As the elements in Period 2 of the Periodic Table are considered in succession from left to right, there is a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the

A. number of protons increases, and the number of shells of electrons remains the same

B. number of protons increases, and the number of shells of electrons increases

C. number of protons decreases, and the number of shells of electrons remains the same

D. number of protons decreases, and the number of shells of electrons increases

Question

Chemistry

Angel Nichols

2 September, 20:38

As the elements in Period 2 of the Periodic Table are considered in succession from left to right, there is a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the

A. number of protons increases, and the number of shells of electrons remains the same

B. number of protons increases, and the number of shells of electrons increases

C. number of protons decreases, and the number of shells of electrons remains the same

D. number of protons decreases, and the number of shells of electrons increases

+2

Answers (1)

Know the Answer?

Leslie Baker · Answer 1

The most probable answer, and the correct one, of the options presented in this problem would be A. The number of protons increases, and the number of shells of electrons remains the same.

As per what is used to classify the elements in the periodic table of elements, groups are utilized to easily identify them and easily remember the elements. Periods, on the other hand. are more or less left out in the cold. This might be because the only significant difference that it presents is that every period, which is the rows, all elements in that period has the same number of shells of electrons or we could refer to them as atomic orbitals.