Question

explain the type of bond formation between mgcl2 with the help of dot structure​

Answer 1

Answer:

The atomic number of magnesium is 12

Electronic configuration of magnesium: 2, 8, 2

Number of electrons in outermost orbit = 2

Valence electron = 2

Atomic number of chlorine = 17

Electronic configuration of chlorine: 2, 8, 7

Electrons in outermost orbit = 7

Therefore, valence electrons = 7

lewis dot structure magnesium chloride

Magnesium loses two electrons in order to obtain stable electronic configuration. Each of the two chlorine atoms gains one electron lost by magnesium to obtain stable electronic configuration. The bonds so formed between magnesium and chlorine are ionic bonds and compound (magnesium chloride) is an ionic compound.

Answer 2

$\huge\sf\red{Answer}$

➝ Magnesium chloride (MgCl₂) is formed by the ionic bond formed between magnesium and chlorine atoms.

➝ The electronic configuration of Mg is 2,8,2. Hence, magnesium needs to loose 2 electrons to become stable.

➝ Electronic configuration of chlorine is 2,8,7. Hence, chlorine needs to gain 1 electron to become stable.

➝ Therefore, during the formation of the ionic bond, a single magnesium atom loses two electrons.

➝ On the other hand, two chlorine atoms gain one electron each.

➝ Hence, magnesium atom becomes cation (positively charged ion) and each chlorine atoms become anions (negatively charged ion).

$\rule{150}1$

$\large\bullet\sf{\pink{\;Formation \:of\: Magnesium\: Chloride}}$

$\dashrightarrow\sf{\underset{\sf{2,8,2}}{Mg}\longrightarrow{}\underset{\sf{2,8}}{Mg^{2+}}+2e^-}$

$\sf{\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\:(Magnesium\:cation)}$

$\dashrightarrow\rm{\underset{\sf{2,8,7}}{Cl}+e^-\longrightarrow{}\underset{\sf{2,8,8}}{Cl^-}}$

$\sf{\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\:(Chloride\:anion)}$

Refer attachment for clear understanding!

$\rule{150}1$