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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
Draw an electron dot diagram to show the formation of the following compound:
Methane
[H = 1, C = 6]
Draw an electron dot diagram to show the formation of each of the following compounds:
Magnesium Chloride
[H = 1, C = 6, Mg = 12, Cl = 17]
Arrange the elements of second period in increasing order of their electron affinity. Name the elements which do not follow the trend in this period.
An element in period 3 whose electron affinity is zero.
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 element A is more than that of element C.
- lonization energy of element C is less than that of element A.
- Electron affinity of B is zero.
State whether the following statement is true or false
The elements with higher electron affinity have higher ionization potential.
Choose the correct answer:
Among the period 2 elements the one which has high electron affinity is
In a period, increase in electron affinity increases ______.
The electron affinity of an element X is greater than that of element Y.
State whether X is likely to be placed to the left or to the right of Y in the periodic table.
Among period 2 elements A, B, C and D, the one which has highest electron affinity is ______.
