Answer: Electronegativity is not relevant here because F-F bonds are exactly non polar. So F2 have lowest boiling point than other.
Explanation:
1.Weak intermolecular forces exist for H2S . Hydrogen sulfide boil at -60.7 °C .
2.Nitrogen tribromide is extremely explosive in its pure form, even at −100 °C
3.Boiling point of F2 is -188°C
4.Boiling point of CF2H2 is −52 °C
5.The boiling point of H2O2 has been extrapolated as being 150.2 °C, approximately 50 °C higher than water.
Electronegativity is not relevant here because F-F bonds are exactly non polar.
All these molecules have only London dispersion forces as their intermolecular force.
The bigger the molecules the stronger the London dispersion forces.
The stronger an intermolecular force the higher the boiling point of the substance will be
Because stronger intermolecular bonds require more energy to break and this energy is supplied in the form of heat when boiling.
Dipole–Dipole Interactions
a) Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.
b) This force is much weaker than ionic and covalent bonds.
c) The partially positive end of a polar molecule is attracted to the partially negative end of another.
London Dispersion Forces
a) The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction.
b) Dispersion forces are present between all molecules, whether they are polar or nonpolar.
c) Larger and heavier atoms and molecules exhibit stronger dispersion forces than smaller and lighter ones.
