SPM Chemistry

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 | 1 Exercise

2.1.1 The Particle Theory of Matter

2.1.2 The Three States of Matter

2.1.3 Basic Concepts of Matter

2.2 The History of Development of the Atomic Model

1 Lesson | 1 Exercise

2.2.1 The History of Development of the Atomic Model

2.2 Development of the Atomic Model

2.3 The Structure of Atom

2 Lessons | 1 Exercise

2.3.1 The Structure of Atom

2.3.2 Electrons Arrangement in Atom

2.3 Atomic Structure

2.4 Isotopes and Their Uses

1 Lesson | 1 Exercise

2.4.1 Isotopes and Their Uses

2.4 Isotopes and Their Uses

03 Concept of Mole, Formulae and Equations

3.1 Relative Atomic Mass and Relative Molecular Mass

1 Lesson | 1 Exercise

3.1.1 Relative Atomic Mass and Relative Molecular Mass

3.1 Relative Atomic Mass and Relative Molecular Mass

3.2 Concept of Mole

3 Lessons | 1 Exercise

3.2.1 Concept of Mole

3.2.2 Number of Mole and Mass

3.2.3 Number of Mole and Volume of Gases

3.2 Mole Concept

3.3 Chemical Formulae

2 Lessons | 1 Exercise

3.3.1 Chemical Formulae

3.3.2 Formula of Ionic Compounds and Molecule

3.3 Chemical Formula

3.4 Chemical Equations

1 Lesson | 1 Exercise

3.4.1 Chemical Equations

3.4 Chemical Equation

04 Periodic Table of Elements

4.1 The Development of Periodic Table

1 Lesson | 1 Exercise

4.1.1 Development of Periodic Table

4.1 Development of the Periodic Table of Elements

4.2 Arrangement of Element in Periodic Table

1 Lesson | 1 Exercise

4.2.1 Arrangement of Electrons in Periodic Table

4.2 Arrangement of Elements in the Modern Periodic Table of Elements

4.3 Group 18 Elements

1 Lesson | 1 Exercise

4.3.1 Group 18 Elements

4.3 Elements in Group 18

4.4 Group 1 Elements

2 Lessons | 1 Exercise

4.4.1 Group 1 Elements

4.4.2 Chemical Properties of Group 1 Elements

4.4 Elements in Group 1

4.5 Group 17 Elements

2 Lessons | 1 Exercise

4.5.1 Group 17 Elements

4.5.2 Chemical Properties of Group 17 Elements

4.5 Elements in Group 17

4.6 Elements in Period 3

1 Lesson | 1 Exercise

4.6.1 Elements in Period 3

4.6 Elements in Period 3

4.7 Transition Elements

1 Lesson | 1 Exercise

4.7.1 The Transition Elements

4.7 Transition Elements

05 Chemical Bonds

5.1 Formation of Compounds

1 Lesson | 1 Exercise

5.1.1 Formation of Compounds

5.1 Basics of Compound Formation

5.2 Ionic Bonds

2 Lessons | 1 Exercise

5.2.1 Formation of Ion

5.2.2 Ionic Bonding

5.2 Ionic Bonds

5.3 Covalent Bonds

1 Lesson | 1 Exercise

5.3.1 Covalent Bonding

5.3 Covalent Bonds

1 of 4

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5.1 Basics of Compound Formation

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SPM Chemistry 5.1 Formation of Compounds 5.1 Basics of Compound Formation

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Question 1 of 10

1. Question
1 point(s)
Why are almost all naturally occurring chemicals in the form of compounds?
- Because atoms do not have room to move on their own.
- Individual elements do not have enough mass.
- Because single elements are more explosive.
- Compounds are more stable than individual elements.
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Question 2 of 10

2. Question
1 point(s)
The Group 18 elements are known as the highly stable noble gases. What is the main reason for their stability?
- They exist in solid form at room temperature.
- They have a stable doublet or octet electron arrangement.
- They always share electrons with other elements.
- They have a very high number of protons.
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Question 3 of 10

3. Question
1 point(s)
Which of the following describes the doublet electron arrangement of the Helium (He) atom?
- Shares two pairs of electrons with another atom.
- Has eight electrons in the valence shell.
- Donates two electrons to become stable.
- Its valence shell is fully filled with two electrons.
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Question 4 of 10

4. Question
1 point(s)
How does a sodium (Na) atom with an electron configuration of 2.8.1 achieve stability?
- Shares one electron with another metal atom.
- Accepts seven more electrons to achieve an octet configuration.
- Releases one valence electron to form the Na⁺ ion.
- Eliminates the innermost electron shell.
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Question 5 of 10

5. Question
1 point(s)
What type of bond is formed through the strong electrostatic attraction between cations and anions?
- Double Bond
- Covalent Bond
- Metallic Bond
- Ionic Bond
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Question 6 of 10

6. Question
1 point(s)
In the formation of a covalent bond, what happens to the valence electrons of the atoms involved?
- Only one atom contributes all the electrons to be shared.
- Valence electrons are shared between non-metal atoms.
- Electrons are transferred completely from one atom to another.
- Valence electrons move freely between all atoms in a compound.
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Question 7 of 10

7. Question
1 point(s)
Which of the following is a characteristic of nonmetal atoms from Groups 15, 16, or 17 during the formation of ionic bonds?
- Does not change its electron arrangement during the reaction.
- Forms positive ions when reacting with metals.
- Tends to accept electrons to form anions.
- Tends to donate valence electrons.
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Question 8 of 10

8. Question
1 point(s)
If a chlorine atom (Cl) has an electron configuration of 2.8.7, what will happen to form the chloride ion (Cl⁻)?
- It will give up all its electrons to become stable.
- It will accept one electron to achieve a configuration of 2.8.8.
- It will give up seven valence electrons.
- It will share one electron with another chlorine atom.
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Question 9 of 10

9. Question
1 point(s)
How many electron pairs are shared in a double triple bond?
- Four pairs of electrons
- Two pairs of electrons
- Three pairs of electrons
- One pair of electrons
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Question 10 of 10

10. Question
1 point(s)
Which part of the electron is involved in the process of forming a chemical bond?
- The electrons in the nucleus.
- All the electrons that the atom possesses.
- Valence electrons (outermost shell).
- Electrons in the innermost shell only.
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