Question

Two elements x and y have atomic number 12 and 15 respectively write the electronic configuration of this elements what type of bond is formed if these two elements

Answer 1

The element x has atomic number 12. So the electronic configuration of x will be - 2.8.2

Again the element y has atomic number 15. So the electronic configuration of y will be- 2.8.5

The element x is Magnesium and the element y is Phosphorus.

Hope it helps...

Answer 2

Answer: a) $x=1s^22s^22p^63s^2$

b) $y=1s^22s^22p^63s^23p^3$

c) ionic bond

Explanation:

An ionic bond is formed when an element completely transfers its valence electron to another element. The element which donates the electron is known as electropositive element and forms a positively charged ion called as cation. The element which accepts the electrons is known as electronegative element and forms a negatively charged ion called as anion.

Electronic configuration for element x with atomic number 12 is magnesium

$Mg=1s^22s^22p^63s^2$

Electronic configuration of element y with atomic number 15 is phosphorous

$P=1s^22s^22p^63s^23p^3$

x atom will loose two electrons to gain noble gas configuration and form  cation with +2 charge.

$[Mg^{2+}]=1s^22s^22p^6$

y atom will gain three electrons to gain noble gas configuration and form  anion with -3 charge.

$[P^{3-}]=1s^22s^22p^63s^23p^6$

Thus $Mg^{2+}$ and $P^{3-}$ combine together and exchange their valencies to form neutral ionic compound $Mg_3P_2$