Why is nf5 unstable

Favourite answer. There are valent d-orbitals in the outer most orbit of phosphorus and hence it shows variable covalence 3 and 5 in ground state and excited state respectively. Octet configuration is defined as the atom that should contain 8 electrons in the valence shell.

So, Nitrogen is unable to give pentahalides, Nitrogen only forms trihalides. Nitrogen is gas but phosphorus is a solid because Nitrogen pairs up, into the N2 molecule which has a very strong triple bond. In phosphorus, the atoms do not pair up, they bond to their neighboring atoms, thus forming a network of bonding that holds the atoms together into a solid. That is because the nitrogen atom is small and there is simply not enough room around the atom to shoe-horn in five atoms.

Nitrogen is found to have either 3 or 5 valence electrons and lies at the top of Group 15 on the periodic table. Why are the dihalides of carbon unstable but the dihalides of tin and lead are stable? Which of the following arrangement of molecule is correct on the basis of their dipole moment?

Distinguish between stable, unstable and neutral equilibrium of a body. Are heavy nuclei stable or unstable? Give reason. When is the equilibrium of a current carrying coil is stable or unstable?

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Efficient iterative schemes for ab initio total-energy calculations using a plane-wave basis set. B 54, — From ultrasoft pseudopotentials to the projector augmented-wave method.

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Grimme, S. A consistent and accurate ab initio parametrization of density functional dispersion correction DFT-D for the 94 elements H-Pu. Effect of the damping function in dispersion corrected density functional theory. On the basis of this definition, scandium and zinc do not count as transition metals — even though they are members of the d block. The zinc ion has full d levels and does not meet the definition either.

Transition elements are defined as elements that form at least one ion that contains partially filled d orbitals. The electronic configuration for a zinc atom is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d As none of the d orbitals are partially, zinc cannot be classified as an transition element. Therefore, copper is a transition elements.

Therefore, zinc is not considered as a true transition element, but its electronic configuration does not fit in the quantum mechanical definition. Stability depends on the hydration energy enthalpy of the ions when they bond to the water molecules.