(a) If the valence atomic orbitals of an atom are sp hybridized,how many unhybridized p orbitals remain in thevalence shell? How many p bonds can the atom form?(b) Imagine that you could hold two atoms that are bondedtogether, twist them, and not change the bond length.Would it be easier to twist (rotate) around a single s bondor around a double 1s plus p2 bond, or would they be thesame?
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.
(a) If the valence atomic orbitals of an atom are sp hybridized,
how many unhybridized p orbitals remain in the
valence shell? How many p bonds can the atom form?
(b) Imagine that you could hold two atoms that are bonded
together, twist them, and not change the bond length.
Would it be easier to twist (rotate) around a single s bond
or around a double 1s plus p2 bond, or would they be the
same?
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