SPM Chemistry (KSSM) Paper 1

01 Introduction to Chemistry
1.1 Chemistry and Its Importance
1 Lesson
1.1.1 Chemistry and Its Importance
1.2 Scientific Investigation
1 Lesson
1.2.1 Scientific Investigation
02 The Structure of Atoms
2.1 The Basic Concept of Matter
2 Lessons
2.1.1 The Particle Theory of Matter
2.1.2 The Three States of Matter
2.2 The History of Development of the Atomic Model
1 Lesson
2.2.1 The History of Development of the Atomic Model
2.3 The Structure of Atom
2 Lessons
2.3.1 The Structure of Atom
2.3.2 Electrons Arrangement in Atom
2.4 Isotopes and Their Uses
1 Lesson
2.4.1 Isotopes and Their Uses
2.5 The Structure of Atom - Practices
03 Concept of Mole, Formulae and Equations
3.1 Relative Atomic Mass and Relative Molecular Mass
1 Lesson
3.1.1 Relative Atomic Mass and Relative Molecular Mass
3.2 Concept of Mole
3 Lessons
3.2.1 Concept of Mole
3.2.2 Number of Mole and Mass
3.2.3 Number of Mole and Volume of Gases
3.3 Chemical Formulae
2 Lessons
3.3.1 Chemical Formulae
3.3.2 Formula of Ionic Compounds and Molecule
3.4 Chemical Equations
1 Lesson
3.4.1 Chemical Equations
3.5 Chemical Formulae and Equations - Practices (Coming Soon)
04 Periodic Table of Elements
4.1 The Development of Periodic Table
1 Lesson
4.1.1 Development of Periodic Table
4.2 Arrangement of Element in Periodic Table
1 Lesson
4.2.1 Arrangement of Electrons in Periodic Table
4.3 Group 18 Elements
1 Lesson
4.3.1 Group 18 Elements
4.4 Group 1 Elements
2 Lessons
4.4.1 Group 1 Elements
4.4.2 Chemical Properties of Group 1 Elements
4.5 Group 17 Elements
2 Lessons
4.5.1 Group 17 Elements
4.5.2 Chemical Properties of Group 17 Elements
4.6 Elements in Period 3
1 Lesson
4.6.1 Elements in Period 3
4.7 Transition Elements
1 Lesson
4.7.1 The Transition Elements
4.8 Periodic Table - Practices (Coming Soon)
1 of 3
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2.3.2 Electrons Arrangement in Atom

SPM Chemistry (KSSM) Paper 1 2.3 The Structure of Atom 2.3.2 Electrons Arrangement in Atom
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Electron Arrangement in Atom

  1. We have learnt that electrons occupy orbits with definite energy level of an atom, as suggested by Neils Bohr.
  2. These orbits with definite energy level are known as the shell.
  3. Every single shell is capable of holding up to certain amount of electrons.
  4. The first shell can hold up to two electrons. This is called a duplet.
  5. The second shell can hold up to eight electrons. This is called an octet.
  6. The third shell can hold up to eighteen electrons.
  7. However, with the third shell, when eight electrons are present, extra stability is gained. The additional electrons go into the fourth shell before the third shell is completely filled.
  8. The way in which the electrons are distributed in the shells of an atom is called the electron arrangement of the atom
  9. The examples below show the electron arrangement of some elements:
Atom
Notes
Electrons Arrangement
  1. Lithium has 3 protons and 3 neutrons and three electrons as well.
  2. All the three electrons are arrange as follows:
  • Two electrons are filled in the first shell.
  • One electron is filled in the second shell.
  • The electron arrangement of carbon is 2.1
2.1 
  1. Chlorine has 17 protons and 18 neutrons and 17 electrons.
  2. All the three electrons are arrange as follows:
  • Two electrons are filled in the first shell.
  • Eight electrons are filled in the second shell.
  • Seven electrons are filled in the third shell.
  • The electron arrangement of chlorine is 2.8.7.
2.8.7
  1. Calcium has 20 protons and 20 neutrons and 20 electrons.
  2. All the three electrons are arrange as follows:
  • Two electrons are filled in the first shell.
  • Eight electrons are filled in the second shell.
  • Eight electrons are filled in the third shell.
  • Two electrons are filled in the forth shell.
  • The electron arrangement of carbon is 2.8.8.2.
2.8.8.2
Table below shows the arrangement of electrons of the first 20 elements in the periodic table. We shall learn periodic table in chapter 4.
Element Proton Number Number of Electron
Number of electron in
 Electron Arrangement
1st shell 2nd shell 3rd shell 4th shell
Hydrogen
1
1
1
0
0
0
 1
Helium
2
2
2
0
0
0
 2
Lithium
3
3
2
1
0
0
 2.1
Beryllium
4
4
2
2
0
0
 2.2
Boron
5
5
2
3
0
0
 2.3
Carbon
6
6
2
4
0
0
 2.4
Nitrogen
7
7
2
5
0
0
 2.5
Oxygen
8
8
2
6
0
0
 2.6
Fluorine
9
9
2
7
0
0
 2.7
Neon
10
10
2
8
0
0
 2.8
Sodium
11
11
2
8
1
0
 2.8.1
Magnesium
12
12
2
8
2
0
 2.8.2
Aluminium
13
13
2
8
3
0
 2.8.3
Silicon
14
14
2
8
4
0
 2.8.4
Phosphorus
15
15
2
8
5
0
 2.8.5
Sulphur
16
16
2
8
6
0
 2.8.6
Chlorine
17
17
2
8
7
0
 2.8.7
Argon
18
18
2
8
8
0
 2.8.8
Potassium
19
19
2
8
8
1
 2.8.8.1
Calcium
20
20
2
8
8
2
 2.8.8.2

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Electron arrangement in an atom

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Valence Electron

Valence electrons are the electrons in the outermost shell.
  1. The electrons in the outermost shell of an atom are called valence electrons.
  2. The valence electrons have great significance in determining the chemical properties of an atom.
  3. Elements with the same number of valence electron have the same chemical properties.
 
Example:
Given that a sodium atom has 11 protons 12 neutrons. Find the number of valence electron in a sodium atom.Answer:
For an atom,
 
Number of electrons = number of protons = 11
 
Electron arrangement of sodium = 2.8.1
 
Therefore, sodium has 1 valence electron.
 
 
 
 
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