The two molecules shown below have different arrangements of atoms but the same chemical formula. Which molecule has a larger dipole moment?

Which diagram correctly shows the direction of polarity for P—O and P—H using the ?+/?− notation?

The compound IBr has an experimental dipole moment of 0.70 D. Assuming that the bond length of IBr is the sum of the atomic radii, determine the partial charges on the atoms in IBr using the experimental dipole moment.

Consider the following nonmetals: C, O, Br, Se

Identify the pair among the given elements that would form the most polar bond.

Calculate the magnitude of the bond dipole of the S-H bonds using the following data. The S-H bond lengths in the Hydrogen sulfide (H₂S) molecule are 134 pm and the H-S-H angle is 92.1°. The dipole moment of the ammonia molecule is 0.95 D.

Refer to the following pairs of atoms:
a. Cl and F
b. S and O
c. K and Cl
d. N and Cl
Identify if the bond between each pair will be ionic or covalent. If the bond is covalent, identify the bond as polar or nonpolar.

Calculate the effective charge (in terms of e) for the S atom in the SO molecule given that the dipole moment is 1.55 D and the bond length is 1.48 Å.