Question

Direction (Q. no. 14-17) The electronic configurations of the
elements A, B and C are given below. Answer the questions from
14 to 17 on the basis of these configurations.
A 1s² 2s² 2p⁶
B 1s² 2s² 2p⁶ 3s² 3p³
C 1s² 2s² 2p⁶ 3s² 3p⁵

Answer 1

Stable form of A will be A.

Compound between B and C will be BC3.

Nature of bond between B and C will be ionic bond.

Stable form of C will be C2.

Explanation:

• A is the element with electronic configuration 1s² 2s² 2p⁶.

• So atomic number of A will be $2+2+6$ =10.

• So,A is an inert gas with fulfilled K amd L shell.

• So A will exist as A only.

• In B the atomic number is $2+2+6+2+3$ = 15.

• In C, the atomic number is $2+2+6+2+5$= 17.

• So,B will get rid of 3 electrons while C will accept 1 electron.

• So the compound formed will be BC3.

• In the bond there's direct transfer of charges.

• So the bond will be ionic bond.

• C has electronic configuration of chlorine and chlorine exist as Cl2.

• So C will exist as C2.

For more information about electronic configuration,

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Which of the following electronic configurations is the general electronic configuration of elements of group 16?Select the proper choice from the given multiple choices.

(A) ns²np³

(B) ns²np⁴

(C) ns²np⁶

(D) ns²np⁵

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a) Give the electronic configurations of sodium and chlorine.

(b) Write the electron-dot structures for sodium and chlorine atoms.

(c) Describe the formation of sodium chloride from sodium and chlorine by the transfer of electrons. What changes take place in the electronic configurations of sodium and chlorine during the formation of sodium chloride?

​(d) Write any two properties of ionic compounds.