Question

24
identify the correct order of increasing first ionization energy. * (0.5 points)
ne < f < he
f< he < ne
he < ne < f
f < ne < he
25
which of the following would you put in box d? * (0.5 points)
s block
p block

Explanation:

Ionization energy is the energy required to remove an electron from an atom. In general, ionization energy increases across a period (from left to right) and decreases down a group. Helium (\(He\)) is in the first period and is a noble gas with a very stable electron configuration (\(1s^{2}\)). Neon (\(Ne\)) is in the second period (\(2s^{2}2p^{6}\)), also a noble gas. Fluorine (\(F\)) is in the second period (\(2s^{2}2p^{5}\)). Since \(F\) is not a noble gas and has one less electron in its valence shell compared to \(Ne\), its ionization energy is lower than \(Ne\). \(He\) has a smaller atomic radius and a more stable electron configuration than \(Ne\), so its ionization energy is higher than \(Ne\).

Answer:

\(F < Ne < He\)