Course: General Chemistry I

General

An- Najah National University

Faculty of Science

Chemistry Department

course name : General Chemistry (I)

Course number :23101

Instructor(s):Dr. Ahmad A. Abu-Obaid

Compulsory / Elective: Compulsory

________________________________________________

Course Contents (description):

This course is designed to give students a working knowledge of the most important chemical principles as the foundation for study of more advanced topics such as chemical analysis, applied chemistry, inorganic and organic chemistry

Course Objectives

To introduce basic chemical concepts and calculations, relate atomic structure to chemical systems, calculate the amount of material used in chemical reactions, use the periodic table as an aid to understanding chemical systems and interpret chemical reactions.

Intended learning Outcomes and Competences At the end of this course

Students should be able to:

Describe matter and its measurement, including calculations done on measurements.

Demonstrate an understanding of basic chemical nomenclature.

Explain concepts of basic atomic theory and relate the theory to the periodic table.

Write chemical reactions and solve problems involving chemical stoichiometry.

Describe the nature of aqueous solutions and reactions occurring in aqueous solution.

To apply the Ideal Gas Law equation, Avogadro’s Law and Dalton’s Law.

Apply concepts of thermochemistry to physical and chemical changes.

Describe the electronic structure of atoms and relate the electronic structure to atomic properties.

Demonstrate an understanding of chemical bonding and its application to molecular structure.

TextBook:

Chemistry ,Ninth Edition, Zumdal & Zumdal

To see full course outline click here
Forum

Announcements Forum
File

101Course outline File
Quiz

First Quiz 19/04/2020
Quiz

Quiz 3-ch3,4-101
Quiz

Final 101 4+5+7 Quiz
Quiz

Final 101 8+9 Quiz

Topic 1

Topic one: Atoms, Molecules, and Ions. (Chapter 2)

Introduction:

Since ancient times humans have pondered the nature of matter. Our modern ideas of the structure of matter began to take shape in the early nineteenth century with Dalton’s atomic theory. We now know that all matter is made of atoms, molecules, and ions. All of chemistry is concerned in one way or another with these species.

Objectives:

Study the historical perspective of the search for the fundamental units of matter. The modern version of atomic theory was laid by John Dalton in the nineteenth century. (2.1)

Conclude that, through experimentation, scientists have learned that an atom is composed of three elementary particles: proton, electron, and neutron. (2.2)

Learn the following ways to identify atoms. Atomic number is the number of protons in a nucleus; atoms of different elements have different atomic numbers. (2.3)

Understand how elements can be grouped together according to their chemical and physical properties in a chart called the periodic table. (2.4)

Learn how the atoms of most elements interact to form compounds, which are classified as molecules or ionic compounds made of positive (cations) and negative (anions) ions. (2.5)

Use chemical formulas (molecular and empirical) to represent molecules and ionic compounds and models to represent molecules. (2.6)

Learn a set of rules that help you to name the inorganic compounds. (2.7)

Explore the organic world to which we will return in a later chapter. (2.8)

Plan :

First :Study the following presentation .
File

Zumdahl9e PPT Ch02 File
المحاضرات المصورة للمساق
URL

https://lectures.najah.edu/ar/course/general-chemistry-1/ URL
File

ch5-lectures File

Topic 2

Topic Tow :Mass Relationships in Chemical Reactions (Chapter 3)

Introduction:

In this chapter we will consider the masses of atoms and molecules and what happens to them when chemical changes occur. Our guide for this discussion will be the law of conservation of mass.

Objectives:

Study the mass of an atom, which is based on the carbon-12 isotope scale to work with the more convenient scale of grams, we use the molar mass. (3.1 and 3.2)

Discuss the atomic mass and then the molecular mass. (3.3 and 3.4)

Expand your knowledge of molecules and ionic compounds, then learn how to calculate the percent composition of these species from their chemical formulas. (3.5)

Understand how the empirical and molecular formulas of a compound are determined by experiment. (3.6)

Learn how to write a chemical equation to describe the outcome of a chemical reaction. (3.7)

Proceed to study the mass relationships of chemical reactions. A chemical equation enables you to use the mole method to predict the amount of product(s) formed. (3.8 and 3.9)

Learn that the actual yield of a reaction is almost always less than that predicted from the equation (theoretical yield) because of various complications. (3.10)

Plan:

First:Study the following presentaion
File

Zumdahl9e PPT Ch03 File

Topic 3

Topic Three :Reactions in Aqueous Solutions (Chapter 4)

Introduction:

Many chemical reactions and virtually all biological processes take place in water. In this chapter, we will discuss three major categories of reactions that occur in aqueous solutions: precipitation reactions, acid-base reactions, and redox reactions. In later chapters, we will study the structural characteristics and properties of water—the so-called universal solvent— and its solutions.

Obiectives:

Study the properties of solutions prepared by dissolving substances in water, called aqueous solutions. (4.1)

Understand that precipitation reactions are those in which the product is an insoluble compound. Learn to represent these reactions using ionic equations and net ionic equations. (4.2).

Learn acid-base reactions, which involve the transfer of proton (H1) from an acid to a base. (4.3)

Learn oxidation-reduction (redox) reactions in which electrons are transferred between reactants. (4.4)

Carry out quantitative studies of solutions, learn how to express the concentration of a solution in molarity. (4.5)

Apply your knowledge of the mole method from Chapter 3 to the three types of reactions studied here. (4.6, 4.7, and 4.8)

Plan:

First:Study the following presentaion
Seventh :Solve the following assignment
File

Zumdahl9e PPT Ch04 File

Topic 4

Topic Four: Gases (Chapter 5)

Introduction:

Under certain conditions of pressure and temperature, most substances can exist in any one of three states of matter: solid, liquid, or gas. Water, for example, can be solid ice, liquid water, steam, or water vapor. The physical properties of a substance often depend on its state.

Gases, the subject of this chapter, are simpler than liquids and solids in many ways. Molecular motion in gases is totally random, and the forces of attraction between gas molecules are so small that each molecule moves freely and essentially independently of other molecules. Subjected to changes in temperature and pressure, it is easier to predict the behavior of gases. The laws that govern this behavior have played an important role in the development of the atomic theory of matter and the kinetic molecular theory of gases.

Obiectives:

Describe the substances that exist as gases and their general properties. (5.1)

Learn the units for expressing gas pressure and the characteristics of atmospheric pressure. (5.2)

Study the relationship among pressure, volume, temperature, and amount of a gas in terms of various gas laws. (5.3 and 5.4)

Impliment the ideal gas equation which can be used to study the stoichiometry involving gases. (5.5)

Learn that the behavior of a mixture of gases can be understood by Dalton’s law of Partial pressures. (5.6)

Study the kinetic molecular theory of gases, which is based on the properties of individual molecules, it can be used to describe macroscopic properties such as the pressure and the temperature of a gas. (5.7)

Study the correction for the non-ideal behavior of gases using the van der Waals equation. (5.8)

Plan:

First:Study the following presentaion
Third:For manual solution look to the following word file
File

Zumdahl9e PPT Ch05 File

Topic 5

Topic Five :Thermochemistry (Chapter six)

Introduction:

Every chemical reaction obeys two fundamental laws: the law of conservation of mass and the law of conservation of energy. We discussed the mass relationship between reactants and products in Chapter 3; here we will look at the energy changes that accompany chemical reactions.

Objectives

Study the nature and different types of energy. (6.1)

Build up your vocabulary, in order to better study thermochemistry. (6.2)

Understand that thermochemistry is part of a broader subject called the “first law of thermodynamics”. (6.3)

Acquaint yourself with a new term for energy, called “enthalpy”. (6.4)

Familiarize yourself with ways to measure the heats of reaction or calorimetry, and the meaning of specific heat and heat capacity. (6.5)

Know the standard enthalpies of formation of reactants and products. Discuss ways to determine these quantities either by the direct method from the elements or by the indirect method. (6.6)

Observe the heat changes when a solute dissolves in a solvent (heat of solution) and when a solution is diluted (heat of dilution). (6.7)

Plan:

First:Study the following presentaion
Third:For manual solution look to the following word file
File

Zumdahl9e PPT Ch06 File

Topic 6

Topic Six :Quantum Theory and the Electronic Structure of Atoms (chapter Seven)

Introduction:

Quantum theory enables us to predict and understand the critical role that electrons play in chemistry. In one sense, studying atoms amounts to asking the following questions:

How many electrons are present in a particular atom?

What energies do individual electrons possess?

Where in the atom can electrons be found?

Objectives

Discuss the transition from classical physics to quantum theory. (7.1)

Explain experimental observations, such as light behaving like a bundle of particles called photons. (7.2)

State Bohr’s theory for the emission spectrum of the hydrogen atom. (7.3)

Recognize that electrons can behave like waves (suggested by de Broglie). (7.4)

Relate the Heisenberg uncertainty principle with the Schrödinger wave equation which describes the behavior of electrons in atoms and molecules. (7.5)

Interpret that there are four quantum numbers to describe an electron in an atom. (7.6 and 7.7)

Assess magnetic properties and the properties of electronic configuration. (7.8)

Apply the rules in writing electron configurations to the entire periodic table. (7.9)

Plan:

First:Study the following presentaion
Second:To understand Electronic Structure of Atoms watch the following video
Third:For manual solution look to the following word file
File

Zumdahl9e PPT Ch07 File

Topic 7

Topic seven: Periodic Relationships Among the Elements(chapter eight)

Introduction:

Many of the chemical properties of the elements can be understood in terms of their electron configurations. Because electrons fill atomic orbitals in a fairly regular fashion, it is not surprising that elements with similar electron configurations, such as sodium and potassium, behave similarly in many respects and that, in general, the properties of the elements exhibit observable trends. Chemists in the nineteenth century recognized periodic trends in the physical and chemical properties of the elements, long before quantum theory came onto the scene. Although these chemists were not aware of the existence of electrons and protons, their efforts to systematize the chemistry of the elements were remarkably successful. Their main sources of information were the atomic masses of the elements and other known physical and chemical properties.

Objectives:

Recall the development of the periodic table and the contributions made by nineteenth-century scientists, in particular by Mendeleev. (8.1)

State the rules for writing the electron configurations of cations and anions. (8.2)

Examine the periodic trends in physical properties such as the size of atoms and ions in terms of effective nuclear charge. (8.3)

Explore chemical properties like ionization energy and electron affinity. (8.4 and 8.5)

Reproduce the knowledge acquired in the chapter to systematically study the properties of the representative elements as individual groups and also across a given period. (8.6)

Plan:

First:Study the following presentaion
Second:For manual solution look to the following word file
File

Zumdahl9e PPT Ch08 File

Topic 8

Topic Eight:Chemical Bonding I:Basic Concepts (chapter nine)

Introduction:

Why do atoms of different elements react? What are the forces that hold atoms together in molecules and ions in ionic compounds? What shapes do they assume? These are some of the questions addressed in this chapter and in Chapter 10. We begin by looking at the two types of bonds—ionic and covalent—and the forces that stabilize them.

Objectives

Recognize Lewis dot symbols, which shows the valence electrons on an atom. (9.1)

Express the formation of ionic bonds and learn how to determine lattice energy. (9.2 and 9.3)

Learn how to write Lewis structures, which are governed by the octet rule. (9.4)

Understand that electronegativity is an important concept in understanding the properties of molecules. (9.5)

Learn to use formal charges to study the distribution of electrons in these species. (9.6 and 9.7)

Identify that there are exceptions to the octet rule. (9.8 and 9.9)

Examine the strength of covalent bonds, which leads to the use of bond enthalpies to determine the enthalpy of a reaction. (9.10)

Plan:

First:Study the following presentaion
File

Zumdahl9e PPT Ch09 File

Topic 9

Topic Nine:Chemical Bonding II:Molecular Geometry and Hybridization of Atomic Orbitals(chapter ten)

Introduction:

In Chapter 9, we discussed bonding in terms of the Lewis theory. Here we will study the shape, or geometry, of molecules. Geometry has an important influence on the physical and chemical properties of molecules, such as density, melting point, boiling point, and reactivity. We will see that we can predict the shapes of molecules with considerable accuracy using a simple method based on Lewis structures. The Lewis theory of chemical bonding, although useful and easy to apply, does not explain how and why bonds form. A proper understanding of bonding comes from quantum mechanics. Therefore, in the second part of the chapter we will apply quantum mechanics to the study of the geometry and stability of molecules.

Objectives

Restate the role of chemical bonds and lone pairs on the geometry of a molecule in terms of a simple approach called the VSEPR model. (10.1)

Express the factors that determine whether a molecule possesses a dipole moment. (10.2)

Apply a quantum mechanical approach, called the valence bond (VB) theory, in the study of chemical bonds. (10.3)

Report that the VB approach accounts for both chemical bond formation and molecular geometry. (10.4 and 10.5)

Deduce that the MO theory considers the formation of molecular orbitals as a result of the overlap of atomic orbitals, and is able to explain the paramagnetism of the oxygen molecule. (10.6)

We can learn about the strength of a bond as well as general magnetic properties from the molecular orbital configurations (Pauli’s exclusion principle and Hund’s rule). (10.7)

The concept of molecular orbital formation is extended to delocalized molecular orbitals, which cover three or more atoms. We see that these delocalized orbitals impart extra stability to molecules like benzene. (10.8)

Plan:

First:Study the following presentaion
File

Zumdahl9e PPT Ch10 File

Topic outline

General

An- Najah National University

Faculty of Science

Chemistry Department

course name : General Chemistry (I)

Course number :23101

Instructor(s):Dr. Ahmad A. Abu-Obaid

Compulsory / Elective: Compulsory

Course Contents (description):

This course is designed to give students a working knowledge of the most important chemical principles as the foundation for study of more advanced topics such as chemical analysis, applied chemistry, inorganic and organic chemistry

Course Objectives

To introduce basic chemical concepts and calculations, relate atomic structure to chemical systems, calculate the amount of material used in chemical reactions, use the periodic table as an aid to understanding chemical systems and interpret chemical reactions.

Intended learning Outcomes and Competences At the end of this course

Describe matter and its measurement, including calculations done on measurements.

Demonstrate an understanding of basic chemical nomenclature.

Explain concepts of basic atomic theory and relate the theory to the periodic table.

Write chemical reactions and solve problems involving chemical stoichiometry.

Describe the nature of aqueous solutions and reactions occurring in aqueous solution.

To apply the Ideal Gas Law equation, Avogadro’s Law and Dalton’s Law.

Apply concepts of thermochemistry to physical and chemical changes.

Describe the electronic structure of atoms and relate the electronic structure to atomic properties.

Demonstrate an understanding of chemical bonding and its application to molecular structure.

TextBook:

Chemistry ,Ninth Edition, Zumdal & Zumdal

To see full course outline click here

Topic 1

Topic one: Atoms, Molecules, and Ions. (Chapter 2)

Introduction:

Objectives:

Study the historical perspective of the search for the fundamental units of matter. The modern version of atomic theory was laid by John Dalton in the nineteenth century. (2.1)

Conclude that, through experimentation, scientists have learned that an atom is composed of three elementary particles: proton, electron, and neutron. (2.2)

Learn the following ways to identify atoms. Atomic number is the number of protons in a nucleus; atoms of different elements have different atomic numbers. (2.3)

Understand how elements can be grouped together according to their chemical and physical properties in a chart called the periodic table. (2.4)

Learn how the atoms of most elements interact to form compounds, which are classified as molecules or ionic compounds made of positive (cations) and negative (anions) ions. (2.5)

Use chemical formulas (molecular and empirical) to represent molecules and ionic compounds and models to represent molecules. (2.6)

Learn a set of rules that help you to name the inorganic compounds. (2.7)

Explore the organic world to which we will return in a later chapter. (2.8)

First :Study the following presentation .

المحاضرات المصورة للمساق

Topic 2

Topic Tow :Mass Relationships in Chemical Reactions (Chapter 3)

Introduction:

In this chapter we will consider the masses of atoms and molecules and what happens to them when chemical changes occur. Our guide for this discussion will be the law of conservation of mass.

Objectives:

Study the mass of an atom, which is based on the carbon-12 isotope scale to work with the more convenient scale of grams, we use the molar mass. (3.1 and 3.2)

Discuss the atomic mass and then the molecular mass. (3.3 and 3.4)

Expand your knowledge of molecules and ionic compounds, then learn how to calculate the percent composition of these species from their chemical formulas. (3.5)

Understand how the empirical and molecular formulas of a compound are determined by experiment. (3.6)

Learn how to write a chemical equation to describe the outcome of a chemical reaction. (3.7)

Proceed to study the mass relationships of chemical reactions. A chemical equation enables you to use the mole method to predict the amount of product(s) formed. (3.8 and 3.9)

Learn that the actual yield of a reaction is almost always less than that predicted from the equation (theoretical yield) because of various complications. (3.10)

Plan:

First:Study the following presentaion

Topic 3

Topic Three :Reactions in Aqueous Solutions (Chapter 4)

Introduction:

Obiectives:

Study the properties of solutions prepared by dissolving substances in water, called aqueous solutions. (4.1)

Understand that precipitation reactions are those in which the product is an insoluble compound. Learn to represent these reactions using ionic equations and net ionic equations. (4.2).

Learn acid-base reactions, which involve the transfer of proton (H1) from an acid to a base. (4.3)

Learn oxidation-reduction (redox) reactions in which electrons are transferred between reactants. (4.4)

Carry out quantitative studies of solutions, learn how to express the concentration of a solution in molarity. (4.5)

Apply your knowledge of the mole method from Chapter 3 to the three types of reactions studied here. (4.6, 4.7, and 4.8)

Plan:

First:Study the following presentaion

Seventh :Solve the following assignment

Topic 4

Topic Four: Gases (Chapter 5)

Introduction:

Under certain conditions of pressure and temperature, most substances can exist in any one of three states of matter: solid, liquid, or gas. Water, for example, can be solid ice, liquid water, steam, or water vapor. The physical properties of a substance often depend on its state.

Obiectives:

Describe the substances that exist as gases and their general properties. (5.1)

Learn the units for expressing gas pressure and the characteristics of atmospheric pressure. (5.2)

Study the relationship among pressure, volume, temperature, and amount of a gas in terms of various gas laws. (5.3 and 5.4)

Impliment the ideal gas equation which can be used to study the stoichiometry involving gases. (5.5)

Learn that the behavior of a mixture of gases can be understood by Dalton’s law of Partial pressures. (5.6)

Study the kinetic molecular theory of gases, which is based on the properties of individual molecules, it can be used to describe macroscopic properties such as the pressure and the temperature of a gas. (5.7)

Study the correction for the non-ideal behavior of gases using the van der Waals equation. (5.8)

Plan: