Question

Explain diagonal relationship between Li and Mg? Why noble gases have exceptionally high ionisation rnthalpyi​

Answer 1

$\huge{\boxed{Answer:-}}$

$\mathfrak{\huge{Digonal Relationship:-}}$

✳First part

Li & Mg :-

• Have similar electonegatives.
• Li & mg are quite hard.
• LiOH & Mg(OH)2 are weak base.
• Both form ionic nitride while heating in air.
• Both decompose on heating and form super oxide & peroxide .
• Both are soluble in ethanol
• Cannot able to form sodium bicarbonate.
• Both have high Polarizing power.

LI. & Mg.

Elecronegaitivity | 1.0. | 1.2.

Atomic Radii. | 1.23 | 1.36

Ionic Radii. | 0.60 | 0.65 ___

Atomic Volume. |__12.97__|____13.97____

✳ Second part

✳Inert gases are in their most stable form.

✳It is more unfavorable to remove their valence electrons than those of any other atom in the same period.

✳ More energy is required to "pull" a valence electron away from inert gases.

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Answer 2

1)Question :-

Explain diagonal relationship between Li and Mg?

SOLUTION:-

The, lithium shows similarities to magnesium and beryllium to aluminium in many of their properties. This type of diagonal similarity is commonly referred to as diagonal relationship in the periodic table. The diagonal relationship is due to the similarity in ionic sizes and /or charge /radius ratio of the elements.

2)Question :-

Why noble gases have exceptionally high ionisation enthalpy?

SOLUTION:-

Because they have stable , filled shell configurations, it is difficult to remove an electron from any of the noble gases. ... Each peak is one of the noble gases. Note that ionization energy decreases from top to bottom of each column because the outer shell electrons become farther removed from the nucleus.