Concept explainers
(a)
Interpretation:Thecharacteristics that can be used to distinguish between crystalline and amorphous solids needs to be explained.
Concept Introduction:
Solid state has strong intermolecular force of attraction between particles whereas the gaseous particles have weakest intermolecular forces between particles. Due to intermolecular force of attraction between particles, different interconversions are possible between these three states like evaporation, condensation, sublimation, etc.
On the basis of structure and intermolecular interactions, solids can further classified as:
- Crystalline solids - Molecular solids, network solid, ionic solids, metallic solids
- Amorphous solid
(a)
Answer to Problem 33E
| Crystalline solid | Amorphous solid |
| Particles have ordered arrangement of particles. | Particles do not have ordered arrangement of particles. |
| They have fix melting and boiling point. | They do not have fix melting and boiling points. |
| Example; diamond | Example; glass |
Explanation of Solution
Crystalline solids have well defined ordered arrangement of particles whereas amorphous solids have disordered at an atomic level because particles are held together in a completely random formation.
Because of the ordered arrangement, crystalline solids have fix melting and boiling point, whereas amorphous solids melt and boil at certain range of temperature.
Diamond is an example of crystalline solid whereas glass is an example of amorphous solid.
(b)
Interpretation:The characteristics that can be used to distinguish between ionic and molecular solids needs to be explained.
Concept Introduction:
Solid state has strong intermolecular force of attraction between particles whereas the gaseous particles have weakest intermolecular forces between particles. Due to intermolecular force of attraction between particles, different interconversions are possible between these three states like evaporation, condensation, sublimation, etc.
On the basis of structure and intermolecular interactions, solids can further classified as:
- Crystalline solids - Molecular solids, network solid, ionic solids, metallic solids
- Amorphous solid
(b)
Answer to Problem 33E
| Ionic solid | Molecular solid |
| These solids are composed of ions | These solids are composed of molecules. |
| Ions are held together with ionic bonds. | Molecules are held together with weak intermolecular forces. |
| Example; NaCl | Example; water, CO2 |
| They usually have very high melting and boiling points. | They have less melting and boiling points. |
Explanation of Solution
Crystalline solids have well defined ordered arrangement of particles. Ionic solids and molecular solids are types of crystalline solids. Ionic solids are mainly composed of oppositely charged ions; cation and anion. Here due to opposite charges, they are held together with strong ionic bonds. Molecular solids are composed of molecules which have weak intermolecular forces. In these solids, the constituent particle must be some molecule. Water and CO2 are good examples of molecular solids.
(c)
Interpretation:The characteristics that can be used to distinguish between network and molecular solids needs to be explained.
Concept Introduction:
Solid state has strong intermolecular force of attraction between particles whereas the gaseous particles have weakest intermolecular forces between particles. Due to intermolecular force of attraction between particles, different interconversions are possible between these three states like evaporation, condensation, sublimation, etc.
On the basis of structure and intermolecular interactions, solids can further classified as:
- Crystalline solids - Molecular solids, network solid, ionic solids, metallic solids
- Amorphous solid
(c)
Answer to Problem 33E
| Network solid | Molecular solid |
| These solids are composed of atoms. | These solids are composed of molecules. |
| Atoms are held together with covalent bonds to form cross network. | Molecules are held together with weak intermolecular forces. |
| Example; diamond, graphite | Example; water, CO2 |
| They usually have very high melting and boiling points. | They have less melting and boiling points. |
Explanation of Solution
Crystalline solids have well defined ordered arrangement of particles. Network solids and molecular solids are types of crystalline solids. Network solids are mainly composed of atoms which are bonded through covalent bonds to form a large cross network. Molecular solids are composed of molecules which have weak intermolecular forces. In these solids, the constituent particle must be some molecule. Water and CO2 are good examples of molecular solids.
(d)
Interpretation:The characteristics that can be used to distinguish between network and metallic solids needs to be explained.
Concept Introduction:
Solid state has strong intermolecular force of attraction between particles whereas the gaseous particles have weakest intermolecular forces between particles. Due to intermolecular force of attraction between particles, different interconversions are possible between these three states like evaporation, condensation, sublimation etc.
On the basis of structure and intermolecular interactions, solids can further classified as:
- Crystalline solids - Molecular solids, network solid, ionic solids, metallic solids
- Amorphous solid
(d)
Answer to Problem 33E
| Network solid | Metallic solid |
| These solids are composed of atoms. | These solids are composed of metal atoms. |
| Atoms are held together with covalent bonds to form cross network. | Metal atoms are held together with metallic bonds |
| Example; diamond, graphite | Example; Cu, Fe |
| They usually have very high melting and boiling points. | They are conductor and malleable. |
Explanation of Solution
Crystalline solids have well defined ordered arrangement of particles. Network solids and molecular solids are types of crystalline solids. Network solids are mainly composed of atoms which are bonded through covalent bonds to form a large cross network. Metallic solids are composed of metal atoms which are bonded with metallic bonds. Metallic bonds are the electrostatic force of attraction between positive charge metal ions and free mobile electrons. Because of that they are good conductor of electricity.
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Chapter 16 Solutions
Chemical Principles
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