Anonymous
Anonymous asked in Science & MathematicsChemistry · 1 month ago

Chem help?

Which of the following statements are true?

1.For the noble gases, the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table.

2. All other factors being the same, dispersion forces between linear molecules are greater than dispersion forces between molecules whose shapes are nearly spherical.

3. In terms of the total attractive forces for a given substance, dipole-dipole interactions, when present, are always larger than dispersion forces.

4. For molecules with varying molecular weights, the dispersion forces may not become stronger as the molecules become more polarizable.

5. The smaller the atom, the less polarizable it is.

2 Answers

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  • 1 month ago
    Favorite Answer

    London dispersion forces are one of the three types of van der Waals forces.  The other two are Keesom forces (dipole-dipole attraction) and Debye forces (induced attraction).

    London forces are often the strongest of the three van der Waals forces and second only to hydrogen bonding.  (This is contrary to what you may have read which suggests that London forces are always the weakest.  That simply isn't true.)

    London forces are present between all molecules regardless if other intermolecular forces exist.  The strength of London forces depends on the polarizability of the molecule, which in turn, depends on the total number of electrons and the area over which they are spread.

    1. FALSE.  The strength of London forces increases going down column 18 (the inert gases).

    2. TRUE.  All other factors being the same, London forces are stronger for linear molecules which have greater area.

    3. FALSE.  Often London forces are stronger than Keesom forces or Debye forces and second only to hydrogen bonds.

    4. FALSE. The strength of London forces has nothing to do with molecular weight (except by coincidence, since molecules with greater atomic weight often have greater numbers of electrons.)

    5. TRUE.... much of the time. Polarizability depends on the total number of electrons and the area over which they are spread.  For two molecules with the same number of electrons, the one with the greater area (larger) will be more polarizable.

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  • Dylan
    Lv 6
    1 month ago

    1) TRUE

    2) TRUE

    3) FALSE ge Hydrogen vs Octane

    4) TRUE

    5) FALSE 

    • Bo1 month agoReport

      WOW.  This is certainly at odds with the other answer given above.

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