NO2 - Molecular Geometry / Shape and Bond Angles
161.6 هزار بار بازدید -
5 سال پیش
-
A quick explanation of the
A quick explanation of the molecular geometry of NO2 - (the Nitrite ion) including a description of the NO2 - bond angles.
Looking at the NO2 - Lewis structure we can see that there are three atoms attached to the central Nitrogen (N) atom as well as a lone pair of electrons. Based on VSEPR Theory (Valence Shell Electron Pair Repulsion Theory) the electron clouds on atoms and lone pair of electrons around the N atom will repel each other. As a result they will be pushed apart giving the NO2 - molecule a bent molecular geometry or shape.
The NO2 - bond angle will be about 120 degrees since it has a bent molecular geometry (it will be a bit less since the lone pair will push down – the actual value is 115.4).
The electron geometry is Trigonal Planar since there are three things bonded to the central atom.
--How to Determine the Molecular Geometry--
1) Draw the Lewis Structure for the compound.
2) Predict how the atoms and lone pairs will spread out when the repel each other.
3) Use a chart based on steric number (like the one in the video) or use the AXN notation to find the molecular shape. This will be determined by the number of atoms and lone pairs attached to the central atom.
Helpful Resources:
• How to Draw Lewis Structures: How to Draw Lewis Structures: Five Ea...
• Molecular Geometry and VSEPR Explained: Molecular Geometry: Rules, Examples, ...
• Molecular Geo App: https://phet.colorado.edu/sims/html/m...
Get more chemistry help at http://www.breslyn.org
Drawing/writing done in InkScape. Screen capture done with Camtasia Studio 4.0. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo).
Looking at the NO2 - Lewis structure we can see that there are three atoms attached to the central Nitrogen (N) atom as well as a lone pair of electrons. Based on VSEPR Theory (Valence Shell Electron Pair Repulsion Theory) the electron clouds on atoms and lone pair of electrons around the N atom will repel each other. As a result they will be pushed apart giving the NO2 - molecule a bent molecular geometry or shape.
The NO2 - bond angle will be about 120 degrees since it has a bent molecular geometry (it will be a bit less since the lone pair will push down – the actual value is 115.4).
The electron geometry is Trigonal Planar since there are three things bonded to the central atom.
1) Draw the Lewis Structure for the compound.
2) Predict how the atoms and lone pairs will spread out when the repel each other.
3) Use a chart based on steric number (like the one in the video) or use the AXN notation to find the molecular shape. This will be determined by the number of atoms and lone pairs attached to the central atom.
Helpful Resources:
• How to Draw Lewis Structures: How to Draw Lewis Structures: Five Ea...
• Molecular Geometry and VSEPR Explained: Molecular Geometry: Rules, Examples, ...
• Molecular Geo App: https://phet.colorado.edu/sims/html/m...
Get more chemistry help at http://www.breslyn.org
Drawing/writing done in InkScape. Screen capture done with Camtasia Studio 4.0. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo).
5 سال پیش
در تاریخ 1397/11/21 منتشر شده
است.
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