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1. The radius of anion is greater than atom while that of cation is lesser than atom.

2.Half-filled and fully-filled orbitals are more stable.

3. The first ionization energy of carbon atom is greater than that of boron whereas the reverse is true for the second ionization energy. Explain.

4. The first ionization potential of N is maximum as compared to those of C and 0.

5. The ionic size of Cl- ions is greater than that of K+, though the two Ions are isoetectronic, Give reasons.

6. The electron affinity of chlorine is greater than that of F.

7. The electron affinity of sulphur is greater than that of oxygen.

8. The electron affinity of phosphorus is greater than that of nitrogen.

9. The first ionization energy of B is less than that of Be.

10. Atomic radius of N is creater than that of 0.

11. Atomic radii decrease from left to right in a period.

12. Atomic size increases down a periodic group.

13. First Ionisatioii potential of nitrogen is higher than the first ionisation potential of oxygen.

14. Explain why Be and Mg atoms do not impart colour to the flame.

15. The values of IE1 and IE2 (kJ/ mol ) of few elements designated by Roman numerals are shown below:

IE1 IE2

I 2372 5251

II 520 7300

III 900 1760

IV 1680 3380

Whichof the above eleiiietits islikely tobe

(A) reactive metal

(B) a reactive non-metal

(C) a noble gas

(D) a metal that forms a binary halide of formula AX2 (X is halogen)

16. Arrange the following in the required order of the properties

(A) C02, N205, SiO2, S03 (increasing acid character)

(B) N 3-, Na+, F-, 02-, Mg2+ (increasing ionic size)

(C)MgO, SrO, K20, NiO, CS20 (increasing base character)

(D) H20, OH-, CH 30- (increasing basically)

(E) HCI, HB2, HF, HI (increasing acid strength)

Note: (^)-stands for raise to the power. (A)-angstronm