Both PCl5 and PBr5 have trigonal bipyramidal geometry. This is not a regular structure and is not very stable. Therefore, PCl5 splits up into more stable octahedral and tetrahedral structures.
Q. How do you tell if it is ionic or covalent compound?
Classifying compounds as ionic or covalent
- If a compound is made from a metal and a non-metal, its bonding will be ionic.
- If a compound is made from two non-metals, its bonding will be covalent.
Q. Does PCl5 have ionic character?
Solid phosphorus pentachloride exhibits some ionic character.
Q. Why does PCl6 not exist?
PCl6- and PI6- does not exist as the maximum valency of P is 5. So in the given compound the existing compound is XeOF and FCl. The logic behind is the compound can exist with the maximum valency of the particular element.
Q. Why does PCl6 minus exist?
PCl5 is unstable due to electronic repulsion at axial bond. it exists as ions (PCl4+, PCl6+) as ionic bonding stabilises crystalline nature. PCl4+ and PCl6- having tetrahedral and octahedral structures respectively fit into each other providing extra stability.
Q. Why NCl 5 is not known but PCl5 is known?
It does not have d orbitals to expand its covalency beyond four. Hence, NCl5 is not known. PCl5 is known as P has vacant 3d orbital to which 3s electrons can be excited to make available five half filled orbitals needed for the formation of five P−Cl bonds. Was this answer helpful?
Q. Why PCl5 is possible?
Phosphorus can form PCl5 since it has vacant d-orbitals in its valence shell. NCl5 is not possible because of no vacant d-orbitals.
Q. Why does PCl3 and PCl5 exist?
Phosphorus is a period 3 element. Hence it has an empty d-orbital which the period 2 elements do not have. As phosphorus initially has valency as 3 it forms PCl3, and due to this expanded octet, PCl5 can also be formed.
Q. Which species does not exist?
(CCl6)2− species does not exist. Carbon cannot accept 6Cl−, since it has no vacant d-orbitals.
Q. Which does not exist sncl6?
Correct option d [CCl6] 2− Explanation:Carbon atom cannot expand its valency shell due to non availability of 2d sub shell so [CCl6]2− does not exist.
Q. Does H2 exist under normal conditions?
The ionization enthalpy of hydrogen is very high (1312kJmol-1). Hence, it is very hard to remvoe its only electron. As a result, its tendency to exist in the monoatomic form is rather low. Istead, hydrogen forms a covalent bond with another hydrogen atom and exists as a diatomic (H2), molecule.
Q. Which one of the following is not paramagnetic?
And S2− has no unpaired electron in its MO’s, so, it is diamagnetic.
