Question

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. \(\mathrm{CsCl}\) b. \(\mathrm{CH}_{3} \mathrm{OH}\) c. \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\) d. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

Short answer

a. Yes, Cl conducts electricity. b. No, _{3} OH does not conduct electricity well. c. Yes, (O}_{2})_{2} conducts electricity. d. No, _{6} _{12} _{6} does not conduct electricity.

Step-by-step solution

- Understanding Electrolytes

An electrolyte is a compound that dissociates into ions when dissolved in water. These ions allow the solution to conduct electricity. Ionic compounds typically dissociate into their constituent cations and anions, making them good electrolytes. Covalent compounds, on the other hand, do not usually dissociate into ions and are typically non-electrolytes.

- Analyzing ing ing ()

Cesium Chloride (Cl) is an ionic compound that will dissociate into + ions and - ions in water. This dissociation allows the solution to conduct electricity because there are free-moving ions in solution.

- Analyzing _{3} OH

Methanol (_{3} OH) is a molecular compound with covalent bonds. It does not dissociate into ions in solution, thus does not conduct electricity well. It can release a very small amount of ions, so it is a weak electrolyte but is usually considered a nonelectrolyte for practical purposes.

- Analyzing (O}_{2})_{2}

Calcium nitrite ((O}_{2})_{2}) is an ionic compound. It will dissociate into 2+ cations and O_{2} - anions in water. This makes it a good conductor of electricity due to the presence of these mobile ions.

- Analyzing _{6} _{12} _{6}

Glucose (_{6} _{12} _{6}) is a molecular compound with covalent bonds. It does not dissociate into ions when dissolved in water, making it a non-electrolyte. Therefore, a solution of glucose does not conduct electricity.

Key concepts

Ionic and Covalent Compounds

When we dive into the world of chemistry, we encounter various types of compounds, but most notably, ionic and covalent compounds. Ionic compounds are formed through the electrostatic forces between positively and negatively charged ions. In simpler terms, they're like partners in a dance, held together because they're opposites that attract. A classic example is table salt ($NaCl$), where sodium ($Na+$) and chloride ($Cl-$) ions come together.

On the flip side, covalent compounds are all about sharing. Atoms in these compounds share electrons to achieve stability, much like best friends sharing secrets. Water ($H\_2O$) showcases this beautifully with hydrogen and oxygen atoms sharing electrons to make a stable molecule.

Understanding these two types of bonds is key to predicting the behavior of substances in different conditions. For instance, ionic compounds tend to dissolve in water and split into their ions, a property that makes them vital in electrical conductivity. Covalent compounds, however, don't usually break up this way and thereby more often do not conduct electricity when dissolved.

Dissociation of Electrolytes

So, what happens when an ionic compound hits water? It's party time for its ions! This process is called dissociation. Imagine throwing a handful of sugar into a cup of tea; the sugar dissolves and disperses evenly. Similarly, when ionic compounds like Cesium Chloride ($CsCl$) dive into water, they split into cations ($Cs+$) and anions ($Cl-$).

This breaking down is what turns the solution into an electric playground. The newly-freed ions can move around, and it's their movement that carries electrical current through the solution. It's as if they are tiny, charged cars on a superhighway, creating a flow of charge. However, not all compounds are keen to dissociate. Covalent compounds like Methanol ($CH\_\{3\}OH$) mostly stick together, failing to create many charged particles, and hence, they don't conduct electricity well.

Conductivity in Aqueous Solutions

Understanding conductivity in aqueous solutions is like figuring out why some roads are better at handling traffic than others. It's about how well the 'cars' (ions) can move. In a solution where an ionic compound has dissolved, like Calcium nitrite ($Ca(NO\_\{2\})\_\{2\}$), ions ($Ca^\{2+\}$) and ($NO\_\{2\}^\{-\}$) act as express lanes for electric current. Because these ions are free to move, they can carry a charge, making the solution a good conductor.

But just as some roads have restrictions, so do some solutions. Solutions with covalent compounds such as glucose ($C\_\{6\}H\_\{12\}O\_\{6\}$) don't have this kind of ionic movement. That means there's no real path for the current to travel along, making the solution a poor conductor. To sum it up, only when particles are free to move and are electrically charged does a solution conduct electricity effectively. It's the presence or absence of these tiny movers that determines whether turning on a lightbulb in an electrolyte solution is a bright idea or not.