Is PCl5 reactive or non reactive?

Correct option 4 PCl5 molecule is non-reactiveExplanation:3. TrueAxial bond : 240 pm Equatorial bond : 202 pm4 FalseDue to longer and hence weaker axial bonds PCl5 is a reactive molecule.

What’s the difference between PCl3 and PCl5?

Phosphorus Trichloride is more stable than Phosphorus pentachloride because PCl5 has more density (trigonal bipyramidal and sp3d2 hybridisation) than PCl3 (structure of the trigonal planet and sp3 hybridisation).

Which is more reactive PCl5 or sf6?

Since it suffers more repulsion it is longer than the other bonds. Also these are weak bondsand therefore these bonds can break easily . Because of these reasons,PCl5 is very reactive.

Why PCl5 is more common than PCl3?

The p-Block Elements. Account for the following: (i) PCl5 is more covalent than PCl3. (i) Greater the positive oxidation state of the central metal atom, greater is its polarising power and thus more is the covalent character of the bond formed between the central metal atom and other atoms.

What happens when PCl3 reacts with water?

Overview. Phosphorus trichloride (phosphorus chloride, PCl3) is a colorless fuming liquid that reacts violently with water to liberate phosphoric acid and hydrogen chloride (HCL) gas.

Is PCl3 stable or unstable?

PCl3 – is a STABLE molecule because all the atoms of the molecule have 8 valence electrons…

Why SF6 is stable than pf5?

SF6 is extremely stable for purely steric reasons, because S is completely blocked by fluorine atoms from all directions, so the reactions starting with an attack on S that otherwise would readily occur (hydrolysis, etc.) never have the chance to occur. This has nothing to do with electronegativity.

Is pf5 less stable than SF6?

Statement 1: PF_(5) molecule is little less stable as compared to SF_(6) molecule.

Is PCl5 a chlorinating agent?

(a) PCl5 has a trigonal bipyramidal shape in which P—Cl (axial) bonds are slightly larger than the P—Cl (equatorial) bonds. This makes the molecule, rather, unstable. It dissociates to lose two chlorine atoms involved in the axial bonds and thus, acts as a chlorinating agent.