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The choices that should have accompanied this question were:
A. 1 
B. 2 
C. 3 
D. 4 

My answer is B. 2.
Below is an explanation, I found while doing the research.

Phosphate needs 3 electrons each totaling 6 electrons so each zinc will need to give up 2 electrons.

Phosphate wants to imitate the electron configuration of Argon because noble configurations are the most stable. With P getting the extra electrons the valence shell will be 3s2 3p6, which is the same as Argon. Without the extra electrons, the P valence shell looks like this 3s2 3p3, now you can see why each phosphorus wants 3 more electrons, that will make it 3s2 3p6, just like Argon.
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Valence electron refers to the number of electrons in the outermost shell of an atom. Since the valence shell of phosphorus is the M shell, then it need 8 electrons to achieve a stable state, Hence, each Zinc atom will lose 2 electrons.

  • Number of atoms required by each phosphorus atom = (8 - 5) = 3

  • Number of phosphorus atoms = 2

  • Total number of atoms required = (2 × 3) = 6 atoms

  • Number of Zinc atoms = 3

Each zinc atom will lose the same number of electrons ;

  • Number of electron lost by each = 6/3 = 2 atoms

Therefore, each Zinc atom will lose 2 electrons.

Learn more :https://brainly.com/question/8526630

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