The electron domain and molecular geometry of BrO2-is _. A)tetrahedral, bent B)trigonal pyramidal, linear C)tetrahedral, trigonal planar
D)trigonal pyramidal, seesaw E)trigonal planar, trigonal planar
The Correct Answer and Explanation is :
The correct answer is:
A) Tetrahedral, Bent
Explanation:
To determine the electron domain and molecular geometry of BrO₂⁻ (bromite ion), we follow these steps:
- Determine the Total Valence Electrons:
- Bromine (Br): 7 valence electrons
- Oxygen (O): Each oxygen has 6 valence electrons, so two oxygens contribute 12 electrons
- Negative charge (-1): Adds 1 extra electron
- Total valence electrons: (7 + 12 + 1 = 20) electrons
- Draw the Lewis Structure:
- Place Br as the central atom.
- Distribute the oxygens around Br.
- Connect each oxygen atom to Br with a single bond.
- Complete the octets of oxygen first.
- Assign the remaining electrons to Br as lone pairs.
- Determine the Electron Domain Geometry:
- Br has two bonded atoms (O) and two lone pairs.
- This gives four electron domains around Br.
- According to VSEPR (Valence Shell Electron Pair Repulsion) theory, a molecule with four electron domains adopts a tetrahedral electron domain geometry.
- Determine the Molecular Geometry:
- The presence of two lone pairs affects the molecular shape.
- Lone pairs repel more strongly than bonding pairs, pushing the oxygen atoms down and creating a bent shape (similar to water, H₂O).
- This results in a bent molecular geometry instead of a tetrahedral shape.
Conclusion:
- Electron Domain Geometry: Tetrahedral
- Molecular Geometry: Bent
- This corresponds to Option A.
Now, I’ll generate an image of the molecular structure.
Here is the 3D molecular structure representation of the bromite ion (BrO₂⁻). It visually demonstrates the tetrahedral electron domain geometry and the bent molecular shape due to the presence of two lone pairs on bromine. Let me know if you need any modifications!