FAJANS RULES PDF

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When a cation approaches an anion, the electron cloud of the anion is attracted towards a cation and hence gets distorted. The effect is called polarisation of the anion. The greater is the polarisation produced, more is the neutralisation of the charges and hence the ionic character decreases or the covalent character increases.

The polarising power of the cation and the polarisability of the anion and hence the formation of covalent bond depends on:. Covalent character of lithium halides is in the order:. Larger the charge on the cation, greater is its polarising power. Hence covalent character increases.

If two cations have the same size and charge, then the one with 18 electrons in the outermost shell has greater polarising power than the other with 8 electrons in the outermost shell. They usually consists of molecules rather than ions. Hence, atoms in a molecule can take up different directional arrangement and thus show structural and stereoisomerism. University and has many years of experience in teaching.

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Fajans' rules

According to this rule covalent character is more , when :. In ionic compound , cation attracts the electrons of anion towards itself. The ability of cation to attract the electrons of anion is called polarizing power. The electrons of anion get attracted towards the cation. Due to this, anion is distorted.

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Fajan’s Rules

When a cation approaches an anion, the electron cloud of the anion is attracted towards a cation and hence gets distorted. The effect is called polarisation of the anion. The greater is the polarisation produced, more is the neutralisation of the charges and hence the ionic character decreases or the covalent character increases. The polarising power of the cation and the polarisability of the anion and hence the formation of covalent bond depends on:. Covalent character of lithium halides is in the order:.

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Fajans' Rules for Chemical Bonds

By using our site, you acknowledge that you have read and understand our Cookie Policy , Privacy Policy , and our Terms of Service. Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. It only takes a minute to sign up. Fajans' rules note the difference were formulated in by Kazimierz Fajans.

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Fajan’s rule

In inorganic chemistry , Fajans' rules , formulated by Kazimierz Fajans in , [1] [2] [3] are used to predict whether a chemical bond will be covalent or ionic , and depend on the charge on the cation and the relative sizes of the cation and anion. They can be summarized in the following table:. The "size" of the charge in an ionic bond depends on the number of electrons transferred. That positive charge then exerts an attractive force on the electron cloud of the other ion, which has accepted the electrons from the aluminium or other positive ion. Two contrasting examples can illustrate the variation in effects.

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