Write the electron configuration for Ne. Then write the Lewis symbol for Ne and indicate which electrons from the electron configuration are included in the Lewis symbol.

Verified step by step guidance

1. Identify the atomic number of Neon (Ne), which is 10, indicating it has 10 electrons.
2. Write the electron configuration for Ne: Start by filling the 1s orbital, then the 2s orbital, and finally the 2p orbital until all 10 electrons are accounted for.
3. The electron configuration for Ne is: 1s^2 2s^2 2p^6.
4. Draw the Lewis symbol for Ne: Since Ne is a noble gas with a full outer shell, represent it with the element symbol 'Ne' surrounded by 8 dots, indicating the 8 valence electrons (2s^2 2p^6).
5. Explain that the Lewis symbol includes only the valence electrons, which are the electrons in the outermost shell (2s^2 2p^6) for Ne.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For neon (Ne), which has 10 electrons, the configuration is 1s² 2s² 2p⁶. This notation indicates that the first energy level (1s) holds 2 electrons, the second energy level has 2 in the s orbital and 6 in the p orbitals, filling the atom's electron shells according to the Aufbau principle.

Lewis Symbols

Lewis symbols represent the valence electrons of an atom using dots around the element's symbol. For neon, the Lewis symbol is represented as 'Ne' with no dots, indicating that it has a complete octet of valence electrons (8 electrons) in its outer shell, making it chemically inert and stable. This visual representation helps in understanding bonding and reactivity.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for chemical bonding. In neon, all 8 valence electrons are in the 2s and 2p orbitals, which are fully occupied. These electrons determine the atom's reactivity; since neon has a complete octet, it does not readily form bonds with other elements, exemplifying the concept of noble gas stability.