How does an oxygen atom obey the octet rule in most of its compounds?

• A. By having only six electrons in its valence shell
• B. By sharing three electrons with other atoms
• C. By losing two electrons to form a stable cation
• D. By forming two covalent bonds to achieve eight valence electrons

Answer: (D)

Verified step by step guidance

1. Recall that the octet rule states atoms tend to form bonds to have eight electrons in their valence shell, achieving a stable electron configuration similar to noble gases.
2. Identify the number of valence electrons in an oxygen atom. Oxygen has 6 valence electrons because it is in group 16 of the periodic table.
3. Understand that oxygen can gain, lose, or share electrons to complete its octet. Losing two electrons to form a cation is unlikely because oxygen is more electronegative and tends to gain or share electrons.
4. Recognize that oxygen typically forms two covalent bonds by sharing two pairs of electrons with other atoms, which adds 4 electrons to its 6 valence electrons, reaching a total of 8 electrons.
5. Conclude that by forming two covalent bonds, oxygen obeys the octet rule, achieving a stable configuration with eight electrons in its valence shell.