Question

which of the following would you put in box f? * (0.5 points)
1 $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}$
2 $1s^{2}2s^{2}2p^{4}$
3 $1s^{2}$
4 $xe6s^{2}4f^{4}$
5 $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{7}$
6 $ne3s^{2}$

Explanation:

Step1: Identify the block of each option

• Option 1: Ends with \(4p^{5}\), so it is in the \(p -\)block.
• Option 2: Ends with \(2p^{4}\), so it is in the \(p -\)block.
• Option 3: Ends with \(1s^{2}\), so it is in the \(s -\)block.
• Option 4: Ends with \(4f^{4}\), so it is in the \(f -\)block.
• Option 5: Ends with \(3d^{7}\), so it is in the \(d -\)block.
• Option 6: Ends with \(3s^{2}\), so it is in the \(s -\)block.

Step2: Match with the \(f -\)block (box F)

Since box F is in the \(f -\)block, we look for the electron - configuration that has an \(f -\)orbital in its outer - most occupied orbital.

Answer:

1. \([Xe]6s^{2}4f^{4}\)