Question

The electron affinity of \[Be\] is almost similar to that of:
A.$He$
B.$B$
C.$Li$
D.$Na$

Answer 1

Hint:To answer this question, recall the trends in the periodic table. The modern periodic law developed by Moseley states that the physical and chemical properties of elements are the periodic function of their atomic number.

Complete step by step answer:
The systematic arrangement of elements according to Moseley’s law discloses certain periodic trends in the properties of elements. Beryllium atom occurs in the group of alkaline earth metal atoms and possesses an atomic number of 4. In powdered form it acts as a greyish-white hard light metal. It has a higher density compared to water. Can act as a toxin by inhalation. It can act as a carcinogenic agent and may also act as a metal allergen.
\[Be\] has filled s-subshell and thus possesses a highly stable configuration.
Hence, \[Be\] does not tend to accept electrons like \[He\] .

Hence, the correct option is A.

Note:
Let us summarize the trends of fundamental properties of an element: Atomic Radii and Ionic radii: The atomic radii and ionic radii of elements decrease while moving from left to right in a period. Ionization Enthalpy: Across a period in the periodic table, ionization energy generally increases. For the trend in a group, ionization enthalpy decreases from top to bottom. Electron gain enthalpy: Electron gain enthalpy becomes more negative as we move from left to right in a period. Electron gain enthalpy is negative when energy is released while accepting an electron. While it is positive when energy is supplied to an atom while adding an electron.