Week 9 Achieve 6
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Re: Week 9 Achieve 6
To solve this, find the charge of each of the ligands and anions (everything except the metal species). Since the overall charge of the complex is 0, you can figure out the charge that will make everything add up to 0.
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Re: Week 9 Achieve 6
NH3 has a charge of 0, the two Chlorines have a combined charge of -2, therefore Cobalt has a charge of +2 to create a neutral coordination compound.
Re: Week 9 Achieve 6
You must first find the hypothetical charges (oxidation states) of all of the other components in the coordination compound. NH3 has no charge (oxidation state=0), and the 2 Cl each have an oxidation state of -1. Therefore 2 times -1= -2. Since the compound is a neutral compound (the overall charge is 0), the metal ion, cobalt, must have an oxidation state of +2.
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Re: Week 9 Achieve 6
You know that NH3, ammonia, is neutrally charged so that has to be 0. Moreover, you know Chlorine has an oxidation state of -1. With the knowledge that the complex is neutrally charged, you can then work backwards to solve for Cobalt's oxidation state.
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Re: Week 9 Achieve 6
Hi Amanda, since the coordination compound is neutral and has no net charge, we know that the sum of the charges of all the components in the compound must equal to zero. We know that NH3 has a net charge of 0, both Cl's have a net charge of -1, totaling to -2. Therefore, we know that Co must have a charge of +2 to give us an overall net charge of 0. So Co, the metal species, would have an oxidation state of +2. Hope this helps!
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Re: Week 9 Achieve 6
NH3 is neutral, and Cl has an oxidation number of -1. Since the compound is neutral and bonded to 2 chlorine anions, each with an oxidation number of -1, the complex should have a +2 charge. If the Cl has an oxidation number of -1, the metal species must have an oxidation number of +3 to compensate.
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