Chemical bonding is one of the most important topics in chemistry because it explains how atoms join together to form substances around us. From water to metals, everything depends on bonding.
In this chapter, you will learn about different types of bonds, properties of metals and non-metals, and the forces that hold molecules together. These notes are designed according to the 2026 new syllabus and written in simple English for quick understanding and exam preparation.
MCQs – Chemical Bonding (Chapter 3)
1. Which form of carbon is used as a lubricant?
(a) Coal
(b) Diamond
(c) Graphite ✅
(d) Charcoal
2. Which compound contains both covalent and ionic bonds?
(a) MgCl₂
(b) NH₄Cl ✅
(c) CaO
(d) PCl₃
3. Why do atoms form chemical bonds?
(a) To increase size
(b) To lower their energy and gain stability ✅
(c) To increase mass
(d) To form isotopes
4. What are formed when sodium reacts with chlorine?
(a) Molecules only
(b) Ions only
(c) Positively charged sodium and negatively charged chloride ions ✅
(d) Uncharged atoms
5. What type of bond is formed in a hydrogen molecule (H₂)?
(a) Polar covalent
(b) Ionic
(c) Non-polar covalent ✅
(d) Metallic
6. In a coordinate bond, the atom donating the electron pair is called:
(a) Acceptor
(b) Donor ✅
(c) Neutral
(d) Receptor
7. Dipole-dipole forces exist between:
(a) Non-polar molecules
(b) Ionic compounds
(c) Polar molecules ✅
(d) Atoms of noble gases
8. Which compounds show hydrogen bonding?
(a) CH₄
(b) NH₃
(c) H₂O ✅
(d) H₂S
What is a Chemical Bond?
A chemical bond is the force that holds atoms together to form molecules or compounds. Atoms form bonds to become stable, usually by completing their outer shell of electrons.
👉 In simple words:
Atoms join together so they can become stable.
Metallic Bond
A metallic bond is found in metals where positive metal ions are surrounded by a “sea of free electrons.”
✔ Key Features:
-
Electrons can move freely
-
Metals conduct electricity and heat
-
Metals are malleable (can be shaped)
-
Metals are ductile (can be stretched into wires)
👉 This is why metals are used in wires and construction.
Electropositive Character of Metals
Electropositive character means the ability of metals to lose electrons easily.
✔ Important Points:
-
Metals form positive ions (cations)
-
Increases down the group in the periodic table
-
Alkali metals are highly electropositive
👉 Example: Sodium easily loses one electron.
Electronegative Character of Non-Metals
Electronegativity is the ability of non-metals to gain electrons.
✔ Important Points:
-
Non-metals form negative ions (anions)
-
Decreases down the group
-
Halogens (like chlorine) are highly electronegative
👉 Example: Chlorine gains one electron to become stable.
Intermolecular Forces of Attraction
These are weak forces between molecules (not inside them).
✔ Types:
-
Dipole-Dipole Forces
-
Hydrogen Bonding
-
Van der Waals Forces
✔ Why Important?
-
Control boiling point
-
Control melting point
-
Affect physical state (solid, liquid, gas)
👉 Stronger forces = higher boiling point
Nature of Bonding and Properties
The type of bonding directly affects the properties of a substance.
Ionic Compounds
-
High melting and boiling points
-
Conduct electricity in molten or dissolved form
-
Usually hard and crystalline
Covalent Compounds
-
Low melting and boiling points
-
Do not conduct electricity
-
Usually gases or liquids
Metallic Substances
-
Good conductors of heat and electricity
-
Malleable and ductile
-
Shiny appearance
👉 Conclusion:
Bonding type decides the behavior of matter.
📥 Download Chapter 3 Notes – Chemical Bonding (PDF)
Skip to PDF contentClick the button below to download the Class 9 Chemistry Chapter 3 Chemical Bonding Notes according to the 2026 new syllabus.
These notes are:
✔ Easy to understand
✔ Exam-focused
✔ Perfect for revision