Write the Lewis symbol for each atom or ion. d. S2-

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Identify the number of valence electrons in a neutral sulfur (S) atom. Sulfur is in Group 16 of the periodic table, which means it has 6 valence electrons.

Determine the charge of the ion. For S2-, the ion has gained 2 additional electrons, giving it a total of 8 valence electrons.

Draw the Lewis symbol for sulfur. Start with the symbol for sulfur, 'S', and surround it with dots representing the 6 valence electrons of a neutral sulfur atom.

Add the extra electrons due to the 2- charge. Place two more dots around the sulfur symbol, ensuring that electrons are paired as much as possible to reflect the gain of electrons.

The final Lewis symbol for S2- should show the sulfur atom surrounded by eight electrons (four pairs), indicating a full outer shell typical of a stable ion.

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주요 개념

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Lewis Symbols

Lewis symbols, also known as Lewis dot diagrams, represent the valence electrons of an atom or ion. Each dot corresponds to a valence electron, and the arrangement of these dots around the chemical symbol indicates how the atom can bond with others. Understanding Lewis symbols is essential for visualizing electron sharing and transfer in chemical bonding.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom interacts with others. For sulfur (S), which is in group 16 of the periodic table, there are six valence electrons. When forming the sulfide ion (S2-), sulfur gains two additional electrons, resulting in a total of eight valence electrons, which is a stable configuration.

Ionic Charge

The ionic charge of an atom or ion indicates the difference between the number of protons and electrons. In the case of the sulfide ion (S2-), the negative charge signifies that sulfur has gained two electrons, leading to a total of 18 electrons compared to its 16 protons. This charge is important for understanding the ion's behavior in chemical reactions and its interactions with other ions.