(i). Low I.E. Values
Ionization Energy is the minimum amount of energy which is required to eject the electron completely from the outermost shell of neutral gaseous atom so as to form a positive ion. Thus, smaller the I.E., easier is to remove the electron to form cation. Hence ionic bond is readily formed.
Ionization Energy is the minimum amount of energy which is required to eject the electron completely from the outermost shell of neutral gaseous atom so as to form a positive ion. Thus, smaller the I.E., easier is to remove the electron to form cation. Hence ionic bond is readily formed.
(ii). High E.A. Values
The atom which gains the electron must possess strong tendency to accept the additional electrons. Halogens possess high electron affinity & thus show high tendency for ionic bonding. The elements of oxygen family also exhibit remarkable electron affinity & form ionic compounds but not so readily as halogens.
(iii). High Lattice Energy
The atom which gains the electron must possess strong tendency to accept the additional electrons. Halogens possess high electron affinity & thus show high tendency for ionic bonding. The elements of oxygen family also exhibit remarkable electron affinity & form ionic compounds but not so readily as halogens.
(iii). High Lattice Energy
The lattice energy is defined as the energy released when one mole of an ionic compound is formed from the gaseous ions. The higher the value of lattice energy of the resulting ionic compound, greater will be the ease of its formation.
An ionic bond is formed between a cation A and an anion B. How would the energy of the ionic bond be affected by the following changes?
ReplyDelete(a) doubling the radius of a.
(b) Explain the ionic character of the lithium-to-fluorine bond in LiF.
y
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