What Are Common Mistakes in Naming Complex Ions?

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SUMMARY

The discussion centers on the correct naming conventions for complex ions, specifically addressing the example of [HgCl4]2-. The established rules include naming negative ligands first, followed by neutral ligands, and concluding with the central ion, which is indicated with Roman numerals for oxidation states. The suffix "-ate" is applied to negatively charged complex ions. The provided answer, "tetrachloromercurate(II)," is confirmed as correct.

PREREQUISITES
  • Understanding of complex ion nomenclature rules
  • Familiarity with ligands and their classifications
  • Knowledge of oxidation states and Roman numeral representation
  • Basic chemistry concepts related to coordination compounds
NEXT STEPS
  • Study the IUPAC naming conventions for coordination compounds
  • Learn about different types of ligands and their properties
  • Explore examples of complex ions with varying charges and their names
  • Review the role of oxidation states in naming complex ions
USEFUL FOR

Chemistry students, educators, and anyone involved in the study of coordination chemistry and complex ion nomenclature.

skander
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Homework Statement


I'm having trouble with naming complex ions. My textbook has given me a few rules but the examples they give seem to contradict them. These are all the rules I know, can someone tell me if they are right and if I am missing any?


Homework Equations


Start naming with negative ligands then neutral and then the central ion using roman numerals such as di, tri, tetra, penta, and hexa.
Write in parantheses the oxidation of the central ion.
If the complex ion is negatively charged add the suffix -ate.


The Attempt at a Solution



So [HgCl4]2- should be tetrachloromercurate(II)

Is this answer and the equations correct? Thanks.
 
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