Question

5. CH4-CH4 interactions: Do the CH4 molecules appear to attract each other much? Briefly describe their interaction.

6. CH3F-CH3F interactions: Do the CH3F molecules appear to attract each other much? Briefly describe their interaction.

7. CH3OH-CH3OH interactions: Do the CH3OH molecules appear to attract each other much? Briefly describe their interaction.

8. CH3OH-water interactions: What happens when the CH3OH molecules are surrounded by water molecules? Briefly describe their interaction

Answer 1

6=Do the ch3f molecules appear to attract each other much? briefly describe their interaction. Answer by Guest Neither attract much nor allows it to be free. How the molecules behave in such way? Because fluorine has a higher electronegativity than carbon and hydrogen, CH3F possesses a non-zero dipole moment.

5=T he CH₄ molecules appear to attract each other because it's non-polar molecule.

7 = The presence of a lone pair decreases the bond angle between the bonding pair of electrons, due to their high electric charge which causes great repulsion between the electrons Lewis structure def is meant to represent chemical bonding and the distribution of electrons - as bonds and lone pairs - in the strucure ball and stick model

8 = A CH 3 OH is decomposed into molecules, a formaldehyde and an H 2, in water, while it is converted into radicals in a gas phase reaction at a high temperature. H 2 O molecules located near a CH 3 OH form a first hydration shell and act as catalyst for the oxidation of CH 3 OH in water.