A p bond is the result of the
sideways overlap of two parallel p orbitals.
The P-P-P bond angle in white phosphorus is approximately 60 degrees.
The P-Cl bond is more polar than the P-Br bond. This is because chlorine (Cl) is more electronegative than bromine (Br), so it attracts the shared electrons in the bond more strongly, leading to a greater difference in electronegativity and thus a more polar bond in P-Cl compared to P-Br.
Among s-s,s-p,p-p sigma P-P is strong enough because of greater overlapping.The bond strengths for sigma S-S is 1.0 ,for sigma S-P is 1.71 and for sigma P-P is 3.0. so sigma P-P is stronger it means that it is more stable. But many books they have given that s-s overlapping is more than p-p overlapping .This is not true because due spherical shape of the s orbital the charge is symmetrically distributed and also small size there will not effective overlapping of orbitals as P-P overlapping .So P-P bond is stronger than S-S bond.
the f-p-f bond angle is 120the cl -p-cl bond angle is 180and the f - p - cl bond angle is 90
A covalent bond forms between Cl and P. In this bond, the atoms share electrons to achieve a stable electron configuration.
A nitrogen-phosphorus bond (N-P) is a covalent bond, where the atoms share electrons to form a stable molecule. This type of bond is typical in compounds such as phosphazenes and phosphoranes.
The bond order of P-O in PO4^3- is 1.33. This is calculated by taking the total number of bonds and dividing by the total number of bond groups present. In the case of PO4^3-, there are 4 P-O bonds and 3 bond groups, so the bond order is 1.33.
180
The P=O bond in phosphorus pentoxide (P2O5) is a double bond with one sigma bond and one pi bond. The oxygen atom donates an electron pair to form the sigma bond, while the second bond is formed by the sideways overlap of p orbitals from phosphorus and oxygen atoms.
The bond in C2H4 is a double bond, specifically a pi bond formed by the side-to-side overlap of two p orbitals. This type of bond is stronger than a single bond but weaker than a triple bond.
It means bond is very stable or strong.
The side-by-side overlap of p orbitals produces a pi bond. This type of bond is formed when two p orbitals share electrons through sideways overlap, resulting in a network of electron density above and below the bonding axis. Pi bonds are weaker than sigma bonds, which form from the head-on overlap of orbitals.