List all types of IMFs that would occur in each of the following a. CH_3CF_3 b.

Question

List all types of IMFs that would occur in each of the following a. CH_3CF_3 b. CCI4 c. SO_2 d. BrF List the dominant type of IMF for the pure substances, then rank the strength of each compound based on IMFs within the samples. Circle all of the species below that can form a hydrogen bond in its pure form. Explain why the other species couldn't hydrogen bond. C_2H_6 CH_3NH_2 KCI CH_3CH_2CH_2OH CH_3OCH_3 Rank the following compounds from weakest intermolecular forces to strongest. Justify your answers. I_2 H_2S H_2O Which of the following will have the highest melting point a. naphthalene, C_8H_10 b. methane b. methane CH_4 c. SiO_2 d. C_2H_5OH Circle all the compounds which would be expected to form intermolecular hydrogen bonds in the liquid state: (a) CH_3OCH_3 (b) CH_4 c) HF d) CH_3CO_2H e) Br_2 f) CH_3OH

Explanation / Answer

SO2 is a polar molecule,dipole-dipole forces exists between polar molecules.

There are also dispersion forces between SO2 molecules.

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CCl4 is a non-polar molecule, so only london dispersion forces.

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BrF only Dipole-dipole interactions and london dispersion forces exist.

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CH3CF3 only hydrogen bonding and  london dispersion forces exists.

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