noble gasses have a full outer shell of 8 electrons which makes them fairly stable as they have no more room in that shell for another electron nor do they have the need to share there electrons with another element to gain a full outer shell
The atomic radius decrease, with several exceptions in periods 6 and 5.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
decreases
The atomic radius decrease from left to right.
When there is an anion (negative charge) the radius will be larger because it is more full whereas it will be smaller if it is a positive charge because of less electrons. ex largest to smallest radius (K-,K, K+)
The atomic radius decrease, with several exceptions in periods 6 and 5.
The atomic radius decreases as you go from left to right. or atomic radius cation radius && anion radius -barbie=]
Atomic radius decreases horizontally in periodic table. This is due to increase in nuclear charge.
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
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.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
decreases
Decreases. Look at the images under atomic radius, on wikipedia.
An increase in atomic number would be accompanied by a decrease in radius, and an increase in electronegativity.
The atomic radius decrease from left to right.
Going across a row in the peiodic table, the atoms have more protons and electrons causing a stronger attractive force, pulling the electrons closer to the nucleus, making the atomic radius decrease. As a new shell is added ( next row down) the atomic radius increases
In a group the ionization energy decrease when the atomic radius increase; in a period this relation is not generally valid.