Table of Contents
Anomalous behaviour of Lithium is due to 2) higher polarising power of Li+ resulting in increased covalent character of its compounds which is responsible for their solubility in organic solvents. 3) comparatively high ionization enthalpy and low electropositive character of lithium as compared to other alkali metals.
What is anomalous behavior of lithium?
The anomalous behaviour of lithium is as follows: Lithium is harder than other metals of the respective group. It has higher Melting and boiling point than other metals. It is least reactive. Unlike other metals LiCl is deliquescent and exist as LiCl.
Why does Li show anomalous Behaviour than rest of the elements of group1?
Lithium differs in many respects from the remaining characteristic properties of the metals of Group 1, due to the following reasons: a) The size of lithium atom and ion is very small.
What is the reason for anomalous Behaviour?
Carbon shows anomalous behavior due to various properties as exceptional size, high electrification, high ionization energy, and absence of d-orbitals. Carbon has high melting and boiling point compared to the other elements of the same group.
Why is lithium in the S block?
Lithium and Beryllium, the first members of the s-block family differ much from the rest of their members. The anomaly of these elements is due to their, Low atomic and ionic size. Greater charge density (charge/volume of the atom).
Why lithium is different from rest of its family members?
➡️ Actually , Among the alkali metals, Llithium has the smallest atomic and ionic size and has the highest polarising power. Due to this, lithium compounds are covalent. Therefore, lithium shows anomalous behaviour as compared to with other alkali metals.
Does lithium has high Polarising power?
Therefore, lithium ion (Li+) has the highest polarizing power. This polarizing power of the lithium is explained by the size and charge of the ion, as we know that the size of the lithium in the alkali metal ions is the smallest, due to which the ratio of charge and size is very high.
Which of the following is incorrect reasons for anomalous Behaviour of lithium?
1) Lithium is harder while all other alkali metals are soft. 2)The melting and boiling point of lithium are comparatively high. 3) Lithium forms monoxides with oxygen while other alkali metals from peroxides as well as superoxide.
What are the similarities between Li and Mg?
Both are quite hard. The hydroxides of both the elements are weak bases and decompose on heating. Both of these elements have covalent characters.
Why lithium is most powerful reducing agent?
Lithium ion is small in size and has high ionization enthalpy. Thus, Li has a greater tendency to lose electrons in solution than other alkali metals. The Large amount of hydration energy makes it the strongest reducing agent in spite of its highest ionisation enthalpy.
What is the anomalous Behaviour of water?
The anomalous expansion of water is an abnormal property of water whereby it expands instead of contracting when the temperature goes from 4°C to 0°C, and it becomes less dense. The density becomes less and less as it freezes because molecules of water normally form open crystal structures when in solid form.
Which metal show anomalous Behaviour as water does?
Antimony shows anomalous behavior. It too is less dense than the liquid at the freezing point.
Why do elements of second period show and anomalous Behaviour?
The anomalous properties of the second period because of the absence of d-orbital. Thus they require higher energy to form bonds. Thus anomalous behavior of any group second period element is due to small size, large charge/radius ratio, and high electronegativity of the elements, and covalence cannot exceed four.
Does beryllium have similar properties to lithium?
Lithium and beryllium are the first elements of Group 1 and 2 respectively exhibit some properties which are different from those of the other members of the respective group. They both show similarity in properties of the second element of the following group.
Why are lithium salts commonly hydrated?
Lithium is the smallest in size among the alkali metals. Hence, Li+ ion can polarise water molecules more easily than other alkali metals. As a result, water molecules get attached to lithium salts as water of crystallization. Hence, lithium salts such as trihydrated lithium chloride are commonly hydrated.
What are P block elements called?
The p-block elements are found on the right side of the periodic table. They include the boron, carbon, nitrogen, oxygen and flourine families in addition to the noble gases.
Why does lithium not form an Alkalide?
Reactivity. Lithium is part of the Group 1 Alkali Metals, which are highly reactive and are never found in their pure form in nature. This is due to their electron configuration, in that they have a single valence electron (Figure 1) which is very easily given up in order to create bonds and form compounds.
Why does lithium behave more like magnesium than sodium?
Chemical reactivity Both lithium and magnesium reacts with carbon or nitrogen to form the corresponding carbide and nitride. Whereas sodium and the other Group 1 metals show no reaction under ambient conditions. Many of the compounds of lithium have a similar reactivity to those of magnesium rather than sodium.
Can lithium form Ethynide?
Lithium has very small size and high polarising power and hence high ionization energy due to which it is difficult to remove the outermost electron. So, lithium is the only alkali metal which does not react with ethyne to give ethynide.
What is the correct order of Polarising power?
D. K+ < Cs+ < Mg2+ < Al3+ Hint: We should know that the polarizing power of a cation is the ability to distort an anion. Polarising power is dependent on the charge of cation and the radius of the cation.
Does Li and Mg have same Polarising power?
In option (C), the pair of cations given consists of Li+ and Mg2+ ions. Though lithium is categorised as the alkali metals in the periodic table, it shows many similarities with the alkaline earth metal, magnesium. Therefore, the value of polarising power of Li+ and Mg2+ ions will be almost the same.
Which ion has a higher polarizing power?
Al+3, thus has the highest polarising power.
