Match List I with List II.
List-I (Elements) | List-II (Properties)
A. Ba | (i) Organic solvent solu

Q: Why are Lithium compounds covalent while other alkali metals form ionic compounds?

Due to its exceptionally small size, the $Li^+$ ion has a very high charge density and polarizing power. According to Fajan's rules, it distorts the electron cloud of the anion significantly, introducing covalent character.

Q: What does 'monoacidic base' mean?

A monoacidic base is a base that yields only one hydroxide ion ($OH^-$) per molecule in aqueous solution, such as $NaOH$ or $KOH$. It can neutralize one proton ($H^+$) from an acid.

Q: Why is Calcium oxalate insoluble in water?

The lattice energy of calcium oxalate is significantly higher than its hydration energy. The strong electrostatic attraction between the $Ca^{2+}$ ions and the oxalate ($C_2O_4^{2-}$) ions makes it difficult for water molecules to pull them apart.

Q: How do I quickly find the outer electronic configuration of an s-block element?

The group number tells you the number of valence electrons (Group 1 = $ns^1$, Group 2 = $ns^2$), and the period number gives you the principal quantum number ($n$). For example, Barium is in Group 2, Period 6, so it's $6s^2$.

Q: Are all s-block oxalates insoluble?

No, the solubility of alkaline earth metal oxalates generally decreases down the group. Beryllium oxalate is soluble, while calcium, strontium, and barium oxalates are insoluble in water.

Question

Match List I with List II. \begin{array}{ll} 	ext{List-I (Elements)} & 	ext{List-II (Properties)} \ 	ext{A. Ba} & 	ext{(i) Organic solvent soluble compounds} \ 	ext{B. Ca} & 	ext{(ii) Outer electronic configuration } 6s^2 \ 	ext{C. Li} & 	ext{(iii) Oxalate insoluble in water} \ 	ext{D. Na} & 	ext{(iv) Formation of very strong monoacidic base} \end{array} Choose the correct answer from the options given below

Options:

(A) A-(ii), B-(iii), C-(i), D-(iv)

(B) A-(iv), B-(i), C-(ii), D-(iii)

(C) A-(iii), B-(ii), C-(iv), D-(i)

(D) A-(i), B-(iv), C-(ii), D-(iii)

Sigma Percentile · Accepted Answer

### Analyzing the Setup
When we look at the s-block elements, we see a fascinating array of properties that vary systematically down the groups and across the periods. In this problem, we are tasked with matching four distinct s-block elements—Barium, Calcium, Lithium, and Sodium—with their most defining chemical or physical characteristics. Let's break them down one by one.

### Barium: The Heavy Alkaline Earth Metal
Let's start with Barium ($Ba$). Barium is a heavy alkaline earth metal located in Group 2 and Period 6 of the periodic table.

Because it resides in Group 2, it has two valence electrons. And since it is in the sixth period, its outermost electrons are in the 6s subshell. Therefore, its outer electronic configuration is exactly $6s^2$. This makes matching Barium straightforward: **A matches with (ii)**.

### Calcium: The Insoluble Oxalate
Next up is Calcium ($Ca$). A classic fact about calcium chemistry—often related to biology and medicine, particularly in the formation of kidney stones—is its reaction with oxalate ions.

Calcium forms calcium oxalate ($CaC_2O_4$), a compound that is notoriously insoluble in water. The strong electrostatic attraction between the $Ca^{2+}$ ions and the $C_2O_4^{2-}$ ions creates a lattice energy that far exceeds its hydration energy. Thus, **B matches perfectly with (iii)**.

### Lithium: The Anomalous Alkali Metal
Moving on to Lithium ($Li$), we encounter the first element of the alkali metals. Lithium is unique because of its exceptionally small atomic and ionic size.

According to **Fajan's rules**, a smaller cation has a higher polarizing power. Lithium's high polarizing power allows it to distort the electron cloud of anions significantly, introducing a strong covalent character into its compounds. Because "like dissolves like," these covalent lithium compounds are highly soluble in organic (non-polar or weakly polar) solvents, unlike the typical ionic compounds of other alkali metals. Therefore, **C matches with (i)**.

### Sodium: The Strong Base Former
Finally, we have Sodium ($Na$). Sodium is a highly reactive alkali metal that reacts vigorously with water to form sodium hydroxide ($NaOH$).

Sodium hydroxide is a classic example of a very strong monoacidic base. It completely dissociates in water to yield one hydroxide ion ($OH^-$) per molecule, ready to neutralize a single proton from an acid. This leads us to our final connection: **D matches with (iv)**.

### Final Calculation
Putting all our logical deductions together, we arrive at the final sequence:
- **A** $\rightarrow$ **(ii)**
- **B** $\rightarrow$ **(iii)**
- **C** $\rightarrow$ **(i)**
- **D** $\rightarrow$ **(iv)**

This sequence corresponds exactly to the first option provided in the question. By understanding the periodic trends and anomalous behaviors of s-block elements, we can confidently solve such matrix match problems!

Select Answer:

Visualized Solution

$Problem Setup$

$Barium (Ba)$

$Calcium (Ca)$

$Lithium (Li)$

$Sodium (Na)$

$Final Answer$

The Sigma Insight: Alkali Metals

Analyzing the Setup When we look at the s-block elements, we see a fascinating array of properties that vary systematically down the groups and across the periods

Barium

Calcium

Lithium

Sodium

Final Calculation

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