are extremely chemically reactive, while gold (Au) is

typical of the other.

2- The surface tension of a liquid is the resistance of the surface of a liquid to an increase in

its volume.

3- When lattice energy is larger than the hydration energy of the ions, the formation of the

solution is endothermic, and ΔH_solution is positive(+)..

4- Capillary action is the drawing of a liquid up the inside of a small bore tube when cohesive

forces exceed adhesive forces.

5- Colligate properties of solutions are physical properties of the solution that depend on the

nature, charge and kind of solute's properties.

6- When the total vapor pressure of a solution is less than that predicated by raoult's law. This

is known as negative deviation.

7- The osmotic pressure (π) of a solution measures its ability to pull additional solute

molecule into itself by osmosis.

8- Fractional distillation is the process in which a liquid solution can be separated into volatile

and nonvolatile components.

9- The effect of pressure on the solubility of a gas is given quantitatively by Raoult’s law (Cg

= Kg x Pg).

10- The outer shells of metals contain normally four or more electrons except hydrogen and

helium.

Q- 2: A/ The partial pressure of ethane (C₂H₆) over a saturated solution containing 6.56 x 10^-2

g of ethane at 25C^o is 751 torr. What is the partial pressure when the saturated solution

contains 1 x 10^-2g of ethane at 25C^o?

B/ The concentration of fluoride (F^-1) ion in sea water is approximately 0.001-g per 1000

gram sea water. Express this concentration in:

1- w%w percent. 2- Parts per million (ppm) 3- parts per billion (ppb).

Q- 3: A/ A mixture was prepared from 50-g of carbon tetrachloride CCl₄ (M. wt. = 153.8 g/mol) and 50-g of Chloroform CH₃Cl (M.wt. = 119.4 g/mol). At 50 C^o, the vapor pressure of pure (P^o) CCl₄= 317 torr and that of pure (P^o) CH₃Cl = 526 torr. Answer the following:

1- Calculate the mole fraction of each component in the solution.

2- Find the total vapor pressure of the mixture. Name the law of calculation.

3- Calculate the mole fraction of each component in the vapor phase. Name the law of calculation.

4- Which component is more volatile?

B/ Name the common units of concentration measurements:

Q-4: A/ A 2-g of non-dissociating protein is dissolved in 100-ml of water and find the osmotic pressure to be 16 torr at 25 C. Estimate the molecular weight of the protein.

(R= 0.0821 L. atm / mol. K)

B/ Briefly describe the kinds of liquid mixtures (solutions).

Q- 5:A/ When 15-g of ethyl alcohol, C₂H₅OH (M.wt = 46 g/mol) is dissolved in 750-g of formic acid HCOOH. The freezing point of pure formic acid is 8.4 C. Evaluate molal freezing point constant (K_f) for formic acid.

B/ A 50-g of sucrose C₁₂H₂₂H₁₁ is dissolved in 117-g of water H₂O. If K_b for H₂O = 0.512 C^o/m and M. wt of sucrose = 342 g/mol. Answer the following:

Calculate the change in the boiling point ΔTb of pure water.
Find the boiling point of the solution Tb (solution) if Tb of pure water = 100 Co.

University of Sulaimani First year class

Faculty of Agriculture Sciences Subject: General Chemistry

Dept. of Soil and Water Sciences Time: 3 Hours

Theoretical Part

Q1/ Verify the sentences below with True (T) or False (F):

1. Liquids take the shape of their container, but they do have their own volume.

2. If homogeneous matter cannot be separated by physical means, then the matter is a pure substance.

3. If matter is not uniform throughout, it is heterogeneous mixtures.

4. The human body consists mostly of 3 main elements.

5. There are 118 elements known in periodic table.

6. Extensive physical properties depend on how much of the substance is present.

7. When a substance changes its composition, it undergoes a chemical change:

8. Mixtures can be separated if their physical properties are different.

9. Femto is a prefix of 10^-6 derived unit.

10. There are 7 derived units in the SI system (International System of Units).

Q2/ Choose only the most appropriate answer for the following expressions:

1- Measurements that are close to the “correct” value are ……………..

a- accurate, b- precise, c- significant.

2- ……………..bond results from sharing electrons between the atoms. Usually found between nonmetals.

a- Covalent, b- Ionic, c- Metallic.

3- All noble gases except ………….. have an s²p⁶ configuration.

a- argon (Ar), b- neon (Ne), c- helium (He)

4- …………….energy is the energy required to completely separate an ionic solid into its gaseous ions.

a- Thermal, b- Lattice, c- Nuclear, d- Solar

5- We represent the electrons as ………… around the symbol for the element.

a- dots, b- circles, c- coma.

6- The SI unit for length is the ………, whereas the SI unit for amount of chemicals substance is the………………..

a-meter, b-liter, c-gram, d-mol, , e- molarity, f- normality,

7- …………liter is a prefix of 10^-6 liter, whereas…………meter is a prefix of 10^-12meter, but …………..gram is a prefix of 10⁹gram.

a- micro, b- mega, c-femto, d- pico, e- giga, f- nano, g- milli, h-kilo, i- deci

Q3/ Your grandmother has a piece of gold of 1.0 cm thick, 2.0 cm wide and 4.0 cm long. If the gold has a density of 19.32 g/cm³ and an atomic weight 196.97 g/mol, calculate the following:

1- How many grams of gold has your grandmother?

2- How many moles of gold has your grandmother?

3- How many gigaatoms of gold has she?

4- Write the Chemical symbols of gold.

Q4-A/ Which of the following contains the largest number of molecules: 6.00 g CH₄, 9.00 g H₂O,

15.0 g NO₂. If the molecular weights are; CH₄= 16 g/mol, H₂O = 18 g/mol, NO₂ = 46

g/mol and Avogadro's number = 6.022 x10²³.

B/ Make the following temperature conversions: (a) 60 ^oF to ^oC; (b) -60 ^oC to ^oF.

Practical Part

Q1-A/ Verify the sentences below with True (T) or False (F):

1. Anions are divided into four groups, whereas cations into five groups.

2. The cations of group (I11) include Fe³⁺, Al³⁺, Cr³⁺, and Mn⁺².

3. We separated the filtrate from the precipitate (ppt.) by means of a filter paper and funnel.

4. The Amphoteric cation in group (I) is Ag²⁺.

5. The metals of group (1) are characterized by their precipitation as chloride.

B/ After adding of the reagent NH₄Cl for precipitating group (III), the solution should be heated. Explain why?

Lecturer: Dr. Salih N. Majid

Faculty of Agricultural Sciences

University of Sulaimani

Course book peer review:

This course book has been reviewed by Dr. Burhan Tahir Kader

Reviewer Signature

Dr. Burhan Tahir Kader

4.7.2015

Analytical Chemistry Course Book for the Academic Year 2015-2016

First year students

Second Part

Name of the Lecturer: Dr. Salih N. Majid

Contents

1- Course coordinator and list of lecturer on this course.

2- Course overview

3- Course objectives.

4- Course contents and syllabus

5- Course grading

6- Cheating

7- Some general policies

8- References or Texts (Required Materials)

9- Samples of the exam and questions

Course coordinator and list of instructors on this course:

Course coordinator: Bzhwen Khalid Majeed

E-mail Address of the Course Coordinator: Bzhwen.majeed@univsul.edu.iq

Mobile No. 07701468930

Lecturers on this course.

1- Dr. Salih N. Majid: (Lecturer)

E-mail: salih.majeed@univsul.edu.iq; salihnm@yahoo.de.

Mobile No.: 07701589206

2- Zana Hama Gafur

E-mail: zana.canny@yahoo.com

Mobile No.: 07701489009

2-Course overview:

Analytical chemistry course is targeted for first year graduate students and will require students to become familiar with the important of analytical theories, concepts, equations, reactions, and methods of analysis processes needed in the different agricultural sectors and environment fields, by using different analytical tools and instruments. Furthermore, studying of analytical chemistry is an integration part for understanding the other related chemistry branches. Current studying in analytical chemistry and applied methods for analytical techniques and measurements will help the students to solve major agriculture problems. Scientific subjects will be presented for the students. These presentations will summarize the basic analytical concepts and significant information for investigating the composition of concern samples and matters (soil, water, plant, food product, animal product, etc.) in agriculture and environment.

3-Course objectives:

Analytical chemistry is a remarkable domain of chemistry. It is an area that has to take the techniques and knowledge of all chemical composition or chemical properties of substances. This course aims to introduce students to the many types of basic theoretical concepts, general problem-solving strategies, technology (chemical, instrumental, and statistical), and communication requirements associated with the ubiquitous problems of agricultural and environmental analysis. The business of the analyst is not only a matter of experts knowing what to do with samples brought to them for investigation, but, just as importantly, it involves communication - accurate statements of the problem requiring analysis, as well as accurate reports of the results of the analysis work. Therefore, the objective of this course is to help each student learn something new about analytical chemistry and equip him/her with knowledge that they can apply this knowledge in their own future’s fields.

As a matter of fact, as agrarians, we all need and use analytical principles and techniques, and I hope that the students do not use them blindly. It is my goal that each student finishes this course with a better understanding of how analytical basics and tools that will be applied in their concern specification and what are their limitations.

The following objectives and skills are targeted:

(1) To provide a thorough background in those chemical principle that are particularly important to analytical chemistry

(2) To introduce basic techniques that is useful in modern analytical chemistry.

(3) Understanding of the principles of analytical methods, expression units and results outline.

(4) Rigorous analytical interpretation and statistical analysis of data.

(5) Improvement of scientific communication skills

4-Course contents and syllabus:

Outline and schedule of the topics

5- Course Grading:

The grade in this course is similar to others courses and will be based on the student performance on 3 examinations (2 monthly exams and the final). The lecture portion will constitute 80% of the final grade and the laboratory 20% of the final grade. Sometime quizzes will also cover theoretical material presented in lecture and studied through

homework problems.

The hundredth grading scale for this class is as follows:

6- Cheating:

According to University policy and regulations, there is zero tolerance for cheating in any of student's test or examination. If you are caught cheating in any way, you will fail the course. In addition, any student caught cheating will be subject to disciplinary action that could result in expulsion from the faculty. Plagiarism of another student’s work or from any other source, talking during an exam, looking at another student’s work during an exam, using a calculator as a memory device, opening a book, using notes, or changing an answer on an exam once it’s been returned are some examples of cheating. In these cases, the student will be immediately dismissed from the room and given a zero score, because it may be assumed that he/she intended to use such materials unlawfully, and he/she may be penalized accordingly. Such behavior will result in disciplinary sanctions resulting in suspension, dismissal or expulsion from the University.

Copying pre-lab, lab write-up, or post-lab answers from other students is also cheating and will not be tolerated.

7- Some general policies:

No cell phones or texting in lecture or lab and it should be completely off or in silent mode. No food, drinks, or gum in lab although you can go outside to eat or drink during lab. No food in lecture although drinks are permitted. During lecture, remain in your seats for the duration. No earphones in either lecture or lab. Don't hurt yourself or others by doing something stupid. Let’s say you are doing a lab that you use highly toxic and flammable chemicals and if misused could kill you. Regular class attendance should be kept. A student who persists in being absent from class will be reported to the student’s affairs section. If you miss an exam because of illness or other extenuating circumstance (travel for family matters is not considered to be an emergency circumstance), you must contact the instructor to discuss your situation prior to the absence.

While the laboratory is generally a safe place to explore chemical principles and phenomena, there are things (equipment, reagents, etc.) that can cause injury when misused. For this reason, it is important to be fully alert and focused when in the laboratory. If you attend lab and you fail to follow general laboratory safety practices and procedures, disregard the written and/or verbal instructions associated with the lab, or are otherwise perceived to be a risk to you or others, you will be asked to leave the lab and may receive a zero for the day.”

8- References or Texts (Please find below some images of books cover)

1- Skoog, D. A., West, D. M., Holler, F. J., and Crouch, S. R. (2004). Fundamentals of Analytical Chemistry. Eighth Edition. Thomson-Brooks/Cole. Australia. Canada. Mexico. Singapore. Spain. United Kingdom. United States.

2- Harris, D. C. (2005). Exploring Chemical Analysis. Third edition. W.H. Freeman & Company. New York.

3- Higson, S. P. J. (2004). Analytical chemistry. Oxford University Press.

9-Samples of the exam and questions

University of Sulaimani Time: 3 Hours

Faculty of Agricultural Sciences Subject: Analytical Chemistry Exam

________________________________________________________________________

Answer only (4) questions:

Q1-A/ Define only (5) of the following.

Precipitating agent; Oxidant; Disproportionation; End point; Titration error;

Stoichiometric calculations;

B/ If 5.585-g of Fe⁺³was reduced to Fe⁺²in the reaction:

Fe⁺³+ V^{+2 _____________________} Fe⁺²+ V⁺³

How many coulombs (C) of charge must have been transferred from V⁺² to Fe⁺³.

(Faraday constant -F) = 9.649 x 10⁴C/mole and A. wt. of Fe = 55.85 g/mole).

Q2-A/ How many milliliters (mL) of 0.5 M NaOH should be added to 10 g of tris

hydrochloride (BH⁺) to give a pH of 7.6 in final volume of 250 mL. ( PKa of tris

hydrochloride (BH⁺) = 8.07 and its M.wt = 157.6 g/mol).

B/ Write the most important steps of the chemical analysis.

Q3-A/ If the solubility product constant (Ksp) of PbI₂ = 1.5 x 10^-9and the molar mass

(M. wt. = 461 g/mol).

The solubility reaction is: PbI₂ __________ Pb⁺² + 2 I^-.

Calculate:

1-The molar solubility of the ion product species of Pb⁺²and I^-.

2-How many grams of PbI₂ can be dissolved in 2 Liter of water?

B/ Write the basic requirements of primary standard substance.

Q4-A/ Balance the following redox reaction and indicate the oxidant and reductant

substances.

H₂O₂ + MnO₄^–1 ____________ Mn⁺² + O_2(g)

B/ An acid –base indicator (HIn) with dissociation constant (Ka) of 1 x 10^—5.

Find the pH range that shows a complete color change.

Q5-A/ A 0.1278-g sample of primary standard oxalic acid H₂C₂O₄ required 33.31 ml

of the permanganate solution (KMnO₄) to reach the end point. Calculate the

molarities of the (KMnO₄).

(M. wt. of H₂C₂O₄= 90 g/mol). The chemical reaction s:

2 MnO₄^—1 + 5 H₂C₂O₄ + 6H⁺ ____ 2Mn⁺² + 10 CO₂ + 8H₂O

B: Distinguish between: 1- The equivalence point and end point 2- Normality and

Molarity 3- Iodometry and iodimetry.

All the best for you

University of Sulaimani Time: 3:00 hours

Faculty of Agricultural Sciences Subject: Analytical chemistry

Q1 / Complete the following by filling in the blank spaces with the correct expression given:

Monodenate ; Volumetric analysis ; Common ion effect ;

Equilibrium Molarity ; Titration ; Ksp ; precipitate ; Electrolyte ;

Titration error.

Q 2 – A / If the concentration of H⁺in a solution is 1.0 × 10^-3M (kW = 1.0 × 10^-14).

Calculate: The molar concentration of OH ^-.

The pH and pOH of this solution.
What is the type of this solution (Acidic, Basic or medium)?

B / what is the pH of a buffer solution prepared by dissolving 12.43 g of a weak bases B

(121.14 g /mol) plus 4.67 g of its conjugate acid BH⁺ (157.6 g / mol) and pka= 8.07 in

1.0 L of water.

Q 3 / from the following stoichiometric chemical equation:

2 AgNO_{3 (aq) +}1 Na₂CO_{3 (aq)} 1Ag₂ CO_{3(s) +} 2NaNO₃

Calculate :

What mass of AgNO₃ in grams (169.87 g / mol) is needed to convert 100ml.of 0.4 M Na₂CO₃ (106.0 g / mol) to Ag₂CO₃ (275.7 g /mol).

2. What mass of Ag₂CO₃ (275.7 g /mol) in grams will be formed from AgNO₃ (169.87 g / mol).

Q 4 – A / Write the main uses of complexation reactions in analytical chemistry.

B / A 25ml. solution containing Ni⁺² ion (nickel ion) was titrated with 50 ml. of 0.05 M

Na₂ – EDTA (Y^-4). Then the excess Na₂ – EDTA was back titrated with 20 ml. of 0.05 M

Zn⁺² ions (zinc solution) calculate:

1. The number of millmoles of Zn⁺² and excess of Na₂ – EDTA in the solution.

2. The equivalence volume of Na₂ – EDTA with Ni⁺²in milliliter.

3. The molarity of Ni⁺² ion solution.

4. Write the chemical equation and the formation constant for the titration reactions.

All the best for you

Atmospheric chemistry and air pollution course book for the academic year 2015-2016

Fourth year students (senior class)

Second (spring) Semester

Name of the Lecturer: Dr. Salih N. Majid

Contents

1- Course coordinator and list of lecturer on this course.

2- Course overview

3- Course objectives.

4- Course contents and syllabus

5- Course grading

6- Cheating

7- Some general policies

8- References or Texts (Required Materials)

9- Samples of the exam and questions

1- Course coordinator and list of instructors on this course:

Ø Course coordinator: Mahtab Hama Salih

E-mail Address of the Course Coordinator: mahtab-78@hotmail.com

Mobile No. 07715001203

Ø Lecturers on this course.

1- Dr. Salih N. Majid: (Lecturer)

E-mail: salih.majeed@univsul.edu.iq; salihnm@yahoo.de.

Mobile No.: 07701589206

2- Bzhwen Khalid Majeed

E-mail: bzhwen.majeed@univsul.edu.iq

Mobile No.: 07705021187

2-Course overview:

Atmospheric Chemistry provides students with a basic knowledge of the chemistry of Earth's atmosphere, and an understanding of the role that chemical transformations play in this vital part of our environment. The composition of the 'natural' atmosphere (troposphere, stratosphere and mesosphere) is described in terms of the physical and chemical cycles.

Therefore, dealing with the composition and chemistry of natural and pollutant compounds in the atmosphere; transport, cycling and reactivity of atmospheric material; atmospheric measurements, air quality and human health issues; air pollution trends and climate change are the most important topics of this course.

On the hand, the formation of air pollution is an important scientific problem that must be understood to ultimately protect human health, since air pollution has significant effects on human health and the environment, through interrelated problems of ozone and particulate matter air pollution, acid rain, visibility degradation, mercury, stratospheric ozone depletion, and climate change. Air pollution is formed through the interaction of hundreds of nonlinear chemical reactions involving thousands of different chemical species.

In current time, scientists turn to computer models to simulate this complex chemistry. In turn, they use these models to make policy aimed at improving air quality.

3-Course objectives:

Atmospheric chemistry is one of the fastest growing fields in the earth sciences. This course is intended to provide students with the knowledge for understanding the atmospheric Chemistry and the phenomena of atmospheric pollution. The course covers the atmospheric chemistry of air pollutants, the sources as well as the fate and transport of air pollutants, the legislative framework for air pollution control, the techniques for air pollution monitoring, risk assessment of air pollution effects, and air pollution control strategies.

Course Objectives:

Through this course, the student will be able:

1) To explain the structure (layers) and composition of atmosphere

2) To determine the properties of atmospheric gases and aerosols.

3) To explain the atmospheric ozone formation via photochemical reactions of NO_x and VOC in the ambient.

4) To explore the chemistry, physics, and dynamics of natural and anthropogenic impacts to the atmosphere.

5) To learn regulation and policies on air pollution and their effectiveness.

6) To develop an understanding of air pollution data management, analysis, and quality assurance and control.

7) To describe the air pollution monitoring instruments

8) To explain the atmospheric, health and welfare effects of air pollution.

9) To describe the principles of gaseous and particulate monitoring systems

Major Topics

Introduction
Fundamental Laws of Gases and Particles
Atmospheric Composition and Structure
Gas Phase Pollutants
Gas phase Pollutant: Ozone formation
Particulate Pollutants
Kinetics and Equilibrium Constant
Atmospheric Effects
Health Effects
Energy Sources and Combustion
Air Monitoring
Atmospheric Motion
Atmospheric Dispersion, Transport, and Deposition
Air Quality Modeling
Air Regulation
Welfare Effects

4-Course contents and syllabus ( Course outline):

Outline and schedule of the topics

Course syllabus

5- Course Grading:

The grade in this course is similar to others courses and will be based on the student performance on 3 examinations (2 monthly exams and the final). The lecture portion will constitute 80% of the final grade and the laboratory 20% of the final grade. Sometime quizzes will also cover theoretical material presented in lecture and studied through

homework problems.

The hundredth grading scale for this class is as follows:

6- Cheating:

According to University policy and regulations, there is zero tolerance for cheating in any of student's test or examination. If you are caught cheating in any way, you will fail the course. In addition, any student caught cheating will be subject to disciplinary action that could result in expulsion from the faculty. Plagiarism of another student’s work or from any other source, talking during an exam, looking at another student’s work during an exam, using a calculator as a memory device, opening a book, using notes, or changing an answer on an exam once it’s been returned are some examples of cheating. In these cases, the student will be immediately dismissed from the room and given a zero score, because it may be assumed that he/she intended to use such materials unlawfully, and he/she may be penalized accordingly. Such behavior will result in disciplinary sanctions resulting in suspension, dismissal or expulsion from the University.

Copying pre-lab, lab write-up, or post-lab answers from other students is also cheating and will not be tolerated.

7- Some general policies:

No cell phones or texting in lecture or lab. No food, drinks, or gum in lab although you can go outside to eat or drink during lab. No food in lecture although drinks are permitted. During lecture, remain in your seats for the duration. No earphones in either lecture or lab. Don't hurt yourself or others by doing something stupid. Let’s say you are doing a lab that you use highly toxic and flammable chemicals and if misused could kill you. Regular class attendance should be kept. A student who persists in being absent from class will be reported to the student’s affairs section. If you miss an exam because of illness or other extenuating circumstance (travel for family matters is not considered to be an emergency circumstance), you must contact the instructor to discuss your situation prior to the absence.

While the laboratory is generally a safe place to explore chemical principles and phenomena, there are things (equipment, reagents, etc.) that can cause injury when misused. For this reason, it is important to be fully alert and focused when in the laboratory. If you attend lab and you fail to follow general laboratory safety practices and procedures, disregard the written and/or verbal instructions associated with the lab, or are otherwise perceived to be a risk to you or others, you will be asked to leave the lab and may receive a zero for the day.”

8- References or Textsbooks (Please find below some images of books cover)

1. Atmospheric Chemistry by Ann Holloway and Richard Wayne.

2. Chemistry of Atmospheres: An Introduction to the Chemistry of the Atmospheres of Earth, the Planets, and their Satellites by Richard Wayne.

3. Air Composition and Chemistry by Peter Brimblecombe.

4. Air Pollution and Global Warming: History, Science, and Solutions by Mark Jacobson.

5. Introduction to Atmospheric Chemistry by Daniel Jacob.

6. Atmospheric Chemistry: Fundamentals and Experimental Techniques by Barbara Finlayson-Pitts and James Pitts.

7. Atmospheric Chemistry and Physics by John Seinfeld and Spyros Pandis.

8. Chemistry of the Upper and Lower Atmosphere: Theory, Experiments, and Applications by James N. Pitts, Jr; Barbara J. and Finlayson-Pitts.

9. Fundamentals of Air Pollution, Fifth Edition (2014) by Daniel Vallero.

10. Air Pollution: Measurement, Modelling and Mitigation, Third Edition (2009) by Jeremy Colls and Abhishek Tiwary.

11. Air Pollution (Global Viewpoints) Library Binding (2011) by Margaret Haerens.

12. Air Pollution Control Engineering (2010) by Noel de Nevers.

13. Air Pollution: Its Origin and Control” 3rd edition by Kenneth Wark, Cecil F.Warner and Wayne T. Davis. Addison-Wesley, 1998.

14. Environmental Policy and Public Health: Air Pollution, Global Climate Change (2011) by William N. Rom.

15. Air Pollution and Health by: Stephen T. Holgate, Jonathan M. Samet, Hillel S. Koren and Robert L. Maynard.

9- Samples of the exam and questions

University of Sulaimani Subject: Atmospheric chemistry and air pollution Faculty of Agricultural Sciences Time: 3 hours

Dept. of Soil and Water Sciences

Q.1A/ Define any (5) the following items: (7.5 Marks)

Soot; Armstrong line; Smog; particulate matter (PM); Ionosphere; Hazes.

Q.1B/ Name five (5) biogenic hydrocarbon that could be released into the atmosphere from the

plants. (2.5 Marks)

Q.2 A/ Earth's atmosphere is divided into many layers. Describe the characteristics of each layer in the

atmosphere (7.0 Marks)

Q.2 B/ What are the principal measures (units) of atmospheric composition. (3.0 Marks)

Q.3A/ Calculate the number densities of air and SO₂ at sea level for P = 1.013 x 10⁵ Pa, T = 273 K . If

the mixing ratio of SO₂ = 139 ppbv.

(Note: Avogadro's Number (Av) = 6.023 x10²³; Gas constant ( R) = 8.314 J mol^-1 K^-1;

and 1ppbv = 1x10^-9 mol/mol). (5.0 Marks)

Q.3B/ Determine the concentration in μg m^{- 3}for O₃ corresponding to a mixing ratio of 120 ppb at

p = 1 atm and T = 298 K. (Note: molar mass of O₃ = 48g/mol; 1 atm= 1.013 x 10⁵ Pa; Gas

constant ( R) = 8.314 J mol^-1 K^-1 and 1 ppbv = 1x10^-3 ppm). (5.0 Marks)

Q.4/ Summarize the changes in soil with change in climate as a table up to the timescale of 100 (10²)

year. The changes in soil should include (soil parameter; properties and characteristics; horizons

and phases; and regimes. (10.0 Marks)

Q.5A/ Tropospheric ozone (ground ozone) cuts plant growth and causes many detrimental effects for

plants. Write the most ozone’s effects on plant growth. (5.0 Marks)

Q.5B/ Express the most chemical reaction steps for the tropospheric ozone formation. (5.0 Marks)

All the best for you