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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.
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The trend in the atomic radii as you move down the group 1A elements is partially due to what?
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.
What trend in atomic radii do periods 3 through 6 have in common in the periodic table?
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.
What is the Atomic polarizability trend?
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.
What best explains the observed trend in atomic radii going down periodic table?
The more energy levels that are occupied by electrons, the larger the atomic radius.
Which atom has larger atomic radius Rb or Xe?
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.
What trend do you note for the atomic radii of period 3?
The size of atom decreasing.
What trend can be observed among the atomic radii of main-group elements down a group?
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.
What element does not fit atomic radii trend?
In the context of atomic radii trends, helium is an element that does not fit the general trend. Typically, atomic radii decrease across a period from left to right due to increasing nuclear charge, but helium has an unexpectedly small atomic radius compared to other noble gases. This is primarily due to its strong effective nuclear charge and the limited electron shielding in its small electron cloud, leading to a compact atomic size.
What explains the observed trend in the atomic radii going down the periodic table?
The more energy levels that are occupied by electrons, the larger the atomic radius.
What trend in atomic radius occurs down a group in the periodic table?
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.
How does atomic radii increase or decrease in the table?
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.
Why does the change for the atomic radii of elements in period 3 from sodium to argon look similar to period 2?
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.
What periodic trends exist for atomic radii?
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.
Why does the change for the atomic radii of the elements for period 3 from sodium to argon look similar to period 2?
Because the trend is the same. Atomic radius decreases from left to right across a period.
What happens to the radii of the elements between 2 highest peaks?
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.
Which best explains that observed trend in atomic radii going down the periodic table?
Atomic radii increase down a group in the periodic table primarily due to the addition of electron shells. As new electron shells are added, the distance between the nucleus and the outermost electrons increases, resulting in a larger atomic size. Furthermore, the increased shielding effect from the inner electron shells reduces the effective nuclear charge felt by the outer electrons, allowing them to spread out further from the nucleus. This combination of added shells and shielding leads to the observed trend of increasing atomic radii.
What trend in atomic radius occurs going down on the periodic table and why?
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.
