Question

Several periodic trends are evident as we move across a row or period. In this case, compare the trend in atomic radii of the elements to the trend in electronegativity.

A) The atomic radii and electronegativity both increase.
B) The atomic radii and electronegativity both decrease.
C) The atomic radii increase and electronegativity decreases.
D) The atomic radii decrease and electronegativity increases.

Answer 1

D) The atomic radii decrease and electronegativity increases.

Step-by-step explanation:

Atomic radii and electronegativity trend across period:

As we move from left to right across the periodic table the number of valance electrons in an atom increase. The atomic size tend to decrease in same period of periodic table because the electrons are added with in the same shell. When the electron are added, at the same time protons are also added in the nucleus. The positive charge is going to increase and this charge is greater in effect than the charge of electrons. This effect lead to the greater nuclear attraction and electronegativity increases.

The electrons are pull towards the nucleus and valance shell get closer to the nucleus. As a result of this greater nuclear attraction atomic radius decreases and ionization energy increases because it is very difficult to remove the electron from atom and more energy is required.