Question

In the compound MgCl2, the subscript 2 indicates that

Answer 1

Answer : The correct option is D.

Explanation :

The given compound is $MgCl_2$.

When $MgCl_2$ is dissolve in water then they dissociates into two ions such as magnesium ion and chloride ion.

It is represented as,

$MgCl_2+H_2O\rightarrow Mg^{2+}+2Cl^-$

The charge on magnesium ion is +2 and on chloride ion is -1. To neutralize the charge on magnesium ion, two chloride ions must be used.

Answer 2

In ${\text{MgC}}{{\text{l}}_2}$ , the subscript 2 indicates that

$\boxed{{\text{D}}{\text{. There are two chloride ions for each magnesium ion}}{\text{.}}}$

Further Explanation:

The attraction between atoms, molecules or ions which results in the formation of chemical compounds is known as a chemical bond. It is formed either due to electrostatic forces or by the sharing of electrons. There are many strong bonds such as ionic bonds, covalent bonds, and metallic bonds while some weak bonds like dipole-dipole interactions, London dispersion forces, and hydrogen bonding.

Ionic compounds are the compounds that are formed from the ions of the respective species. Ions are the species that are formed either due to loss or gain of electrons. A neutral atom forms cation by the loss of electrons and anion by the gain of electrons.

There is formation of ionic bond in case of ${\text{MgC}}{{\text{l}}_2}$. Magnesium, being a metal loses two electrons and ${\text{M}}{{\text{g}}^{2 + }}$ is formed. These electrons are accepted by two chlorine atoms and two ${\text{C}}{{\text{l}}^ - }$ ions are formed.

The dissociation of ${\text{MgC}}{{\text{l}}_2}$ occurs as follows:

${\text{MgC}}{{\text{l}}_2} \rightleftharpoons {\text{M}}{{\text{g}}^{2 + }} + {\text{2C}}{{\text{l}}^ - }$

Here, one ${\text{M}}{{\text{g}}^{2 + }}$ and two ${\text{C}}{{\text{l}}^ - }$ are formed. This indicates that there are two chlorine ions for each magnesium ion. So the subscript in the chemical formula of ${\text{MgC}}{{\text{l}}_2}$ indicates the presence of two chlorine atoms per ion of magnesium. This implies statement A is incorrect and statement D is correct.

The chemical formula of the compound has nothing to do with the size of the ions formed during the compound formation. So subscript gives no idea about the size of the ions. This implies statement B is incorrect.

A covalent bond requires mutual sharing of electrons between the bonded atoms. But there is an ionic bond formation between magnesium and chlorine due to difference in their electronegativities. So a double covalent bond cannot be formed between chlorine and magnesium. This implies statement C is incorrect.

Learn more:

1. Identification of ionic bonding: brainly.com/question/1603987

2. Basis of investigation for the scientists: brainly.com/question/158048

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Ionic and covalent compounds

Keywords: chlorine, magnesium, ionic bond, electronegativity, covalent bond, compound, chemical formula, mutual sharing, chemical bond, electrostatic forces, cation, anion.