MCQ Detailed View

Metals are chemical elements characterized by their ability to conduct heat and electricity, their malleability, ductility, and their shiny appearance. The most important chemical property of metals is that they are highly electropositive.

Electropositivity refers to the tendency of an atom to donate or lose electrons and form positively charged ions (cations). Metals have relatively low ionization energies, which means they can lose electrons from their outermost shell with ease. Once they lose electrons, they attain a stable electronic configuration, often resembling the nearest noble gas.

For example:

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  Sodium (Na) loses one electron to form Na⁺.

  
  


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  Calcium (Ca) loses two electrons to form Ca²⁺.

  
  


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  Aluminum (Al) loses three electrons to form Al³⁺.

  
  

This ability to lose electrons makes metals strongly electropositive. In contrast, nonmetals are generally electronegative, as they prefer to gain electrons.

Electropositivity increases down a group in the Periodic Table because atomic size increases, making it easier to lose electrons. On the other hand, electropositivity decreases across a period from left to right, because nuclear charge increases, holding electrons more tightly.

Key Points to Remember:

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  Metals → Electropositive (lose electrons easily).

  
  


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  Nonmetals → Electronegative (gain electrons easily).

  
  


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  Alkali metals (like Na, K, Rb, Cs) are the most electropositive elements.

  
  


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  Electropositivity trend → increases down a group, decreases across a period.

  
  

Therefore, the correct answer is Electropositive because metals characteristically form positive ions due to their strong tendency to lose electrons.