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.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

if you're asking what comes out, it's steam.