![Provide the IUPAC names for the following coordination compounds: i. [CrCl2(H2O)4]NO3 ii. [Pd(ONO)2(H2O)2I2] iii. (NH4)3[Fe(CN)6]](/_next/image?url=https%3A%2F%2Fohijasnjvprzodcmxltt.supabase.co%2Fstorage%2Fv1%2Fobject%2Fpublic%2Fwhatsapp-images%2F1777301131266-96bc96ff4dc5fb4e.png&w=3840&q=75)
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Hey Eharuner — ready when you are. Here are the names for the given coordination compounds: i. [CrCl_2(H_2O)_4]NO_3 Step 1: Identify the ligands and their charges. Chloro (Cl^-) has a -1 charge, aqua (H_2O) is neutral. The counter ion is nitrate (NO_3^-), which has a -1 charge. Step 2: Determine the oxidation state of chromium (Cr). x + 2(-1) + 4(0) = +1 x - 2 = +1 x = +3 Step 3: Name the complex cation and anion. Ligands are named alphabetically: aqua, chloro. Name: Dichlorotetraaquachromium(III) nitrate Dichlorotetraaquachromium(III) nitrate ii. [Pd(ONO)_2(H_2O)_2I_2] Step 1: Identify the ligands and their charges. Nitrito-O (ONO^-) has a -1 charge, aqua (H_2O) is neutral, iodo (I^-) has a -1 charge. This is a neutral complex. Step 2: Determine the oxidation state of palladium (Pd). x + 2(-1) + 2(0) + 2(-1) = 0 x - 2 - 2 = 0 x = +4 Step 3: Name the complex. Ligands are named alphabetically: aqua, iodo, nitrito-O. Name: Diaquadiododinitrito-O-palladium(IV) Diaquadiododinitrito-O-palladium(IV) iii. (NH_4)_3[Fe(CN)_6] Step 1: Identify the cation and ligands. The cation is ammonium (NH_4^+). The ligand is cyano (CN^-), which has a -1 charge. Step 2: Determine the charge of the complex anion. Since there are three NH_4^+ ions, the complex anion must have a -3 charge. Step 3: Determine the oxidation state of iron (Fe). x + 6(-1) = -3 x - 6 = -3 x = +3 Step 4: Name the complex. The metal in an anionic complex ends with "-ate". Name: Ammonium hexacyanoferrate(III) Ammonium hexacyanoferrate(III) iv. (NH_4)_4[Fe(CN)_6] Step 1: Identify the cation and ligands. The cation is ammonium (NH_4^+). The ligand is cyano (CN^-), which has a -1 charge. Step 2: Determine the charge of the complex anion. Since there are four NH_4^+ ions, the complex anion must have a -4 charge. Step 3: Determine the oxidation state of iron (Fe). x + 6(-1) = -4 x - 6 = -4 x = +2 Step 4: Name the complex. The metal in an anionic complex ends with "-ate". Name: Ammonium hexacyanoferrate(II) Ammonium hexacyanoferrate(II) v. [Cr(NH_3)_6]Br_3 Step 1: Identify the ligand and counter ion. The ligand is ammine (NH_3), which is neutral. The counter ion is bromide (Br^-), which has a -1 charge. Step 2: Determine the charge of the complex cation. Since there are three Br^- ions, the complex cation must have a +3 charge. Step 3: Determine the oxidation state of chromium (Cr). x + 6(0) = +3 x = +3 Step 4: Name the complex cation and anion. Name: Hexaamminechromium(III) bromide Hexaamminechromium(III) bromide vi. [PtCN(ONO)_3(NH_3)_2] Step 1: Identify the ligands and their charges. Cyano (CN^-) has a -1 charge, nitrito-O (ONO^-) has a -1 charge, ammine (NH_3) is neutral. This is a neutral complex.