Question
Rank the following ions in order of increasing electrical conductivity in aqueous solution.Na+, Rb+, Cs+,Li+, K+
Answers
Answered by
GPT-4o mini
The electrical conductivity of ions in aqueous solution is influenced by several factors, including the size of the ion and its mobility in water. Generally, larger cations have higher mobility because they can move through the solution more easily, which increases their contribution to electrical conductivity.
In the case of the alkali metal cations you listed, the order of ionic radius (and hence general mobility) is as follows, from smallest to largest:
1. Li⁺ (lithium)
2. Na⁺ (sodium)
3. K⁺ (potassium)
4. Rb⁺ (rubidium)
5. Cs⁺ (cesium)
Given that larger ions tend to be more conductive due to their higher mobility in solution, you can rank the cations in order of increasing electrical conductivity as follows:
**Li⁺ < Na⁺ < K⁺ < Rb⁺ < Cs⁺**
So, the correct order from lowest to highest conductivity is:
**Li⁺ < Na⁺ < K⁺ < Rb⁺ < Cs⁺**.
In the case of the alkali metal cations you listed, the order of ionic radius (and hence general mobility) is as follows, from smallest to largest:
1. Li⁺ (lithium)
2. Na⁺ (sodium)
3. K⁺ (potassium)
4. Rb⁺ (rubidium)
5. Cs⁺ (cesium)
Given that larger ions tend to be more conductive due to their higher mobility in solution, you can rank the cations in order of increasing electrical conductivity as follows:
**Li⁺ < Na⁺ < K⁺ < Rb⁺ < Cs⁺**
So, the correct order from lowest to highest conductivity is:
**Li⁺ < Na⁺ < K⁺ < Rb⁺ < Cs⁺**.
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