Final answer:
Neon, a noble gas with a full valence shell, is true to not form a chemical bond with oxygen, adhering to the octet rule. so, option a is the correct answer.
Step-by-step explanation:
The statement that the element neon, with the electron configuration 1s² 2s² 2p⁶, will not form a chemical bond with another element like oxygen is true. Neon is a noble gas and has a full outer shell of electrons, which means it has a stable noble gas configuration. According to the octet rule, atoms strive to have eight electrons in their valence shell to achieve stability like the noble gases. Since neon already has eight electrons in its outer shell, it is not inclined to form bonds with other elements, making it predominantly inert. Other noble gases also exhibit similar properties, and while some compounds containing noble gases have been synthesized, they are not common and generally require extreme conditions.
The statement is True. Neon, with the electron configuration 1s2 2s2 2p6, has a full outer shell with 8 electrons, which makes it stable. According to the octet rule, elements tend to transfer or share electrons with other elements to achieve a filled valence shell, which is the electron configuration of noble gases like neon. Since neon already has a full valence shell, it does not need to form a chemical bond with another element.