Identify the intermolecular forces holding the molecules together in each sample. ch3nh2 f2 : nof : c2h6 : h2o : b. arrange the molecules in order of increasing boiling point. justify the order you chose. 7. a simple cubic crystalline solid contains 48% empty space. a body centered crystalline solid

CH3NH2 : Hydrogen bonding and London dispersion forces

F2 : Hydrogen bonding, dipole-dipole and London dispersion forces

NOF : Dipole-dipole forces

C2H6 : London dispersion forces

H2O : Hydrogen bonding and London dispersion forces

Increasing order of boiling point:

F2

C2H6

NOF

CH3NH2

H20

Explanation:

London dispersion forces exist in all substances

CH3NH2 : The hydrogen bonding in the amine group and the assymetry of the molecule makes the hydrogen bonding and dipole-dipole bonds from the methyl group.

F2 : The bond is non polar because its a homonuclear bond

NOF : Dipole-dipole forces due to difference in elecronegativity between all the atoms involved and assymetry

C2H6 : London dispersion forces because all dipole-dipole forces are cancelled out due to the symmetry of the molecule

H2O : Hydrogen bonding between hydrogen and oxygen and the assymetry of the molecule

Order of boiling points: London dispersion forces, followed by dipole-dipole forces and hydrogen bonding is the strongest

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