Electronic configuration of four elements A, B, C, and D are given below
A. $1 s^{2} 2 s^{2} 2 p^{6}$ B. $1 s^{2} 2 s^{2} 2 p^{4}$ C. $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$
D. $1 s^{2} 2 s^{2} 2 p^{5}$
Whilch of the following is the correct order of increasing tendency to gain electron?
(a) A < C <B <D (b) A < B < C < D (c) D <B < C < A (d) D < A < B <C

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Solution

Electronic configuration of elements indicate that A is a noble gas (i.e. ne)I B is oxygen (group 16) , C is sodium metal (group 1 ) and D is fluorine (group 17).
(i) Noble gases have no tendency to gain electrons since all their orbitals are completely filled. Thus element a has the least electron gain enthalpy
(ii) Since element D ahs one electron less and element B has Two electrons less than the corresponding noble gas configuration, hence element D has the highest electron gain enthalpy followed by element B
(iii) Since, element C has one electron in the s- orbital and hence needs one more electron to complete it, therefore, electron gain enthalpy of C is less than that of element B. Combining all the facts given above the electron gain enthalples of the four elements increase in the order A < C< B< D.

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Similar questions

A, B, C

D

1 s^{2} 2 s^{2} 2 p^{6}

1 s^{2} 2 s^{2} 2 p^{4}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}

1 s^{2} 2 s^{2} 2 p^{5}

1 s^{2}

1 s^{2} 2 s^{2} 2 p^{2}

1 s^{2} 2 s^{2} 2 p^{5}

1 s^{2} 2 s^{2} 2 p^{4}

Question 17

The electronic configurations of the elements A, B and C are given below. Answer the question on the basis of these configurations.

A $1 s^{2}$ $2 s^{2}$ $2 p^{6}$

B $1 s^{2}$ $2 s^{2}$ $2 p^{6}$ $3 s^{2}$ $3 p^{3}$

C $1 s^{2}$ $2 p^{6}$ $2 p^{6}$ $3 s^{2}$ $3 p^{5}$

The bond between B and C will be

(a) ionic

(b) covalent

(d) coordinate

[H e] 2 s^{1}, [N e] 3 s^{1}

[A r] 4 s^{1}

(i n K J m o l^{1})

Which of the following represent the correct electronic configuration of $O_{2}$ ?

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