Which of the highlighted elements in Figure P7.3: a. forms...

Which of the highlighted elements in Figure P7.3:
a. forms common monatomic ions smaller than the parent atoms? (More than one answer is possible.)
b. has the largest first ionization energy, IE $_{1} ?$
c. has the largest second ionization energy, $1 \mathrm{E}_{2} ?$

Key Concepts

Atomic and Ionic Radii

When atoms lose one or more electrons to form monatomic ions, the balance between nuclear attraction and electron-electron repulsion changes. The loss of electrons, especially those from the outer shell, reduces electron repulsion, often causing the remaining electrons to be drawn closer to the nucleus, which decreases the size of the ion relative to the neutral atom.

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. The first ionization energy pertains to removing one electron from a neutral atom, while the second ionization energy concerns the removal of an electron from an already positively charged ion, often requiring significantly more energy due to the increased effective nuclear charge experienced by the remaining electrons.

Periodic Trends

Periodic trends refer to the systematic variation in atomic properties across periods and down groups on the periodic table. Trends in ionization energy, atomic size, and electron affinity are largely determined by factors such as nuclear charge, electron shielding, and electron configurations, which help predict behaviors such as the ease of forming ions or the energy needed to remove electrons.

Electronic Configuration and Stability

The electronic configuration of an atom or ion determines its chemical stability. Atoms with configurations that yield especially stable arrangements—such as those with filled or half-filled subshells—can exhibit unusually high ionization energies, particularly for removing electrons beyond the first, as the removal disrupts a stable electronic arrangement.

Transcript

Please give Ace some feedback