Become A Chemistry Master - Basic Principles Of Chemistry

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

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.

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

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

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.

What is science?

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

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

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.

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

Know all this in this lecture !!! 

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

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

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

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.

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

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

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

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

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 !!!

This is the summary for this section

Regards

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

An introduction to early Greek theories and Dalton atomic theory.

Know how Atomic Symbols and Models were derived.

Understand the law of conservation of mass with one example.

What is The law of multiple proportions?

You will know it in this lecture.

Learn the structure of the atom.

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

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.

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.

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

you will know this in this lecture.

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

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

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

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.

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.

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

you will know that in this lecture.

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

A full guide about Naming of Ionic Compounds

(Chemical Nomenclature)

How to write the formula of ionic compound correctly??

you will know now!!!

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

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.

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

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

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.

Ethane reacts with oxygen to form carbon dioxide and water.

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

This is the summary for this section

Regards

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

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.

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.

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

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.

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

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

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

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.

What is the Empirical Formula?

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

Learn how here.

In this lecture:

Determining the Molecular Formula from Percentage Composition and Molecular Mass

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.

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.

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.

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.

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. 

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

Know all details through this lecture.

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

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

Know all this in this lecture.

In this lecture we will study:

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

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

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.

In this lecture we will study:

• Molar Concentration
• Dilution Analysis

In this lecture we will study:

• Gravimetric Analysis
• Volumetric Analysis - Titration 

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.

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

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 1787 was a French physicist continued these kinds of experiments.

Know what is his law.

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.

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.

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

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.

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

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

Stoichiometry calculations can be applied on Gases.

We will study it with example.

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

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 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 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

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.

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.

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.

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.

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. 

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.

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).

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.

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.

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.

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.

• 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?

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.

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.

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.

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

Lets study now:

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

How to Write Lewis Structures for any compound?

In this lecture we will know

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.

In this lecture we will study:

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

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 – 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 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)