Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

5. Molecules and Compounds

Polyatomic Ions

Introduction to Chemistry

5. Molecules and Compounds

Polyatomic Ions

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Multiple Choice

Give the systematic name for the following polyatomic ion.
IO₃^–

iodite

hypoiodate

iodide

iodate

periodate

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Verified step by step guidance

Identify the central atom in the polyatomic ion. In this case, it is iodine (I).

Recognize the number of oxygen atoms bonded to the central iodine atom. The formula IO3– indicates there are three oxygen atoms.

Understand the naming convention for polyatomic ions with oxygen. The suffix '-ate' is typically used for the most common or typical oxyanion of an element.

Compare the given options with the standard naming conventions: 'iodite' would imply one less oxygen than 'iodate', 'hypoiodate' would imply even fewer oxygens, and 'iodide' refers to the anion of iodine without oxygen.

Conclude that the systematic name for IO3–, with three oxygens, is 'iodate', as it follows the standard naming convention for the most common oxyanion of iodine.