Question

Given below are two statements: Statement I: The formation of \([O_2]^+[PtF_6]^-\) is the basis for the formation of xenon fluorides. Statement II: \(O_2\) and Xe have almost the same first ionization enthalpies.

• A. Both Statements I and II are correct
• B. Statement I is correct, but Statement II is not correct
• C. Statement I is not correct, but Statement II is correct
• D. Both Statements I and II are not correct

Hint:

The discovery of xenon compounds began with Bartlett's reaction: \[ O_2 + PtF_6 \rightarrow [O_2]^+[PtF_6]^- \] Because \(O_2\) and Xe have similar ionization energies, xenon chemistry was born.

Answer 1

The Correct Option is A

Step 1: Set the background.
Noble gases were once thought to form no compounds. The first noble gas compound came from a clever observation by Neil Bartlett.

Step 2: Read Statement I.
Bartlett saw that platinum hexafluoride could pull an electron from oxygen to form the salt $[O_2]^+[PtF_6]^-$. \[ O_2 + PtF_6 \rightarrow [O_2]^+[PtF_6]^- \] This idea led him to try the same with xenon.

Step 3: Judge Statement I.
Because this reaction inspired the making of xenon fluorides, Statement I is correct.

Step 4: Read Statement II.
Bartlett's reasoning worked only because the first ionisation enthalpy of $O_2$ is very close to that of xenon.

Step 5: Judge Statement II.
The first ionisation enthalpy of $O_2$ (about 1175 kJ/mol) is nearly the same as that of Xe (about 1170 kJ/mol). So Statement II is also correct, and it explains Statement I.

Step 6: Combine the judgements.
Both statements are correct, and the second one supports the first.

Step 7: State the final answer.
The correct choice is:
\[ \boxed{\text{Both Statements I and II are correct}} \]