For each of these Lewis symbols, indicate the group in the periodic table in which the element X belongs: (a)

Verified step by step guidance

1. Identify the number of valence electrons represented in the Lewis symbol for element X.
2. Recall that the number of valence electrons corresponds to the group number for main group elements in the periodic table.
3. Determine the group number by matching the number of valence electrons to the appropriate group in the periodic table.
4. Consider that elements in the same group have similar chemical properties due to having the same number of valence electrons.
5. Conclude which group in the periodic table element X belongs to based on the number of valence electrons.

Key Concepts

Lewis Symbols

Lewis symbols are a way to represent the valence electrons of an atom using dots around the element's symbol. Each dot corresponds to a valence electron, and the arrangement of these dots can help predict how an element will bond with others. Understanding Lewis symbols is essential for determining the group of an element in the periodic table, as elements in the same group typically have similar valence electron configurations.

Periodic Table Groups

The periodic table is organized into columns known as groups, where each group contains elements with similar chemical properties and the same number of valence electrons. For example, Group 1 elements have one valence electron, while Group 17 elements have seven. Identifying the group of an element based on its Lewis symbol involves counting the dots and relating that to the periodic table's structure.

Valence Electrons

Valence electrons are the outermost electrons of an atom and play a crucial role in chemical bonding and reactivity. The number of valence electrons determines how an element interacts with others, influencing its placement in the periodic table. By analyzing the Lewis symbol, one can ascertain the number of valence electrons and thus identify the corresponding group in the periodic table.