Explain the following:
a. Which of the following `Na, Mg, Si` and `P` would have the greatest difference between the `IE_(1)` and `IE_(2)`? Explain?
b. The `EN's` of `B, Al` and `Ga` are `2.0, 1.5` and `1.6` respectively. The trends is not regular.Explain?
c. `Li_(2)CO_(3)` decomposes on heating but other alkali metal barbonate ( e.g. `Na_(2)CO_(3)`) does not. Explain?
d. Expalin why `Cu^(o+)` is found only is solid state and not solutions.
e. `Be` of `N` have extremely low value of `EA` (i.e. less negative value)against the trend. Explain?
f. Arrange the following in decreasing order of their properties indicated:
`Na^(o+)Mg^(2+)` and `Al^(3+)`
i. Ionic mobillity in `H_(2)O`
ii. Size of ions
iii. Standard reduction protential `(E_(M^(x+(aq.)))^(ɵ)//M_(s))`
iv. Extent of hydration
v. Hydration energy
vi. Size of hydrated ions
g. In iodomentry. why `KI` is not added dropwise to an acidified solution of `KMnO_(4)` but reverse is done?
h. Why the decrease in size between `Li` and `Be` is much greater than that between `Na` and `Mg` or `K` and `Ca`?
i. `K_(2)CO_(3)` is less soluble than `Cs_(2)CO_(3)` or `Rb_(2)CO_(3)` while among group `2` elements `MgCO_(3)` is more soluble than `BaCO_(3)`.
j. Expalin the decreasing order of solubility of sulphate of group `2` elements.
k. `'EA'` of `Cl` is the highest among the halogens, yet `F` is the strongest oxidising agent'. Why?