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Course: Become A Chemistry 1 Master - Basic Principles Of Chemistry

Become A Chemistry 1 Master - Basic Principles Of Chemistry

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  • Self-Paced
About this Course

Hi!!!

Are you one of the high school students: Chemist student, Pharmacy student, biology student, Nursing student or Engineering student and you have problems in studying General Chemistry 101???

Do you Like Chemistry but you don’t know how to study the basics in Chemistry???

Are you suffering from understanding the basics of Chemistry which makes the General Chemistry Exam as a nightmare for you???

Do you want to be a master in Chemistry and pass the Chemistry exam getting a high score easily???

Whatever the reason you have for thinking about studying chemistry , Whether you were Chemistry student, Pharmacy student, Biology student, Nursing student or Engineering student, this course will help you to understand the essential basics of Chemistry.

This course will help you in covering everything you will need to know as you prepare for possible future exams. It doesn't matter how much, or how little, prior knowledge of Chemistry you've got as this course will take you through all the necessary stages.

Have a look at some awesome reviews about this course!!!

★★★★★ "This is an awesome course in General Chemistry 1, the explanation are very easy to be understood, the examples in this course helped me to understand the Chemistry 1 completely." - Amin

★★★★★ "I have learned more in this course than I did in school" - Jari -chan

★★★★★ "EXCELLENT CONTENT - simple and easy to be understood !!!!" - Mstluchy

★★★★★ "This course is a mini introduction to 101 Chemistry, it serves to build further interest in the subject. I found it engaging; however, it left me wanting more, which is good. It drives home the fact that chemistry in integrated into all aspects of our daily lives and existence, so there is nothing to fear. After all, cooking is in fact chemistry, most of us do this experiment on a daily basis." - DL Lieberman 

★★★★★ "very easy to understand..." - Mohammed demachkie 

★★★★★ "The course is really informative and it has help me lot." - Mr. SHEIKH SAJJAD SHEIKH 

★★★★★ "Great chemistry course!" - Matt F.

★★★★★ "Very detailed and well thought out explanations. Covers each concept very well and in simple steps.!" - MacSabu.

★★★★★ "This is the best Course in chemistry I have watched !!!!!!" - Tanjib.

★★★★★ "I am a popular science fan with a background in Chemistry. I needed this course to be able to understand the terminology of chemistry and its applications in daily life.!" - Noyon.

★★★★★ "Great and full experienced instructor....!" - Sssujon.

★★★★★ "Well organized and easy explanation , I liked this course....!" - Zihad.

If You just love chemistry!!!! OR Whatever the reason you have for thinking about studying Chemistry further, ENROLL in this course to help you learn and understand the Chemistry basics very easily.

Hey!!!

Am Mohammad Abualrub, I have PhD in Chemistry and am Expert in pharmaceutical Industry - +8Years & Expert in teaching Chemistry +4Years.

In this Course we will cover the following topics:

Section 1 - Matter and Measurement

  • An Introduction To Chemistry
  • Methods Of Science
  • Categories Of Science
  • Steps Of Scientific Method
  • Theory And Law
  • The Scientific Method
  • Law of Conservation of Mass
  • Matter, Element And Compound
  • Types Of Mixtures
  • The Three States Of matter
  • Properties And Changes Of matter
  • Units Of Measurements
  • Scientific Notations
  • Significant Figures
  • Accuracy And Precession
  • Units and Dimensional Analysis

Section 2 - Atoms, Molecules, and Ions

  • Dalton’s Atomic Theory
  • Atomic Symbols and Models
  • Law of Conservation of Mass
  • Law of multiple proportions
  • The Structure of The Atom
  • Discovery of the Electron
  • The nuclear model of the atom
  • Atomic Mass, Mass Number and Isotopes
  • Mass number and Atomic Masse
  • Periodic Table of the Elements
  • Metals, Nonmetals, and Metalloids
  • Molecular Substances
  • Ionic Substances
  • Organic Compounds
  • Ionic Compounds
  • Rules for predicting Charges
  • Naming of Ionic Compounds
  • Formula of Ionic Compounds
  • Naming of Binary Molecular Compounds
  • Acids and Corresponding Anions
  • Naming of Hydrates
  • Writing Chemical Equations
  • Balancing Chemical Equations

Section 3 - Calculations With Chemical Formulas And Equations

  • Introduction to Calculations in Chemistry
  • Mass and Moles of Substance
  • Molecular Mass and Formula Mass
  • The Mole Concept
  • Mole Calculations
  • Determining Chemical Formulas
  • Elemental Analysis, Percentage of C, H and O
  • Determining Formulas
  • Molecular Formula from Empirical Formula
  • Stoichiometry: Quantitative Relations in Chemical Reactions
  • Limiting Reactant
  • Theoretical Yield

Section 4 – Chemical Reactions

  • Introduction to Chemical Reactions
  • Ionic Theory of Solutions and Solubility Rules
  • Electrolytes and Non-electrolytes
  • Solubility Rules
  • Molecular and Ionic Equations
  • Acid Base, Neutralization and Oxidation-Reduction Reactions
  • Oxidation number
  • Types of Oxidation-Reduction Reactions
  • Working with solutions
  • Quantitative Analysis

Section 5 – Gaseous State

  • Introduction to the Gaseous State
  • Gas Pressure and Its Measurement
  • Boyle’s Law: Relating Volume and Pressure
  • Charles’s Law: Relating Volume and Temperature
  • Gay-Lussac’s Law : Relating Pressure and Temperature
  • Combined Gas Law : Relating Pressure, Temperature and Volume
  • Avogadro’s Law: Relating Volume and Amount
  • The Ideal Gas Law
  • Standard Temperature and Pressure (STP)
  • Gas Density; Molecular-Mass Determination
  • Gas Stoichiometry
  • Gas Mixtures; Law of Partial Pressures
  • Real Gases

Section 6 –  Thermochemistry

  • Introduction to Thermochemistry
  • Thermodynamics
  • Thermodynamic Equations
  • Heat Capacity (C)
  • Standard Enthalpy of Formation ΔH formation

Section 7 –  Quantum Theory and the Electronic Structure of Atoms

  • Properties of Waves
  • Bohr’s Model of the Atom
  • Schrodinger Wave Equation
  • Aufbau principle and Hund's Rule 
  • Electron configuration

Section 8 –  Periodic Relationships

  • Ground State Electron Configurations and Classification of Elements
  • Electron Configurations of Cations and Anions 
  • Effective nuclear charge (Zeff)
  • The Atomic Radius
  • The Ionization Energy
  • The Electron Affinity
  • Groups Elements Properties

Section 9 –  Ionic and Covalent Bonding

  • The Ionic and Covalent Bonding
  • Electronegativity and Polar Covalent Bond
  • Writing Lewis Structures
  • Formal Charge

Section 10 –  Molecular Geometry and Chemical Bonding Theory

  • Valence shell electron pair repulsion (VSEPR) model
  • Dipole Moments and Polar Molecules
  • Valence Bond Theory
  • Hybridization

You have everything to gain and nothing to lose! I will stress this as well and stand behind this course.

Lets start success together! Click on the “take this course" link at the top right of this page right NOW! Don't let another minute go by not living your dreams.

Dr Mohammad Abualrub

PhD in Chemistry Expert in pharmaceutical Industry +8Years & Expert in teaching Chemistry +4Years.

Who this course is for:

  • This course is for High School Students, Chemists, Pharmacy student, biology student, Nursing student and Engineering student,under graduated or graduated.
  • Everyone who has a big passion with chemistry and want to discover more about it.
Basic knowledge
  • There are no essential course requirements, just a desire to learn more about Chemistry and a willingness to make the necessary effort
  • This course is very simple and no need for any techniques to be understood
What you will learn
  • Know exactly what is Matter, Element and Compound
  • Learn the scientific methods and type of Mixtures
  • Know the Three State of Maters and Units of Measurements
  • Calculate Scientific Notation and Significant Figures
  • Determine if the results you obtained are Accurate and Precise
  • Understand the Units and Dimensional Analysis
  • Understand the Atomic Theory and Models of the Atom
  • know the Law of Conservation and law of Multiple Proportions
  • Learn Atomic Mass, Mass Number and Isotopes
  • Know how elements are organized in the Periodic Table
  • Learn how to name the Ionic Compounds
  • Know how to write Chemical equations
  • Learn how to make a Chemical Balance
  • Understand The Mole Concept
  • Be able to do Mole calculations successfully
  • Learn determination of Chemical formulas
  • Understand the Stiochiometry
  • To calculate the Limiting Reactant and the Yield of the reaction
  • Study all the Solubility Rules
  • Understand the Electrolyte and Non-Electrolyte solutions
  • Know all the Types of Chemical Reactions
  • Be able to do Calculations on Molar Concentration and Dilution Analysis
  • Understand the Gravimetric Analysis and the Titration
  • Understand Boyle’s Law, Charles’s Law, Gay-Lussac’s Law, Avogadro’s Law, Combined Gas Law, The Ideal Gas Law, Real Gases, Gas Density and Gas Stoichiometry.
  • You will understand Thermochemistry the study of heat change in chemical reactions
  • You will be able to distinguish between Exothermic & Endothermic reactions
  • You will learn Enthalpy and the First Law of Thermodynamics
  • You will be able to calculate Heat Capacity (C) for any element
  • Learn how to calculate standard enthalpy of reaction (ΔH0) for any chemical reaction
  • You will understand the Properties of Waves
  • You will know how Bohr’s Model of the Atom works
  • Understand Schrodinger Wave Equation.
  • Be able to find the four quantum numbers in Schrodinger Equation
  • You will be bale to write the Electron configuration for any element
  • Understand the Ground State Electron Configurations and Classification of Elements
  • know the Electron Configurations of Cations and Anions
  • You will learn The Atomic Radius, The Ionization Energy, Effective nuclear charge (Zeff) and The Electron Affinity
  • You will be able to understand Groups Elements Properties
  • You will be able to understand the difference between ionic bond and covalent bond
  • You will understand electronegativity and formal charge
  • You will be able to write Lewis structure
  • You will understand the VSEPR theory
  • You will understand the Hybridization
Curriculum
Number of Lectures: 106
Total Duration: 06:58:15
Introduction
  • Contents of This Course - Promotional Video  

    In this Course we will cover the following topics:

    Section 1 - Matter and Measurement

    • An Introduction To Chemistry
    • Methods Of Science
    • Categories Of Science
    • Steps Of Scientific Method
    • Theory And Law
    • The Scientific Method
    • Law of Conservation of Mass
    • Matter, Element And Compound
    • Types Of Mixtures
    • The Three States Of matter
    • Properties And Changes Of matter
    • Units Of Measurements
    • Scientific Notations
    • Significant Figures
    • Accuracy And Precession
    • Units and Dimensional Analysis

    Section 2 - Atoms, Molecules, and Ions

    • Dalton’s Atomic Theory
    • Atomic Symbols and Models
    • Law of Conservation of Mass
    • Law of multiple proportions
    • The Structure of The Atom
    • Discovery of the Electron
    • The nuclear model of the atom
    • Atomic Mass, Mass Number and Isotopes
    • Mass number and Atomic Masse
    • Periodic Table of the Elements
    • Metals, Nonmetals, and Metalloids
    • Molecular Substances
    • Ionic Substances
    • Organic Compounds
    • Ionic Compounds
    • Rules for predicting Charges
    • Naming of Ionic Compounds
    • Formula of Ionic Compounds
    • Naming of Binary Molecular Compounds
    • Acids and Corresponding Anions
    • Naming of Hydrates
    • Writing Chemical Equations
    • Balancing Chemical Equations

    Section 3 - Calculations With Chemical Formulas And Equations

    • Introduction to Calculations in Chemistry
    • Mass and Moles of Substance
    • Molecular Mass and Formula Mass
    • The Mole Concept
    • Mole Calculations
    • Determining Chemical Formulas
    • Elemental Analysis, Percentage of C, H and O
    • Determining Formulas
    • Molecular Formula from Empirical Formula
    • Stoichiometry: Quantitative Relations in Chemical Reactions
    • Limiting Reactant
    • Theoretical Yield

    Section 4 – Chemical Reactions

    • Introduction to Chemical Reactions
    • Ionic Theory of Solutions and Solubility Rules
    • Electrolytes and Non-electrolytes
    • Solubility Rules
    • Molecular and Ionic Equations
    • Acid Base, Neutralization and Oxidation-Reduction Reactions
    • Oxidation number
    • Types of Oxidation-Reduction Reactions
    • Working with solutions
    • Quantitative Analysis

    Section 5 – Gaseous State

    • Introduction to the Gaseous State
    • Gas Pressure and Its Measurement
    • Boyle’s Law: Relating Volume and Pressure
    • Charles’s Law: Relating Volume and Temperature
    • Gay-Lussac’s Law : Relating Pressure and Temperature
    • Combined Gas Law : Relating Pressure, Temperature and Volume
    • Avogadro’s Law: Relating Volume and Amount
    • The Ideal Gas Law
    • Standard Temperature and Pressure (STP)
    • Gas Density; Molecular-Mass Determination
    • Gas Stoichiometry
    • Gas Mixtures; Law of Partial Pressures
    • Real Gases

    Section 6 –  Thermochemistry

    • Introduction to Thermochemistry
    • Thermodynamics
    • Thermodynamic Equations
    • Heat Capacity (C)
    • Standard Enthalpy of Formation ΔH formation

    Section 7 –  Quantum Theory and the Electronic Structure of Atoms

    • Properties of Waves
    • Bohr’s Model of the Atom
    • Schrodinger Wave Equation
    • Aufbau principle and Hund's Rule 
    • Electron configuration

    Section 8 –  Periodic Relationships

    • Ground State Electron Configurations and Classification of Elements
    • Electron Configurations of Cations and Anions 
    • Effective nuclear charge (Zeff)
    • The Atomic Radius
    • The Ionization Energy
    • The Electron Affinity
    • Groups Elements Properties

    Section 9 –  Ionic and Covalent Bonding

    • The Ionic and Covalent Bonding
    • Electronegativity and Polar Covalent Bond
    • Writing Lewis Structures
    • Formal Charge

    Section 10 –  Molecular Geometry and Chemical Bonding Theory

    • Valence shell electron pair repulsion (VSEPR) model
    • Dipole Moments and Polar Molecules
    • Valence Bond Theory
    • Hybridization
  • Welcome - About Me  

    Hi. Am Dr Mohammad Abualrub Assistant Professor in Chemistry, I have +8 years experience in the Pharmaceutical Field, currently I work in teaching in private university, I have a lot of research publications, so you will take this course from an expert.

  • Contents of The Course  

    Section 1 - Matter and Measurement

    • An Introduction To Chemistry
    • Methods Of Science
    • Categories Of Science
    • Steps Of Scientific Method
    • Theory And Law
    • The Scientific Method
    • Law of Conservation of Mass
    • Matter, Element And Compound
    • Types Of Mixtures
    • The Three States Of matter
    • Properties And Changes Of matter
    • Units Of Measurements
    • Scientific Notations
    • Significant Figures
    • Accuracy And Precession
    • Units and Dimensional Analysis

    Section 2 - Atoms, Molecules, and Ions

    • Dalton’s Atomic Theory
    • Atomic Symbols and Models
    • Law of Conservation of Mass
    • Law of multiple proportions
    • The Structure of The Atom
    • Discovery of the Electron
    • The nuclear model of the atom
    • Atomic Mass, Mass Number and Isotopes
    • Mass number and Atomic Masse
    • Periodic Table of the Elements
    • Metals, Nonmetals, and Metalloids
    • Molecular Substances
    • Ionic Substances
    • Organic Compounds
    • Ionic Compounds
    • Rules for predicting Charges
    • Naming of Ionic Compounds
    • Formula of Ionic Compounds
    • Naming of Binary Molecular Compounds
    • Acids and Corresponding Anions
    • Naming of Hydrates
    • Writing Chemical Equations
    • Balancing Chemical Equations

    Section 3 - Calculations With Chemical Formulas And Equations

    • Introduction to Calculations in Chemistry
    • Mass and Moles of Substance
    • Molecular Mass and Formula Mass
    • The Mole Concept
    • Mole Calculations
    • Determining Chemical Formulas
    • Elemental Analysis, Percentage of C, H and O
    • Determining Formulas
    • Molecular Formula from Empirical Formula
    • Stoichiometry: Quantitative Relations in Chemical Reactions
    • Limiting Reactant
    • Theoretical Yield

    Section 4 – Chemical Reactions

    • Introduction to Chemical Reactions  
    • Ionic Theory of Solutions and Solubility Rules  
    • Electrolytes and Non-electrolytes  
    • Solubility Rules  
    • Molecular and Ionic Equations  
    • Acid Base, Neutralization and Oxidation-Reduction Reactions  
    • Oxidation number  
    • Types of Oxidation-Reduction Reactions  
    • Working with solutions  
    • Quantitative Analysis

    Section 5 – Gaseous State

    • Introduction to the Gaseous State
    • Gas Pressure and Its Measurement
    • Boyle’s Law: Relating Volume and Pressure
    • Charles’s Law: Relating Volume and Temperature
    • Gay-Lussac’s Law : Relating Pressure and Temperature
    • Combined Gas Law : Relating Pressure, Temperature and Volume
    • Avogadro’s Law: Relating Volume and Amount
    • The Ideal Gas Law
    • Standard Temperature and Pressure (STP)
    • Gas Density; Molecular-Mass Determination
    • Gas Stoichiometry
    • Gas Mixtures; Law of Partial Pressures
    • Real Gases

    Section 6 –  Thermochemistry

    • Introduction to Thermochemistry
    • Thermodynamics
    • Thermodynamic Equations
    • Heat Capacity (C)
    • Standard Enthalpy of Formation ΔH formation

    Section 7 –  Quantum Theory and the Electronic Structure of Atoms

    • Properties of Waves
    • Bohr’s Model of the Atom
    • Schrodinger Wave Equation
    • Aufbau principle and Hund's Rule 
    • Electron configuration

    Section 8 –  Periodic Relationships

    • Ground State Electron Configurations and Classification of Elements
    • Electron Configurations of Cations and Anions 
    • Effective nuclear charge (Zeff)
    • The Atomic Radius
    • The Ionization Energy
    • The Electron Affinity
    • Groups Elements Properties

    Section 9 –  Ionic and Covalent Bonding

    • The Ionic and Covalent Bonding
    • Electronegativity and Polar Covalent Bond
    • Writing Lewis Structures
    • Formal Charge

    Section 10 –  Molecular Geometry and Chemical Bonding Theory

    • Valence shell electron pair repulsion (VSEPR) model
    • Dipole Moments and Polar Molecules
    • Valence Bond Theory
    • Hybridization
Matter and Measurement
  • Contents of This Section  

    In this section we will cover the following topics:

    1) Chemistry: A Science for the 21st Century

    2) Methods of Science

    3) Categories of Science

    4) Steps of Scientific Method

    5) Theory and Law

    6) Matter, Element and Compound

    7) Type of Mixtures

    8) The Three States of Matter

    9) Properties and Changes of Matter

    10) Units of Measurement

    11) Scientific Notation

    12) Significant Figures

    13) Accuracy And Precession

    14) Units and Dimensional Analysis

  • Introduction to Chemistry  

    Chemistry as the science of the composition and structure of materials and of the changes that materials undergo. Introduction to Chemistry, Modern Chemistry and the main Applications of Chemistry in the 21st Century.

  • Methods of Science  

    What is science?

    Science is not just a subject in school. It is a method for studying the natural world.

  • Categories of Science  

    Science covers many different topics that can be classified according to three main categories. Life science, Earth science and physical science.

  • Steps of Scientific Method  

    Although scientists do not always follow a rigid set of steps, investigations often follow a general pattern. The pattern of investigation procedures is called the scientific methods. Six common steps found in the scientific methods are shown in this lecture.

  • Theory and Law  

    What is Theory, and what is Law??? and what is the difference between them??

    Know all this in this lecture !!! 

  • Matter, Element and Compound  

    In this lecture we will understand distinguish between Matter, Element and Compound.

  • Types of Mixtures  

    In this lecture, You will know the two types of Mixtures.

  • The Three States of Matter  

    In this lecture, We will know the Three States of Matters and we will study the properties of each state.

  • Properties and Changes of Matter  

    In this lecture, We will study the Changes of Matters whether it was Chemical Change or Physical Change, also extensive and intensive properties will be studied.

  • Units of Measurement  

    In this lecture, International System of Units (SI) will be studies.

  • Scientific Notation  

    In this lecture, we will understand the Scientific notation expression and examples of the calculation process.

  • Significant Figures  

    In this lecture, we will understand the Significant Figures and the calculation process on it.

  • Accuracy And Precession  

    In this lecture, We will understand how to distinguish between the Accuracy and Recovery for any data you have.

  • Units and Dimensional Analysis  

    Converting between SI units, sometimes quantities are measured using different units. A conversion factor is a ratio that is equal to one. It is used to change one unit to another. How much mL are in 1.255 L? in this lecture you will learn how to convert from any unit to another, enjoy !!!

  • Summary For This Section  

    This is the summary for this section

    Regards

Atoms, Molecules, and Ions
  • Contents of The Section  

    In this section we will cover the following topics:

    1. Dalton’s Atomic Theory
    2. Atomic Symbols And Models 
    3. Law Of Conservation Of Mass 
    4. Law Of Multiple Proportions 
    5. The Structure Of The Atom 
    6. Discovery Of The Electron 
    7. The Nuclear Model Of The Atom
    8. Atomic Mass, Mass Number And Isotopes 
    9. Mass Number And Atomic Mass 
    10. Periodic Table Of The Elements 
    11. Metals, Nonmetals, And Metalloids 
    12. Molecular Substances 
    13. Ionic Substances
    14. Organic Compounds 
    15. Ionic Compounds 
    16. Rules For Predicting Charges Naming Of Ionic Compounds 
    17. Formula Of Ionic Compounds 
    18. Naming Of Binary Molecular Compounds 
    19. Acids And Corresponding Anions 
    20. Naming Of Hydrates 
    21. Writing Chemical Equations 
    22. Balancing Chemical Equations
  • Dalton's Atomic Theory  

    An introduction to early Greek theories and Dalton atomic theory.

  • Atomic Symbols and Models  

    Know how Atomic Symbols and Models were derived.

  • Law of Conservation of Mass  

    Understand the law of conservation of mass with one example.

  • Law of Multiple Proportions  

    What is The law of multiple proportions?

    You will know it in this lecture.

  • The Structure of The Atom  

    Learn the structure of the atom.

  • Discovery of The Electron  

    This section focus on the stages of electron discovery by Thomson and Millikan.

  • The Nuclear Model of The Atom  

    Ernest Rutherford a British scientist, proposed the idea of the nuclear model of the atom in 1911, know how he discovered this model in this lecture.

  • Atomic Number, Mass Number and Isotopes  

    In this lecture you will know what is Atomic Number, Mass Number, and Isotopes. In addition to this you will know how to calculate the number of protons, electrons and neutrons for any atom.

  • Mass Number and Atomic mass  

    What's the difference between Mass Number and Atomic Mass?

    you will know this in this lecture.

  • Metals, Nonmetals, and Metalloids  

    What differences between Metals, Nonmetals, and Metalloids???

  • Periodic Table of The Elements  

    An awesome trip inside the periodic table let you know how elements are ordered in periods and groups.

  • Molecular Substances  

    Molecules are assemblies of two or more atoms bonded together. Know more in this lecture.

  • Ionic Substances  

    An ion is an electrically charged particle obtained from an atom or chemically bonded group of atoms by adding or removing electrons. Learn what is cation and anion?

    Learn the formulas of ionic compounds and how to write this formula.

  • Organic Compounds  

    You encounter organic compounds in both living and nonliving materials every day. The proteins, amino acids, enzymes, and DNA that make up your body are all either individual organic molecules or contain organic molecules.

    Learn more about organic compounds in this lecture.

  • Ionic Compounds  

    Do you know what is mono-atomic compound, poly-atomic compound, oxoanion?

    you will know that in this lecture.

  • Rules for predicting the charge for mono-atomic ions  

    Know the four Rules for predicting the charge for mono-atomic ions in this lecture.

  • Naming of Ionic Compounds Chemical Nomenclature  

    A full guide about Naming of Ionic Compounds

    (Chemical Nomenclature)

  • Formula of Ionic Compounds  

    How to write the formula of ionic compound correctly??

    you will know now!!!

  • Naming of Binary Molecular Compounds  

    Binary Compound is a compound composed of only two elements. Learn how to name them in this lecture.

  • Acids and Corresponding Anions  

    An Acid is a molecular compound that yields hydrogen ions, H+, and an anion for each acid molecule when the acid dissolves in water. Know how to name Acids in this lecture.

  • Naming of Hydrates  

    Hydrate: is a compound that contains water molecules weakly bound in its crystals.

    How to name Hydrate? this lecture will show you that.

  • Writing Chemical Equations  

    A process in which one or more substances is changed into one or more new substances is a chemical reaction.

    In this lecture you will learn how to read and represent the chemical equation in the correct form.

  • Balancing Chemical Equations  

    Ethane reacts with oxygen to form carbon dioxide and water.

    Learn how you can make a correct balance for reactants and products.

  • Summary For The Section  

    This is the summary for this section

    Regards

Calculations With Chemical Formulas And Equations
  • Contents of The Calculations Section  

    Calculations With Chemical Formulas And Equations

    In this section we will cover the following topics:

    • Introduction to Calculations in Chemistry
    • Mass and Moles of Substance
    • Molecular Mass and Formula Mass
    • The Mole Concept
    • Mole Calculations
    • Determining Chemical Formulas
    • Elemental Analysis, Percentage of C, H and O
    • Determining Formulas
    • Molecular Formula from Empirical Formula
    • Stoichiometry: Quantitative Relations in Chemical Reactions
    • Limiting Reactant
    • Theoretical Yield
  • Introduction to Calculations in Chemistry  

    How do you determine the chemical formula of a substance such as acetic acid or acetaldehyde? How much acetic acid can you prepare from a given quantity of ethanol or a given quantity of acetaldehyde? These types of questions are very important in chemistry. 

    Learn more in this lecture.

  • Mass and Moles of Substance  

    We buy a quantity of items in several ways. You often purchase items such as oranges and lemons by counting out a particular number. Some things, such as eggs and soda, can be purchased in a “package” that represents a known quantity.

    Learn how We Measure Items in Chemistry here.

  • Molecular Mass and Formula Mass  

    Learn what is the Molecular Mass and what is the Formula Mass in this lecture.

  • The Mole Concept  

    Chemist have adopted the mole concept as a convenient way to deal the enormous number of molecules or ions in the samples they work with.

    Learn More in this lecture about the concept of mole.

  • Mole Calculations  

    In this lecture you will learn the basic calculation of Mole conversions to mass.

  • Determining Chemical Formulas  

    Percentage Composition is, as the mass percentages of each element in the compound.

    Learn here how to find element percentage in any organic compound.

  • Elemental Analysis, Percentage of C, H and O  

    Suppose you have a newly discovered compound whose formula you wish to determine. The first step is to obtain its percentage composition. Learn more here.

  • Determining Formulas  

    What is the Empirical Formula?

    How we can make Determining the Empirical Formula from Masses of Elements?

    Learn how here.


  • Molecular Formula from Empirical Formula  

    In this lecture:

    Determining the Molecular Formula from Percentage Composition and Molecular Mass

  • Stoichiometry: Quantitative Relations in Chemical Reactions  

    Stoichiometry is the calculation of the quantities of reactants and products involved in a chemical reaction.

    It is based on the chemical equation and on the relationship between mass and moles. Such calculations are fundamental to most quantitative work in chemistry.

    Learn how to apply it on chemical equations.

  • Limiting Reactant  

    In this lecture:

    The limiting reactant (or limiting reagent) is the reactant that is entirely consumed when a reaction goes to completion.

    The moles of product are always determined by the starting moles of limiting reactant.

    How to calculate the limiting reactant?

    You will know now.

  • Theoretical Yield  

    What is the Theoretical Yield?

    What is The Actual Yield?

    What is the Percentage Yield?

    How to calculate Yield?

    You will know everything in this lecture.

  • Summary  
Chemical Reactions
  • Introduction to Chemical Reaction  

    In this section, we will discuss the major types of chemical reactions, including precipitation reactions. Some of the most important reactions we will describe involve ions in aqueous (water) solution. Therefore, we will first look at these ions and see how we represent by chemical equations the reactions involving ions in aqueous solution.

  • Ionic Theory of Solutions and Solubility Rules  

    Chemists began studying the electrical behavior of substances in the early nineteenth century, and they knew that you could make pure water electrically conducting by dissolving certain substances in it. In 1884, the Swedish chemist Arrhenius proposed the ionic theory of solutions to account for this conductivity. 

  • Electrolytes and Non-Electrolytes  

    We can divide the substances that dissolve in water into two broad classes, electrolytes and non-electrolytes.

    Know all details through this lecture.

  • Solubility Rules  

    In this lecture you will learn all the rules of solubility.

  • Molecular and Ionic Equations  
    • What is Molecular equation?
    • What is Net Ionic Equation?
    • How to find the net ionic equation?

    Know all this in this lecture.


  • Acid base, Neutralization and Oxidation reactions  

    In this lecture we will study:

    • Acid Base Reactions
    • Neutralization Reactions
    • Oxidation - Reduction Reactions
  • Types of Oxidation-Reduction Reactions  

    In this lecture we will study the five types of oxidation reduction reactions with examples.

  • Oxidation number  

    Oxidation number is the charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred.

    • What are the seven rules of oxidation numbers?
    • How to calculate oxidation numbers?

    Find that in this lecture.

  • Working with solutions  

    In this lecture we will study:

    • Molar Concentration
    • Dilution Analysis
  • Quantitative Analysis  

    In this lecture we will study:

    • Gravimetric Analysis
    • Volumetric Analysis - Titration 


The Gaseous State
  • The Gaseous State  

    In this lecture - Introduction to Gases.

    Gases have several characteristics that distinguish them from liquids and solids. You can compress gases into smaller and smaller volumes.

  • Gas Pressure and Its Measurement  

    This lecture will cover:

    • Important units in pressure
    • Pressure at different heights on the earth
    • Mercury Barometer
    • Flask equipped with a closed-tube manometer
    • Empirical Gas Laws
  • Boyle’s Law: Relating Volume and Pressure  

    Robert Boyle in 1661. When he poured mercury into the open end of a J-shaped tube, the volume of the enclosed gas decreased.

    we will study in this lecture Boyle law with example.

  • Charles’s Law: Relating Volume and Temperature  

    Charles 1787 was a French physicist continued these kinds of experiments.

    Know what is his law.

  • Gay-Lussac’s Law : Relating Pressure and Temperature  

    According to Gay-Lussac’s Law: The pressure exerted by a gas at constant volume is directly proportional to its absolute temperature. 

    All details included in this lecture.

  • Combined Gas Law : Relating Pressure, Temperature and Volume  

    In this lecture we will study that If all three parameters, P, V, and T, are changing so there is no constant, their combined relationship of Combined Gas Law.

  • Avogadro’s Law: Relating Volume and Amount  

    We will study the Avogadro’s Law at Constant temperature and pressure.

  • The Ideal Gas Law  

    If we combined the three laws Boyle’s law, Charles’ law and Avogadro’s law together we will obtain the ideal gas law PV=nRT. Will be studied in this lecture.

  • Standard Temperature and Pressure (STP)  

    In this lecture we will study the STP conditions, The conditions 0 C and 1 atm are called standard temperature and pressure (STP).

  • Gas Density; Molecular-Mass Determination  

    In this lecture you will be able to get the density of any gas from the ideal gas law.

  • Gas Stoichiometry  

    Stoichiometry calculations can be applied on Gases.

    We will study it with example.

  • Gas Mixtures; Law of Partial Pressures  

    In this lecture, Dalton’s Law of Partial Pressures will be studied to explain gas mixtures.

  • Real Gases  

    Ideal gases assume:

    • No interaction between molecules (either attractive nor repulsive).
    • Volume of molecules is negligibly small compared to container.

    While Real gases know:

    • Molecules have a finite molecule number volume.
    • Interaction between molecules exist.

    In this lecture you will learn how to use Van der Waals equation on real gases.

Thermochemistry
  • Introduction to Thermochemistry  

    Thermochemistry is the study of heat change in chemical reactions.

    In this lecture we will study:

    • Thermochemistry
    • Energy Changes in Chemical Reactions
    • Open, Closed and Isolated systems.
    • Exothermic & Endothermic reactions
  • Thermodynamics  

    Thermodynamics is the scientific study of the inter-conversion of heat and other kinds of energy.

    we will study here:

    • state of the system
    • First Law of Thermodynamic
    • Another form of the first law for ΔE system
    • Work Done on the System
    • one example on work
    • Enthalpy and the First Law of Thermodynamics
  • Thermodynamic Equations  

    In converting H2O (solid) to H2O (liquid) heat is absorbed by the system from the surroundings, Is ΔH negative or positive? you will know in this lecture.

    moreover: 

    • The stoichiometric coefficients always refer to the number of moles of a substance.
    • The physical states of all reactants and products. 
    • A Comparison of ΔH and ΔE.
  • Heat Capacity (C)  

    In this lecture we will study the specific heat (s) and the heat capacity (C) 

    then you will be able to calculate the heat capacity (C) for any element.

  • Standard Enthalpy of Formation (ΔH formation)  

    Because there is no way to measure the absolute value of the enthalpy of a substance, must I measure the enthalpy change for every reaction of interest?

    You will know in this lecture.

Quantum Theory and the Electronic Structure of Atoms
  • Properties of Waves  

    It is important to realize that a wave is quite a different object than a particle.

    In this lecture we will study the properties of the waves.

  • Bohr’s Model of the Atom  

    In this lecture we will study the Bohr Model of the Atom, The Bohr model is a relatively primitive model of the hydrogen atom, compared to the valence shell atom. As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics and thus may be considered to be an obsolete scientific theory. 

  • Schrodinger Wave Equation  

    In 1926 Schrodinger wrote an equation that described both the particle and wave nature of the e-

    Wave function psi - describes:

    1. energy of e- with a given psi

    2. probability of finding e- in a volume of space

     Schrodinger equation will be studied here.

    Psi = fn(n, l, ml, ms), all the four quantum numbers will be studied with examples.

  • Aufbau principle and Hund's Rule  

    In this lecture we will study:

    • Fill up” electrons in lowest energy orbitals (Aufbau principle)
    • The most stable arrangement of electrons in subshells is the one with the greatest number of parallel spins (Hund’s rule).


  • Electron configuration  

    In atomic physics and quantum chemistry, the electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbitals.

    We will study the Electron Configuration of Elements with some examples.

Periodic Relationships
  • Ground State Electron Configurations and Classification of Elements  

    The electron configuration of an atom is the representation of the arrangement of electrons distributed among the orbital shells and sub-shells. Commonly, the electron configuration is used to describe the orbitals of an atom in its ground state, but it can also be used to represent an atom that has ionized into a cation or anion by compensating with the loss of or gain of electrons in their subsequent orbitals.

    In this lecture you will know:

    • When the Elements Were Discovered?
    • Ground State Electron Configurations of the Elements.
    • Classification of the Elements.
  • Electron Configurations of Cations and Anions  

    The electronic configuration of many ions is that of the closest noble gas to them in the periodic table. An anion is an ion that has gained one or more electrons, acquiring a negative charge. A cation is an ion that has lost one or more electrons, gaining a positive charge.

    we will study here:

    • Electron Configurations of Cations and Anions of Representative Elements.
    • The isoelectronic of elements.
    • Electron Configurations of Cations of Transition Metals.
  • Effective nuclear charge (Zeff)  

    The effective nuclear charge is the net positive charge experienced by valence electrons.

    In this lecture you will know how to find the  effective nuclear charge (Zeff) for elements.

  • Atomic Radius  
    • How to calculate the atomic radius for elements?
    • What is the trend of atomic radius in the periodic table?
    • What about Cations and Anions Atomic Radius?
  • Ionization Energy  

    What is Ionization energy?

    • Why third ionization energy is higher than second ionization energy which is also higher then the first ionization energy?
    • Why there is a significant jump between some ionization energies for the same elements?
    • What is the general Trend in First Ionization Energies?

    All these questions will answered in this lecture.

  • Electron Affinity  

    In this lecture we will study:

    • What is the electron affinity.
    • Electron affinities of some representative elements and noble gases.
    • Variation of Electron Affinity With Atomic Number.


  • Groups Elements Properties  

    In this lecture we will study:

    • The group elements from 1A to 8A.
    • The general reactions of those elements.
    • we will see an awesome pure elements shapes.
    • Some properties of Oxides Across a Period.


Ionic and Covalent Bonding
  • The Ionic and Covalent Bonding  

    In this lecture we will study:

    • Valence electrons
    • Lewis Dot Symbols 
    • The Ionic Bond
    • Electrostatic (Lattice) Energy
    • Born-Haber Cycle 
    • The Covalent Bond
    • Lengths of Covalent Bonds
  • Electronegativity and Polar Covalent Bond  

    Lets study now:

    • Polar Covalent Bond
    • Electronegativity
    • Classification of bonds by difference in electronegativity
  • Writing Lewis Structures  

    How to Write Lewis Structures for any compound?

    In this lecture we will know

  • Formal Charge  

    An atom’s formal charge is the difference between the number of valence electrons in an isolated atom and the number of electrons assigned to that atom in a Lewis structure.

    Lets start calculating the formal charge for any element in any compound.

    In addition to that, we will study the Resonance Structure and Bond Energies (BE) and Enthalpy changes in reactions.

Molecular Geometry and Chemical Bonding Theory
  • Valence shell electron pair repulsion (VSEPR) model)  

    In this lecture we will study:

    • Valence shell electron pair repulsion (VSEPR) model
    • Predicting Molecular Geometry


  • Dipole Moments and Polar Molecules  

    Which of the following molecules have a dipole moment, H2O, CO2, SO2, and CH4?

    Here you will know that by studying the Dipole Moments and Polar Molecules.

  • Valence Bond Theory  

    Valence bond theory – bonds are formed by sharing of e- from overlapping atomic orbitals.

    In this lecture:

    • Change in Potential Energy of Two Hydrogen Atoms as a Function of Their Distance of Separation.
    • Valence Bond Theory and NH3.


  • Hybridization  

    Hybridization is mixing of two or more atomic orbitals to form a new set of hybrid orbitals.

    In this lecture we will study:

    • Formation of sp3 Hybrid Orbitals
    • Formation of sp2 Hybrid Orbitals
    • Formation of sp1 Hybrid Orbitals
    • How do I predict the hybridization of the central atom
    • Sigma (sig) and Pi Bonds (pi)
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