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

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, $\mathrm{Na}, \mathrm{Cl}$ $\mathrm{Na}, \mathrm{Cl}, \mathrm{K}$

Solution

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: