Questions: Given the following information for element E, identify the element's group in the periodic table: The electron affinity is positive. The first ionization energy of E is less than the second ionization energy, which in turn is very much less than its third ionization energy A. Group 1A B. Group 2A C. Group 3A D. Group 8A

Solution Steps

The problem states that the electron affinity of element \( E \) is positive. Electron affinity is the energy change when an electron is added to a neutral atom. A positive electron affinity indicates that the atom does not readily accept an additional electron, which is typical for elements that are not highly electronegative.

The first ionization energy is less than the second, which is much less than the third. This pattern suggests that the element has two electrons in its outer shell that are relatively easy to remove, but removing a third electron requires significantly more energy. This is characteristic of elements in Group 2A, which have two valence electrons.

Given the information:

• Positive electron affinity suggests the element is not highly electronegative.
• The ionization energy pattern (first < second << third) is typical for elements with two valence electrons.

These characteristics align with elements in Group 2A of the periodic table, which are alkaline earth metals.

Final Answer