In spite of being an odd electron molecule `ClO_(2)` does not dimerise because.a) The odd electron is localised in the chlorine atom of "p `pi`-p `pi` bonding in the central atom b) The two "Cl-O" bonds do not have the same length c) The odd electron is delocalised

which of the following is odd electron molecule A) MgO B) NO_(2) C) C Cl_(4) D)HF

The molecule exhibiting maximum number of non-bonding electron pairs (l.p.) around the central atom is :

Assertion : The double bond in C_(2) molecule consider of both pi bonds Reason :Four electrons are presents in two pi bonding molecule orbital in C_(2)

Write the electron-dot structure for sodium and chlorine atoms. How do these form a chemical bond? Name the type of bond so formed. Why does a compound so formed have high melting point?

A : Heavier elements of 14th group do not form p pi - p pi bonds . R : Atomic orbital of heavier elements are too large and do not have effective overlapping .

A central atom in a molecule has two lone pairs of electrons and forms three single bonds. The shape of this molecule is :

The difference in the total number of lone pairs of electrons on all atoms and bond pair of electrons in P_(4)O_(6) is

Assertion : To obtain effefctive p pi-p pi overlap, the size of the de-orbital must be similar to the p- orbital so the chlorine p pi-p pi bonding is strongest in their oxoanions. Reason :On moving period from left to right in the periodic table, the nuclear charge is incresed and more s and p-electrons are added. Since these s- and p- electron shield the nuclear charge incompletely, the size of the atom and that of the d- orbital decreases .This leads to progressively stronger p pi-d pi bonding.