Question

identify the position of AL =(z=13 ) AND S= (Z=16) in periodic table with help of electronic configuration and also find compound form between them

Answer 1

Electronic configuration of al-2,8,3

Hence , it is placed in the 13th group and 3rd period

Electronic configuration of s-2,8,6

Hence it is placed in the 16th group and 3rd period

The compound formed is al2s3

Answer 2

Answer:

Position of Al : 3rd period and group 13

Position of S : 3rd period and group 16

The compound of Al and S is Al₂S₃.

Explanation:

• The atomic number of aluminium is 13. The electronic configuration of aluminium is 1s² 2s² 2p⁶ 3s² 3p¹. Because the valence electrons filled in third shell. Therefore, the aluminium is present in 3rd period. The aluminium has three valence electrons in its valence shell. The elements of group 13 has three valence electrons with configuration ns²np¹. Therefore, Al is present in group 13.
• The atomic number of Sulphur is 16. The electronic configuration of Sulphur is 1s² 2s² 2p⁶ 3s² 3p⁴. The valence electrons present in third shell. Therefore, the Sulphur is present in third period. Sulphur has six valence electrons in its valence shell. The elements of group 16 (oxygen family) has six valence electrons with configuration ns²np⁴. Therefore, S is present in group 16 in periodic table.
• Valency of aluminium is 3 and the valency of sulphur is 2. When two elements formed compound their valency becomes the subscript of each other. So the compound formed between Al and S will be Al₂S₃.