Question

which of the following would you put in box d? * (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: Determine the block and period of box D

Box D is in the p - block. The p - block elements have their outermost electrons in p orbitals. Also, since it is in the highest - numbered period among the given options (by comparing the electron configurations).

Step2: Analyze the electron configurations

• Option 1: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}\) is in the p - block (4p orbital), but let's check others.
• Option 2: \(1s^{2}2s^{2}2p^{4}\) is in the p - block (2p orbital), but period 2.
• Option 3: \(1s^{2}\) is in the s - block (1s orbital).
• Option 4: \([Xe]6s^{2}4f^{4}\) is in the f - block.
• Option 5: \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{7}\) is in the d - block.
• Option 6: \([Ne]3s^{2}\) is in the s - block.

The electron configuration \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}\) (Option 1) has the highest - numbered p orbital among the valid p - block options.

Answer:

1. \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{5}\)