How many valence electrons does each of the following contribute to a Lewis structure?
(g) S

Verified step by step guidance

1. Step 1: Recall the concept of valence electrons. Valence electrons are the electrons in the outermost shell of an atom that are involved in chemical bonding. The number of valence electrons for an element can be determined from its position in the periodic table.
2. Step 2: Locate sulfur (S) on the periodic table. Sulfur is in Group 16 (also known as Group VI-A), which means it has six valence electrons.
3. Step 3: Write the electron configuration for sulfur to confirm the number of valence electrons. Sulfur has an atomic number of 16, so its electron configuration is: ${\mathrm{1s}}^2{\mathrm{2s}}^2{\mathrm{2p}}^6{\mathrm{3s}}^2{\mathrm{3p}}^4.\; The\; electrons\; in\; the\; 3s\; and\; 3p\; orbitals\; (a\; total\; of\; 6)\; are\; the\; valence\; electrons.$
4. Step 4: Understand that these six valence electrons are the ones sulfur contributes to a Lewis structure. In a Lewis structure, these electrons are represented as dots around the sulfur atom.
5. Step 5: Conclude that sulfur contributes six valence electrons to a Lewis structure, which is consistent with its group number and electron configuration.

Key Concepts

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for determining how an atom will bond with others. In the context of Lewis structures, these electrons are represented as dots around the chemical symbol of the element. The number of valence electrons varies by element and is determined by its position in the periodic table.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw and interpret Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Sulfur's Valence Electrons

Sulfur (S) is located in group 16 of the periodic table and has six valence electrons. This is important for constructing its Lewis structure, as these electrons will participate in bonding with other atoms. Recognizing the number of valence electrons helps in predicting how sulfur will interact with other elements in chemical reactions.