Short Answer TypeArrange the following in the decreasing order of their basic strength in aqueous solutions:
CH3NH2, (CH3)2NH, (CH3)3 N and NH3
(a) Complete the following chemical reactions equations:
(i) P4+SO2Cl2 -->
(ii) XeF6+H2O -->
(b) Predict the shape and the asked angle (90° or more or less) in each of the following cases:
(i) and the angle O - S - O
(ii) ClF3 and the angle F - Cl - F
(iii) XeF2 and the angle F - Xe - F
Complete the following chemical equations:
(i) NaOH+Cl2 -->
(ii) XeF4+O2F2--->
(b) Draw the structures of the following molecules:
(i) H3PO2
(ii) H2S2O7
(iii) XeOF4
State reasons for each of the following:
The N-O bond in is shorter than the N-O bond in
State reasons for each of the following:
(i) All the P-Cl bonds in PCl5 molecule are not equivalent.
(ii) Sulphur has a greater tendency for catenation than oxygen.
Long Answer Type(i) NF3 is an exothermic compound whereas NCl3 is not.
(ii) F2 is most reactive of all the four common halogens.
(b) Complete the following chemical equations:
(i) C + H2SO4 (conc.)-->
(ii) P4 + NaOH + H2O-->
(iii) Cl2+F2 ------>
(excess)
(a) Account for the following:
(i) The acidic strength decreases in the order HCl > H2S > PH3
(ii) Tendency to form pentahalides decreases down the group in group 15 of the periodic table.
(b) Complete the following chemical equations:
(i) P4 + SO2Cl2-->
(ii) XeF2 + H2O--->
(iii) I2+HNO3(conc.)--->
(i) The acidity of a molecule depends on the polarity of the bond between central atom and the hydrogen atom. Greater the polarity higher will be the acidity.
And the polarity of the bond depends on the electronegativity of the central atom. In a period, the electronegativity decreases in the order Cl > S > P. As a result, the loss of H+ ions decreases.
Thus, the acidic strength of the hydrides decreases in the
Following order:
HCl > H2S > PH3
(ii) Nitrogen does not form pentahalide because it does not have d-orbital. P, As, Sb form pentahalide. Bi does not form pentahalide. The tendency to form pentahalide decrease down the group. This because of inert pair effect.
Due to the inert pair effect, ns2 electron remains inert in a chemical reaction and element shows -2 oxidation state. Inert pair effect increases down the group. Thus the tendency to form pentahalides decrease down the group 15.
(b)
(i) P4 + 10SO2Cl2---> 4PCl5 + 10SO2
(ii) 2XeF2 + 2H2O----> 2Xe + 4HF + O2
(iii) I2 + 10HNO3--> 2HIO3+10NO2+4H2O
is not likely to exist and why?
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