According to increasing ionization energy, which of the sequences is correct?

Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous state.

As we move across a period (from left to right) in the periodic table, the ionization energy generally increases. This is because the atomic size decreases, and the electrons are held more tightly by the increased effective nuclear charge, making it more difficult to remove an electron.

In the given options, the correct sequence is:

• Li (lithium) has the lowest ionization energy among the elements listed.
• Si (silicon) has a higher ionization energy than lithium.
• C (carbon) has a higher ionization energy than silicon.
• F (fluorine) has a higher ionization energy than carbon.
• Ne (neon) has the highest ionization energy among the elements listed.

So, the correct sequence of increasing ionization energy is:

 Li < Si < C < F < Ne.