The S-block Elements
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4 months agoContributor-Level 10
Li+ has maximum degree of hydration due to its small size and for this reason lithium salts are mostly hydrated.
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4 months agoContributor-Level 10
Hydration energy decreases down the group from Be to Ba and lattice energy remains almost constant.
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4 months agoContributor-Level 10
Lithium, sodium, potassium, rubidium, caesium and Francium are group I elements and collectively known as the alkali metals.
They are called as the alkali metals because they form hydroxides on reaction with water which are strongly alkaline in nature.
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4 months agoContributor-Level 10
The ionic radius of Be2+ is estimated to be 31 pm; the charge/radius ratio is nearly the same as that of the Al3+ ion. Hence beryllium resembles aluminium in some ways. Some ofthe similarities are:
(i) Like aluminium, beryllium is not readily attacked by acids because of the presence of an oxide film on the surface of the metal.
(ii) Beryllium hydroxide dissolves in excess of alkali to give a beryllate ion, [Be (OH)4]2– just as aluminium hydroxide gives aluminate ion, [Al (OH)4]–.
(iii) The chlorides of both beryllium and aluminium have Cl– bridged chloride structure in vapour phase. Both the chlorides are solubl
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4 months agoNew answer posted
4 months agoContributor-Level 10
(c) Reason is wrong a statement. More negative is the electrode potential, higher is the tendency of the element to lose electrons and hence, stronger is the reducing agent.
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4 months agoContributor-Level 10
(b) Both the statements are correct but not the reason for the assertion.
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4 months agoNew answer posted
4 months agoContributor-Level 10
(d) The ionization enthalpies of the alkali metals are considerably low and decrease down the group from Li to Cs. This is because the effect of increasing size outweighs the increasing nuclear charge, and the outermost electron is very well screened from the nuclear charge.
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