What is the predominant intermolecular force in the liquid state of each of these compounds: methanol (ch3oh), carbon tetrafluoride (cf4), and hydrogen sulfide (h2s)? drag the appropriate items to their respective bins. dipole-dipole forces- hydrogen bonding- dispersion forces-?

The inter-molecular forces are the force of attraction between molecules.

Hydrogen bond : it is an effective force of attraction between a highly electronegative element (F, O or N) and a hydrogen bonded to a highly electronegative element (F, O or N).

Dipole dipole force: it is present in polar molecules.

Dispersion force: these forces are present in all molecules however in non polar molecules this force of attraction is primary force.

Methanol : hydrogen bond

carbon tetrafluoride : dispersion force

Hydrogen sulfide : dipole-dipole forces

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.