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.
Part 1: Nomenclature
- What are covalent compounds (molecules)? Give two examples of covalent compounds and their formula.
- What are binary ionic compounds (formula units)? Give two examples of binary ionic compounds and their formula
- What is the difference between naming of cations with variable charge and compounds with fixed charge? Give two examples of each and their formula
- What are polyatomic ions? Give two examples of polyatomic ions and their formula
- Give two examples of compounds containing polyatomic ions and their formula
- Give an example of names of binary acids (not containing a polyatomic ion) in aqueous solution and its formula.
- Give an example of an oxyacid (containing a polyatomic ion) inn aqueous solution and its formula.
Part 2: Structure, Shape and polarity
- Draw the Lewis structure of PH3
- draw the electronic geometry and name the geometry (hint: very similar to NH3)
- draw the molecular geometry and name the geometry
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