Chapter 21, Problem 13PS

(a)

Interpretation Introduction

Interpretation: The complete balanced equation should be written for the given reaction.

Concept introduction: Main group elements are categorized as s-block and p-block elements. The s-block elements include metals belonging to group $\text{1A}$ and group $\text{2A}$ and elements from group $\text{3A}$ to $\text{8A}$ are referred to as p-block elements. The reaction of the metals with the nonmetals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which is gained by the nonmetals. The metal gets positively charge and the non-metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  $\text{M}\to {\text{M}}^{n+}+n{e}^{-}$

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    $\text{X}+n{e}^{-}\to {\text{X}}^{n-}$

The metals of group $\text{1A}$ form $+1$ ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group $\text{1A}$ elements is $+1$. Similarly, group $\text{2A}$ elements form $+2$ ions by losing two electrons and have an oxidation number of $+2$. The non-metal gains these electrons to form anions with $-1$ and $-2$ charge.

The compounds of non-metals with oxides and hydrides are covalent compounds. This is because non-metals are less electropositive and the difference in electronegativity between two elements is less than $2$. If the difference in electronegativity is more than $2$ then ionic compounds are formed.

(b)

Interpretation Introduction

Interpretation: The complete balanced equation should be written for the given reaction.

Concept introduction: Main group elements are categorized as s-block and p-block elements. The s-block elements include metals belonging to group $\text{1A}$ and group $\text{2A}$ and elements from group $\text{3A}$ to $\text{8A}$ are referred to as p-block elements. The reaction of the metals with the nonmetals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which is gained by the nonmetals. The metal gets positively charge and the non-metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  $\text{M}\to {\text{M}}^{n+}+n{e}^{-}$

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    $\text{X}+n{e}^{-}\to {\text{X}}^{n-}$

The metals of group $\text{1A}$ form $+1$ ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group $\text{1A}$ elements is $+1$. Similarly, group $\text{2A}$ elements form $+2$ ions by losing two electrons and have an oxidation number of $+2$. The non-metal gains these electrons to form anions with $-1$ and $-2$ charge.

The compounds of non-metals with oxides and hydrides are covalent compounds. This is because non-metals are less electropositive and the difference in electronegativity between two elements is less than $2$. If the difference in electronegativity is more than $2$ then ionic compounds are formed.

(c)

Interpretation Introduction

Interpretation: The complete balanced equation should be written for the given reaction.

Concept introduction: Main group elements are categorized as s-block and p-block elements. The s-block elements include metals belonging to group $\text{1A}$ and group $\text{2A}$ and elements from group $\text{3A}$ to $\text{8A}$ are referred to as p-block elements. The reaction of the metals with the nonmetals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which is gained by the nonmetals. The metal gets positively charge and the non-metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  $\text{M}\to {\text{M}}^{n+}+n{e}^{-}$

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    $\text{X}+n{e}^{-}\to {\text{X}}^{n-}$

The metals of group $\text{1A}$ form $+1$ ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group $\text{1A}$ elements is $+1$. Similarly, group $\text{2A}$ elements form $+2$ ions by losing two electrons and have an oxidation number of $+2$. The non-metal gains these electrons to form anions with $-1$ and $-2$ charge.

The compounds of non-metals with oxides and hydrides are covalent compounds. This is because non-metals are less electropositive and the difference in electronegativity between two elements is less than $2$. If the difference in electronegativity is more than $2$ then ionic compounds are formed.

(d)

Interpretation Introduction

Interpretation: The complete balanced equation should be written for the given reaction.

Concept introduction: Main group elements are categorized as s-block and p-block elements. The s-block elements include metals belonging to group $\text{1A}$ and group $\text{2A}$ and elements from group $\text{3A}$ to $\text{8A}$ are referred to as p-block elements. The reaction of the metals with the nonmetals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which is gained by the nonmetals. The metal gets positively charge and the non-metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  $\text{M}\to {\text{M}}^{n+}+n{e}^{-}$

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    $\text{X}+n{e}^{-}\to {\text{X}}^{n-}$

The metals of group $\text{1A}$ form $+1$ ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group $\text{1A}$ elements is $+1$. Similarly, group $\text{2A}$ elements form $+2$ ions by losing two electrons and have an oxidation number of $+2$. The non-metal gains these electrons to form anions with $-1$ and $-2$ charge.

The compounds of non-metals with oxides and hydrides are covalent compounds. This is because non-metals are less electropositive and the difference in electronegativity between two elements is less than $2$. If the difference in electronegativity is more than $2$ then ionic compounds are formed.