As a general rule, when moving left to right on the periodic table the atomic radius decreases due to increasing electromagnetic attraction of the nucleus to the electrons.
The trend in atomic radii as you move down Group 1A elements is partially due to the increase in the number of electron shells or energy levels. As you move down the group, each subsequent element has an additional electron shell, leading to an overall larger atomic size.
Atomic radii generally decrease across periods 3 through 6 in the periodic table. This is because as you move from left to right across a period, the number of protons and electrons increases, leading to stronger attraction between the nucleus and the electrons, pulling the outer electrons closer to the nucleus, thus decreasing the atomic radius.
The atomic polarizability generally increases down a group and decreases across a period. This trend occurs because atoms with larger electron clouds (such as larger atomic size) are more easily polarized. Additionally, atoms with higher electronegativity tend to have lower polarizability due to stronger electron-electron repulsion.
The more energy levels that are occupied by electrons, the larger the atomic radius.
Xe has a larger atomic radius than Rb because atomic radius generally increases from top to bottom within a group in the periodic table. Xe is located below Rb in the periodic table, so it has more electron shells, resulting in a larger atomic radius.
The size of atom decreasing.
The atomic radii of main-group elements generally increase down a group. This is because as you move down a group, the principal quantum number increases, leading to larger atomic orbitals and a greater distance between the nucleus and the outermost electron, resulting in a larger atomic radius.
The more energy levels that are occupied by electrons, the larger the atomic radius.
Atomic radii increases moving down a group in the Periodic Table due to the increasing energy levels in the electron configuration and electrons filling in energy levels further away from the nucleus.
Atomic radii generally increase from top to bottom within a group (with more electron shells) and decrease from left to right across a period (due to increasing nuclear charge). This trend is influenced by the balance between the increasing positive nuclear charge and the increasing number of electron shells, which can shield the outer electrons from the nucleus.
The atomic radii of elements in period 3 from sodium to argon decrease due to a greater nuclear charge pulling electrons closer to the nucleus. This trend is similar to period 2 because both periods follow the same pattern of increasing nuclear charge as you move across the period, leading to a similar decrease in atomic radii.
Because the trend is the same. Atomic radius decreases from left to right across a period.
As you move across a row on the periodic table, the atomic radii becomes smaller due to the attraction between positive protons and negative electrons. As you move down a column, the radii increase due to the addition of valance electrons.
The radii of elements generally decrease as you move from left to right across a period in the periodic table. The radii then increase as you move down a group in the periodic table. This trend is due to changes in the atomic structure of the elements.
Atomic radii increases moving down a group in the Periodic Table due to the increasing energy levels in the electron configuration and electrons filling in energy levels further away from the nucleus.
The trend of atomic radius increases down a group on the periodic table. This occurs because each successive element down a group has another energy level. As more electrons are added, more energy levels are needed to hold the electrons.
The trend in atomic radii as you move down Group 1A elements is partially due to the increase in the number of electron shells or energy levels. As you move down the group, each subsequent element has an additional electron shell, leading to an overall larger atomic size.