Question

Compare the trends of the ionization energy and electron affinity within the group and across the period with the help of examples. Mention at least four valid reasons under each headin​

Answer 1

Answer:

Electronegativity measures an atom's tendency to attract and form bonds with electrons. This property exists due to the electronic configuration of atoms. Most atoms follow the octet rule (having the valence, or outer, shell comprise of 8 electrons). Because elements on the left side of the periodic table have less than a half-full valence shell, the energy required to gain electrons is significantly higher compared with the energy required to lose electrons. As a result, the elements on the left side of the periodic table generally lose electrons when forming bonds. Conversely, elements on the right side of the periodic table are more energy-efficient in gaining electrons to create a complete valence shell of 8 electrons. The nature of electronegativity is effectively described thus: the more inclined an atom is to gain electrons, the more likely that atom will pull electrons toward itself.

Answer 2

Answer:

its help the build up

Explanation:

The ionization energy of the elements within a period generally increases from left to right. This is due to valence shell stability.The ionization energy of the elements within a group generally decreases from top to bottom. This is due to electron shielding.The noble gases possess very high ionization energies because of their full valence shells as indicated in the graph. Note that helium has the highest ionization energy of all the elements.