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Arrange the elements according to atomic radius Largest radius Ar P S Si Mg Al Na Smallest radius
Answer “Arrange these elements according to atomic radius”.
The periodic table can be described as a progression in elements according to their increasing atomic number. These elements can be either metals or metalloids. The atomic radius is one of the most important periodic trends.
Atomic radius refers to the distance between the nucleus of the nucleus, and the valence shell. Atomic radius increases on moving downwards in a group and decreases on moving in the right in a period from left.
The position of an element in the periodic table determines its atomic radius. Generally, as we go down in a particular group, we see a rise in the atomic radius.
The distance between the nucleus’ inner core and the outermost shell is called the atomic radius. This trend can vary depending on the time period or the group.
The effective nuclear charge is decreased when there are more shells of an atom in a group. The lower attraction between nucleus and electrons can cause an increase in the atomic radii. As the atomic number increases, so does the effective nuclear charge. All atoms have the same number shells. This results in a decrease in atomic radii.
All of these elements are included in the same period.
Along the period, atomic radii decrease.
All these facts allow us to arrive at the following order of decreasing atomic radiations:
Na, Mg, Al, Si, P, S, Cl, Ar.
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