Explanations 
Textbooks 
Flashcards 
91影视 AI 
Notes 
Study Plans 
Study Sets 
Find a degree 
Magazine Chapter 22: Problem 47
Write the IUPAC name for each of the following coordination compounds. \(\mathrm{K}_{3}\left[\mathrm{FeF}_{6}\right]\) \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]^{2+}\) \(-\) \(\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{F}_{5}\right] \quad\) d \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\)
Short Answer
Expert verified
Potassium hexafluoroferrate(III), Diamminediaquacopper(II) ion, Ammonium aquapentafluoroferrate(III), Dicyanoargentate(I) ion.
Step by step solution
01
Understanding Coordination Compounds
Coordination compounds consist of a central metal atom or ion bonded to surrounding ligands. The ligands can be ions or molecules. It is important to identify the central metal and the attached ligands to correctly name the compound.
02
Naming the Anionic Coordination Compound \\(\mathrm{K}_{3}\left[\mathrm{FeF}_{6}\right]\\)
1. Identify the central metal: \(\mathrm{Fe}\) (Iron).2. Recognize that the complex \(\left[\mathrm{FeF}_{6}\right]^{3-}\) is an anionic coordination entity.3. Use the suffix '-ate' for the metal name because the complex is an anion, making it 'ferrate'.4. Identify the oxidation state of \(\mathrm{Fe}\): The total charge is \(-3\), and each \(\mathrm{F}^{-}\) has \(-1\) charge. Hence, \(x - 6 = -3 \, \Rightarrow x = +3\).5. Name the ligands (fluoride) and count their number (hexafluoride).6. Combine to get the full name: Potassium hexafluoroferrate(III).
03
Naming the Cationic Coordination Compound \\(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{H}_{2}\mathrm{O}\right)_{2}\right]^{2+}\\)
1. Identify the central metal: \(\mathrm{Cu}\) (Copper).2. Recognize that this is a cationic complex.3. Name the ligands: \(\mathrm{NH}_{3}\) (ammine), \(\mathrm{H}_{2}\mathrm{O}\) (aqua).4. Indicate the number of each ligand: diamine, diaqua.5. Determine the oxidation state of \(\mathrm{Cu}\): The charge of complex is \(+2\).6. Assemble the name: Diamminediaquacopper(II) ion.
04
Naming the Neutral Coordination Compound \\(\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{Fe}\left(\mathrm{H}_{2}\mathrm{O}\right) \mathrm{F}_{5}\right]\\)
1. Identify the central metal: \(\mathrm{Fe}\) (Iron).2. Recognize the complex \(\left[\mathrm{Fe}\left(\mathrm{H}_{2}\mathrm{O}\right) \mathrm{F}_{5}\right]^{2-}\) is an anionic entity.3. Use '-ate' suffix for iron, making it 'ferrate'.4. Identify ligands: \(\mathrm{H}_{2}\mathrm{O}\) (aqua), \(\mathrm{F}^{-}\) (fluoride).5. Determine the oxidation state of \(\mathrm{Fe}\): \(x + (0) + 5(-1) = -2 \, \Rightarrow x = +3\).6. Combine to name: Ammonium aquapentafluoroferrate(III).
05
Naming the Anionic Coordination Compound \\(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\\)
1. Identify the central metal: \(\mathrm{Ag}\) (Silver).2. The complex is an anionic entity.3. Use '-ate' suffix for the metal when the complex is negatively charged, turning 'silver' into 'argentate'.4. Identify and count ligands: \(\mathrm{CN}^{-}\) (cyano), total two (dicyano).5. Determine oxidation state for \(\mathrm{Ag}\): \(x + 2(-1) = -1 \, \Rightarrow x = +1\).6. Full name: Dicyanoargentate(I) ion.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with 91影视!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Coordination Compounds
Coordination compounds are fascinating structures in chemistry that consist of a central metal atom or ion surrounded by various molecules or ions known as ligands. This central unit is frequently called a coordination complex. These compounds can display an extraordinary variety of properties and structures, which is why they are studied in fields ranging from bioinorganic chemistry to materials science. For proper understanding:
- The central metal atom or ion is usually transition metals like iron (Fe), copper (Cu), or silver (Ag).
- Ligands are the ions or neutral molecules that surround the metal center. They possess lone pairs of electrons that form coordinate covalent bonds with the metal.
- The overall structure, including the central metal and ligands, can carry a positive, negative, or neutral charge.
Oxidation States
Oxidation states refer to the apparent charges on atoms within a compound that indicate their degree of oxidation. Especially in coordination compounds, accurate determination and presentation of oxidation states are essential for correct nomenclature and understanding the compound's reactivity and properties. When naming a coordination complex:
- The oxidation state of the metal is shown in Roman numerals within parentheses after the metal's name.
- It allows us to balance the total charge of the coordination complex.
- For instance, if a coordination compound is given as [FeF鈧哴鲁鈦�, the total charge on all ligands (each F being -1) indicates the Fe must be in the +3 oxidation state, resulting in ferrate(III).
Ligands
Ligands are the key to understanding how coordination compounds form and behave. They are atoms, ions, or molecules that can donate a pair of electrons to the metal center, creating a coordinate covalent bond. Here are some points to remember about ligands:
- They can be negative ions, like fluoride ( F^{-} ) or CN鈦�, molecules like water (H鈧侽) and ammonia (NH鈧�, called ammine when part of a complex).
- The names and prefixes of ligands depend on whether they are simple ions or more complex molecules; numerical prefixes (di-, tri-,) are often used to indicate the number of each ligand present.
- The nature of the ligand (size, charge, donating ability) influences the complex's geometry, reactivity, and even color.
Anionic and Cationic Complexes
Coordination complexes can be either anionic (negatively charged), cationic (positively charged), or neutral. This classification is key in nomenclature and physical and chemical properties. Here is how they differ:
- Anionic Complexes: When a coordination complex carries a negative charge, it is referred to as an anionic complex. The nomenclature often ends with 'ate', such as in ferrate in [FeF鈧哴鲁鈦�. Identifying the overall charge involves summing the oxidation state of the metal with the charges of the ligands.
- Cationic Complexes: If the complex possesses a positive charge, it usually retains the typical metal name since it behaves like a cation (e.g., the diamminediaquacopper(II) in [Cu(NH鈧�)鈧�(H鈧侽)鈧俔虏鈦�). Like anionic complexes, calculating the total charge is crucial for accuracy.
