The correct order of density is
Be > Mg > Ca > Sr
Sr > Ca > Mg > Be
Sr > Be > Mg > Ca
Be > Sr > Mg > Ca
The Correct Option is C
Solution and Explanation
The question asks us to determine the correct order of density among the given alkaline earth metals: Beryllium (Be), Magnesium (Mg), Calcium (Ca), and Strontium (Sr). This requires an understanding of the periodic trends in the density of elements, particularly within the same group (group 2 of the periodic table).
Density is a measure of mass per unit volume and is influenced by both atomic mass and atomic volume. As we move down the group in the periodic table, the atomic mass of elements increases. Even though atomic size increases as well, the increase in mass tends to have a more significant impact on density compared to the increase in volume. Accordingly, heavier elements in a group often have higher densities.
Below is the order based on the general trend of density in group 2 (alkaline earth metals):
- Strontium (Sr): Out of the given elements, strontium is expected to have the highest density due to its larger atomic mass and relatively compact crystalline structure compared to lighter elements.
- Beryllium (Be): While beryllium is lighter, it has a very compact crystalline structure leading to relatively high density for its position in the periodic table.
- Magnesium (Mg): Typically follows beryllium in density, as it is directly below beryllium in the same group.
- Calcium (Ca): Even though it comes after magnesium and is heavier, calcium's crystal structure contributes to a slightly lower density than magnesium.
Therefore, the correct order of density is:
Sr > Be > Mg > Ca
This order is represented by the correct answer choice: Sr > Be > Mg > Ca.
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Concepts Used:
S-Block Elements
S-block elements, also known as alkali and alkaline earth metals, constitute the first two groups of the periodic table.
Group 1 elements, including hydrogen, lithium, sodium, potassium, rubidium, cesium, and francium, are alkali metals characterized by low density, high reactivity, and the ability to form strong bases when combined with water. They showcase a single valence electron in their outermost shell, making them eager to lose it in chemical reactions.
Group 2 elements, beryllium, magnesium, calcium, strontium, barium, and radium, make up the alkaline earth metals in Group 2. These metals share similar properties, such as higher densities and melting points compared to alkali metals. They also have a tendency to form ionic compounds with nonmetals.
S-block elements play vital roles in various industrial and biological processes. Alkali metals find applications in batteries, while alkaline earth metals are crucial for construction materials and are essential nutrients for living organisms. Despite their importance, the reactivity of alkali metals requires careful handling, often stored in oil to prevent reactions with moisture or oxygen. Overall, s-block elements contribute significantly to the diverse applications of chemistry in our daily lives.