Consider the following mechanism for the reaction between t-butyl chloride and water: (CH_3)_3 CCl(aq) rightarrow (CH_3)_3 C^+ (aq) + Cl^- (aq) (CH_3)_3 C^+ (aq) + H_2O(l) rightarrow (CH_3)_3 CHOH^+ (aq) (CH_3)_3 CHOH^+ (aq) + H_2O(l) rightarrow (CH_3)_3 COH(aq) + H_3 O^+ (aq) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? yes no If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one.

Explanation:

CH_3)_3 CCl(aq) --> (CH_3)_3 C^+ (aq) + Cl^- (aq)

(CH_3)_3 C^+ (aq) + H_2O(l) --> (CH_3)_3 CHOH^+ (aq)

(CH_3)_3 CHOH^+ (aq) + H_2O(l) --> (CH_3)_3 COH(aq) + H_3 O^+(aq)

Write the chemical equation of the overall reaction

CH_3)_3 CCl(aq) + 2H_2O(l) --> (CH_3)_3 COH(aq) + H_3 O^+(aq)  +  Cl^- (aq)

Are there any intermediates in this mechanism?

Yes

Intermediates; (CH_3)_3 C^+(aq), (CH_3)_3 CHOH^+ (aq)

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.

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