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.
NO₂^–

nitrate

nitrite

nitrous

pernitrate

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Verified step by step guidance

Identify the chemical formula of the polyatomic ion given in the problem, which is NO2–.

Recognize that NO2– is a polyatomic ion composed of nitrogen and oxygen atoms.

Understand that the naming of polyatomic ions often involves recognizing common patterns or suffixes. In this case, ions with the suffix '-ate' typically have more oxygen atoms than those with the suffix '-ite'.

Recall that NO3– is known as nitrate, which has one more oxygen atom than NO2–. Therefore, NO2– is named nitrite, following the pattern where '-ite' indicates fewer oxygen atoms compared to '-ate'.

Conclude that the systematic name for NO2– is nitrite, based on the established naming conventions for polyatomic ions.