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write notes on diftenent types of atomic
radius.
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Three widely used definitions of atomic radius are: Van der Waals radius, ionic radius, and covalent radius.
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Types of Radius with Respect to the Types of Bonds
1. Van Der Waals Radius:
Van-der-Waals radii are determined from the contact distances between unbonded atoms in touching molecules or atoms.
2. Ionic Radius:
The ionic radius is the radius of an atom forming an ionic bond or an ion.
The electrons and nucleus are restricted by the atomic bonds and due to this reason the ions or atoms don’t have a specific shape.
The measuring unit for the ionic radius is Armstrong(A0) or picometers(pm). The characteristic radius ranges from 30 to 200 pm.
The ionic radius is not static but differs with respect to spin state of the electrons, coordination number and numerous other parameters.
Ionic size grows with increasing coordination number. The ionic size also grows for an ion with the high spin state of an electron than an ion with a low spin state of the electron.
The ion with a positive charge will have a smaller size than the ion with negative charge if we will take charge of the ion into consideration.
3. Metallic Radius:
The metallic radius is the radius of an atom joined by the metallic bond. The metallic radius is half of the total distance between the nuclei of two adjacent atoms in a metallic cluster.
4. Covalent Radius:
The covalent radius of an atom is stated as the radius of an atom which is under the covalent bond with another atom(s) of a similar element.
The covalent radius of an atom can be determined by measuring bond lengths between pairs of covalently-bonded atoms: if the two atoms are of the same kind, then the covalent radius is simply one half of the bond length.
Whilst this is straightforward for some molecules such as Cl2 and O2, in other cases, one has to infer the covalent radius by measuring bond distances to atoms whose radii are already known (e.g., a C–X bond, in which the radius of C is known).
Hope these notes will help.
1. Van Der Waals Radius:
Van-der-Waals radii are determined from the contact distances between unbonded atoms in touching molecules or atoms.
2. Ionic Radius:
The ionic radius is the radius of an atom forming an ionic bond or an ion.
The electrons and nucleus are restricted by the atomic bonds and due to this reason the ions or atoms don’t have a specific shape.
The measuring unit for the ionic radius is Armstrong(A0) or picometers(pm). The characteristic radius ranges from 30 to 200 pm.
The ionic radius is not static but differs with respect to spin state of the electrons, coordination number and numerous other parameters.
Ionic size grows with increasing coordination number. The ionic size also grows for an ion with the high spin state of an electron than an ion with a low spin state of the electron.
The ion with a positive charge will have a smaller size than the ion with negative charge if we will take charge of the ion into consideration.
3. Metallic Radius:
The metallic radius is the radius of an atom joined by the metallic bond. The metallic radius is half of the total distance between the nuclei of two adjacent atoms in a metallic cluster.
4. Covalent Radius:
The covalent radius of an atom is stated as the radius of an atom which is under the covalent bond with another atom(s) of a similar element.
The covalent radius of an atom can be determined by measuring bond lengths between pairs of covalently-bonded atoms: if the two atoms are of the same kind, then the covalent radius is simply one half of the bond length.
Whilst this is straightforward for some molecules such as Cl2 and O2, in other cases, one has to infer the covalent radius by measuring bond distances to atoms whose radii are already known (e.g., a C–X bond, in which the radius of C is known).
Hope these notes will help.
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