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.
Explain the influence of the electronegative atoms like chlorine on radical stability.
Introduction to Electronegativity
It is a measure of the atom's ability to attract electrons to itself. Electronegativity is commonly defined on Pauling's scale, which ranges from zero to four. Atoms with higher electronegativity values are more likely to attract electrons and form a covalent bond with another atom. For example, Oxygen has a higher electronegativity than Nitrogen, and so it is more likely to form a covalent bond with Hydrogen than Nitrogen. Electronegativity values can vary widely from one element to another, and from one bond to another. Electronegativity is an important concept in chemistry and is widely used to explain and predict chemical reactivity.
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