Match List-I with List-II.
List-I
A. Be
B. Mg
C. Ca
D. Ra
List-II
1. Treatment of cancer
2. Extracti

Q: Why is Beryllium specifically used for X-ray windows and not other light metals like Lithium?

Beryllium is used because it has a very low atomic number (Z=4), meaning it absorbs very few X-rays. While Lithium (Z=3) is lighter, it is highly reactive and chemically unstable in air, making Beryllium the practical choice for durable X-ray tube windows.

Q: How does Calcium act as a reducing agent?

Calcium has a very strong affinity for oxygen and halogens. In metallurgical processes, it readily reacts with the oxides or halides of metals like Uranium or Zirconium, stripping away the oxygen/halogen and leaving the pure metal behind.

Q: Are incendiary bombs the only use for Magnesium?

Not at all! While its bright, hot flame makes it ideal for flares and incendiaries, Magnesium is also widely used in lightweight alloys for aircraft and car engines because of its low density and high strength.

Q: Is Radium still widely used for cancer treatment today?

Radium was historically significant in early radiotherapy. However, today it has largely been replaced by safer and more effective radioisotopes like Cobalt-60 and linear accelerators, which are easier to control and pose fewer long-term risks.

Q: What are the bearings for motor engines made of, if not these metals?

Bearings for motor engines are typically made of alloys like Babbitt metal (containing tin, copper, and antimony) or bronze. None of the Group 2 metals listed here are primarily used for engine bearings.

Question

Match List-I with List-II.
\begin{array}{|l|l|}
\hline
	ext{List-I} & 	ext{List-II} \
\hline
	ext{A. Be} & 	ext{1. Treatment of cancer} \
	ext{B. Mg} & 	ext{2. Extraction of metals} \
	ext{C. Ca} & 	ext{3. Incendiary bombs and signals} \
	ext{D. Ra} & 	ext{4. Windows of X-ray tubes} \
& 	ext{5. Bearings for motor engines.} \
\hline
\end{array}
Choose the most appropriate answer the option given below.

Options:

(A) 4, 3, 1, 2

(B) 4, 3, 2, 1

(C) 3, 4, 5, 2

(D) 3, 4, 2, 5

Sigma Percentile · Accepted Answer

### The Magic of Alkaline Earth Metals

Have you ever wondered what makes the windows of an X-ray tube transparent to radiation, or what gives a signal flare its blinding white light? The answers lie in Group 2 of the periodic table—the Alkaline Earth Metals. This problem is a beautiful journey through the practical applications of these elements, connecting their fundamental atomic properties to real-world uses.

### Beryllium: The Transparent Shield

Let's start with Beryllium ($Be$). Beryllium is the first element in Group 2, possessing a very low atomic number ($Z=4$). Because it has so few electrons, it interacts very weakly with high-energy electromagnetic radiation like X-rays.

Imagine trying to block a stream of water with a net that has massive holes; the water just passes right through. Similarly, X-rays pass right through Beryllium without being absorbed. This unique property makes it the perfect material for constructing the windows of X-ray tubes, allowing the rays to exit the machine and create the medical images we rely on.

### Magnesium: The Blinding Flare

Next up is Magnesium ($Mg$). If you've ever been in a chemistry lab, you might have witnessed the classic experiment of burning a magnesium ribbon. It ignites to produce a dazzling, intensely bright white flame.

This happens because Magnesium reacts vigorously with oxygen at high temperatures, releasing a tremendous amount of energy in the form of heat and light. Because of this brilliant and energetic combustion, Magnesium is widely used in military and emergency applications, specifically in **incendiary bombs** and **signal flares**.

### Calcium: The Oxygen Thief

Moving down the group, we encounter Calcium ($Ca$). Calcium is a highly reactive metal with a notorious appetite for oxygen and halogens. In the world of metallurgy, this makes Calcium an exceptional **reducing agent**.

When we need to extract certain heavy metals like Uranium, Zirconium, or Thorium from their naturally occurring oxide ores, we introduce Calcium. Calcium essentially "steals" the oxygen away from these heavy metals, leaving behind the pure metal we need. It's a chemical heist that is fundamental to modern nuclear and structural engineering!

### Radium: The Radioactive Healer

Finally, we reach Radium ($Ra$), the heaviest element in the group. Unlike the others, Radium is highly radioactive. Its unstable nucleus constantly decays, emitting high-energy radiation in the process.

Historically, this radiation was harnessed in the medical field for **radiotherapy**. By carefully directing the radiation emitted by Radium, doctors could target and destroy malignant cancer cells. While modern medicine has largely shifted to safer radioisotopes, Radium's legacy in the treatment of cancer remains a monumental milestone in science.

### Bringing It All Together

By understanding the unique "personality" of each element, the matching becomes intuitive:
- **Beryllium** ($Be$) $\rightarrow$ Windows of X-ray tubes
- **Magnesium** ($Mg$) $\rightarrow$ Incendiary bombs and signals
- **Calcium** ($Ca$) $\rightarrow$ Extraction of metals
- **Radium** ($Ra$) $\rightarrow$ Treatment of cancer

This perfectly aligns with our option, proving that chemistry isn't just about memorizing facts—it's about understanding how the universe works on an atomic level!

Select Answer:

Visualized Solution

$Alkaline Earth Metals$

$Beryllium (Be)$

$Magnesium (Mg)$

$Calcium (Ca)$

$Radium (Ra)$

$Final Match$

The Sigma Insight: Alkaline Metals

The Magic of Alkaline Earth Metals

Beryllium

Magnesium

Calcium

Radium

Bringing It All Together

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