Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
![**Title: Understanding Basicity in Organic Compounds**
**Introduction:**
In organic chemistry, the basicity of a compound refers to its ability to accept protons. The basicity of amines and related compounds can vary significantly based on their structure. Below, we will arrange a series of compounds in order of increasing basicity.
**Compounds to Arrange:**
1. **Compound [I]:** Aniline - A benzene ring with an amino group (NH₂) attached.
2. **Compound [II]:** Nitroaniline - A benzene ring with both an amino group (NH₂) and a nitro group (NO₂) attached.
3. **Compound [III]:** Ethylamine - A straightforward aliphatic amine with the structure CH₃CH₂NH₂.
4. **Compound [IV]:** Isopropylamine - An aliphatic amine with the structure (CH₃)₂CHNH₂.
5. **Compound [V]:** Ammonia - NH₃, a simple inorganic compound.
**Analysis:**
The basicity of these compounds is influenced by the electronic effects of substituents and the availability of the lone pair on the nitrogen atom for protonation.
1. **Aniline** is less basic due to the resonance stabilization of the lone pair on nitrogen with the benzene ring.
2. **Nitroaniline** is even less basic compared to aniline because the electron-withdrawing nitro group further reduces the electron density on the nitrogen, making it less available to accept protons.
3. **Ethylamine** and **Isopropylamine**, being aliphatic amines, are generally more basic than aromatic amines like aniline because aliphatic chains donate electron density via inductive effects, making the lone pair on nitrogen more available.
4. **Ammonia** is the reference basic compound and, in this series, is more basic than aromatic amines like aniline and nitroaniline but less basic than aliphatic amines due to less electron-donating ability.
**Conclusion:**
Based on these considerations, the order of increasing basicity is as follows:
\[ \text{II (Nitroaniline)} < \text{I (Aniline)} < \text{V (Ammonia)} < \text{III (Ethylamine)} < \text{IV (Isopropylamine)} \](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2a1b3fd2-2e90-43fb-8484-e4a13c72498e%2F7e25b20b-393e-425e-a964-4b372be043a3%2Fgvkn9co_processed.jpeg&w=3840&q=75)
The tendency to donate the electron pairs to any other element is known as basicity. The presence of electron withdrawing groups decrease the basicity while electron donating group increase the basicity.
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