Question

Based on reference table S, atoms of which of these elements have the strongest attraction for the electrons in a chemical bond?

A) Si
B) P
C) Al
D) S

Answer 1

D

Step-by-step explanation:

Answer: Option (D) is the correct answer.

Step-by-step explanation:

Atomic number of Si is 14 and its electronic configuration is .

Atomic number of P is 15 and its electronic configuration is .

Atomic number of Al is 13 and its electronic configuration is .

Atomic number of S is 16 and its electronic configuration is .

To completely fill 3p orbital, sulfur will readily accept two electrons as it is more electronegative. Thus, by gaining two electrons it will become stable in nature.

Therefore, we can conclude that atoms of sulfur (S) will have the strongest attraction for the electrons in a chemical bond

Answer 2

Answer: Option (D) is the correct answer.

Step-by-step explanation:

Atomic number of Si is 14 and its electronic configuration is
`1s^(2)2s^(2)2p^(6)3s^(2)3p^(2)`.

Atomic number of P is 15 and its electronic configuration is
`1s^(2)2s^(2)2p^(6)3s^(2)3p^(3)`.

Atomic number of Al is 13 and its electronic configuration is
`1s^(2)2s^(2)2p^(6)3s^(2)3p^(1)`.

Atomic number of S is 16 and its electronic configuration is
`1s^(2)2s^(2)2p^(6)3s^(2)3p^(4)`.

To completely fill 3p orbital, sulfur will readily accept two electrons as it is more electronegative. Thus, by gaining two electrons it will become stable in nature.

Therefore, we can conclude that atoms of sulfur (S) will have the strongest attraction for the electrons in a chemical bond.