What conclusion can be drawn from the statement that an element has a high ionization energy and small atomic size?A) The element is most likely from Group 1A or 2A and in period 1 or 2

B) The element is most likely from Group 2A or 3A and in period 2 or 3.

C) The element is most likely from Group 4A or 5A and in period 4 or 5.

D) The element is most likely from Group 6A or 7A and in period 6 or 7​

Answer:

The list of answer choices is wrong.

The correct list is:

A) The element is most likely from Group 1A or 2A and in period 1 or 2.

B) The element is most likely from Group 2A or 3A and in period 6 or 7.

C) The element is most likely from Group 4A or 5A and in period 4 or 5.

D) The element is most likely from Group 6A or 7A and in period 2 or 3.

The correct answer is:

• Option D) The element is most likely from Group 6A or 7A and in period 2 or 3.

Explanation:

The ionization energy increases from left to right on the periodic table. So the elements with higer ionization energies are in the right end of the table. The right most columns are 6A (16) and 7A(17). The column 8A (18) which is that of the noble gases is not normally taken into acccount for this predictions because noble gases are nearly inert.

Hence, the fact that the statement indicates high ionization energy suggests that the element is most likely from group 6A or 7A.

The atomic radius increases from top to bottom, so the smallest elements are in the top rows, which is the periods 1, 2, or 3. The period 1 only has two elements, hydrogen in group 1 and helium in group 8A, so they are not considered in the choices. Thus, that leaves you with the periods 2 or 3.

Adding the two considerations, the conclusion is that the element is most likely from group 6A or 7A and in period 2 or 3.

Answer:

Explanation:

The answer is A) The element is most likely from Group 1A or 2A and in period 1 or 2