To understand the compound HNO3 (nitric acid) thoroughly, let’s explore its Lewis dot structure, hybridization, electron geometry, molecular geometry, and polarity.
Lewis Dot Structure
The Lewis dot structure for HNO3 shows the arrangement of valence electrons among the constituent atoms. In HNO3, nitrogen (N) is the central atom bonded to three oxygen (O) atoms and one hydrogen (H) atom. The structure can be represented as:
O
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H - N - O
|
O
The nitrogen atom forms one double bond with one oxygen atom, a single bond with another oxygen, and a single bond with hydrogen, ensuring all atoms have their valence shells fulfilled.
Hybridization
The hybridization of HNO3 can be determined by the number of bonds around the nitrogen atom. Nitrogen in HNO3 has three regions of electron density (two single bonds and one double bond), leading to an sp2 hybridization.
Electron Geometry
The electron geometry around the nitrogen atom, which includes lone pairs and bonds, is trigonal planar. This geometry indicates that the electron groups are spread out as far as possible to minimize repulsion.
Molecular Geometry
The molecular geometry of HNO3 is also trigonal planar. Since there are no lone pairs of electrons on the nitrogen atom, the shape reflects that of the electron geometry.
Polarity
HNO3 is a polar molecule. The difference in electronegativity between nitrogen and oxygen creates polar bonds, and the asymmetrical arrangement of these bonds, along with the attached hydrogen, results in an overall dipole moment. Therefore, HNO3 is classified as a polar molecule.
In conclusion, HNO3 can be summarized as follows:
- Lewis Dot Structure: Represents N bonded to three oxygens and one H.
- Hybridization: sp2
- Electron Geometry: Trigonal planar
- Molecular Geometry: Trigonal planar
- Polarity: Polar