Not for electron affinity but i have for electronegativity.
i.e. फोन कल
F>O>N>Cl
and for electron affinity just reverse it.

Electron affinity is defined as the amount of energy released when an electron is added to a neutral atom to form a negative ion. Remembering electron affinities can be challenging, but there are some shortcut tricks that can help make the task easier. Here are some strategies to remember electron affinities:

Understanding the Concept:
Before diving into the shortcuts, it is important to have a clear understanding of the concept of electron affinity. Remember that electron affinity is a measure of an atom's tendency to attract an electron. A higher electron affinity indicates a stronger attraction for an electron.

Shortcut Tricks:

1. Group Trends:
- Group 1 elements (alkali metals) have low electron affinities. They readily lose electrons to form positive ions, so their electron affinity values are generally low.
- Group 7 elements (halogens) have high electron affinities. They strongly attract electrons to achieve a stable octet, so their electron affinity values are generally high.

2. Periodic Trends:
- Electron affinity generally increases from left to right across a period. This is because as you move from left to right, the atomic radius decreases and the effective nuclear charge increases, leading to a stronger attraction for an electron.
- There are some exceptions to this trend, such as the electron affinities of group 2 elements (alkaline earth metals) being slightly lower than expected due to their relatively larger atomic size.

3. Noble Gases:
- The noble gases (group 18 elements) have a complete octet and do not readily accept additional electrons. Therefore, their electron affinities are close to zero or even slightly positive.

4. Metalloids:
- Metalloids (such as boron, silicon, and arsenic) have moderate electron affinities. They are located on the boundary between metals and nonmetals and exhibit properties of both.

5. Comparisons:
- Compare the electron affinities of elements within a group or period. For example, oxygen has a higher electron affinity than nitrogen because it is closer to achieving a stable octet.
- Compare the electron affinities of elements with similar atomic radii. Smaller atoms tend to have higher electron affinities due to the stronger attraction between the nucleus and the incoming electron.

In conclusion, understanding periodic trends, group characteristics, and making comparisons can help remember electron affinities. By applying these shortcut tricks, you can enhance your knowledge of electron affinities and their patterns in the periodic table.