Question

Show formation of sodium oxide by transfer of electrons ? Why compound formed conducts electricity in molten state

Answer 1

$\huge {ANSWER}$

▶Sodium is a metal which lies in group one peroid 3 of the periodic table.

According to which its,

◼ELECTRONIC CONFIGURATION =2,8,1

◼VALENCE ELECTRON = +1.

So, to be stable like nearest noble gas neon it need to lose one electron.

▶Oxygen is a non metal which lies in group 16 and period 2.

According to which,

◼ELECTRONIC CONFIGURATION =2,6.

◼VALENCE ELECTRONS =-2.

So, to be stable like nearest noble gas neon it is need gains two two electrons.

⚫In the formation of sodium oxide,

Sodium (Na) loses its one electron to be stable and oxygen(O) needs two electrons, since sodium has only one valence electrons so two atoms of sodium reacts in this.

▶Before losing electrons,

${Na}^{+1} \longrightarrow {O}^{-2} \longleftarrow {Na}^{+1}$

(2,8,1).......(2,6).........(2,8,1)

▶After losing electrons,

$[{Na}^{+1}] [{O}^{-2}][{Na}^{+1}]$

(2,8)....(2,8)....(2,8)

▶FORMULA = $Na_2O$

$\bold {REASON}$

◼The compound formed conducts electricity because its a ionic compound which when dissolved in water dissociate to form ions while when its in it solid state its held by strong electrostatic force which needs a really high amount of kinetic energy to dissociate and form ions.