Question:
Identify the incorrect set from the following:
Identify the incorrect set from the following:
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Ionic solids like MgO have high melting points and conduct electricity in molten state, unlike covalent solids.
Updated On: May 18, 2025
- SiO₂, covalent solid, insulator, high melting point
- MgO, covalent solid, insulator, high melting point
- H₂O (ice), molecular solid, insulator, low melting point
- Ag(s), metallic solid, conductor, high melting point
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The Correct Option is B
Approach Solution - 1
Step 1: Understanding the Classifications
- SiO₂ is correctly classified as a covalent solid.
- MgO is incorrectly classified as a covalent solid (it is an ionic solid).
- H₂O (ice) is correctly classified as a molecular solid.
- Ag is correctly classified as a metallic solid.
Thus, MgO's classification is incorrect.
- SiO₂ is correctly classified as a covalent solid.
- MgO is incorrectly classified as a covalent solid (it is an ionic solid).
- H₂O (ice) is correctly classified as a molecular solid.
- Ag is correctly classified as a metallic solid.
Thus, MgO's classification is incorrect.
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Approach Solution -2
Step 1: Understanding the Classifications of Solids
- Solids can be broadly classified into four types based on the nature of particles and bonding: **covalent solids, ionic solids, molecular solids, and metallic solids**.
Step 2: Classification of SiO₂ (Silicon Dioxide)
- SiO₂ forms a three-dimensional network where atoms are connected by strong covalent bonds throughout the structure.
- This extended network structure gives it high melting points and hardness, typical of **covalent solids**.
- Hence, SiO₂ is correctly classified as a covalent solid.
Step 3: Classification of MgO (Magnesium Oxide)
- MgO consists of Mg²⁺ and O²⁻ ions held together by strong electrostatic (ionic) forces in a crystal lattice.
- These ionic bonds result in properties such as high melting points, electrical conductivity when molten, and brittleness, characteristic of **ionic solids**.
- Therefore, classifying MgO as a covalent solid is incorrect; it should be classified as an **ionic solid**.
Step 4: Classification of H₂O (Ice)
- Solid water (ice) consists of discrete H₂O molecules held together by hydrogen bonds and van der Waals forces.
- These intermolecular forces are weaker than ionic or covalent bonds, leading to relatively low melting points.
- Ice is thus correctly classified as a **molecular solid**.
Step 5: Classification of Ag (Silver)
- Silver atoms are arranged in a lattice where valence electrons are delocalized over the entire structure.
- This “sea of electrons” accounts for metallic properties such as electrical conductivity, malleability, and ductility.
- Hence, silver is correctly classified as a **metallic solid**.
Step 6: Summary and Conclusion
- SiO₂ is a covalent solid due to strong covalent networks.
- MgO should be classified as an ionic solid, not a covalent solid.
- H₂O (ice) is a molecular solid with hydrogen bonding.
- Ag is a metallic solid with delocalized electrons.
- The only incorrect classification in the list is that of MgO.
- Solids can be broadly classified into four types based on the nature of particles and bonding: **covalent solids, ionic solids, molecular solids, and metallic solids**.
Step 2: Classification of SiO₂ (Silicon Dioxide)
- SiO₂ forms a three-dimensional network where atoms are connected by strong covalent bonds throughout the structure.
- This extended network structure gives it high melting points and hardness, typical of **covalent solids**.
- Hence, SiO₂ is correctly classified as a covalent solid.
Step 3: Classification of MgO (Magnesium Oxide)
- MgO consists of Mg²⁺ and O²⁻ ions held together by strong electrostatic (ionic) forces in a crystal lattice.
- These ionic bonds result in properties such as high melting points, electrical conductivity when molten, and brittleness, characteristic of **ionic solids**.
- Therefore, classifying MgO as a covalent solid is incorrect; it should be classified as an **ionic solid**.
Step 4: Classification of H₂O (Ice)
- Solid water (ice) consists of discrete H₂O molecules held together by hydrogen bonds and van der Waals forces.
- These intermolecular forces are weaker than ionic or covalent bonds, leading to relatively low melting points.
- Ice is thus correctly classified as a **molecular solid**.
Step 5: Classification of Ag (Silver)
- Silver atoms are arranged in a lattice where valence electrons are delocalized over the entire structure.
- This “sea of electrons” accounts for metallic properties such as electrical conductivity, malleability, and ductility.
- Hence, silver is correctly classified as a **metallic solid**.
Step 6: Summary and Conclusion
- SiO₂ is a covalent solid due to strong covalent networks.
- MgO should be classified as an ionic solid, not a covalent solid.
- H₂O (ice) is a molecular solid with hydrogen bonding.
- Ag is a metallic solid with delocalized electrons.
- The only incorrect classification in the list is that of MgO.
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