Chapter 2, Problem 2.50QP

(a)

Interpretation Introduction

Interpretation:

Formula for copper (I) cyanide has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• Generally many ionic compounds are binary in which the metal cations are named first which then followed by naming nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula for Copper (I) cyanide is written as $CuCN$.

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

Cyanide is $C{N}^{-}$ anion and copper (I) is cuprous cation $C{u}^{+}.$ Hence formula of the given compound is written as $CuCN$.

(b)

Interpretation Introduction

Interpretation:

Formula for Strontium chlorite has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula for Strontium chlorite is written as $Sr{\left(Cl{O}_2\right)}_2$

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

Chlorite is $Cl{O}_2^{-}$ anion and Strontium here is cation $S{r}^{2+}.$ Charge on the anion has to be written on the subscript of the cation. Charge on the cation is written on the subscript of the anion. Hence formula of the given compound is written as $Sr{\left(Cl{O}_2\right)}_2$

(c)

Interpretation Introduction

Interpretation:

Formula for Perchloric acid has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula for Perchloric acid is written as $HCl{O}_4$.

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

Oxoacids are named on the basis of polyatomic anion present in them. Here the polyatomic anion is perchloro ion $Cl{O}_4^{-}$. Thus formula for Perchloric acid is written as $HCl{O}_4$.

(d)

Interpretation Introduction

Interpretation:

Formula for the given compound hydroiodic acid has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula of the compound hydroiodic acid is written as $HI$.

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

Binary acids are named based on the non-metal atom present in them. Non-metal in this acid is iodine. Thus the formula of the compound is written as $HI$.

(e)

Interpretation Introduction

Interpretation:

Formula for the given compound Disodium ammonium phosphate has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula of the compound Disodium ammonium phosphate is written as $N{a}_2\left(N{H}_4\right)P{O}_4$.

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

The compound $N{a}_2\left(N{H}_4\right)P{O}_4$ has three ions – two cations $N{a}^{+}$, $N{H}_4^{+}$ and one anion $P{O}_4^{3-}$.

The charge on the anion $3-$ is balanced by charge on cation 2, positive charge from sodium ion, i.e. $2N{a}^{+}$ and one positive charge from ammonium ion $N{H}_4^{+}$.

Thus formula of the compound Disodium ammonium phosphate is written as $N{a}_2\left(N{H}_4\right)P{O}_4$.

(f)

Interpretation Introduction

Interpretation:

Formula for the given compound Lead(II) carbonate has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula of the compound Lead(II) carbonate is written as $PbC{O}_3$.

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

The cation and anion in Lead(II) carbonate are lead(II) ion $P{b}^{2+}$ and carbonate ion $C{O}_3^{2-}$ respectively.  Charge on the anion is written on the subscript of the cation.  Charge on the cation is written on the subscript of the anion.

Hence the formula is $P{b}_2{\left(C{O}_3\right)}_2$

The formula can be simplified and written as the same number in subscript gets called and thus the formula of the compound Magnesium phosphate is written as $PbC{O}_3$.

(g)

Interpretation Introduction

Interpretation:

Formula for the given compound Tin(II) fluoride has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula for the compound Tin(II) fluoride is written as $Sn{F}_2$.

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

The cation and anion in Tin(II) fluoride are Tin(II) ion $S{n}^{2+}$ and fluoride ion $F^{-}$ respectively.  Charge on the anion is written on the subscript of the cation.  Charge on the cation is written on the subscript of the anion.

Hence the formula is $Sn{F}_2$

(h)

Interpretation Introduction

Interpretation:

Formula for the given compound Tetraphosphorus decasulfide has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula for the compound Tetraphosphorus decasulfide is written as $P_4{S}_{10}$.

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

The prefix ‘tetra’ indicates 4 P atoms and ‘deca’ indicates 10 S atoms.

Hence the formula is $P_4{S}_{10}$

(i)

Interpretation Introduction

Interpretation:

Formula for the given compound Mercury (II) oxide has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula of the compound Mercury (II) oxide is written as $HgO$

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

The cation and anion in Mercury(II) oxide are mercury(II) ion $H{g}^{2+}$ and oxide ion $O^{2-}$ respectively.  Charge on the anion is written on the subscript of the cation.  Charge on the cation is written on the subscript of the anion.

Hence the formula is $H{g}_2{O}_2$

The formula can be simplified and written as the same number in subscript gets called and thus the formula of the compound Mercury(II) oxide is written as $HgO$

(j)

Interpretation Introduction

Interpretation:

Formula for the given compound Mercury (I) iodide has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula of Mercury (I) iodide is written as $H{g}_2{I}_2$

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

The cation and anion in Mercury(I) iodide are mercury(I) ion $H{g}^{1+}$ and iodide ion $I^{-}$ respectively.  Experimental studies show that $H{g}^{1+}$ exists as dimer - $H{g}_2^{2+}$ Charge on the anion is written on the subscript of the cation.  Charge on the cation is written on the subscript of the anion.

Hence the formula is ${\left(H{g}_2\right)}_1{I}_2$ and it is written as $H{g}_2{I}_2.$

(k)

Interpretation Introduction

Interpretation:

Formula for the given compound cobalt $\left(II\right)$ chloride hexahydrate has to be written.

Concept Introduction:

Generally the ionic compound consists of cation and anion.

Cation: When electrons are removed from the atom that results to form positively charged ion called cation.

Anion: Addition of electron to atom results to form negatively charged ion called anion.

The nomenclature of inorganic compounds involves following rules:

• For ionic compounds first, metal cations are named first which then followed by nonmetallic anion.
• In ionic compound the metal cations generally hold their metal name itself and the metal anions hold their respective metal name with suffix $\text{"-ide"}$ with it.
• The prefixes on each atom indicate the number of those atoms in the compound.
• The number written on the subscript of the anion is numerically equal to the charge on the cation and vice versa.
• Subscripts are discarded when the numerical charge on cation and anion are equal.
• When a metal has more than one positive oxidation state, its lowest oxidation number has name of the metal ion ending with ‘ous’ and highest oxidation number has name of the metal ion ending with ‘ic’. This rule is applicable when oxidation number of metal is not more than three.
• If a metal ion has multiple numbers of oxidation states more than three, then Roman numeral has to be used within square brackets to indicate the oxidation number of metal ion.
• Nomenclature of binary acids and oxoacids are not similar. Binary acids are named based on the non-metal atom present in them. Oxoacids are named on the basis of polyatomic anion present in them.
• Naming binary molecular compounds is also similar to binary ionic compounds.
• The first element is named as such while second element is added with prefix which describes the number of respective atoms present.

Answer to Problem 2.50QP

Formula of cobalt $\left(II\right)$ chloride hexahydrate is written as $CoC{l}_2.6H_{2}O$

Explanation of Solution

With reference to table 2.3 in the text book, anions and cations formed by various elements are named.

In cobalt $\left(II\right)$ chloride the cation is $C{o}^{2+}$ and the anion is $2C{l}^{-}$ ions. Charge on the anion is written on the subscript of the cation. Charge on the cation is written on the subscript of the anion. The term hexahydrate says that the compound has six water molecules with it.

Hence the formula is written as $CoC{l}_2.6H_{2}O$.