Examples of stable odd-electron molecules and their structures

🧪 Quick Study Guide

• ⚛️ Odd-electron molecules contain an odd number of valence electrons. This means they cannot satisfy the octet rule for all atoms.
• ⚡ These molecules are often paramagnetic, meaning they are attracted to magnetic fields due to the presence of unpaired electrons.
• 💥 Odd-electron molecules tend to be highly reactive because of their unpaired electron, which seeks to form a bond.
• 🌡️ Stability depends on the specific molecule, but resonance, delocalization, and steric protection can enhance stability.
• 📝 Some examples include:
• $\\cdot NO$ (Nitric oxide)
• $\\cdot ClO_2$ (Chlorine dioxide)
• $\\cdot NO_2$ (Nitrogen dioxide)
• ⚗️ Structures: These molecules often exhibit resonance, leading to delocalization of the unpaired electron. For example, in $NO_2$, the unpaired electron is delocalized over the nitrogen and oxygen atoms.

🧪 Practice Quiz

1. Which of the following is an example of a stable odd-electron molecule?
   1. $N_2O_4$
   2. $O_3$
   3. $NO$
   4. $H_2O$
2. What property is commonly associated with odd-electron molecules due to the presence of unpaired electrons?
   1. Diamagnetism
   2. Paramagnetism
   3. Ferromagnetism
   4. Antiferromagnetism
3. Why are odd-electron molecules generally reactive?
   1. Due to high electronegativity
   2. Due to the presence of lone pairs
   3. Due to their complete octet
   4. Due to the presence of an unpaired electron
4. Which factor can enhance the stability of an odd-electron molecule?
   1. High polarity
   2. Steric hindrance
   3. Limited resonance
   4. Absence of delocalization
5. In $NO_2$, where is the unpaired electron primarily delocalized?
   1. Only on the nitrogen atom
   2. Only on one oxygen atom
   3. Over the nitrogen and oxygen atoms
   4. Only in the space between the atoms
6. Which of the following molecules does *not* have an odd number of valence electrons?
   1. $ClO_2$
   2. $NO$
   3. $O_2$
   4. $NO_2$
7. What is the main reason odd-electron molecules don't satisfy the octet rule?
   1. They always have too many electrons.
   2. They always have too few electrons.
   3. They contain an odd number of valence electrons.
   4. They form ionic bonds instead of covalent bonds.