Draw a Lewis structure for dihydrogen phosphate ion, H₂PO4, adding charges and lone electron pairs to the appropriate atoms. O Explicitly draw all H atoms. • Include all valence lone pairs in your answer. ●
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.
![### Drawing the Lewis Structure for Dihydrogen Phosphate Ion (H₂PO₄⁻)
**Task Description:**
Draw a Lewis structure for dihydrogen phosphate ion, H₂PO₄⁻, adding charges and lone electron pairs to the appropriate atoms.
**Instructions:**
- Explicitly draw all H atoms.
- Include all valence lone pairs in your answer.
The image provided shows a blank workspace from the ChemDoodle software, which is a tool for drawing chemical structures. At the top of the workspace, there are various drawing tools and options that can be used to create the desired structure.
### Steps to Draw the Lewis Structure for H₂PO₄⁻:
1. **Identify the Total Number of Valence Electrons:**
- Hydrogen (H): 1 electron × 2 H = 2 electrons
- Phosphorus (P): 5 electrons
- Oxygen (O): 6 electrons × 4 O = 24 electrons
- Additional electron for the charge: +1 electron
- Total: 2 + 5 + 24 + 1 = 32 valence electrons
2. **Determine the Central Atom:**
- Phosphorus (P) will be the central atom since it can form more bonds compared to hydrogen or oxygen.
3. **Draw the Skeleton Structure:**
- Place the phosphorus (P) atom in the center.
- Connect it to four oxygen (O) atoms.
4. **Distribute Electrons to Complete the Octet Rule:**
- First, distribute the remaining valence electrons around the oxygen atoms to complete their octets.
- Then, if any electrons remain, place them around the central phosphorus atom.
5. **Consider Formal Charges and Resonance:**
- Adjust the structure to minimize formal charges, ensuring that the overall charge of the ion is -1.
6. **Add Hydrogen Atoms:**
- Attach the two hydrogen (H) atoms to two of the oxygen (O) atoms.
### Example of the Lewis Structure for H₂PO₄⁻:
```
O O
| |
H - O - P - O⁻
|
H
```
In this structure:
- Phosphorus (P) is the central atom.
- Two oxygen (O) atoms are bonded to two hydrogens (H).
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