Questions: Arrange the following elements from lower to higher ionization energy. K, Cl, Na Na, K, Cl Cl, K, Na K, Na, Cl Na, Cl, K

Arrange the following elements from lower to higher ionization energy. K, Cl, Na Na, K, Cl Cl, K, Na K, Na, Cl Na, Cl, K
Transcript text: Arrange the following elements from lower to higher ionization energy. $\mathrm{K}, \mathrm{Cl}, \mathrm{Na}$ $\mathrm{Na}, \mathrm{K}, \mathrm{Cl}$ $\mathrm{Cl}, \mathrm{K}, \mathrm{Na}$ K, $\mathrm{Na}, \mathrm{Cl}$ $\mathrm{Na}, \mathrm{Cl}, \mathrm{K}$
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Solution

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Solution Steps

Step 1: Understanding Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. Generally, ionization energy increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table.

Step 2: Locate Elements on the Periodic Table

The elements given are potassium (K), chlorine (Cl), and sodium (Na).

  • Potassium (K) is in Group 1, Period 4.
  • Sodium (Na) is in Group 1, Period 3.
  • Chlorine (Cl) is in Group 17, Period 3.
Step 3: Compare Ionization Energies
  • Sodium (Na) and potassium (K) are both in Group 1, but potassium is below sodium, so potassium has a lower ionization energy than sodium.
  • Chlorine (Cl) is in Group 17 and is to the right of sodium in the same period, so chlorine has a higher ionization energy than sodium.
Step 4: Arrange Elements by Ionization Energy

From the above analysis, the order from lower to higher ionization energy is:

  1. Potassium (K)
  2. Sodium (Na)
  3. Chlorine (Cl)

Final Answer

\(\boxed{\text{K, Na, Cl}}\)

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