Explain why N(2) has a greater bond diss...

Explain why `N_(2)` has a greater bond dissociation energy than `N_(2)^(+)` while `O_(2)` has lesser bond dissociation energy than `O_(2)^(+).`

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How many nodal planes are present in the following MO's (Taking Z-axis as the internuclear axis) (i) sigma ls (ii) sigma^(**) ls (iii) sigma2p_(z) (iv) sigma^(**)2p_(z) (v) pi 2p_(y) (vi) pi^(**)2p_(x) or pi^(**)2p_(y) Give the number of electrons which occupy the bonding orbitals in H_(2)^(o+) H_(2) and O_(2)^(o+) (c ) Why N_(2) has greater bond dissociation energey than N_(2)^(o+) whereas O_(2)^(o+) has greater bond dissociation energy than O_(2) .

State the bond order and indicate whether the species is paramagnetic (i) B_(2) (ii) C_(2) (iii) N_(2) (iv) O_(2) (v) Br_(2) (vi) CI_(2)^(o+) Which of the following molecules has the highest bond order (i) Ne_(2) (ii) F_(2) (c) Explain why N_(2) has a greater dissociation energy than N_(2)^(o+) , whereas O_(2) has a lower dissociation energy tnan O_(2)^(o+) (b) The bonding sigma 2s orbital has a higher energy than the antibonding sigma^(**) 1s orbitals Why is the former a bonding orbital while the latter is an antibonding .

N_(2)^(+) has greater bond dissociation enthalpy than N_(2) molecule.

(a) H_(2)^(+)and H_(2)^(-) ions have same bond order but H_(2)^(-) ion is more stable. Explain. (b) N_(2) has a greater bond dissociation enthalpy than N_(2)^(+) ion hals more bond dissociation enthalpy than O_(2). Why ? (c ) Can we have ahomonuclear diatomic molecule with all its ground state molecular orbitals full of electrons ? (d) When a magnet is dipped in a jar of liquid oxygen, some oxygen clings to it. Assign reason :

Which has the largest bond dissociation energy?

F_2 has lower bond dissociation enthalpy than Cl_2. Why?

Molecular orbitals are formed by the overlap of atomic orbitals. The combining orbitals must have proper orientation so that they can overlap to a considerable extent. Two atomic orbitals combine to form two molecular orbitals called bonding molecular orbital and antibonding molecular orbital. Bonding molecular orbital is stable and antibonding molecular orbital is unstable. sigma MO is formed by head on overlap while pi MO is formed by sidewise overlap. The MOs are filled with electrons according to the same rules as followed for filling atomic orbitats. Bond order is one of the most important parameter to compare the bond strength and bond length of bonds. Why has N_2 a larger dissociation energy than N_2 ^(+) whereas O_2 has a lower dissociation energy than O_(2)^(+) ?

The distribution of electrons among molecular orbitals is called the electronic configuration of the molecule which provides us the following very important informations about the molecule. (A)Stability of molecule : The molecule is stable if number of bonding moleculer orbital electrons (N_b) is greater than the number of antibonding molecular orbital electrons (N_a) . (B) Bond order : Bond order =1/2(N_b-N_a) A positive bond order means a stable molecule while a negative or zero bond order means an unstable molecule. ( C)Nature of the bond : Bond order 1,2 and 3 corresponds to single , double and triple bonds respectively. (D)Bond length: Bond length decreases as bond order increases. (E)Magnetic nature: Molecular orbitals in a molecule are doubly occupied , the substance is diamagnetic and if one or more molecular orbitals are singly occupied, it is paramagnetic. N_2 has greater dissociation energy than N_2^+ , where as O_2 has a lower dissociation energy than O_2^+ because

DINESH PUBLICATION-CHEMICAL BONDING AND MOLECULAR STRUCTURE -COVALENT AND CO-ORDINATE BONDS

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