Ionic and covalent bonds are important in chemistry. Ionic bonds form when atoms transfer electrons. Covalent bonds happen when atoms share electrons. These bonds shape the materials we see around us.
Understanding these bonds is simple with the right explanation. Knowing their differences helps explain how substances are formed and how they behave.
In this blog, you will learn about difference between ionic bond and covalent bond in an easy-to-understand way. Letâs explore their definitions, examples, and key differences!
What is Ionic Bond?
“An ionic bond forms when one atom transfers electrons to another, creating oppositely charged ions.”
Example,
Sodium (Na) donates an electron to Chlorine (Cl), forming Sodium Chloride (NaCl).
What is Covalent Bond?
“A covalent bond forms when two atoms share electrons to achieve stability.”
Example,
Two hydrogen atoms share electrons with one oxygen atom, forming a water molecule (HâO).
Difference between Ionic Bond and Covalent Bond
| Aspect | Ionic Bond | Covalent Bond |
|---|---|---|
| Definition | Ionic bonds form when one atom transfers electrons to another, creating oppositely charged ions. | Covalent bonds form when two atoms share electrons to achieve stability. |
| Formation | Occurs between metals (donors) and non-metals (acceptors). | Occurs between non-metal atoms. |
| Electron Sharing | No sharing; electrons are transferred. | Electrons are shared equally or unequally between atoms. |
| Type of Attraction | Strong electrostatic forces between positively and negatively charged ions. | Strong shared electron cloud binds the nuclei of atoms together. |
| State of Matter | Mostly forms crystalline solids at room temperature. | Forms gases, liquids, or solids, depending on the molecule. |
| Melting/Boiling Points | High melting and boiling points due to strong ionic bonds. | Lower melting and boiling points compared to ionic compounds. |
| Solubility | Soluble in polar solvents like water. | Solubility depends on the polarity of the molecule (polar covalent dissolve in water, non-polar donât). |
| Electrical Conductivity | Conduct electricity when dissolved in water or molten. | Generally non-conductive, except in cases of polar covalent bonds in water. |
| Bond Strength | Strong but brittle. | Generally strong but flexible. |
| Example | Sodium chloride (NaCl): Sodium donates an electron to chlorine, forming Naâş and Clâğ ions. | Water (HâO): Hydrogen atoms share electrons with oxygen to form covalent bonds. |
| Polarity | Highly polar, as complete transfer of electrons creates distinct charges. | Polarity depends on the difference in electronegativity of the bonded atoms. |
| Structure | Forms a rigid lattice structure in the solid state. | Forms discrete molecules with specific geometries. |
| Bond Formation Energy | Requires more energy to form and break bonds. | Requires relatively less energy to form and break bonds. |
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