What is the Difference Between Linear and Bent Molecules?
🆚 Go to Comparative Table 🆚The main difference between linear and bent molecules lies in the arrangement of their atoms. Here are the key differences:
- Linear molecules have atoms bonded to each other, forming a straight molecule with a bond angle of 180°. Examples of linear molecules include carbon dioxide (CO2) and nitrogen (N2).
- Bent molecules have atoms arranged in a bent shape with an angle less than 180°. The bent structure of these molecules is often a result of the presence of lone electron pairs in the central atom. Examples of bent molecules include water (H2O), nitrogen dioxide (NO2), and hydrogen peroxide (H2O2).
Another difference between linear and bent molecules is the presence of lone pairs of electrons on the central atom. For a molecule to be linear, it does not have any lone pairs of electrons on the central atom, while a bent molecule has at least one lone pair.
Comparative Table: Linear vs Bent Molecules
The main difference between linear and bent molecules lies in the arrangement of their atoms and the angles between them. Here is a comparison table highlighting the differences:
| Feature | Linear Molecules | Bent Molecules |
|---|---|---|
| Shape | Straight structure, with a 180° bond angle | Bent structure, with an angle less than 180° |
| Lone Pairs | No lone pairs around the central atom | One or two lone pairs on the central atom, which push the other atoms away and cause the bent shape |
| Electron Pair Repulsion | No repulsion due to lone pairs | Repulsion between electron pairs, leading to the bent structure |
| Examples | Typically have the molecular formula AX2, AX2E4, and AX2E3 | Commonly found in triatomic molecules and ions, such as water, nitrogen dioxide, and CH2 |
To determine if a molecule is linear or bent, you can use the VSEPR (valence shell electron pair repulsion) theory, which helps predict the geometry of molecules based on electron pair repulsion.
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