Chapter 11: Problem 64
\(\Lambda\) metal \(\mathrm{M}\) readily forms water soluble sulphate \(\mathrm{MSO}_{4}\), water insoluble hydroxide \(\mathrm{M}(\mathrm{OII})_{2}\) and oxide MO which becomes inert on heating. The hydroxide is soluble in NaOII. The \(\mathrm{M}\) is (1) Be (2) \(\mathrm{Mg}\) (3) \(\mathrm{Ca}\) (4) Sr
Short Answer
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Be
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
alkaline earth metals
Alkaline earth metals belong to Group 2 of the periodic table.
These elements include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra).
They are all shiny, silvery-white, somewhat reactive metals at standard temperature and pressure.
Unlike alkali metals (Group 1), alkaline earth metals have two electrons in their outer shell.
This gives them distinctive properties such as higher melting points and boiling points.
Alkaline earth metals generally form +2 oxidation state cations (e.g., Be²⁺, Mg²⁺).
They are usually found in their compounded form in nature (e.g., MgCO₃ for magnesium).
These elements are known for forming a variety of compounds, including oxides, hydroxides, sulfates, and carbonates.
These elements include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra).
They are all shiny, silvery-white, somewhat reactive metals at standard temperature and pressure.
Unlike alkali metals (Group 1), alkaline earth metals have two electrons in their outer shell.
This gives them distinctive properties such as higher melting points and boiling points.
Alkaline earth metals generally form +2 oxidation state cations (e.g., Be²⁺, Mg²⁺).
They are usually found in their compounded form in nature (e.g., MgCO₃ for magnesium).
These elements are known for forming a variety of compounds, including oxides, hydroxides, sulfates, and carbonates.
solubility of compounds
Solubility of compounds, especially those formed by alkaline earth metals, varies based on the element and the type of compound.
For example, the solubility of their sulfates decreases down the group (from BeSO₄ to BaSO₄).
Conversely, the solubility of their hydroxides increases from top to bottom within the group (from Be(OH)₂ to Ba(OH)₂).
Solubility is essential in determining how these compounds behave in water and other solvents.
It influences various applications, including industrial, environmental, and pharmacological contexts.
Notably, Beryllium hydroxide is soluble in NaOH, forming a soluble complex.
This property is crucial for identifying Beryllium among other Group 2 elements.
For example, the solubility of their sulfates decreases down the group (from BeSO₄ to BaSO₄).
Conversely, the solubility of their hydroxides increases from top to bottom within the group (from Be(OH)₂ to Ba(OH)₂).
Solubility is essential in determining how these compounds behave in water and other solvents.
It influences various applications, including industrial, environmental, and pharmacological contexts.
Notably, Beryllium hydroxide is soluble in NaOH, forming a soluble complex.
This property is crucial for identifying Beryllium among other Group 2 elements.
chemical properties of elements
The chemical properties of the elements determine how they interact with other substances.
Alkaline earth metals are known for their reactive nature, though less so than alkali metals.
These metals quickly oxidize in air, forming a thin oxide layer that can protect the underlying metal.
Their reactions with water vary in intensity, with increasing reactivity as you move down the group.
For instance, Magnesium reacts slowly with water, whereas Calcium reacts more vigorously.
The hydroxides and oxides formed by these reactions are crucial for understanding their chemical behavior.
Beryllium stands out due to its amphoteric oxide BeO, which makes it inert at high temperatures.
This property was used in the exercise to identify Beryllium accurately.
Alkaline earth metals are known for their reactive nature, though less so than alkali metals.
These metals quickly oxidize in air, forming a thin oxide layer that can protect the underlying metal.
Their reactions with water vary in intensity, with increasing reactivity as you move down the group.
For instance, Magnesium reacts slowly with water, whereas Calcium reacts more vigorously.
The hydroxides and oxides formed by these reactions are crucial for understanding their chemical behavior.
Beryllium stands out due to its amphoteric oxide BeO, which makes it inert at high temperatures.
This property was used in the exercise to identify Beryllium accurately.
Group 2 elements
Group 2 elements, also known as alkaline earth metals, play significant roles in various chemical reactions.
They are characterized by their ability to form stable compounds where the metal has a +2 charge.
Their atomic and ionic sizes increase from Beryllium to Radium, influencing their reactivity and bonding properties.
These metals form insoluble carbonates and hydroxides, except for Beryllium whose hydroxide displays solubility in NaOH.
Calcium compounds like CaCO₃ and CaSO₄ are ubiquitous and essential for environmental and biological processes.
Understanding these characteristics helps in predicting and explaining the behavior of these metals in different contexts.
The understanding of Group 2 elements helps to solve complex chemical identification problems like the exercise discussed.
They are characterized by their ability to form stable compounds where the metal has a +2 charge.
Their atomic and ionic sizes increase from Beryllium to Radium, influencing their reactivity and bonding properties.
These metals form insoluble carbonates and hydroxides, except for Beryllium whose hydroxide displays solubility in NaOH.
Calcium compounds like CaCO₃ and CaSO₄ are ubiquitous and essential for environmental and biological processes.
Understanding these characteristics helps in predicting and explaining the behavior of these metals in different contexts.
The understanding of Group 2 elements helps to solve complex chemical identification problems like the exercise discussed.
