- Why PCl5 is Unsymmetric?
- How stable is PCl5?
- Which is more stable PCl5 or PCl3?
- Why is PCl3 a Lewis acid?
- Why PCl5 is a good chlorinating agent?
- Is PCl5 trigonal bipyramidal?
- Why PCl5 is unstable?
- What is shape of PCl5?
- What is the Lewis dot structure of PCl5?
- Is PCl5 an acid?
- Is PCl5 acid or base?
- What is the use of PCl5?
Why PCl5 is Unsymmetric?
there is a theoretical reason (VSEPR) for PCl5 to be non-polar.
The electron pairs in the five P-Cl bonds repel each other (while being attracted to the phosphorus nucleus).
For a contrast, consider PCl3, which has a trigonal pyramid geometry (with a lone pair on the phosphorus atom) according to VSEPR theory..
How stable is PCl5?
In Phosphorous pentachloride, the central Phosphorous atom is sp3d2 hybridised. … It acquires such a shape so as to minimize the interelectronic repulsion between the Cl atoms. Hence it is fairly stable. In certain conditions, it decomposes to form Phosphorous trichloride(more stable) and chlorine gas.
Which is more stable PCl5 or PCl3?
PCl3 is more stable than PCl5 because PCl5 has steric crowding(triagonal bipyramidal shape and sp3d2 hybridisation) than PCl3(triagonal planar structure and sp3 hybridisation).
Why is PCl3 a Lewis acid?
Answer. Phosphorus trichloride has a lone pair, and therefore can act as a Lewis base. For example with the Lewis acidsBBr3 it forms a 1:1 adduct, Br3B−−+PCl3. … Remember when you draw the Lewis structure for PCl5 that Phosphorous (P) is in Period 3 on the Periodic table.
Why PCl5 is a good chlorinating agent?
PCl5 has a trigonal bipyramidal shape in which P-Cl (a) bonds are slightly larger than the P-Cl (e ) bonds. This makes the molecule rather unstable. It dissociates to lose two chlorine atoms involved in the axial bonds and acts as a chlorinating agent.
Is PCl5 trigonal bipyramidal?
Answer. In case of , P has 5 valence electrons in orbitals. To make 5 bonds with 5 Cl atoms, it will excited one of its electron from 3s to 3d therefore the hybridization will be . And with hybridization the geometry will be trigonal bipyramidal whereas in case of , the Iodine atom has 7 valence electrons in .
Why PCl5 is unstable?
Answer: PCl5 is unstable because phosphorus forms 5 bonds with cl atoms out of which the two axial bonds have more Bond length than three equatorial Bond length this result in repulsion and thereby making the axial bonds weak.
What is shape of PCl5?
Trigonal Bipyramidal Shape PCl5 (phosphorus pentachloride) is a molecule representative of trigonal bipyramidal bond angle geometry & is roughly 300mm (12″) high on the long axis when constructed with Unit model parts.
What is the Lewis dot structure of PCl5?
There are a total of 40 valence electrons in the PCl5 Lewis structure. Remember when you draw the Lewis structure for PCl5 that Phosphorous (P) is in Period 3 on the Periodic table. This means that it can hold more than 8 valence electrons.
Is PCl5 an acid?
Lewis acidity Phosphorus pentachloride is a Lewis acid.
Is PCl5 acid or base?
It is neither a base nor a acid . it is a salt.
What is the use of PCl5?
Uses of Phosphorus Pentachloride – PCl Used as a chlorinating agent and catalyst ш making organic chemicals, intermediates, dyestuffs, etc. Used as a catalyst in the manufacture of acetyl cellulose the plastic film on which motion pictures are printed. Used as a chlorinating agent in organic chemistry.