Energy can be stored in chemical bonds. The amount of energy in a bond is somewhat counterintuitive – the stronger or more stable the bond, the less potential energy there is between the bonded atoms. Strong bonds have low potential energy and weak bonds have high potential energy.

During an exothermic reaction bonds break and new bonds form and protons and electrons go from a structure of higher potential energy to lower potential energy. During this change, potential energy is converted to kinetic energy, which is the heat released in reactions.

It takes roughly 100 kcal of energy to break 1 mol of C–H bonds, so we speak of the bond energy of a C–H bond as being about 100 kcal/mol. A C–C bond has an approximate bond energy of 80 kcal/mol, while a C=C has a bond energy of about 145 kcal/mol.

Among covalent bonds, triple bonds are stronger than double bonds and double are stronger than single bonds. Hydrogen bonds are weaker than all, but they play a big role in determining the properties of important compounds such as proteins and water….Bond Energy.

s orbitals spend more time close to their respective nuclei, and less in the binding region. p orbitals spend more time in the binding region; that is close both the nuclei; thus s-p overlap forming a stronger bond than s-s overlap.

sp3

Since a higher energy level implies lower stability, an sp-sp bond must have the lowest energy level, since it is formed by the overlap of one sigma and two pi bonds in total, more than those in sp2-sp2 or sp3-sp3. Hence, energy level(sp

Since s orbital is closest to the nucleus, thus electron which is present in orbitals with more s character will be more attracted by the nucleus and as a result electronegativity of sp is greater than the other two. Therefore sp is more acidic followed by sp2 and sp3.

Thus a hybrid orbital having more s-character will be more close to the nucleus and thus, more electronegative. This gives us the answer why sp carbon is more electronegative than sp2 and sp3 carbons. Also, more the %s character in the hybrid orbitals, the stronger are the bonds formed.

Re: Are the Sp3 orbital is a stronger base than the sp2 atom? sp2 hybridized atoms are more electronegative than sp3 hybridized ones due to greater s-character. So, the sp2 atoms tend to keep the unshared pair of electrons to themselves rather than giving them away to an acid’s proton.

Now if acids are inverse to basses meaning the stronger something is as an acid the weaker it is as a base we can say that basicity goes in the exact opposite direction. That means something sp is most acidic but less basic and sp3 which was least acidic is going to be most basic.

An increase in s character on an atom increases the electronegativity of that atom which favors acidity and therefore disfavors basicity. Hence sp3-hybridized nitrogen is more basic than either sp2 or sp hybridized nitrogen.

Hybridization only occurs in response to bond formation, that is an atom will not just spontaneously hybridize on its own. Further, an atom will only hybridize if hybridization leads to the formation of a more stable (lower energy) molecule.

Atom Size – As the atom size increases down a column on the periodic table, the acidity increases. As the electronegativity of an atom increases from left to right across a row, the acidity increases. Inductive Effect – An electronegative atom will withdraw electron density, stabilizing the conjugate base.

The bond strength of an acid generally depends on the size of the ‘A’ atom: the smaller the ‘A’ atom, the stronger the H-A bond. When going down a row in the Periodic Table (see figure below), the atoms get larger so the strength of the bonds get weaker, which means the acids get stronger.

3. Acidity Trend #2: The More “Polarizable” The Atom, The Better It Is Able To Stabilize Negative Charge. High charge densities tend to be less stable than low charge densities. The more “spread out” a charge can be, the more stable it will be.

Because resonance allows for delocalization, in which the overall energy of a molecule is lowered since its electrons occupy a greater volume, molecules that experience resonance are more stable than those that do not.

ANSWER: Protons (a) are the most acidic. Method 2. Proton (a) are bonded to SP3 carbons so pka ≈ 50. Proton (b) is bonded to a more electronegative atom (S).