Ionic Compounds: Formation MCQs Quiz | Class 10
This quiz covers Class X Science (Code 086), Unit I: Chemical Substances – Nature and Behaviour, focusing on the topic Ionic Compounds: Formation. It includes questions on ion formation (cations and anions), electron transfer, electrostatic forces, and the nature of ionic bonds. Submit your answers to check your score and download the PDF answer key.
Overview of Ionic Compound Formation
Ionic compounds are chemical compounds formed by the complete transfer of electrons from a metal to a non-metal. This process results in the formation of oppositely charged ions which are held together by strong electrostatic forces of attraction, known as ionic bonds or electrovalent bonds.
Key Concepts
- Cation Formation: Metals lose electrons from their valence shell to achieve a stable octet configuration (noble gas structure), forming positively charged ions called cations (e.g., Sodium loses 1 electron to become Na+).
- Anion Formation: Non-metals gain electrons to complete their valence shell, forming negatively charged ions called anions (e.g., Chlorine gains 1 electron to become Cl-).
- Electrostatic Force: The strong force of attraction between the positive cation and negative anion holds the compound together.
- Charge Balance: The total positive charge equals the total negative charge, making the ionic compound electrically neutral as a whole.
Example: Formation of Magnesium Chloride (MgCl2)
Magnesium (Atomic number 12) has electronic configuration 2, 8, 2. It loses 2 electrons to form Mg(2+). Chlorine (Atomic number 17) has configuration 2, 8, 7. It requires 1 electron. Therefore, one Magnesium atom transfers two electrons to two Chlorine atoms (one to each), resulting in the formula MgCl2.
Practice Questions
- Why do ionic compounds have high melting points?
- Write the electron dot structure for Calcium Oxide (CaO).
- Identify the cation and anion in Potassium Chloride (KCl).
- Does Carbon form ionic bonds? Why or why not?
- Explain why ionic compounds conduct electricity in molten state but not in solid state.
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