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If the IP of Na is 5.48 eV, the ionsatio...

If the IP of Na is 5.48 eV, the ionsation potential of K will be

A

same as that of Na

B

4.4 eV

C

5.68 eV

D

10.88 eV

Text Solution

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The correct Answer is:
To determine the ionization potential (IP) of potassium (K) given the ionization potential of sodium (Na) is 5.48 eV, we can follow these steps: ### Step-by-Step Solution: 1. **Understand Ionization Potential**: Ionization potential (or ionization energy) is the energy required to remove an electron from an isolated gaseous atom. 2. **Identify the Group**: Sodium (Na) and potassium (K) are both alkali metals and belong to Group 1 of the periodic table. 3. **Trends in Ionization Potential**: As we move down a group in the periodic table, the ionization potential generally decreases. This is due to two main factors: - **Increase in Atomic Size**: As we go down the group, the atomic size increases, which means the outermost electron is further from the nucleus. - **Shielding Effect**: The inner electrons shield the outermost electron from the nucleus's positive charge, reducing the effective nuclear charge felt by the outer electron. 4. **Comparison of Ionization Potentials**: Since potassium is below sodium in the periodic table, we expect its ionization potential to be lower than that of sodium. 5. **Evaluate Given Options**: We are given three options for the ionization potential of potassium: - 4.4 eV - 5.68 eV - 10.88 eV Since we established that the ionization potential of potassium should be less than that of sodium (5.48 eV), we can eliminate the options: - 5.68 eV (greater than 5.48 eV) - 10.88 eV (greater than 5.48 eV) This leaves us with 4.4 eV, which is less than 5.48 eV. 6. **Conclusion**: The ionization potential of potassium is 4.4 eV. ### Final Answer: The ionization potential of potassium (K) is **4.4 eV**.
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