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प्रश्न
Explain the following:
The reducing power of element increases down in the group while decreases in a period.
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उत्तर
The reducing property depends on the ionisation potential and electron affinity of the elements. In a period, from left to right in a horizontal row of the periodic table, the atomic size decreases and the nuclear charge increases, so the electron affinity and ionisation energy both increase. Hence, the tendency to lose electrons decreases across the period from left to right and thus the reducing property also decreases across the period from left to right.
The electron affinity and ionisation potential decreases along the group from top to bottom. Hence, the tendency to lose electrons increases, and thus, the reducing property also increases along the group from top to bottom.
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संबंधित प्रश्न
Give one word or phrase for the following:
The amount of energy released when an atom in the gaseous state accepts an electron to form an anion.
Define the term ‘electron affinity’.
Give reason:
Electronegativity of chorine is higher than Sulphur?
An element in period 3, whose electron affinity is zero:
F, B, N, O (In the increasing order of electron affinity)
Why is the electron affinity of fluorine less than chlorine?
A, B, C are three elements in which B is an inert gas other than helium.With this information complete the following table.
| Element | Atomic number | No. of electrons in the valence shell | Group to which the element belongs |
| A | Z - 1 | ||
| B | Z | ||
| C | Z + 1 |
Also, explain the following : Electron affinity of B is Zero.
Explain
Halogens have high electron affinity.
On descending a group, ______ in ionisation potential as well as electron affinity ______ oxidising capacity.
