Chemistry form 4 notes

Chemistry form 4 notes - Welcome to our blog Malaysian, through this post we'll provide and share to you some chemistry form 4 notes and the past collection of chemistry notes form 4. The collection for form 4 begin from chapter 2 to chapter 9.

You can view all notes easily and directly by following the links below:

Chapter 2: The Structure of the Atom.

2.1 - Rutheford atomic model
2.2 - Bohr atomic model

Chapter 3: Chemical Formulae and Equations

3.1 - Understanding of mole concept
3.2 - Mass and moles of an element
3.3 - Empirical formula of magnesium oxide
3.4 - Empirical formula of copper (II) oxide

Chapter 4: Periodic Table of Elements

4.1 - Introduction of periodic table
4.2 - Physical properties of Group 1
4.3 - Reactivity of Group 1
4.4 - Physical properties of Group 17
4.5 - Reactivity of Group 17
4.6 - Characteristics of transition metal

Chapter 5: Chemical Bonds

5.1 - Ionic bond
5.2 - Covalent bond
5.3 - Lewis dot structure of covalent bond
5.4 - Electrical conductivity of ionic compound

Chapter 6: Electrochemistry

6.1 - Understanding of electrolyte
6.2 - Understanding of electrolysis
6.3 - Electrolysis of concentrated sodium chloride
6.4 - Types of electrodes affect product of electrolysis
6.5 - Electrolysis of copper sulphate using carbon and copper
6.6 - Electroplating of metal
6.7 - Purification of metal
6.8 - Extraction of metal
6.9 - Daniell cell
6.10 - Displacement of metal from salt solution
6.11 - Constructing electrochemical series

Chapter 7: Acids and Bases

7.1 - Understanding of acid and base
7.2 - Strength of acid
7.3 - Differences between strong acid and weak acid
7.4 - Strength of alkali
7.5 - pH scale
7.6 - Concentration of solution – molarity
7.7 - Preparing a standard solution
7.8 - Neutralization reaction
7.9 - Titration method
7.10 - Determining molarity of solution

Chapter 8: Salts

8.1 - Preparation of insoluble salt
8.2 - Application of precipitation of salt

Chapter 9: Manufactured Substances in Industry

9.1 - Contact process
9.2 - Haber process
9.3 - Making of alloy

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Mass and moles of an element

Mass and moles of an element - Chemistry Form 4: Chapter 3 - Mass and Moles of an element.

Molar mass is the weight of one mole of any chemical compounds.
Molar mass ==> Relative Molecular Mass

For detail have a look the image below:



SWF Player - Click on the diagram to play.

Hopefully this Mass and moles of an element works! Study smart.

Understanding of Mole concept

Understanding of Mole concept - The next chapter for Chemistry Form 4 is Chapter 3 about The Mole.

There are 2 important point that you need to know:

• A mole is the quantity of anything that has the same number of particles found in 12.000 grams of carbon-12. That number of particles is Avogadro's Number, which is roughly 6.02x1023
• A mole of carbon atoms is 6.02x1023 carbon atoms.

The image below for detail and understand technique as well as core concept for Mole, so please imagine and save it in your memory:



More picture about Mole concept and activity:


Description: Figure 5-2. One mole of sulfur (a), potassium dichromate (b), and graphite (c) has a mass in grams which equals the mass of a single particle of each substance. Each amount shown here contains 6.02 x 10(23) particles for that substance.

Another image below show you about Mole Conversions:

Bohr atomic model

Bohr atomic model - Now we at Chemistry Form 4: Chapter 2 - Bohr's Atomic Model, the information needed as below.

Introduction: Neils Bohr was born on October 7, 1885 in Copenhagen, Denmark. In year 1922 he won the Nobel prize for physics. Bohr was a professor at the unoversity of Copenhagen. Neils Bohr produced a theory about the structure of an atom based on Rutheford's Plum Pudding model. Bohr discovered that the electrons travel in orbits. Outer orbits could hold more electrons than the inner orbits. He suggested that when an electron jumps from an outer orbit to an inner orbit it emits light which called photon.



This model was created by Neils Bohr in 1915. In the center is the nucleus which is composed of protons and neutrons. It is orbited by electrons. The nucleus is about 100,000 times smaller than the radius of the atom.

Rutheford atomic model

Rutheford atomic model - Chemistry Form 4: Chapter 2 - Rutherford Atomic Model.

Rutherford bombarded a very thin leaf of element gold with a stream of high speed positively charged particles. These positively charged particles are alpha radiation from helium nuclei.

As expected, most alpha particles went right through the gold foil but to his amazement, a few alpha particles rebounded almost directly backwards due to same positive charge repulsion force.

Click on the diagram to play!

This proved that:

1. the atom had a dense but very small positive nucleus
2. the electrons were far away from the nucleus
3. the electrons were separated from the nucleus by a lot of empty space

Rutheford atomic model is one of Chemistry Form 4 notes, specially provide to you by http://chemistryform4notes.blogspot.com/