Which of the following atoms best exemplifies the octet rule?

• A. Phosphorus (P)
• B. Hydrogen (H)
• C. Neon (Ne)
• D. Boron (B)

Answer: (C)

Verified step by step guidance

1. Understand the octet rule: it states that atoms tend to gain, lose, or share electrons to have eight electrons in their valence shell, achieving a stable electron configuration similar to noble gases.
2. Examine each atom's position in the periodic table and their typical valence electron count: Hydrogen (H) has 1 valence electron, Boron (B) has 3, Phosphorus (P) has 5, and Neon (Ne) has 8 valence electrons.
3. Recognize that Neon (Ne) is a noble gas with a full valence shell of 8 electrons, naturally satisfying the octet rule without needing to gain, lose, or share electrons.
4. Note that Hydrogen is an exception to the octet rule because it is stable with 2 electrons (duet rule), and Boron and Phosphorus often form compounds to achieve an octet but do not inherently have a full octet in their elemental form.
5. Conclude that Neon (Ne) best exemplifies the octet rule because it naturally has a complete octet in its valence shell.