Explain how the period in which an element is located related to the number of shells that contain electrons.
Question: Explain how the period in which an element is located related to the number of shells that contain electrons.
The period number in the periodic table directly corresponds to the number of electron shells (energy levels) that contain electrons in an atom of an element. Here's how this relationship works:
- Periods: The periodic table is organized into horizontal rows called periods. Each period indicates the number of electron shells present in the elements of that row.
- Shells and Electrons:
- Elements in Period 1 (e.g., Hydrogen and Helium) have only one electron shell occupied.
- Elements in Period 2 (e.g., Lithium to Neon) have electrons in two shells.
- Elements in Period 3 (e.g., Sodium to Argon) have electrons in three shells, and so on.
This means that as you move down the periodic table, the number of occupied electron shells increases by one with each successive period.
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