The question asks for the increasing order of metallic character among the given elements — Beryllium (Be), Calcium (Ca), and Potassium (K). To solve this, we need to understand what determines metallic character and its trend in the periodic table.
Concept: Metallic character refers to how easily an element can lose electrons to form positive ions (cations). The key trends regarding metallic character in the periodic table are:
Metallic character increases down a group. This is because the atomic size increases, making it easier for the element to lose an external electron.
Metallic character decreases across a period from left to right. This is because the increased nuclear charge makes it more difficult to lose electrons.
Explanation: In the given options, we have three elements:
Potassium (K): Located in Group 1, Period 4.
Calcium (Ca): Located in Group 2, Period 4.
Beryllium (Be): Located in Group 2, Period 2.
According to the periodic trends:
Potassium (K) is more metallic than Calcium (Ca) because it is further left in the periodic table and belongs to the alkali metals which have a higher metallic character.
Calcium (Ca) is more metallic than Beryllium (Be) because it is positioned lower within the same group (alkaline earth metals) in the periodic table.
Therefore, the correct order from least metallic to most metallic among the elements is:
Beryllium (Be)
Calcium (Ca)
Potassium (K)
This order corresponds to the correct option:
K > Ca > Be
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