How are solid classified on the basic of an intermolecular forces
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Solids are classified into four types; based on the intermolecular forces operating in them.
Molecular Solids
Ionic Solids
Metallic Solids
Covalent solids
1 - Molecular Solids – Solids having molecules as their constituent particles are called Molecular solids. For, example, Hydrogen, Chlorine, Water, HCl, solid carbon dioxide, sucrose, etc.
Molecular solids are classified into three types on the basis of their bond:
Non-Polar Molecular solids
Polar Molecular Solids
Hydrogen Bonded Molecular Solids
(a) Non Polar Molecular Solids – Solids which are comprised of atoms only, such as helium and argon or molecules; formed because of the non polar covalent bonds are known as Non-Polar Molecular Solids. For example – H2, Cl2, I2, etc.
Characteristic of Non-Polar Molecular Solids –
The molecules of non-polar molecular solids are held together by weak dispersion forces or London forces.
Non-Polar Molecular Solids are soft.
Non-polar molecular solids are non-conductor of electricity.
Non-polar molecular solids have low melting points.
Non-polar molecular solids are usually in liquid or gaseous state at the room temperature and pressure.
(b) Polar Molecular Solids – The solids which are formed by polar covalent bonds are known as Polar Molecular solids. For example – HCl, SO2, NH3, etc.
Characteristic of Polar Molecular Solids –
The molecules in polar molecular solids are held together with dipole-dipole interactions.
Polar molecular solids are generally soft in nature.
Polar molecular solids are non-conductor of electricity.
Polar molecular solids have higher melting points in comparison to non-polar molecular solids.
Most of the polar molecular solids are gases or liquids at room temperature and pressure.
Solid SO2 and solid NH3 are some examples of polar molecular solids.
(c) Hydrogen bonded Molecular Solids – The molecules of hydrogen bonded molecular solids contain polar covalent bond between H and O, F or N. In solids such as H2O (ice) molecules are bound together strongly with hydrogen bond. HF, H2O (ice), etc are the examples of hydrogen bound molecular solids.
Characteristics –
Hydrogen bound molecular solids are generally volatile liquid or soft solids at room temperature and pressure.
Hydrogen bound molecular solids are non-conductor of electricity.
2 - Ionic Solids – Solids, in which ions are the constituent particles, are called ionic solids. These solids are formed because of three dimensional arrangements of cations and anions bound together with strong electrostatic forces (coulombic forces). For example NaCl.
Characteristics of Ionic Solids –
High melting and boiling points.
Non-conductor of electricity in solid state.
Conductor of electricity in molten state.
Conducted electricity when dissolved in water.
3 - Metallic Solids – All metals are referred as Metallic solids. Their constituent particles are positive ions. These positive ions are surrounded by free moving electrons. For example – iron, aluminium, etc.
Characteristics –
High melting points.
Good conductors of electricity and heat.
Lustrous, and are of specific colors.
Hard but malleable and ductile in nature
4 - Covalent Solids – Crystalline solids are formed by non metals because of formation of covalent bonds between the adjacent molecules throughout the crystal. These are also known as Network Solids. These are also called giant molecules. For example – diamond, graphite, silicon carbide, etc.
Characteristic of Covalent Solids –
They are very hard and brittle except graphite which is soft.
Very high melting points.
Do not conduct electricity except graphite.
Also called giant molecules.