bonds in the liquid state: ... (g) NH3. CH4. (h) HCl(g). NaCl. (i) SiC. Cu. 3. Isopropyl alcohol has a melting point ... a) Which substance can form h...
INTERMOLECULAR FORCES #2 1. Circle all the compounds in the following list which would be expected to form hydrogen bonds in the liquid state: (a) CH3OCH3 (dimethyl ether)
(b) CH4
(c) HF
(d) CH3CO2H (acetic acid)
(e) Br2
(f) CH3OH (methanol)
2. Specify the predominant intermolecular force involved for each substance in the space immediately following the substance. Then in the last column, indicate which member of the pair you would expect to have the higher boiling point.
Substance #1 (a) HCl(g) (b) CH3F
Predominant Intermolecular Force
Substance #2 I2 H2S
(d) SiO2
SO2 Kr
(f) CH3OH
CuO
(g) NH3
CH4
(h) HCl(g)
NaCl
(i) SiC
Substance with Higher Boiling Point
CH3OH
(c) H2O (e) Fe
Predominant Intermolecular Force
Cu
3. Isopropyl alcohol has a melting point of -89oC and a boiling point of 82oC at atmospheric pressure. a) Draw a heating curve for isopropyl alcohol. b) If the pressure is decreased, what would expect to happen to melting and boiling points of isopropyl alcohol. 4. When comparing the 4 diatomic molecules for by the halogens, F2, Cl2, Br2, and I2, boiling point increases as you go down the halogen group on the periodic table. Provide and explanation for this trend. 5. The following questions relate to following compounds: CH4, H2S, and HF. a) b) c) d) e)
Which substance can form hydrogen bonds? Which substance has the lowest boiling point? Explain why none of these have London dispersion forces. How would waters boiling point compare to the above compounds? Why are the HF intermolecular forces stronger than waters?