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Chapter 3: Problem 80

Of the atoms \(\mathrm{Na}, \mathrm{Mg}\), and \(\mathrm{K}\), which should be the most difficult to ionize? Which has the smallest first ionization energy?

Short Answer

Expert verified
The most difficult element to ionize is Mg, as it has a larger ionization energy compared to Na and K. The smallest first ionization energy belongs to K, as it is lower in the same group as Na.

Step by step solution

01

Identify the atomic numbers and positions of the elements in the periodic table

First, we need to find the atomic numbers for each element and locate their positions in the periodic table: Na (Sodium) - Atomic number 11 Mg (Magnesium) - Atomic number 12 K (Potassium) - Atomic number 19 Now, locate them in the periodic table. Na and K belong to group 1, and Mg belongs to group 2. Na is in period 3, Mg is in period 3, and K is in period 4.
02

Compare the ionization energies based on position in the periodic table

As mentioned earlier, the ionization energy generally increases as we move from left to right across a period and decreases as we go down a group. Since Na and K belong to the same group (group 1), and K is below Na, the ionization energy of K is smaller than Na. Mg belongs to group 2 which is on the right side of Na and K, so its ionization energy should be larger.
03

Determine the most difficult element to ionize and the element with smallest first ionization energy

Based on our comparison, Mg (group 2) should be the most difficult to ionize due to having a larger ionization energy compared to Na and K (group 1). Additionally, K has a smaller first ionization energy than Na because it is lower in the same group. So, the most difficult to ionize is Mg and the smallest first ionization energy belongs to K.

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Most popular questions from this chapter

Write the elemental symbols for nitrogen, silicon, phosphorus, potassium, and gold.

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