15. In the Lewis structure for nitrite, what is the formal charge on the nitrogen atom?...

15. The leats structure & for nitrite Ň (NG) Fromal change on the nitrogen atoma nus - [2 Mbp + hub] Mors non numbers of Valance electrone Mbp a numbers of bonding electrons. naba numbers of nonbonding electrons.

Up (0) 5 - 1 kx6 +2] = 6-1342) > 0 (formal change) Ans: option A 20. 16. The molecule AX3 G (a central atom with 3 atoms attached and I lone pairs); A = central atan Xa substituent atomas & lone pairs. According to Vs EPR theory the geometry of the central atom must be tetrahedosal in natura But due to the presence of One Lone pain E. the shape of the molecule becomes Trigonal pynamid.

XX 17. Here inch, the Cl- a bond roepresents a nonpolar Covalent bond, since it is a homonuclear diatomic molecule so, here partial Separation of charge are is not possible. Both atoms have equal electronegativity And option ara In, Nad s Nat a lonie ina nativce and H-f here fis. more electronegative than H, So bond polarisation appears. Sts-

A.

V. B. c. EEN H Among the three ions only in A Nho has only Sigma bonds in ite lewis Structure. In No, and CN- there are one and two ł-bonding present respectively.

19. Brock valance electronic Configuration of central artem Bro - [Ar]3d10 45 4822 Broin 7 Exfox[17] Ex bax! | I Т ГО g a aa a ali el's electrons are preporesented as a sign. and Bro electrons are represented as 7 arrowsign. ence, In Brody, the central atom Bo is spid- hybridised, so the geometry will be octahedral Due to the presence of one lone pairs the molecular Shape will be square pyramid; 90, 188 (Ans :) ata & Bro a- 1 a

20. The given meaction is: CO + H₂ H₂otco Relative bond enthalpies: C-O 358 kJ/mol H-O 463 kJ/mol C=0 743 kJ/ml C=O: 1072 kJ/mol H-H : 436 kJ/mol 0-0 146 kJ/mole Hneactorst : o=C=0 + H H - 2x(c=0) + 1*(H-H) = (2x 743 +436) = 1922 kJ based 44product: Hot & Co 2(0-H) + 1x(co) >(2x463 + 1072) > 1998 KJ przed 2.

A Hooxn 2 Almeactant - Att product (1922 – 1998)Kimata - 76 k3 m