Chapter 4.1, Problem 4.6YT

(a)

Interpretation Introduction

Interpretation:

The chemical formula for sodium hypochlorite has to be given.

Concept Introduction:

Chemical formula of a compound is the symbolic representation of its atomic constituents. To write the chemical formula of a compound one should know the following things,

• ✓  The symbols of the constituent elements
• ✓  The combining capacity of each atom constituting the compound

If a compound contains a metal cation bonded to a non-metal anion then it can be considered as an Ionic compound. The cation and anions are hold together by an electrostatic attraction.

Nomenclature of ionic compounds

Cation (positively charged ion) must be named first then consider anion (negatively charged ion).

Cation:

If the cation has only one possible charge then the element’s name can be used. If cation has more than one possible charge, then charge of the cation in Roman numeral (in parentheses) must be included in its name.

Anion:

If the given ionic compound is binary, use element name and change its ending to –ide.

If the given ionic compound is tertiary, use polyatomic ion chart to the name ion.

Polyatomic ion chart is shown below,

$\begin{array}{cc}\text{Common}\text{polyatomic}\text{ion}& \text{Name}\\ {\text{NH}}_{\text{4}}^{\text{+}}& \text{Ammonium}\\ {\text{C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}^{\text{-}}& \text{Acetate}\\ {\text{OH}}^{\text{-}}& \text{Hydroxide}\\ {\text{ClO}}_{\text{3}}^{\text{-}}& \text{Chlorate}\\ {\text{CO}}_{\text{3}}^{\text{2-}}& \text{Carbonate}\\ {\text{CN}}^{\text{-}}& \text{Cyanide}\\ {\text{HCO}}_{\text{3}}^{\text{-}}& \text{Bicarbonate}\\ {\text{HSO}}_{\text{4}}^{\text{-}}& \text{Bisulfate}\\ {\text{HSO}}_{\text{3}}^{\text{-}}& \text{Bisulfite}\\ {\text{ClO}}^{\text{-}}& \text{Hypochlorite}\\ {\text{NO}}_{\text{3}}^{\text{-}}& \text{Nitrate}\\ {\text{NO}}_{\text{2}}^{\text{-}}& \text{Nitrite}\\ {\text{C}}_{\text{2}}{\text{O}}_{\text{4}}^{\text{2-}}& \text{Oxalate}\\ {\text{ClO}}_{\text{4}}^{\text{-}}& \text{Perchlorate}\\ {\text{MnO}}_{\text{4}}^{\text{-}}& \text{Permangnate}\\ {\text{PO}}_{\text{4}}^{\text{3-}}& \text{Phosphate}\\ {\text{SO}}_{\text{4}}^{\text{2-}}& \text{Sulfate}\\ {\text{SO}}_{\text{3}}^{\text{2-}}& \text{Sulfite}\\ {\text{ClO}}_{\text{2}}^{\text{-}}& \text{Chlorite}\\ {\text{Cr}}_{\text{2}}{\text{O}}_{\text{7}}^{\text{2-}}& \text{Dichromate}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The chemical formula for magnesium carbonate has to be given.

Concept Introduction:

Chemical formula of a compound is the symbolic representation of its atomic constituents. To write the chemical formula of a compound one should know the following things,

• ✓  The symbols of the constituent elements
• ✓  The combining capacity of each atom constituting the compound

If a compound contains a metal cation bonded to a non-metal anion then it can be considered as an Ionic compound. The cation and anions are hold together by an electrostatic attraction.

Nomenclature of ionic compounds

Cation (positively charged ion) must be named first then consider anion.

Cation:

If the cation has only one possible charge then the element’s name can be used. If cation has more than one possible charge, then charge of the cation in Roman numeral (in parentheses) must be included in its name.

Anion:

If the given ionic compound is binary, use element name and change its ending to –ide.

If the given ionic compound is tertiary, use polyatomic ion chart to the name ion.

Polyatomic ion chart is shown below,

$\begin{array}{cc}\text{Common}\text{polyatomic}\text{ion}& \text{Name}\\ {\text{NH}}_{\text{4}}^{\text{+}}& \text{Ammonium}\\ {\text{C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}^{\text{-}}& \text{Acetate}\\ {\text{OH}}^{\text{-}}& \text{Hydroxide}\\ {\text{ClO}}_{\text{3}}^{\text{-}}& \text{Chlorate}\\ {\text{CO}}_{\text{3}}^{\text{2-}}& \text{Carbonate}\\ {\text{CN}}^{\text{-}}& \text{Cyanide}\\ {\text{HCO}}_{\text{3}}^{\text{-}}& \text{Bicarbonate}\\ {\text{HSO}}_{\text{4}}^{\text{-}}& \text{Bisulfate}\\ {\text{HSO}}_{\text{3}}^{\text{-}}& \text{Bisulfite}\\ {\text{ClO}}^{\text{-}}& \text{Hypochlorite}\\ {\text{NO}}_{\text{3}}^{\text{-}}& \text{Nitrate}\\ {\text{NO}}_{\text{2}}^{\text{-}}& \text{Nitrite}\\ {\text{C}}_{\text{2}}{\text{O}}_{\text{4}}^{\text{2-}}& \text{Oxalate}\\ {\text{ClO}}_{\text{4}}^{\text{-}}& \text{Perchlorate}\\ {\text{MnO}}_{\text{4}}^{\text{-}}& \text{Permangnate}\\ {\text{PO}}_{\text{4}}^{\text{3-}}& \text{Phosphate}\\ {\text{SO}}_{\text{4}}^{\text{2-}}& \text{Sulfate}\\ {\text{SO}}_{\text{3}}^{\text{2-}}& \text{Sulfite}\\ {\text{ClO}}_{\text{2}}^{\text{-}}& \text{Chlorite}\\ {\text{Cr}}_{\text{2}}{\text{O}}_{\text{7}}^{\text{2-}}& \text{Dichromate}\end{array}$

(c)

Interpretation Introduction

Interpretation:

The chemical formula for ammonium nitrate has to be given.

Concept Introduction:

Chemical formula of a compound is the symbolic representation of its atomic constituents. To write the chemical formula of a compound one should know the following things,

• ✓  The symbols of the constituent elements
• ✓  The combining capacity of each atom constituting the compound

If a compound contains a metal cation bonded to a non-metal anion then it can be considered as an Ionic compound. The cation and anions are hold together by an electrostatic attraction.

Nomenclature of ionic compounds

Cation (positively charged ion) must be named first then consider anion.

Cation:

If the cation has only one possible charge then the element’s name can be used. If cation has more than one possible charge, then charge of the cation in Roman numeral (in parentheses) must be included in its name.

Anion:

If the given ionic compound is binary, use element name and change its ending to –ide.

If the given ionic compound is tertiary, use polyatomic ion chart to the name ion.

Polyatomic ion chart is shown below,

$\begin{array}{cc}\text{Common}\text{polyatomic}\text{ion}& \text{Name}\\ {\text{NH}}_{\text{4}}^{\text{+}}& \text{Ammonium}\\ {\text{C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}^{\text{-}}& \text{Acetate}\\ {\text{OH}}^{\text{-}}& \text{Hydroxide}\\ {\text{ClO}}_{\text{3}}^{\text{-}}& \text{Chlorate}\\ {\text{CO}}_{\text{3}}^{\text{2-}}& \text{Carbonate}\\ {\text{CN}}^{\text{-}}& \text{Cyanide}\\ {\text{HCO}}_{\text{3}}^{\text{-}}& \text{Bicarbonate}\\ {\text{HSO}}_{\text{4}}^{\text{-}}& \text{Bisulfate}\\ {\text{HSO}}_{\text{3}}^{\text{-}}& \text{Bisulfite}\\ {\text{ClO}}^{\text{-}}& \text{Hypochlorite}\\ {\text{NO}}_{\text{3}}^{\text{-}}& \text{Nitrate}\\ {\text{NO}}_{\text{2}}^{\text{-}}& \text{Nitrite}\\ {\text{C}}_{\text{2}}{\text{O}}_{\text{4}}^{\text{2-}}& \text{Oxalate}\\ {\text{ClO}}_{\text{4}}^{\text{-}}& \text{Perchlorate}\\ {\text{MnO}}_{\text{4}}^{\text{-}}& \text{Permangnate}\\ {\text{PO}}_{\text{4}}^{\text{3-}}& \text{Phosphate}\\ {\text{SO}}_{\text{4}}^{\text{2-}}& \text{Sulfate}\\ {\text{SO}}_{\text{3}}^{\text{2-}}& \text{Sulfite}\\ {\text{ClO}}_{\text{2}}^{\text{-}}& \text{Chlorite}\\ {\text{Cr}}_{\text{2}}{\text{O}}_{\text{7}}^{\text{2-}}& \text{Dichromate}\end{array}$

(d)

Interpretation Introduction

Interpretation:

The chemical formula for calcium hydroxide has to be given.

Concept Introduction:

Chemical formula of a compound is the symbolic representation of its atomic constituents. To write the chemical formula of a compound one should know the following things,

• ✓  The symbols of the constituent elements
• ✓  The combining capacity of each atom constituting the compound

If a compound contains a metal cation bonded to a non-metal anion then it can be considered as an Ionic compound. The cation and anions are hold together by an electrostatic attraction.

Nomenclature of ionic compounds

Cation (positively charged ion) must be named first then consider anion.

Cation:

If the cation has only one possible charge then the element’s name can be used. If cation has more than one possible charge, then charge of the cation in Roman numeral (in parentheses) must be included in its name.

Anion:

If the given ionic compound is binary, use element name and change its ending to –ide.

If the given ionic compound is tertiary, use polyatomic ion chart to the name ion.

Polyatomic ion chart is shown below,

$\begin{array}{cc}\text{Common}\text{polyatomic}\text{ion}& \text{Name}\\ {\text{NH}}_{\text{4}}^{\text{+}}& \text{Ammonium}\\ {\text{C}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}^{\text{-}}& \text{Acetate}\\ {\text{OH}}^{\text{-}}& \text{Hydroxide}\\ {\text{ClO}}_{\text{3}}^{\text{-}}& \text{Chlorate}\\ {\text{CO}}_{\text{3}}^{\text{2-}}& \text{Carbonate}\\ {\text{CN}}^{\text{-}}& \text{Cyanide}\\ {\text{HCO}}_{\text{3}}^{\text{-}}& \text{Bicarbonate}\\ {\text{HSO}}_{\text{4}}^{\text{-}}& \text{Bisulfate}\\ {\text{HSO}}_{\text{3}}^{\text{-}}& \text{Bisulfite}\\ {\text{ClO}}^{\text{-}}& \text{Hypochlorite}\\ {\text{NO}}_{\text{3}}^{\text{-}}& \text{Nitrate}\\ {\text{NO}}_{\text{2}}^{\text{-}}& \text{Nitrite}\\ {\text{C}}_{\text{2}}{\text{O}}_{\text{4}}^{\text{2-}}& \text{Oxalate}\\ {\text{ClO}}_{\text{4}}^{\text{-}}& \text{Perchlorate}\\ {\text{MnO}}_{\text{4}}^{\text{-}}& \text{Permangnate}\\ {\text{PO}}_{\text{4}}^{\text{3-}}& \text{Phosphate}\\ {\text{SO}}_{\text{4}}^{\text{2-}}& \text{Sulfate}\\ {\text{SO}}_{\text{3}}^{\text{2-}}& \text{Sulfite}\\ {\text{ClO}}_{\text{2}}^{\text{-}}& \text{Chlorite}\\ {\text{Cr}}_{\text{2}}{\text{O}}_{\text{7}}^{\text{2-}}& \text{Dichromate}\end{array}$