6. Assign the formal charges of the “heavy" atoms (non-hydrogen atoms, so in this case C's, N, O and P) in the Lewis structure below. Note that you should not add or erase (©) the lone pairs H H H H H. a.
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
Assign the formal charges of the “heavy” atoms (non-hydrogen atoms, so in this case C’s, N, O and P) in the Lewis structure below. Note that you should not add or erase the lone pairs
![**6. Assign the formal charges of the “heavy” atoms (non-hydrogen atoms, so in this case C’s, N, O, and P) in the Lewis structure below. Note that you should not add or erase (⊝) the lone pairs.**
[Image of a Lewis structure]
- The structure includes the following atoms: Carbon (C), Nitrogen (N), Oxygen (O), Phosphorus (P), and Chlorine (Cl). Hydrogen atoms (H) are attached to the carbons and nitrogen.
- Detailed explanation of the Lewis structure:
- Five carbon atoms are present, each with four single bonds (or lone pairs).
- Nitrogen (N) is bonded to one carbon and has one lone pair.
- Phosphorus (P) is bonded to a carbon, chlorine (Cl) which has three lone pairs, and oxygen (O) which has two lone pairs.
For each non-hydrogen atom's formal charge calculation, use the formula:
\[ \text{Formal Charge} = (\text{Valence electrons}) - (\text{Non-bonding electrons}) - \frac{1}{2}\times (\text{Bonding electrons}) \]
where:
- Valence electrons are the number of electrons in the outermost shell of the atom.
- Non-bonding electrons are the electrons not involved in bonds (lone pairs).
- Bonding electrons are the electrons shared in bonds (each bond has 2 electrons).
Apply this formula to each heavy atom to determine its formal charge.
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