Tag: anomalous properties of lithium

Questions Related to anomalous properties of lithium

Which of the following carbonate is not stable to heat.

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. $Li _2CO _3$

  2. $Na _2CO _3$

  3. $K _2CO _3$

  4. $Rb _2CO _3$

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Correct Option: A

Which one of the alkali metals,forms only,the normal oxide $M _2O$ on heating in air?

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. $Li$

  2. $Na$

  3. $Rb$

  4. $K$

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Correct Option: A

Li has chemical properties most similar to :

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. Al

  2. Ca

  3. Mg

  4. Ti

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Correct Option: C
Explanation:

Li has chemical properties most similar to Mg due to diagonal relationship.
Both exhibits same properties like
(i).

$MgCO _3\, \overset{\Delta}{\rightarrow}\, MgO\, +\, CO _2$
$Li _2CO _3\, \overset{\Delta}{\rightarrow}\, Li _2O\, +\, CO _2$

(ii).
$3Mg\, +\, N _2\, \rightarrow Mg _3N _2$ 
$6Li+ N _2 \rightarrow 2Li _3N$

Hence option C is correct answer.

Li resembles to element X which is not the member of alkali metals. The group of X is?

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. II

  2. III

  3. IV

  4. I

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Correct Option: A
Explanation:

Li resembles to element X which is not a member of alkali metals. The group of X must be II group, because certain elements of 2nd period show similarity with their diagonal elements in the 3rd period as shown below : Thus, Li resembles Mg, Be resembles Al and B resembles Si. This is called diagonal relationship and is due to the reason that these pairs of element have almost identical ionic radii and polarizing power (i.e. charge/size ratio). Element of second period are known as bridge elements.

So Li is I st group element and the diagonal element Mg is II nd group element.
Hence option A is correct.

$Mg$ and $Li$ and similar in their properties due to:

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. same $\dfrac {e}{m}$ ratio

  2. same electron affinity

  3. same group

  4. same radius

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Correct Option: D
Explanation:

$Li$ and $Mg$ show diagonal relationship due to the similarity in size (radius), electronegativity, ionisation enthalpy and charge/radius ratio.

Li resembles to element X which is not the member of alkali metals.
The element X is :

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. Mg

  2. Be

  3. Ca

  4. B

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Correct Option: A
Explanation:

Li resembles to element X which is not the member of alkali metals. The element X is Mg. This is due to diagonal relationship. Certain elements of 2nd period show similarity with their diagonal elements in the 3rd period as shown below : Thus, Li resembles Mg, Be resembles Al and B resembles Si. 


This is called diagonal relationship and is due to the reason that these pairs of element have almost identical ionic radii and polarizing power (i.e. charge/size ratio). Element of second period are known as bridge elements.   
Hence option A is correct.

Lithium borohydride, $LiB{H} _{4}$, crystallizes in an orthorhombic system with four molecules per unit cell. The unit cell dimensions are $a=6.0\mathring { A } ,b=4.4\mathring { A } ,c=7.5\mathring { A } $. The density of crystals is
$\left( Li=7,B=11,{ N } _{ A }=6\times { 10 }^{ 23 } \right) $

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. $0.74g/{cm}^{3}$

  2. $1.48g/{cm}^{3}$

  3. $0.37g/{cm}^{3}$

  4. $0.90g/{cm}^{3}$

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Correct Option: A

Lithium shows similarities with magnesium in its chemical behaviour because :

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. similar size, greater electronegativity and lower polarising power

  2. similar size, same electronegativity, and lower polarising power

  3. similar size, same electronegativity and similar high polarising power

  4. none of the above

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Correct Option: C
Explanation:

Lithium shows similarities with magnesium in its chemical behaviour because they have similar size and charge/size ratio. They have similar electronegativity.


This type of diagonal similarity is commonly referred to as diagonal relationship in the periodic table.

In certain matters, lithium differs from other alkali metals; the main reason for this is :  

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. small size of lithium atom and $Li^+$.

  2. extremely high electropositivity of $Li$.

  3. greater hardness of $Li$.

  4. hydration of $Li^+$ ion.

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Correct Option: A
Explanation:

In certain matters, lithium differs from other alkali metals(anamalous property); the main reason for this is small size of lithium atom and $Li^+$ and high polarizing power.

Hence option A is correct.

In certain matters, lithium differs from other alkali metals, the main reason for this is:

chemistry the s-block elements (alkali and alkaline earth metals) anomalous properties of lithium group 1 elements: alkali metals properties of s block elements

  1. Small size of lithium atom and $Li^+$ ion

  2. Extremely high electro positivity of $Li$

  3. Greater hardness of $Li$

  4. Hydration of $Li^+$ ion

Show answer
Correct Option: A
Explanation:

The chemistry of lithium shows several differences from that of the rest of the group as the small lithium cation polarises anions and gives its compounds as the more covalent character.