Q.1. Explain why sodium is less reactive than potassium.
Q.2. What is the oxidation state of
(i) lithium in Li2O
(ii) sodium in Na2O2
(iii) potassium in KO2
Q.3. Why are potassium and cesium, rather than lithium can be used in photoelectric cells ?
Q.4. When a cation is highly polarising ? Which alkali metal ion has the highest polarising power ?
Q.5. Lithium is the only alkali metal to form nitride directly. Explain.
Q.6. What makes lithium to show properties uncommon to rest of the alkali metals ?
Q.7. Why are lithium salts commonly hydrated and those of other alkali ions usually anhydrous ?
Q.8. Arrange the following alkali metal ions in decreasing order of their mobility:
Li+, Na+, K+, Rb+, Cs+.
Q.9. Arrange the following in order of increasing covalent character:
MCl, MBr, MF and MI (where M= alkali metal)
Q.10. The Eo values are:
Cl–/Cl2 = +1.36V, I–/I2 = +0.53V, Ag+/Ag = +0.79V, Na+/Na = –2.71V, Li+/Li = –3.04V
Arrange the following ionic species in decreasing order of reducing strength:
I–, Ag+, Cl–, Li+, Na+
Q.11. Why is KO2 paramagnetic?
Q.12. Why is that on being heated in excess supply of air, K, Rb, and Cs form superoxides in preference to oxides and peroxides ?
Q.13. What happens when KO2 reacts with water? Write the balanced chemical equation for the reaction.
Q.14. Write balanced equations for reactions between:
(i) Na2O2 and water
(ii) KO2 and water
(iii) Na2O and CO2
Q.15. Sodium metal is kept under kerosene. Explain why.
Q.16. LiCl is soluble in organic solvents. Explain.
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