Stuck again...
"Determine the charge on the complex:
diaquadichloroethylenediaminecobalt(III)"
I'm having problems even writing a formula for this one! Is it [Co(2)(NH2CH2CH2NH2)Cl]Cl ??? Maybe if I could figure out the formula I'd be better at figuring out the charge.
Thank you!
I may not write it in the proper order but the formula is
the diaqua means (H2O)2
dichloro means Cl2
ethylenediamine means (en)
Co(III) means Co^3+.
The only charges are 3+ for Co, 1- each for chloro and that's it. en is neutral. H2O is neutral.
YAY! Thanks, that was a tough one.
Formula didn't matter so much as figuring out the charge. +1 was it! You were a wonderful help, as always!
Well, first let's break down the name of the complex: diaquadichloroethylenediaminecobalt(III).
Diaqua means there are two water ligands, so we have Co(H2O)2.
Dichloro means there are two chloride ligands, so we have CoCl2.
Ethylenediamine is a bidentate ligand, meaning it can bond to the metal in two places. Since it's mentioned once, we have to write it twice: H2NCH2CH2NH2.
Now we can put all the ligands together:
Co(H2O)2Cl2(H2NCH2CH2NH2)2
To determine the charge, we need to consider the oxidation state of cobalt (III). The overall coordination number of the complex is 6 (2 waters, 2 chlorides, and 2 ethylenediamines), which is balanced by the charge on the cobalt ion.
So, the charge on the complex is +3. Now you have it, so you can approach the problem like a real "Co-llector" of complex ions!
To determine the charge on the complex, you need to consider the overall charge of the complex and the charges on its individual ligands and counterions.
The complex you mentioned is diaquadichloroethylenediaminecobalt(III). Let's break it down step-by-step:
1. Start with the central metal atom, which in this case is cobalt (Co).
2. Next, determine the oxidation state of cobalt. The Roman numeral in the name "(III)" tells us that cobalt has an oxidation state of +3.
3. Identify the ligands and their charges in the complex:
- "diaqua" means there are two water (H2O) ligands.
- "dichloro" means there are two chloride (Cl-) ligands.
- "ethylenediamine" refers to the ligand with the formula NH2CH2CH2NH2, which is neutral (has no charge).
4. Determine the overall charge of the complex. Since water and chloride are negatively charged ligands, and ethylenediamine is neutral, the overall charge of the complex depends on the charges of the counterions. In this case, you mentioned there is a chloride counterion (Cl-).
Combining the charges of the ligands and the counterion, we have:
-2 (from two water ligands) + -2 (from two chloride ligands) + -1 (from the chloride counterion) = -5
Therefore, the complex has a charge of -5.
To write the formula for the complex, we write the central metal atom followed by the ligands and counterions in square brackets. Considering the charge of the complex, the formula would be:
[Co(H2O)2Cl2(NH2CH2CH2NH2)]Cl with a charge of -5.
I hope this helps! Let me know if you have any further questions.
To determine the charge on the complex, we need to consider the charges on the ligands and the overall charge of the complex.
The complex is "diaquadichloroethylenediaminecobalt(III)". Let's break down the complex name and analyze it step by step:
1. "diaqua" indicates that there are two water (H2O) molecules coordinated to the central cobalt (Co) atom.
2. "dichloro" suggests that there are two chloride (Cl) ions coordinated to the central cobalt (Co) atom.
3. "ethylenediamine" refers to the organic ligand, which consists of two amine (NH2) groups connected by an ethylene (CH2CH2) bridge.
4. "cobalt(III)" indicates that the central cobalt (Co) ion is in its +3 oxidation state.
Now, let's construct the formula for the complex using this information:
Start with the central cobalt (Co) ion in its +3 oxidation state: Co(III)
Add the ligands one by one:
- Two water (H2O) molecules: Co(III)(H2O)2
- Two chloride (Cl) ions: Co(III)(H2O)2Cl2
- One ethylenediamine ligand: Co(III)(H2O)2Cl2(NH2CH2CH2NH2)
Lastly, let's determine the charge:
To calculate the charge on the complex, we need to consider the overall charge of the complex. This information is usually given in the problem or can be determined based on the oxidation states of the elements.
In this case, we don't have information about the overall charge provided, but we can assume the complex is neutral unless otherwise specified. Therefore, the charge on the complex is 0.
So, the correct formula for the complex is Co(III)(H2O)2Cl2(NH2CH2CH2NH2) with a charge of 0.
It's important to note that the square brackets [] are not typically used in complex formula notation, and we write the ligands directly attached to the central metal ion.