In the periodic table, the charges of ions formed by elements across a row (or period) generally correlate with their positions and the number of valence electrons they possess. As you move from left to right across a period, the number of valence electrons increases from one to eight. Elements on the left side, such as alkali metals (Group 1), tend to lose one electron, forming cations with a +1 charge (e.g., sodium forms Na⁺). Transitioning toward the right, elements like the chalcogens (Group 16) have six valence electrons and typically gain two electrons to achieve a stable electron configuration, resulting in anions with a -2 charge (e.g., oxygen forms O²⁻). This pattern reflects the elements' tendencies to achieve the stable electron configuration of noble gases by either losing or gaining electrons.
The periodic table is arranged by various patterns. Describe the pattern regarding charges of ions formed across a row? In three to five sentences, explain your reasoning and provide specific examples
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