Chapter 22, Problem 22.136SP

Interpretation Introduction

(a)

Interpretation:

The balance net ionic equation for the given reaction needs to be determined.

${\text{Zn}}_{\text{(s})}{\text{+ dil H}}_{\text{2}}{\text{SO}}_{\text{4(aq)}}\underset{}{\to }\text{ ?}$

Concept introduction:

Non-metals forms acidic oxides and tend to form covalent hydride as they have tendency to share their valence electrons to form covalent bond. Metallic oxides are ionic in nature whereas non-metallic oxides are covalent in nature. As the charge on cation increases in oxide, the covalent nature increases due to more polarization of anion from smaller cation.

Interpretation Introduction

(b)

Interpretation:

The balance net ionic equation for the given reaction needs to be determined.

${\text{BaSO}}_{\text{3}}{}_{\text{(s})}{\text{+ HCl}}_{\text{(aq)}}\underset{}{\to }?$

Concept introduction:

Non-metals forms acidic oxides and tend to form covalent hydride as they have tendency to share their valence electrons to form covalent bond. Metallic oxides are ionic in nature whereas non-metallic oxides are covalent in nature. As the charge on cation increases in oxide, the covalent nature increases due to more polarization of anion from smaller cation.

Interpretation Introduction

(c)

Interpretation:

The balance net ionic equation for the given reaction needs to be determined.

${\text{Cu}}_{\text{(s) }}{\text{+ hot, concentrated H}}_{\text{2}}{\text{SO}}_{\text{4(l)}}\underset{}{\to }\text{ ?}$

Concept introduction:

Non-metals forms acidic oxides and tend to form covalent hydride as they have tendency to share their valence electrons to form covalent bond. Metallic oxides are ionic in nature whereas non-metallic oxides are covalent in nature. As the charge on cation increases in oxide, the covalent nature increases due to more polarization of anion from smaller cation.

Interpretation Introduction

(d)

Interpretation:

The balance net ionic equation for the given reaction needs to be determined.

${\text{H}}_{\text{2}}{\text{S}}_{\text{(aq})}{\text{+ I}}_{\text{2}}{}_{\text{(aq)}}\underset{}{\to }\text{ ?}$

Concept introduction:

Non-metals forms acidic oxides and tend to form covalent hydride as they have tendency to share their valence electrons to form covalent bond. Metallic oxides are ionic in nature whereas non-metallic oxides are covalent in nature. As the charge on cation increases in oxide, the covalent nature increases due to more polarization of anion from smaller cation.