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प्रश्न
Arrange the following in increasing order of property indicated
F, Cl, Br, I (electron affinity)
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उत्तर
I < Br < F < Cl
Electron affinity decreases down the group due to increase in atomic size as it results in more distance between nucleus and last shell to which incoming electron enters. Hence, incoming electron feels less attraction from the nucleus.
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संबंधित प्रश्न
Element X is a metal with a valency 2, Y is 3 non- metal with a valency 3.
1) Write an equation to show how Y from an ion.
2) If Y is a diatomic gas, write an equation for the direct combination of X and Y to form a compound.
Define the term ‘electron affinity’.
Electron affinity values generally _______ across the periods left to right and ______ down the group top to bottom.
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.
What is electron affinity?
Among the Period 2 elements, the element which has high electron affinity is
The changes in the properties of elements on moving from left to right across a period of the Periodic Table. For the property, choose the correct answer.
The electron affinity of elements in groups 1 to 7:
On descending a group, ______ in ionisation potential as well as electron affinity ______ oxidising capacity.
Arrange the following as per instruction given in the bracket.
Cl, F, Br, I (increasing electron affinity)
