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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.
The general trend is a decrease in size as you move from left to right . This is apparent in periods 2 and 3 but in period 4 and above we have the transition metals and these have some exceptions. This is due to the fact that as we moves from left to right along a period while the nuclear charge increases we are also adding extra electrons but the effective charge is mainly affected by the inner core electrons that "shield" the outer electrons. The effective nuclear charge, the charge felt by the outer electrons, increases across a period thus causing a contraction in the shell.
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.