Atoms have a pattern in common charge due to the relationship between their valence electrons and the formation of stable electron configurations.
The valence electrons of an atom are the electrons in its outermost energy level or shell, specifically in the s and p orbitals. These electrons play a crucial role in determining the chemical properties and reactivity of the atom.
Atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration, often following the octet rule (except for elements in the first period or hydrogen). The octet rule states that atoms are most stable when they have a full valence shell containing 8 electrons.
When atoms gain or lose electrons, they form ions with a positive or negative charge, respectively. The charge of an ion is related to the number of electrons gained or lost. For example, if an atom gains one or more electrons, it becomes negatively charged (anion), and if it loses one or more electrons, it becomes positively charged (cation).
The common charge of an atom refers to the most common or predictable charge that an atom of a particular element is likely to have when it forms an ion. This common charge is often determined by the number of valence electrons needed to reach a stable electron configuration.
Elements within the same group (vertical column) of the periodic table have the same number of valence electrons and tend to exhibit similar chemical properties and common charges. For example, elements in Group 1 (alkali metals) tend to lose one electron to achieve a stable configuration, resulting in a common charge of +1. Elements in Group 17 (halogens) tend to gain one electron to achieve a stable configuration, resulting in a common charge of -1.
In summary, the pattern in common charge among atoms relates to their valence electrons and the tendency to gain or lose electrons in order to achieve a stable electron configuration, following the octet rule. Elements in the same group of the periodic table often share similar common charges due to their similar valence electron configurations.