Question

Knowing the names of similar chlorine oxyanions and acids, deduce the names of the following: \(\mathrm{IO}^{-}, \mathrm{IO}_{2}^{-}, \mathrm{IO}_{3}^{-}, \mathrm{IO}_{4}^{-}$$\mathrm{HIO}, \mathrm{HIO}_{2}, \mathrm{HIO}_{3}, \mathrm{HIO}_{4}\)

Short answer

The names of the given iodine oxyanions and acids are as follows: - \(\mathrm{IO}^{-}\): hypoiodite, \(\mathrm{HIO}\): hypoiodous acid - \(\mathrm{IO}_{2}^{-}\): iodite, \(\mathrm{HIO}_{2}\): iodus acid - \(\mathrm{IO}_{3}^{-}\): iodate, \(\mathrm{HIO}_{3}\): iodic acid - \(\mathrm{IO}_{4}^{-}\): periodate, \(\mathrm{HIO}_{4}\): periodic acid

Step-by-step solution

Review chlorine oxyanions and acids names

Referring back to the chlorine oxyanions and acids names, we have: - \(\mathrm{ClO}^{-}\): hypochlorite, \(\mathrm{HClO}\): hypochlorous acid - \(\mathrm{ClO}_{2}^{-}\): chlorite, \(\mathrm{HClO}_{2}\): chlorous acid - \(\mathrm{ClO}_{3}^{-}\): chlorate, \(\mathrm{HClO}_{3}\): chloric acid - \(\mathrm{ClO}_{4}^{-}\): perchlorate, \(\mathrm{HClO}_{4}\): perchloric acid Considering these names, we can deduce the naming pattern for iodine oxyanions and acids accordingly.

Name iodine oxyanions

Following the naming convention for chlorine oxyanions, we can deduce the names of iodine oxyanions: - \(\mathrm{IO}^{-}\): hypoiodite - \(\mathrm{IO}_{2}^{-}\): iodite - \(\mathrm{IO}_{3}^{-}\): iodate - \(\mathrm{IO}_{4}^{-}\): periodate

Name iodine oxyacids

Similarly, we can now deduce the names of the iodine oxyacids using the convention from the chlorine oxyacids: - \(\mathrm{HIO}\): hypoiodous acid - \(\mathrm{HIO}_{2}\): iodus acid - \(\mathrm{HIO}_{3}\): iodic acid - \(\mathrm{HIO}_{4}\): periodic acid So, the names of the given iodine oxyanions and acids are as follows: - \(\mathrm{IO}^{-}\): hypoiodite, \(\mathrm{HIO}\): hypoiodous acid - \(\mathrm{IO}_{2}^{-}\): iodite, \(\mathrm{HIO}_{2}\): iodus acid - \(\mathrm{IO}_{3}^{-}\): iodate, \(\mathrm{HIO}_{3}\): iodic acid - \(\mathrm{IO}_{4}^{-}\): periodate, \(\mathrm{HIO}_{4}\): periodic acid

Key concepts

Naming Conventions

When discussing the naming conventions for iodine oxyanions and acids, it helps to understand the step-by-step patterns observed in similar compounds such as chlorine oxyanions. Generally, the names of these compounds are systematically built upon their composition and the oxygens bonded to a central halogen atom like iodine.
For instance, when there is only one oxygen as in \( \mathrm{IO}^{-} \), the prefix 'hypo-' is used, resulting in the name hypoiodite for the anion. Correspondingly, its acid form \( \mathrm{HIO} \) is named hypoiodous acid.
For two oxygens like in \( \mathrm{IO}_{2}^{-} \), the suffix '-ite' is used, leading to the name iodite. The acid form follows the same suit and is called iodus acid, though it’s worth noting that 'iodous' is less commonly used than the others.
When the compound contains three oxygens as seen in \( \mathrm{IO}_{3}^{-} \), the suffix changes to '-ate', thus iodate, and for its acid, iodic acid. With four oxygens \( \mathrm{IO}_{4}^{-} \), the prefix 'per-' and the suffix '-ate' are used to form periodate, and correspondingly, periodic acid for the acid form.
Understanding these conventions makes it easier to deduce or remember the names of these compounds just by looking at their formulas.

Chemical Nomenclature

Chemical nomenclature refers to the system of naming chemical compounds in a standardized way so everyone can understand what specific compounds are being referred to. It's like the language of chemistry, allowing for clear communication among scientists and students alike.
The IUPAC has official guidelines and rules that dictate how each element and compound should be named, considering their structure, function, and bonding. For iodine oxyanions and acids, the IUPAC rules align closely with those used for chlorine oxyanions, reflecting the similarity in their chemical structures.

• The fundamental rule is that anions containing more oxygen atoms use the suffix '-ate', while those with fewer use '-ite.'
• When prefixes are included, like 'hypo-' and 'per-', they indicate less or more oxygen, respectively, than the '-ite' and '-ate' forms. Worked perfectly when naming iodine oxyanions, drawing parallels with chlorine compounds.

The structured nature of chemical nomenclature ensures that when you come across compounds like \( \mathrm{IO}_{3}^{-} \) (iodate) or \( \mathrm{HIO}_{4} \) (periodic acid), you're equipped to understand their composition and even predict their properties based on their names.

Chlorine Oxyanions Comparison

Comparing iodine oxyanions to chlorine oxyanions can be incredibly insightful because they follow similar naming patterns and chemical behavior. Both sets of oxyanions belong to the group of halogens in the periodic table and thus share similarities in how they combine with oxygen.
In the case of chlorine, the sequence from chloride to perchlorate includes:

• \( \mathrm{ClO}^{-} \): hypochlorite
• \( \mathrm{ClO}_{2}^{-} \): chlorite
• \( \mathrm{ClO}_{3}^{-} \): chlorate
• \( \mathrm{ClO}_{4}^{-} \): perchlorate

Similarly, iodine's oxyanion sequence goes from hypoiodite to periodate, mirroring the step-up in oxygen count and thus naming convention.
The parallels arise because, for each additional oxygen, both iodine and chlorine's oxyanions adopt a systematic change in their names that reflect their increased oxidation states. This similar behavior is what makes the direct comparison not just possible, but exceedingly useful in predicting names and understanding reactivity patterns of these compounds in chemical reactions.
By studying the similarities and differences, students can deepen their understanding of periodic trends and the concept of oxyanions, leveraging these patterns to master both iodine and chlorine chemistry.