The extent of sidewise overlapping is less than the axial overlapping. So, the bond formed from the overlapping of two p orbitals laterally is weaker.
During the axial overlap of p-p orbitals, the electron density increases around the axis, so the bond formed is the strongest. Therefore, the strongest bond formed is when p-p orbital overlap occurs.
The ionic bond is generally the weakest of the true chemical bonds that bind atoms to atoms.
The extent of overlap is higher for s orbital than for p orbital. Higher is the extent of overlap, stronger is the bond formed. Was this answer helpful?
The orbital overlap is strongest when the orbitals overlap along the inter nuclear axis because the extent of orbital overlap is maximum.
In a 1s orbital 1 is the principal quantum number. As the principal quantum number increases the extent of overlapping would decrease. Hence by taking this factor into account, we can eliminate options B and C. Because 1s orbital would have a higher bond strength.
The strength of a covalent bond is proportional to the amount of overlap between atomic orbitals; that is, the greater the overlap, the more stable the bond. An atom can use different combinations of atomic orbitals to maximize the overlap of orbitals used by bonded atoms.
The connection formed is the strongest because the electron density increases around the axis during the axial overlap of Orbitals. As a result, the strongest link is formed when the Orbitals overlap.
s orbitals are closer to the nucleus than the p orbitals. Hence, more is the p character, more is the efficiency of overlap.
Thus, we will think of these bonds in the following order (strongest to weakest): Covalent, Ionic, Hydrogen, and van der Waals. Also note that in Chemistry, the weakest bonds are more commonly referred to as “dispersion forces.”
Hydrogen bonds
This interaction is called a hydrogen bond. Hydrogen bonds are common, and water molecules in particular form lots of them. Individual hydrogen bonds are weak and easily broken, but many hydrogen bonds together can be very strong.
The three types of chemical bonds in order of weakest to strongest are as follows: ionic bonds, polar covalent bonds, and covalent bonds.
1s-1s > 2s - 2p > 2p - 2p (axial)
p orbitals when overlap on the same symmetrical axis at 180 degree bond angle the bond formed is the strongest bond.
The extent of overlap is higher for a hybrid orbital than their parent orbital and also s orbital than for a p orbital. Higher the extent of overlap, stronger is the bond formed.
A sigma (σ) bond is stronger than a pi (π) bond.
Negative Overlapping of Atomic Orbitals – When the phase of two interacting atomic orbitals is opposite, then the overlap is negative and in this case, the bond is not formed.
By the axial overlapping of two p-orbitals of the same energy, a strong sigma bond is formed.
Positive Overlap of Atomic Orbitals: Positive overlap occurs when the phase of two participating atomic orbitals is the same. This overlap results in bond formation. Negative Overlap of Atomic Orbitals: When the phase of participating atomic orbitals is opposite to each other, negative overlap takes place.
The overlap between one half filled s orbital of one atom and one half filed p orbital of another atom containing electrons with opposite spins is called as s-p overlapping.
Chemical bonds have different strengths. Atoms that are more strongly attracted to each other have a stronger bond strength and are more stable. More energy is required to break stronger chemical bonds as compared to the energy required to break weaker chemical bonds.
Usually, the shorter the bond the stronger the bond. The longer the bond the weaker the bond.