is clo2-, asf6-, sebr3+, i3-, o3, icl4+ and xebr4 polar or non polar?
The Correct Answer and Explanation is :
To determine whether the given molecules/ions are polar or nonpolar, we need to analyze their molecular geometry and electronegativity differences. A molecule is polar if it has an asymmetrical shape that creates a net dipole moment. Conversely, if the dipole moments cancel out due to symmetry, the molecule is nonpolar.
1. ( ClO_2^- ) (Chlorite ion) – Polar
- Lewis Structure: Bent shape due to lone pairs on chlorine.
- Electronegativity: Oxygen is more electronegative than chlorine.
- Polarity: The bent shape prevents dipoles from canceling, making ( ClO_2^- ) polar.
2. ( AsF_6^- ) (Hexafluoroarsenate) – Nonpolar
- Geometry: Octahedral.
- Electronegativity: Fluorine pulls electrons evenly in opposite directions.
- Polarity: Since the molecule is symmetric, dipoles cancel, making it nonpolar.
3. ( SeBr_3^+ ) (Selenium tribromide cation) – Polar
- Geometry: Trigonal pyramidal due to lone pairs on selenium.
- Electronegativity: Bromine is more electronegative than selenium.
- Polarity: Asymmetry leads to a net dipole moment, making it polar.
4. ( I_3^- ) (Triiodide ion) – Nonpolar
- Geometry: Linear (lone pairs on central iodine).
- Electronegativity: Iodine atoms share electrons symmetrically.
- Polarity: No net dipole moment due to linear shape, making it nonpolar.
5. ( O_3 ) (Ozone) – Polar
- Geometry: Bent due to lone pairs on central oxygen.
- Electronegativity: Oxygen has a strong dipole.
- Polarity: Asymmetrical shape creates a net dipole, making it polar.
6. ( ICl_4^+ ) (Tetrachloroiodate cation) – Polar
- Geometry: See-saw shape due to lone pair on iodine.
- Electronegativity: Chlorine is more electronegative than iodine.
- Polarity: Asymmetrical shape results in a net dipole, making it polar.
7. ( XeBr_4 ) (Xenon tetrabromide) – Nonpolar
- Geometry: Square planar due to lone pairs on xenon.
- Electronegativity: Bromine pulls symmetrically.
- Polarity: Symmetry cancels out dipoles, making it nonpolar.
Final Answer:
| Molecule/Ion | Polarity |
|---|---|
| ( ClO_2^- ) | Polar |
| ( AsF_6^- ) | Nonpolar |
| ( SeBr_3^+ ) | Polar |
| ( I_3^- ) | Nonpolar |
| ( O_3 ) | Polar |
| ( ICl_4^+ ) | Polar |
| ( XeBr_4 ) | Nonpolar |
Conclusion: Polarity depends on both electronegativity and molecular shape. Molecules with symmetrical geometry (e.g., octahedral, square planar, linear) are generally nonpolar, while asymmetrical ones (bent, trigonal pyramidal, see-saw) tend to be polar.