Is this the correct formula for dichlorotetramminechromium (III) nitrate?
(CrCl2(NH3)4 NO3)
[Cr(NH3)4Cl2]NO3
Yes, the formula you provided is correct for dichlorotetramminechromium (III) nitrate.
To determine if the given formula is correct for dichlorotetramminechromium (III) nitrate, we need to check the valence and charge of each element in the compound.
Let's break down the formula into its individual components:
1. CrCl2(NH3)4: This part of the formula represents the coordination complex of the chromium (III) ion with two chloride ions and four ammonia ligands.
The oxidation state of chromium (Cr) in this complex is +3 since "chromium (III)" is mentioned in the name. The chloride ions (Cl) have a -1 charge each. The ammonia ligands (NH3) are neutral.
2. NO3: This is the nitrate ion. It consists of one nitrogen atom (N) and three oxygen atoms (O). The nitrate ion has a -1 charge.
To determine the overall charge of the compound, we need to consider the charges of each component and their respective quantities:
Chromium (Cr) has a +3 charge (from "chromium (III)").
Chloride ions (Cl) each have a -1 charge.
Ammonia ligands (NH3) are neutral.
Nitrate (NO3) has a -1 charge.
Based on this information, let's take a closer look at the formula:
(CrCl2(NH3)4 NO3)
Since we have two chloride ions (Cl) and four ammonia ligands (NH3), the overall charge from these ligands is 2(-1) + 4(0) = -2.
Adding up the charges: +3 - 2 - 1 = 0
The overall charge of the compound is neutral, which is expected for a compound. Thus, the given formula (CrCl2(NH3)4 NO3) is correct for dichlorotetramminechromium (III) nitrate.