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Chapter 23: Problem 57

Give formulas corresponding to the following names: (a) Hexaaquachromium(III) sulfate (b) Barium tetrabromoferrate(III) (c) Bis(ethylenediamine)platinum(II) carbonate

Short Answer

Expert verified
(a) \text{[Cr(H₂O)₆]₂(SO₄)₃}, (b) \text{Ba[FeBr₄]}, (c) \text{[Pt(en)₂]CO₃}

Step by step solution

01

Identify the coordination complex components

For each compound, identify the central metal atom/ion, its oxidation state, and the ligands associated with it.
02

Write the formulas for the ligands

Convert the names of the ligands into their respective chemical formulas. For example, water is H₂O, ethylenediamine is (en), etc.
03

Combine metal and ligands

Combine the central metal atom/ion with its ligands according to the given name. Ensure the correct coordination number and oxidation state of the metal.
04

Balance the charges

Ensure that the overall charge of the coordination compound is balanced by considering the charges of the metal ion and the ligands.
05

Write the final formula

Combine everything from the previous steps to write the complete chemical formula for each coordination compound.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Formulas
Chemical formulas are a way to represent chemical substances using symbols and numbers. They show which elements are present in a molecule and in what quantities. For coordination compounds, chemical formulas become slightly more complex as they need to include the central metal ion and its surrounding ligands. Here are some key points to remember:
  • Identify each component in the name given (metal, ligands).
  • Convert the names of ligands to their chemical formulas (e.g., water is H₂O).
  • Ensure that the metal ion’s oxidation state is accounted for properly.
  • Combine these individual components correctly to write the full formula.
For example, to write the formula for Hexaaquachromium(III) sulfate, recognize that “hexaaqua” refers to six water molecules (ligands) and “chromium(III)” tells us that chromium is in the +3 oxidation state. The formula will be [Cr(H₂O)₆]²(SO₄)₃.
Oxidation States
Oxidation states indicate the degree of oxidation of an atom within a compound. In coordination chemistry, knowing the oxidation state of the metal center is crucial for determining the charge balance between the metal and ligands. Key points to remember:
  • Oxidation state is typically indicated in Roman numerals in parentheses after the metal (e.g., Chromium(III) -> Cr³⁺).
  • This helps in determining how many ligands can attach to the central metal ion.
  • For cations like Cr³⁺ (in Hexaaquachromium(III)), it shows the metal can form bonds with negatively charged or neutral ligands.
For the given problem, Chromium(III) means a +3 oxidation state, which plays a pivotal role in forming robust coordination complexes.
Ligands
Ligands are molecules or ions that donate at least one pair of electrons to a central metal atom or ion to form a coordination complex. Ligands are classified by their charge, size, and the number of donor atoms available for bonding. To understand ligands better, consider the following points:
  • Neutral ligands like water (H₂O) and ammonia (NH₃) have no overall charge.
  • Anionic ligands like chloride (Cl⁻) and hydroxide (OH⁻) carry a negative charge.
  • Polydentate ligands, such as ethylenediamine (en), can form multiple bonds with the central metal ion.
For instance, in Hexaaquachromium(III) sulfate, ‘hexaaqua’ signifies six water molecules, each acting as neutral ligands to bond with the chromium ion.
Coordination Chemistry
Coordination chemistry explores the properties and behaviors of coordination compounds where a central metal ion is bonded to a set of surrounding molecules or ions called ligands. Several essential concepts in coordination chemistry:
  • The 'coordination number' refers to the number of ligand bonds to the central atom (e.g., Hexaaquachromium has a coordination number of 6 because it is bonded to six water molecules).
  • The 'geometry' of a coordination complex can vary (octahedral, tetrahedral, square planar, etc.), depending on the coordination number and type of ligands.
  • The stability of these complexes is influenced by various factors, including the charge of the metal ion and the nature of the ligands.
Understanding how to combine these elements helps you write chemical formulas for coordination compounds correctly and predict their behavior.

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Most popular questions from this chapter

Give formulas corresponding to the following names: (a) Tetraamminezinc sulfate (b) Pentaamminechlorochromium(III) chloride (c) Sodium bis(thiosulfato)argentate(I)

Ionic liquids have many applications in engineering and materials science. The dissolution of the metavanadate ion in chloroaluminate ionic liquids has been studied: $$\mathrm{VO}_{3}^{-}+\mathrm{AlCl}_{4}^{-} \longrightarrow \mathrm{VO}_{2}\mathrm{Cl}_{2}^{-}+\mathrm{AlOCl}_{2}^{-}$$ (a) What is the oxidation number of \(\mathrm{V}\) and \(\mathrm{Al}\) in each ion? (b) In reactions of \(\mathrm{V}_{2} \mathrm{O}_{5}\) with \(\mathrm{HCl}\), acid concentration affects the product. At low acid concentration, \(\mathrm{VO}_{2} \mathrm{Cl}_{2}^{-}\) and \(\mathrm{VO}_{3}^{-}\) form: $$\mathrm{V}_{2} \mathrm{O}_{5}+\mathrm{HCl} \longrightarrow \mathrm{VO}_{2}\mathrm{Cl}_{2}^{-}+\mathrm{VO}_{3}^{-}+\mathrm{H}^{+}$$ At high acid concentration, \(\mathrm{VOCl}_{3}\) forms: $$\mathrm{V}_{2} \mathrm{O}_{5}+\mathrm{HCl} \longrightarrow \mathrm{VOCl}_{3}+\mathrm{H}_{2} \mathrm{O}$$ Balance each equation, and state which, if either, is a redox process. (c) What mass of \(\mathrm{VO}_{2} \mathrm{Cl}_{2}^{-}\) or \(\mathrm{VOCl}_{3}\) can form from \(12.5 \mathrm{~g}\) of \(\mathrm{V}_{2} \mathrm{O}_{5}\) and the appropriate concentration of acid?

(a) What is the maximum number of unpaired electrons in a lanthanide ion? (b) How does this number relate to occupancy of the \(4 f\) subshell?

Two bidentate ligands used extensively in analytical chemistry are bipyridyl (bipy) and ortho-phenanthroline \((o\) -phen \():\) Draw structures and discuss the possibility of isomers for (a) [Pt(bipy) \(\mathrm{Cl}_{2}\) ] (b) \(\left[\mathrm{Fe}(o-\mathrm{phen})_{3}\right]^{3+}\) (c) [Co(bipy) \(\left._{2} \mathrm{~F}_{2}\right]^{+}\) (d) \(\left[\mathrm{Co}(o-\mathrm{phen})\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}\right]^{2+}\)

How many \(d\) electrons \(\left(n\right.\) of \(\left.d^{n}\right)\) are in the central metal ion in (a) \(\left[\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{SO}_{4}\) (b) \(\mathrm{Na}_{2}\left[\mathrm{Os}(\mathrm{CN})_{6}\right] ;\) (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{CO}_{3} \mathrm{I}\right] ?\)
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