Why do atoms form bonds to achieve a full octet in their valence shell?

• A. To increase their chemical stability by attaining a noble gas electron configuration
• B. To become electrically charged
• C. To maximize their atomic radius
• D. To decrease the number of protons in the nucleus

Answer: (A)

Verified step by step guidance

1. Understand that atoms form bonds primarily to achieve greater stability. Stability in atoms is often related to having a full valence shell of electrons, which is commonly an octet (8 electrons) for many elements.
2. Recall the Octet Rule, which states that atoms tend to gain, lose, or share electrons to have eight electrons in their outermost shell, similar to the electron configuration of noble gases.
3. Recognize that noble gases are chemically stable because their valence shells are full, making them less likely to react with other atoms.
4. Note that forming bonds allows atoms to effectively 'share' or 'transfer' electrons, enabling them to complete their octet and thus lower their potential energy, increasing chemical stability.
5. Eliminate incorrect options by understanding that atoms do not form bonds to become electrically charged (though ions can form), to maximize atomic radius (bonding usually affects size differently), or to change the number of protons (which defines the element and does not change during bonding).