Become A Chemistry 1 Master - Basic Principles Of Chemistry

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.

Hi students

I hope that you enjoy in this course and I need your review, after you watch this course then tell me please what is your opinion In this course I hope you rate this course. Really your review is very important to me thank you

Dr Mohammad Abualrub

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.

This quiz is over different types of matter - Elements, Compounds and Mixtures. Select the best answer from the choices.

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.

This َQuiz will determine your level of understanding the previous lectures

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.

Practice Quiz on Scientific Notation !!!

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

This quiz is designed to test your ability on recognizing the exact significant figures at any number you have !!!

Enjoy !!!

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.

A downloadable copy of the periodic Table like this in the resources.

By referring to the periodic table, identify the group and period to which each of the following elements belongs. Then decide whether the element is a metal, nonmetal, or metalloid.

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)

Naming an Ionic Compound from Its Formula

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.

Balancing Simple Equations Quiz

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.

Mole Calculation for atoms, molecules, units and ions

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

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

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

Reactions that take place in the real world go until one of the reactants is used up. The reactant that is used up first is called the limiting reactant (LR)because it limits how much product can be made. The reactant that is left over is called the excess reactant (ER).

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.

Classification of Solutes in Aqueous Solution: Classify each solute if it is strong electrolyte, weak electrolyte or non-electrolyte in aqueous solution.

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

Solubility Rules for Ionic Compounds Decide if the following ionic compounds soluble or insoluble in Water.

• 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

Oxidation-Reduction reactions (also called “redox” reactions) are reactions that involve a shift of electrons between reactants.

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.

An oxidation number is a positive or negative number assigned to an atom according to a set of rules.

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.

Boyle’s Law Quiz: Relating Volume and Pressure

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

Know what is his law.

Charles's law (also known as the law of volumes) is an experimental gas law that describes how gases tend to expand when heated. A modern statement of Charles's law is:

When the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be directly related.

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.

Gay-Lussac's law, Amontons' law or the pressurelaw was found by Joseph Louis Gay-Lussac in 1809. It states that, for a given mass and constant volume of an ideal gas, the pressure exerted on the sides of its container is directly proportional to its absolute temperature.

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.

When we put Boyle's law, Charles' law, and Gay-Lussac's law together, we come up with the combined gas law, which shows that: Pressure is inversely proportional to volume, or higher volume equals lower pressure. Pressure is directly proportional to temperature, or higher temperature equals higher pressure.

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