What element has the following electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6
1 answer:
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Complete Question
The complete question is shown on the first uploaded image
Answer:
X is Be
Y is B
Z is O
Explanation:
In order to understand the solution, we need to that the an element form a bond based on
1 The number of valence electron available in its atom
2 The number of electron it require to attains its stable state i.e its Octet state
The number of valence electron for each of the option are
F = 7, N = 5 , O = 6 , C = 4 , B = 3 , Be = 2
Considering the first element
We see that X is donating two valence electron in its atom and it is donating it to 2 Cl as Cl only requires a single electron to achieve its stable state
Now looking option we can see that Be has two valence electron in it atom and in order for it to attain its stable state it needs to release the electron so the correct option for this question is Be
Considering the second element
We see that Y is donating three valence electron in its atom and it is donating it to 3 Cl as Cl only requires a single electron to achieve its stable state
Now looking option we can see that B has three valence electron in it atom and in order for it to attain its stable state it needs to release the valence electron so the correct option for this question is B
Considering the second element
We see that Z is donating two valence electron in its atom and it is donating it to 2 Cl as Cl only requires a single electron to achieve its stable state, also Z has 2 lone-pair valence electron
Now looking at the option we can see that O has 6 valence electron so if it donates 2 valence electron it will still be left with 4 - pair of electron
Therefore the correct option to this question is O
