Question

1. the complete photoelectron spectrum for an element is shown. what oxide compound would it most likely form? a) xo₂ b) x₃o c) xo d) x₂o₂

Explanation:

To solve this, we analyze the photoelectron spectrum to find the element's electron configuration and oxidation state:

Step 1: Determine Electron Configuration

From the spectrum (assuming typical peaks), if the element has a valence state (oxidation state) of \( +2 \) (e.g., Group 2 metal, losing 2 electrons), oxygen has an oxidation state of \( -2 \).

Step 2: Balance Oxidation States

For a compound \( XO \):

• Oxidation state of \( X \): \( +2 \)
• Oxidation state of \( O \): \( -2 \)
• Sum: \( (+2) + (-2) = 0 \), which is neutral.

Other options:

• \( XO_2 \): \( X \) would need \( +4 \) (unlikely for a Group 2 - like element).
• \( X_2O \): \( X \) would need \( +1 \) (doesn’t match \( +2 \) valence).
• \( X_2O_2 \): Equivalent to \( XO \) (simplified), but \( XO \) is simpler and matches \( +2/-2 \) balance.

Answer:

c) \( \boldsymbol{XO} \)