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Chapter 4: Problem 41

Explain why liquid methanol, \(\mathrm{CH}_{3} \mathrm{OH},\) cannot conduct electricity, whereas molten \(\mathrm{NaOH}\) can.

Short Answer

Expert verified
Short Answer: Liquid methanol (CH鈧僌H) cannot conduct electricity because it is a covalent compound with no free ions available to carry an electrical charge. On the other hand, molten NaOH can conduct electricity because it is an ionic compound with free-moving Na鈦� and OH鈦� ions that can carry electrical current when melted.

Step by step solution

01

Understanding the molecular structure of methanol

Methanol, or CH鈧僌H, is a covalent compound where atoms are held together by covalent bonds, meaning that the electrons are shared between the atoms. In methanol, there are no ions present as each atom forms covalent bonds to create a stable molecule.
02

Explaining why methanol cannot conduct electricity

Electricity is conducted through the movement of charged particles called ions. As mentioned in Step 1, methanol does not have any free ions as it is a covalent compound. Since there are no ions available in the liquid methanol to carry electrical charge, it cannot conduct electricity.
03

Understanding the ionic structure of NaOH

Sodium hydroxide, or NaOH, is an ionic compound. In an ionic compound, the atoms are not held together by covalent bonds but rather by forces of attraction between oppositely charged ions. Sodium hydroxide consists of a sodium cation (Na鈦�) and a hydroxide anion (OH鈦�).
04

Explaining the difference between solid NaOH and molten NaOH

In solid-state sodium hydroxide, the Na鈦� and OH鈦� ions are held together in a strong ionic lattice. In this state, the ions are not free to move around and the substance cannot conduct electricity. However, when NaOH is melted, the ionic lattice breaks down, and the ions become free to move around in the liquid.
05

Explaining why molten NaOH can conduct electricity

When NaOH melts, the Na鈦� and OH鈦� ions are free to move within the liquid. These free-moving ions in the liquid are charged particles and can carry electrical current, allowing the molten NaOH to conduct electricity. In conclusion, liquid methanol cannot conduct electricity because it is a covalent compound with no free ions, while molten NaOH contains free-moving ions that can conduct electrical current.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Covalent Compounds
Methanol, or \( \mathrm{CH}_{3} \mathrm{OH} \), serves as a classic example of a covalent compound. In covalent compounds, the atoms within a molecule are connected by covalent bonds. These bonds involve the sharing of electrons between atoms rather than the transfer of electrons, which occurs in ionic bonds.
  • Methanol is composed of carbon, hydrogen, and oxygen atoms sharing electrons to maintain a stable electron configuration.
  • Because the electrons are shared, no charged particles or ions are present in the structure.
This lack of charge carriers is why liquid methanol cannot conduct electricity. Without ions, there is no vehicle to shift electrical charges through the substance, thus making methanol a non-conductor of electricity.
Ionic Compounds
The nature of ionic compounds is fundamentally different from covalent compounds. An excellent example of this is sodium hydroxide (\( \mathrm{NaOH} \)). Ionic compounds are characterized by the presence of positively and negatively charged ions.
  • In \( \mathrm{NaOH} \), the sodium atom (\( \mathrm{Na}^+ \)) loses an electron to become positively charged, while the hydroxide ion (\( \mathrm{OH}^- \)) gains an electron to become negatively charged.
  • This exchange of electrons results in the creation of ionic bonds due to the electrostatic forces of attraction between oppositely charged ions.
In the solid state, the ions in \( \mathrm{NaOH} \) are locked into place within a crystalline structure and do not move freely. However, when \( \mathrm{NaOH} \) is in its molten form, the structure breaks, allowing ions to move freely, making it a good conductor of electricity, in contrast to solid ionic compounds.
Conductivity in Liquids
The ability of a liquid to conduct electricity depends on the presence and mobility of charged particles. This is especially evident when comparing covalent and ionic compounds in their liquid forms.
  • Covalent compounds like methanol lack free ions or charged particles in their liquid state, therefore, they do not conduct electricity.
  • Conversely, ionic compounds such as molten \( \mathrm{NaOH} \) dissociate into free ions in the liquid state, facilitating the conduction of electricity.
In molten ionic compounds, ions are sufficiently dispersed, enabling them to carry an electrical charge through the liquid. As these ions move, they effectively create a pathway for electricity, leading to good electrical conductivity. In summary, the key to understanding electrical conductivity in liquids lies in the presence of mobile charged particles, which are absent in covalent but prevalent in ionic compounds when melted.

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