Chapter 23, Problem 23.17QP

(a)

Interpretation Introduction

Interpretation: The formulae for each of the given systematic names to be predicted.

Concept Introduction:

The cation is named before the anion.

Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).

When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.

The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.

If the complex ion is an anion, the metal name should end with –ate.

To Identify: The formulae for each of the given systematic names to be predicted.

Answer to Problem 23.17QP

The formula is ${{\text{[Zn(OH)}}_4]}^{2-}$

Explanation of Solution

Predict the formula of $\text{tetrahydroxozincate}\left(\text{II}\right)\text{.}$

$\begin{array}{l}\text{1)}\text{The}\text{ligands}\text{ ; 2)oxidation}\text{state}\text{of}\text{Zn}\text{is}\text{:}\text{+2}\text{}\text{.}\\ \text{tetrahydroxo}\to \text{represented}\text{as}{\text{(OH)}}_{\text{4}}\text{.}\\ \text{Zincate}\to \text{represented}\text{as}\text{Zn}\\ {\text{3)consider,[Zn(OH)}}_4{]}^x\\ \text{overall charge of complex ion = x ; oxidation number of Zn =+2}\\ \text{charge of (OH)ligand = (-1)}\\ \text{2 + (-4) = x}\\ \text{-2 = x}\\ {\text{Thus , the formula is [Zn(OH)}}_4{]}^{2-}.\\ \end{array}$

The formula is ${{\text{[Zn(OH)}}_4]}^{2-}$. The overall charge of the complex ion is $(-2)$,because the Ligand $\text{hydroxo}$ has a charge of $(-1)$.

(b)

Interpretation Introduction

Interpretation: The formulae for each of the given systematic names to be predicted.

Concept Introduction:

1. a) The cation is named before the anion.
2. b) Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).
3. c) When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.
4. d) The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.
5. e) If the complex ion is an anion, the metal name should end with –ate.

To Identify: The formulae for each of the given systematic names to be predicted.

Answer to Problem 23.17QP

The formula is ${\text{[Cr(H}}_{\text{2}}{\text{O)}}_{\text{5}}\text{Cl]}{\text{Cl}}_2$

Explanation of Solution

Predict the formula of $\text{penta-aquachlorochromium(III) chloride}\text{.}$

$\begin{array}{l}\text{1)}\text{The}\text{ligands}\text{ ; 2)oxidation}\text{state}\text{of}\text{Cr}\text{is}\text{:}\text{+3}\text{.}\\ \text{penta-aqua}\to \text{represented}\text{as}{{\text{(H}}_2}_{\text{O)}}\\ \text{chloro}\to \text{represented}\text{as}\text{Cl}\text{.}\\ {\text{3)Consider,[Cr(H}}_{\text{2}}{\text{O)}}_{\text{5}}{\text{Cl]}}^{\text{x}}{\text{Cl}}_x\\ \text{overall charge of complex ion = x ; oxidation number of Cr =+3}\\ {\text{charge of (H}}_2\text{O)ligand = (0) ; charge of (Cl)ligand = (-1)}\\ \text{3 + (-1) = 2}\\ \text{2 = x}\\ {\text{Thus , the formula is [Cr(H}}_{\text{2}}{\text{O)}}_{\text{5}}\text{Cl]}{\text{Cl}}_2.\\ \end{array}$

The formula is ${\text{[Cr(H}}_{\text{2}}{\text{O)}}_{\text{5}}\text{Cl]}{\text{Cl}}_2$. The overall charge of the complex ion is $(+2)$,because the Ligand $\text{chloro}$ has a charge of $(-1)$.

(c)

Interpretation Introduction

Interpretation: The formulae for each of the given systematic names to be predicted.

Concept Introduction:

The cation is named before the anion.

Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).

When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.

The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.

If the complex ion is an anion, the metal name should end with –ate.

To Identify: The formulae for each of the given systematic names to be predicted.

Answer to Problem 23.17QP

The formula is ${{\text{[Cu(Br)}}_4]}^{2-}$

Explanation of Solution

Predict the formula of $\text{tetrabromo-cuprate(II)}\text{.}$

$\begin{array}{l}\text{1)}\text{The}\text{ligands}\&\text{metal ion ; 2)oxidation}\text{state}\text{of}\text{Cu}\text{is}\text{:}\text{+2}\text{.}\\ \text{tetra-bromo}\to \text{represented}\text{as}{\text{Br}}_{\text{4}}\text{.}\\ \text{cuprate (metal anion)}\to \text{represented}\text{as}\text{Cu}\text{.}\\ {\text{3)Consider,[CuBr}}_4{\text{]}}^{\text{x}}\\ \text{overall charge of complex ion = x ; oxidation number of Cu =+2}\\ \text{charge of (Br)ligand = (-1)}\\ \text{2 + (-4) = x}\\ \text{-2 = x}\\ {\text{Thus , the formula is [Cu(Br)}}_4\text{]}{}^{2-}.\\ \end{array}$

The formula is ${{\text{[Cu(Br)}}_4]}^{2-}$. The overall charge of the complex ion is $(-2)$, because the Ligand $\text{Bromo}$ has a charge of $(-1)$.

(d)

Interpretation Introduction

Interpretation: The formulae for each of the given systematic names to be predicted.

Concept Introduction:

The cation is named before the anion.

Within a complex ion, the Ligands are arranged in an alphabetical order followed by the metal ion name. The anionic Ligand should ends with a letter –o, the neutral Ligand are called by the molecules (some common name for some exception).

When more Ligands are present, Greek prefixes like di, tri, tetra, penta, and hexa to specify their number.

The oxidation number of the metal is represented in roman numerals immediately following the metal ion name.

If the complex ion is an anion, the metal name should end with –ate.

To Identify: The formulae for each of the given systematic names to be predicted.

Answer to Problem 23.17QP

The formula is $\text{[Fe(EDTA)]}{}^{2-}$

Explanation of Solution

Find the formula for $\text{ethylenediaminetetraacetatoferrate(II)}\text{.}$

$\begin{array}{l}\text{1)}\text{The}\text{ligands}\&\text{metal ion ; 2)oxidation}\text{state}\text{of}\text{Cu}\text{is}\text{:}\text{+2}\text{.}\\ \text{ethylenediaminetetraacetato}\to \text{represented}\text{as}\text{EDTA}\text{.}\\ \text{ferrate (metal anion)}\to \text{represented}\text{as}\text{Fe}\text{.}\\ {\text{3)Consider,[Fe(EDTA)]}}^{\text{x}}\\ \text{overall charge of complex ion = x ; oxidation number of Fe =+2}\\ \text{charge of (EDTA)ligand = (-4)}\\ \text{2 + (-4) = x}\\ \text{-2 = x}\\ \text{Thus , the formula is [Fe(EDTA)]}{}^{2-}.\\ \end{array}$

The formula is $\text{[Fe(EDTA)]}{}^{2-}$. The overall charge of the complex ion is $(-2)$, because the Ligand $\text{EDTA}$ has a charge of $(-4)$