A skeletal structure for perchlorate (CIO) is shown below. Starting from this structure, complete the Lewis structure that follows the octet rule on all atoms. O I CI O Click to edit mecule O
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.
#### Description of Graph/Diagram:
In the diagram provided, which represents the skeletal structure of the perchlorate ion (ClO₄⁻), a central chlorine (Cl) atom is connected to four surrounding oxygen (O) atoms. Each connection is represented by a single line, which signifies a single bond between the chlorine atom and each oxygen atom.
- **Central Atom:** Chlorine (Cl)
- **Surrounding Atoms:** Four oxygen (O) atoms, each bonded to the central chlorine atom.
#### Steps to Complete the Lewis Structure:
1. **Count the Total Valence Electrons:**
- Chlorine (Cl) has 7 valence electrons.
- Each Oxygen (O) atom has 6 valence electrons, and with four O atoms, this totals 24 valence electrons.
- The perchlorate ion carries a -1 charge, so add an additional electron.
- Total valence electrons = 7 (from Cl) + 24 (from O atoms) + 1 (extra electron for the charge) = 32 valence electrons.
2. **Place Electrons Around Each Atom to Satisfy the Octet Rule:**
- Start by placing a single bond (2 electrons) between Cl and each O atom, which uses up 8 electrons (4 bonds x 2 electrons per bond).
- Distribute the remaining 24 electrons around each O atom to complete their octets.
- Each O atom requires 6 more electrons to complete its octet, resulting in 24 electrons (4 O atoms x 6 electrons per O atom).
3. **Check the Chlorine Atom:**
- The chlorine atom should be checked to ensure it follows the octet rule. Chlorine in this structure may need to share its electrons by forming double bonds with one or more oxygens to fulfill the octet requirement.
This exercise illustrates the importance of understanding the electron configuration around each atom to adhere to the octet rule while also considering the overall charge on the ion.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6895f9cd-8521-4c9a-bc62-df11c4ac3cae%2Fdc41c437-d775-49b7-ad1b-deb3732cd0ef%2Fgrrwfzq_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
