Which of the following ions possess a dipole moment: ClF2+, ClF2-, IF2+, or IF4-?
ClF2- possesses a dipole moment.
To determine which of the given ions possess a dipole moment, we need to consider the molecular geometry and the polarity of the individual bonds.
- ClF2+: This ion consists of a central chlorine atom bonded to two fluorine atoms. Since the chlorine and fluorine atoms have different electronegativities, the Cl-F bonds are polar. However, the molecule has a linear geometry, and the bond polarities cancel each other out, resulting in a nonpolar molecule. Therefore, ClF2+ does not possess a dipole moment.
- ClF2-: Like ClF2+, this ion also consists of a central chlorine atom bonded to two fluorine atoms. Since the Cl-F bonds are polar, the molecule is polar as well. The bond polarities do not cancel, causing a net dipole moment. Therefore, ClF2- possesses a dipole moment.
- IF2+: This ion consists of a central iodine atom bonded to two fluorine atoms. Similar to the ClF2+ ion, the iodine-fluorine bonds are polar. However, the molecule has a linear geometry, and the bond polarities cancel each other out, resulting in a nonpolar molecule. Therefore, IF2+ does not possess a dipole moment.
- IF4-: This ion consists of a central iodine atom bonded to four fluorine atoms. The molecule has a square planar geometry, which creates a symmetrical arrangement of the bond polarities. As a result, the bond polarities cancel each other out, making IF4- a nonpolar molecule. Therefore, IF4- does not possess a dipole moment.
In summary, ClF2- is the only ion among the given options that possesses a dipole moment.
To determine which of the following ions possess a dipole moment (meaning they have a net dipole), we need to assess the molecular geometry and polarity of each ion.
1. ClF2+: The ClF2+ ion has a "trigonal planar" molecular geometry. However, since it carries a positive charge (+), it means it is missing one electron compared to the neutral molecule ClF2. Thus, the ClF2+ ion has a net dipole moment due to the presence of the polar bonds in the molecule, and the positive charge on the central Cl atom.
2. ClF2-: The ClF2- ion also has a "trigonal planar" molecular geometry, but with a negative charge (-). Similar to ClF2+, it has a net dipole moment due to the presence of the polar bonds, but this time due to the extra electron present on the ion.
3. IF2+: The IF2+ ion has a "linear" molecular geometry. However, since it carries a positive charge, it means it is missing one electron compared to the neutral molecule IF2. This ion does not possess a net dipole moment. Although the IF bond is polar, the molecular geometry cancels out the dipoles, resulting in a nonpolar ion.
4. IF4-: The IF4- ion has a "square planar" molecular geometry. The presence of four polar IF bonds in the molecule gives it a net dipole moment, and the negative charge adds to the polarity. Therefore, IF4- possesses a dipole moment.
In summary, the ions that possess a net dipole moment are ClF2+ ClF2-, and IF4-.