Silicones are polymeric compounds containing, among others, the following types of covalent bonds: si–o, c–h, and c–c. which chart below correctly arranges the bonds in order of increasing polarity and designates the positive and negative atoms using the symbols δ+ and δ–? (hint: some bonds can be nonpolar)

Si–O > C–H > C–C

Explanation:

The greater the electronegativity difference between two atoms, the greater the bond polarity.

Atoms that are closest to fluorine are the most electronegative atoms in the periodic table, as fluorine is the most electronegative atom.

Si–O bond in this case would be the most polar bond, as oxygen is the most electronegative atom of Si, O, C and H and Si is the least electronegative. Oxygen would be partially negative and silicon would be partially positive, as O is more electronegative.

C–H bond would be less polar than Si–O, as carbon and hydrogen are close to each other in terms of electronegativity, carbon being slightly more electronegative which makes carbon partially negative and hydrogen partially positive.

The C–C bond would be non-polar, as we have a bond between two same atoms of equal electronegativity, no partially positive or negative charges here.

it is the most commonly accepted one