Video Solution: Which compound in each of the following pairs would you expe...

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Which compound in each of the following pairs would you expect to have the greater dipole moment ? Why? 

HF or BF3

Which of the below molecules has no net dipole moment?

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For the following molecules, use the dipole moment symbol to show the direction of the molecular dipole moment in all molecules that have an overall molecular dipole. Note for this one you do NOT need to draw the individual bond dipole moments, just the overall molecular dipole moment,

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Based on the electronegativities of C, H, and Cl, would you expect the   Cl3CCCH molecule to be  polar or  nonpolar? A molecule is polar if the vector sum of its bond dipole moments is not equal to zero. A molecule is nonpolar if the vector sum of its bond dipole moments is equal to zero. Pauling electronegativity values are listed in the periodic table on the last page of this handout.

A. Polar molecule

B. Nonpolar molecule

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Which pair of elements listed below would be expected to form an ionic bond rather than a covalent bond?

A. C–Mg           B. C–Li            C. Al–Cl            D. H–F               E. O–Na

F. More than one pair, but not all of them, would form ionic bonds rather than covalent bonds.

G. All of these pairs would form ionic bonds.

H. None of these pairs would form ionic bonds.

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Circle the molecule with the smallest dipole moment.

NH3

H2O

CH3CN

CO2

SO2

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Which compound is less polar?

a) CO2                  

or                      

b) SO2

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Five pairs of atoms are listed below with dipole moments. Pick the correct ones (maximum of two). 

                

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Which of the following molecules is polar (hint: It has a molecular dipole)

a. CO2

b. BF3

c. SO2

d. CH4

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