Question

IIalides of alkaline carth metals form hydrates such as \(\mathrm{MgCl}_{2} \cdot 6 \mathrm{II}_{2} \mathrm{O}, \mathrm{CaCl}_{2} \cdot 6 \mathrm{II}_{2} \mathrm{O}, \mathrm{BaCl}_{2} \cdot 2 \mathrm{II}_{2} \mathrm{O}\). This shows that halides of group 2 clements (1) are hygroscopic in nature (2) acts as dehydrating agents (3) can absorb moisturc from air (4) all of theso

Short answer

All of the statements are correct (4).

Step-by-step solution

- Identify Information

Recognize that IIalides of group 2 elements form hydrates. Examples include \( \mathrm{MgCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \), \( \mathrm{CaCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \) and \( \mathrm{BaCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O} \).

- Recognize Hygroscopic Nature

Hydrates are compounds that include water molecules within their structure. This indicates that the halides absorb water to form hydrates, showing hygroscopic nature.

- Assess as Dehydrating Agents

Because these group 2 element halides can collect water and create hydrates, they are also able to act as dehydrating agents.

- Confirm Moisture Absorption

Since these compounds absorb water to form hydrates, they absorb moisture from the air.

- Combine Observations

Based on the observations of their properties: absorbing moisture, forming hydrates, and acting as dehydrating agents, conclude that all of the given properties are true.

Key concepts

hygroscopic nature

Hydrates of Group 2 elements, such as \(\mathrm{MgCl}_{2}\cdot 6 \mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CaCl}_{2}\cdot 6 \mathrm{H}_{2} \mathrm{O}\), showcase a fascinating property known as hygroscopic nature. This means that these compounds have the ability to attract and hold water molecules from the surrounding environment. This is key for their formation as hydrates.
Hygroscopic substances are incredibly useful in various applications:

• Preserving moisture-sensitive products
• Maintaining humidity levels in certain environments
• Serving as indicators of moisture (since they change appearance or properties upon absorbing water)

Understanding this property helps explain why certain materials tend to 'pull' moisture from the air to form more stable compounds.

dehydrating agents

Because Group 2 element hydrates absorb moisture, they can also act as dehydrating agents. A dehydrating agent is a substance that removes water from another material, either by chemical or physical means.
Alkaline earth metal halides such as \(\mathrm{CaCl}_{2}\cdot 6 \mathrm{H}_{2} \mathrm{O}\) are particularly effective. They can attract water molecules and bind them within their structural lattice, forming a stable hydrate complex.
This property makes these compounds useful in a variety of industrial and laboratory settings:

• Drying gases
• Removing moisture from chemical reactions
• Maintaining dry conditions in packaging

By understanding the role of these agents, we appreciate how they support processes that require moisture control.

moisture absorption

Group 2 element halides absorb moisture to form hydrates. This ability is documented in compounds like \(\mathrm{BaCl}_{2}\cdot 2 \mathrm{H}_{2} \mathrm{O}\). These compounds, when exposed to air, readily uptake water molecules from their surroundings.
Moisture absorption is crucial for applications that exploit this property:

• Humidity regulation in environments
• Storing and preserving hygroscopic substances
• Creating desiccants for various applications

The chemical structure of these hydrates enables them to form stable complexes by integrating water molecules, which is essential for their various practical uses. This mechanism helps in controlling the humidity and ensuring the preservation of substances sensitive to moisture.

alkaline earth metals

Alkaline earth metals, found in Group 2 of the periodic table, include elements like Magnesium (Mg), Calcium (Ca), and Barium (Ba). These metals are characterized by their reactivity with water and formation of various compounds, including hydrates.
The formation of hydrates is typical because:

• They have two valence electrons, making them highly reactive
• They readily lose electrons to form cations (e.g., \(\mathrm{Ca}^{2+}\))
• Their compounds readily absorb moisture due to their ionic nature

Studying the properties of these metals helps us understand their widespread applications in industries, from construction materials to chemical manufacturing. Their hydrates are evident in solutions and compounds we frequently encounter, reflecting their significant role in chemical processes.