Want this question answered?
from left to right the atomic radius decreases as the electrons that get added are added in the same shell as they are in the same period. the shielding effect remains constant but the proton number increases which inturn increases the effective nuclear pull on the electrons bringing the electrons closer to the nuclei hence decreasing the radius of the atom
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
The atomic radius decrease, with several exceptions in periods 6 and 5.
decreases
the atomic radius decreses from left to right in periodic table due to increase in the number of succesive element the electrons of the outermost shell are more attracted towards nucleus and the atomic radius or atomic size decreases.
The atomic radius decrease from left to right.
An increase in atomic number would be accompanied by a decrease in radius, and an increase in electronegativity.
Atomic radii generally decrease across a period from left to right due to increasing nuclear charge pulling electrons closer to the nucleus. Atomic radii tend to increase down a group due to additional electron shells being added, increasing the distance between the nucleus and outermost electrons. These trends are not perfectly consistent and can be influenced by other factors such as electron configuration.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
In a group the ionization energy decrease when the atomic radius increase; in a period this relation is not generally valid.
Argon doesnt have the smallest atomic radius, its chlorine.Argon has the largest atomic radius in period 3.