To determine the ionization energies for the given elements, let's analyze the provided data step-by-step. Here is a detailed breakdown organized into a table format for clarity:
[tex]\[
\begin{array}{|c|c|}
\hline
\text{\textbf{Element}} & \text{\textbf{Ionization Energy (kJ/mole)}} \\
\hline
\text{H} & 1311 \\
\hline
\text{He} & 2370 \\
\hline
\text{Li} & 521 \\
\hline
\text{Be} & 899 \\
\hline
\text{B} & 799 \\
\hline
\text{C} & 1087 \\
\hline
\text{N} & 1404 \\
\hline
\text{O} & 1314 \\
\hline
\text{F} & 1682 \\
\hline
\text{Ne} & 2080 \\
\hline
\text{Na} & 496 \\
\hline
\text{Mg} & 737 \\
\hline
\text{Al} & 576 \\
\hline
\text{Si} & 786 \\
\hline
\text{P} & 1052 \\
\hline
\text{S} & 1000 \\
\hline
\text{Cl} & 1245 \\
\hline
\text{Ar} & 1521 \\
\hline
\text{K} & 419 \\
\hline
\text{Ca} & 590 \\
\hline
\end{array}
\][/tex]
### Explanation of Ionization Energy:
- Ionization energy is the energy required to remove an electron from a gaseous atom or ion.
- Generally, ionization energy increases across a period (left to right on the periodic table) due to increasing nuclear charge.
- It decreases down a group (top to bottom on the periodic table) as the outer electrons are farther from the nucleus and experience more shielding.
### Summary of Ionization Energies:
1. Alkali Metals: Li (521), Na (496), K (419)
- Ionization energies are relatively low as they have one electron in their outermost shell.
2. Noble Gases: He (2370), Ne (2080), Ar (1521)
- High ionization energies due to full valence shells, making them stable and inert.
3. Other Elements:
- Be (899), Mg (737), Ca (590): These are alkaline earth metals with slightly higher ionization energies than alkali metals.
- Transition Metals and Metalloids: Al (576), Si (786)
- Non-Metals: B (799), C (1087), N (1404), O (1314), F (1682), P (1052), S (1000), Cl (1245)
By observing and analyzing the pattern, we can gain insights into periodic trends and electron configurations across different elements.
