The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. Based on the Lewis structure given, the formal charge on the central xenon atom is
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.
The image shows a Lewis structure of xenon tetrafluoride (\( \text{XeF}_4 \)). In this diagram:
- The central atom, xenon (\( \text{Xe} \)), is bonded to four fluorine (\( \text{F} \)) atoms.
- Each fluorine atom is surrounded by three pairs of dots, representing lone pairs of electrons.
- Solid lines between the xenon and fluorine atoms depict covalent bonds, indicating shared pairs of electrons.
- The xenon atom also has two lone pairs of dots.
Based on the Lewis structure given, the **formal charge** on the central **xenon** atom is \([ \text{Box for answer} ]\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F22d43075-54d6-45bf-85ef-42ccc8523dda%2F0d9eb075-6b2b-4570-827f-ab38e060ec99%2F3c0u69y_processed.png&w=3840&q=75)
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