The NO2- ion, also known as the nitrite ion, has a nitrogen atom at the center, bonded to two oxygen atoms. To determine its geometry and polarity, we need to consider the electron pairs around the central atom and their repulsion.1. Determine the electron pairs around the central atom:Nitrogen has 5 valence electrons, and each oxygen atom has 6 valence electrons. In the NO2- ion, there is an additional electron due to the negative charge. So, the total number of valence electrons is 5 + 6 + 6 + 1 = 18.2. Distribute the electron pairs:The nitrogen atom forms two single bonds with the two oxygen atoms, which accounts for 4 electrons. The remaining 14 electrons are distributed as lone pairs, with 6 electrons 3 lone pairs on each oxygen atom and 1 lone pair 2 electrons on the nitrogen atom.3. Determine the electron pair geometry:The nitrogen atom has three electron groups around it two bonding groups and one lone pair . According to the VSEPR Valence Shell Electron Pair Repulsion theory, these electron groups will arrange themselves to minimize repulsion. In this case, the electron pair geometry is trigonal planar.4. Determine the molecular geometry:Since there is one lone pair on the nitrogen atom, the molecular geometry will be different from the electron pair geometry. The two oxygen atoms and the nitrogen atom will form a bent or V-shaped geometry.5. Determine the polarity:The electronegativity difference between nitrogen and oxygen causes the N-O bonds to be polar, with oxygen being more electronegative. Due to the bent geometry, the bond dipoles do not cancel each other out, resulting in a net dipole moment. Therefore, the NO2- ion is polar.In summary, the predicted geometry of the NO2- ion is bent or V-shaped, and it is a polar molecule.