Chemical SO3 : Central atom considered: Number of electron groups: Bond angle: Electron geometry: Molecular Geometry: Does this molecule have polar bonds? ( yes or no) Hybrid orbital: Is this molecule polar? (yes or no) Strongest IMF: Chemical: H2SO4 Lewis Structure: �¢ÑƒÑ€�µ: Central atom considered: Number of electron groups: Bond angle: Electron geometry: Molecular Geometry: Does this molecule have polar bonds? (yes or no) Is this molecule polar? (yes or no) Strongest IMF: Hybrid orbital: Chemical: NaHSO4 Lewis Structure: �¢ÑƒÑ€�µ: Central atom considered: S Number of electron groups: Bond angle: Electron geometry: Molecular Geometry: Does this molecule have polar bonds? ( yes or no) Is this molecule polar? |(yes or no) Strongest IMF: Hybrid orbital: Please help filling out Number of electron groups: Bond angle: Electron geometry: Does this molecule have polar bonds? (yes or no) Hybrid orbital: Chemical: H₂SO4 Type: Central atom considered: S Number of electron groups: Bond angle: Electron geometry: Does this molecule have polar bonds? (yes or no) Hybrid orbital: Chemical: NaHSO4 Type: Central atom considered: S Number of electron groups: Bond angle: Electron geometry: Does this molecule have polar bonds? (yes or no) Hybrid orbital: Molecular Geometry: Is this molecule polar? (yes or no) Strongest IMF: Lewis Structure: Molecular Geometry: Is this molecule polar? (yes or no) Strongest IMF: Lewis Structure: Molecular Geometry: Is this molecule polar? (yes or no) Strongest IMF:
The Correct Answer and Explanation is :
Let’s break down each molecule and fill in the required information. I’ll explain the details for each compound based on their molecular structures and bonding properties.
1. SO3 (Sulfur Trioxide)
- Central atom considered: Sulfur (S)
- Number of electron groups: 3 (3 bonds to oxygen atoms)
- Bond angle: 120°
- Electron geometry: Trigonal planar (since there are three electron groups around the central atom)
- Molecular Geometry: Trigonal planar (the arrangement of the atoms is the same as the electron geometry)
- Does this molecule have polar bonds? Yes (the bonds between sulfur and oxygen are polar due to a difference in electronegativity)
- Hybrid orbital: sp² (since the electron geometry is trigonal planar)
- Is this molecule polar? No (despite having polar bonds, the molecule is symmetrical and has no net dipole moment)
- Strongest IMF: London dispersion forces (due to the symmetrical nature of the molecule)
2. H2SO4 (Sulfuric Acid)
- Central atom considered: Sulfur (S)
- Number of electron groups: 4 (2 OH groups and 2 double bonds to oxygen atoms)
- Bond angle: 109.5° (approximately, since the molecule has a tetrahedral electron geometry around the sulfur atom)
- Electron geometry: Tetrahedral (due to the four electron groups around sulfur)
- Molecular Geometry: Tetrahedral (since there are no lone pairs on the central atom)
- Does this molecule have polar bonds? Yes (the bonds between sulfur and oxygen are polar)
- Is this molecule polar? Yes (the molecule is not symmetrical, so it has a net dipole moment)
- Hybrid orbital: sp³ (due to the tetrahedral geometry)
- Strongest IMF: Hydrogen bonding (due to the presence of OH groups)
3. NaHSO4 (Sodium Bisulfate)
- Central atom considered: Sulfur (S)
- Number of electron groups: 4 (1 OH group, 1 single bond to oxygen, and 2 double bonds to oxygen)
- Bond angle: 109.5° (similar to H2SO4)
- Electron geometry: Tetrahedral (due to 4 electron groups around sulfur)
- Molecular Geometry: Tetrahedral
- Does this molecule have polar bonds? Yes (the bonds between sulfur and oxygen are polar)
- Hybrid orbital: sp³ (tetrahedral geometry)
- Is this molecule polar? Yes (the molecule is asymmetric, giving it a dipole moment)
- Strongest IMF: Hydrogen bonding (due to the presence of the OH group)
Explanation:
- Bond angles: The bond angles depend on the number of electron groups around the central atom. For molecules with 3 groups, like SO3, the bond angle is 120°, characteristic of a trigonal planar geometry. For molecules like H2SO4 and NaHSO4 with 4 electron groups, the bond angles are approximately 109.5°, corresponding to a tetrahedral geometry.
- Electron and Molecular Geometry: Electron geometry refers to the arrangement of all electron groups (including bonding and lone pairs), whereas molecular geometry describes the arrangement of only the atoms. In both H2SO4 and NaHSO4, the electron geometry is tetrahedral due to 4 electron groups around sulfur. The molecular geometry is also tetrahedral, as there are no lone pairs on sulfur in these cases.
- Polarity: Even though SO3 has polar bonds, its molecular geometry is symmetrical, meaning the dipoles cancel out, making the molecule non-polar. On the other hand, H2SO4 and NaHSO4 are polar due to their asymmetrical geometries and the presence of polar bonds that don’t cancel out.
- IMFs: The strongest intermolecular forces in SO3 are London dispersion forces due to its molecular symmetry. However, H2SO4 and NaHSO4 exhibit hydrogen bonding due to the presence of OH groups, which is stronger than dispersion forces.
This provides a comprehensive breakdown of each molecule’s properties, hybridization, polarity, and molecular structure.