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FAQs on Mind Map: Coordination Compounds - Chemistry Class 12 - NEET
| 1. What are coordination compounds and how are they formed? |  |
Ans. Coordination compounds are chemical compounds consisting of a central metal atom or ion bonded to surrounding molecules or anions, known as ligands. They are formed when the metal atom donates its empty orbitals to accept electron pairs from the ligands, creating coordinate covalent bonds. This interaction results in the formation of complex ions or neutral coordination compounds.
| 2. What is the significance of ligands in coordination compounds? | |
Ans. Ligands play a crucial role in coordination compounds as they determine the properties and reactivity of the compound. They can be neutral molecules, like water (H₂O), or ions, like chloride (Cl⁻). The type, number, and arrangement of ligands around the central metal ion influence the compound's stability, color, and biological activity.
| 3. Can you explain the different types of ligands found in coordination compounds? | |
Ans. Ligands are categorized based on the number of bonding sites they possess. Monodentate ligands have one donor atom (e.g., NH₃, H₂O), bidentate ligands have two donor atoms (e.g., ethylenediamine), and polydentate ligands can attach through multiple sites (e.g., EDTA). This diversity in bonding allows for various geometrical arrangements in coordination complexes.
| 4. What are some common applications of coordination compounds? | |
Ans. Coordination compounds have numerous applications, including in medicine (e.g., cisplatin for cancer treatment), agriculture (e.g., fertilizers), and industrial processes (e.g., catalysts in chemical reactions). They are also used in materials science for developing new materials with specific properties, such as magnetic or optical characteristics.
| 5. How do you determine the oxidation state of the central metal in coordination compounds? | |
Ans. The oxidation state of the central metal in a coordination compound can be determined by considering the charge of the entire complex and the charges of the ligands. The sum of the oxidation states of the metal and the ligands must equal the overall charge of the complex. For example, in [Cu(NH₃)₄]²⁺, if each NH₃ is neutral, the oxidation state of Cu must be +2 to balance the overall +2 charge of the complex.
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