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To detect how many bonds can be formed without hybridization by Sulfur:
it is electronic configuration of valence electron is: 
3s² 3p⁴ we have here 2 unpaired electrons and 2 lone pairs so it can forms only two bonds  (due to bond is formed by the unpaired electrons)
Note:
Valence electrons: The electrons which are present in the outermost energy level.
Electron configuration: The arrangement of electrons in an atom by a superscript in each sublevel  

Answer:

The bonds formed by Si are 4, P are 3 and F are 1. The S form 2 bonds.

Explanation:

The electronic orbitals are filled up one after the other.

For Si = [tex]\rm 3\;s^2\;3\;p\;^2[/tex]

There are 4 valence electrons in the third orbital. This can form 4 bonds.

For P = [tex]\rm 3\;s^2\;2\;p\;^3[/tex]

There are 5 electrons, it requires 3 electrons to complete its octet. So, it makes 3 bonds.

For, F = [tex]\rm 2\;s^2\;2\;p\;^5[/tex]

It has 7 electrons and requires one electron to complete its octet. So, it will make 1 bond.

For S = [tex]\rm 3\;s^2\;3\;p\;^4[/tex]

There are 6 electrons and 2 are required to complete the octet. So, 2 bonds are formed.

For more information, refer the link:

https://brainly.com/question/14140731?referrer=searchResults

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