Gen Chem - Isomers in a complex ion

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Determining if a complex ion has an optical isomer involves assessing whether its mirror image can be superimposed. In the case of [Co(NH3)4F2]+, the arrangement of ligands is crucial. The structure can exhibit cis/trans isomerism due to the positioning of the fluorine ligands, but it may not have optical isomers if it remains symmetrical. The NH3 ligands are typically considered fixed in a specific arrangement in this context. Therefore, the complex primarily displays cis/trans isomerism without optical isomers.
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How can you know if a complex ion has an optical isomer or not? I understand that it's when the mirror image can't be superimposed but am having trouble recognizing it. For example, take
[Co(NH3)4F2]+. Does this have an optical isomer or just cis/trans?
 
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Try to draw it.
 
right, I did that. but I'm not sure if the NH3s are fixed or if they can move around etc.
I have:
NH3
l
NH3 - Co - NH3
l
NH3

And one F coming out of the screen and the other in the back. So I think it has cis/trans, but I'm not sure about optical.

EDIT: the picture isn't coming out right but the metal has 4 NH3 ligands on surrounding it.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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