Define atomic radii discuss its trend in periodic table?
Question: Define atomic radii discuss its trend in periodic table?
Atomic radii are the distances between the nuclei of atoms and their outermost electrons. They are measured in picometers (pm) or angstroms (Å). Atomic radii vary depending on the type of bond and the number of atoms involved. For example, covalent radii are the distances between two atoms that share electrons in a covalent bond, while metallic radii are the distances between two atoms in a metallic lattice. Atomic radii also depend on the number of protons and electrons in an atom, as well as the arrangement of electrons in shells and subshells.
One way to discuss the trend of atomic radii in the periodic table is to compare the elements in the same group (vertical column) or period (horizontal row). Generally, atomic radii increase from top to bottom in a group, because each successive element has an additional shell of electrons that increases the size of the atom. However, atomic radii decrease from left to right in a period, because each successive element has an additional proton that increases the nuclear charge and pulls the electrons closer to the nucleus. There are some exceptions to this trend, such as the lanthanides and actinides, which have similar atomic radii due to the shielding effect of their inner f-electrons.
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