Table of Contents
- 1 What is the molecular shape of No 2?
- 2 What shapes can molecules form?
- 3 What is the shape and bond angle of No 2?
- 4 How is the shape of a diatomic molecule determined?
- 5 Which is an example of a triatomic molecule with a linear shape?
- 6 How are non bonding electrons included in the shape of a molecule?
What is the molecular shape of No 2?
We can see that NO2 has a bent molecular geometry and the angle is around 120 degrees.
What shapes can molecules form?
Molecular Geometries. The VSEPR theory describes five main shapes of simple molecules: linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral.
What is the shape and bond angle of No 2?
Hybridization of NO2
| Name of the Molecule | Nitrogen Dioxide |
|---|---|
| Molecular Formula | NO2 |
| Hybridization Type | sp2 |
| Bond Angle | 134° |
| Geometry | Bent |
What defines the shape of a molecule?
The shape of a covalent molecule can be predicted using the Valence Shell Electron Pair Repulsion (VSEPR) theory. VSEPR theory is based on the idea that the geometry (shape) of a molecule is mostly determined by repulsion among the pairs of electrons around a central atom.
What makes up the shape of a molecule?
Since electrons are negatively charged and repel one another, electrons on the central atom of a molecule always maximize their distance from one another. These repulsions give rise to the five basic molecular geometries (or shapes) for molecules in which the central atom has no lone pairs.
How is the shape of a diatomic molecule determined?
For diatomic molecules (i.e., those made up of two atoms), the shape has to be linear. For molecules with three of more atoms, the shape depends on the number and type of electrons (bonding versus nonbonding) around the central atom.
Which is an example of a triatomic molecule with a linear shape?
Examples of triatomic molecules for which VSEPR theory predicts a linear shape include BeCl 2 (which does not possess enough electrons to conform to the octet rule) and CO 2. When writing out the electron dot formula for carbon dioxide, notice that the C-O bonds are double bonds; this makes no difference to VSEPR theory.
How are non bonding electrons included in the shape of a molecule?
For molecules of water and ammonia, however, the non-bonding electrons must be included in the calculation. In each case there are four regions of electron density associated with the valence shell so that a tetrahedral bond angle is expected.