Compute the formal charge (FC) on each atom in the following structures. (a) Methane (CH₂) H H:C:H H two nonbonding electrons (b) The hydronium ion, H, O+ HAO H H three bonds, six bonding electrons) Boron has four bonds, eight bonding electrons HH (c) H₂N-BH, H&N BH HH Nitrogen has four bonds, eight bonding electrons (d) [H,CNH,]* H>C=N
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.
please explain answer
- The central carbon atom is single-bonded to four hydrogen atoms (H).
The formal charge on the central carbon (C) and each hydrogen (H) atom in methane is calculated as follows:
- For Carbon (C):
\[
FC = \text{Valence electrons} - \left(\frac{\text{Bonding electrons}}{2}\right) - \text{Nonbonding electrons}
\]
\[
FC_{\text{C}} = 4 - \left(\frac{8}{2}\right) - 0 = 4 - 4 - 0 = 0
\]
- For each Hydrogen (H):
\[
FC_{\text{H}} = 1 - \left(\frac{2}{2}\right) - 0 = 1 - 1 = 0
\]
#### (b) The Hydronium Ion (H₃O⁺)
- **Structure:**
- The central oxygen atom is single-bonded to three hydrogen atoms (H) and has one lone pair. The ion carries a positive charge.
The formal charge on central oxygen (O) and each hydrogen (H) atom in the hydronium ion is:
- For Oxygen (O):
\[
FC_{\text{O}} = 6 - \left(\frac{6}{2}\right) - 2 = 6 - 3 - 2 = 1
\]
- For each Hydrogen (H):
\[
FC_{\text{H}} = 1 - \left(\frac{2}{2}\right) - 0 = 1 - 1 = 0
\]
#### (c) Ammonia-Borane (H₃N−BH₃)
- **Structure:**
- The nitrogen atom (N) is single-bonded to three hydrogen atoms (H).
- The boron atom (B) is single-bonded to three hydrogen atoms (H).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1cf81ca3-2485-4010-80d9-cb2da241c90c%2F1ee316e3-2fc6-4fa4-8176-49f0bf427a4c%2Flgwbfp_processed.png&w=3840&q=75)
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