For each of the following pairs, indicate which element has...

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) $\mathrm{Ti}, \mathrm{Ba} ;(\mathrm{b}) \mathrm{Ag}, \mathrm{Cu} ;(\mathrm{c}) \mathrm{Ge}$ $\mathrm{Cl} ;$ (d) $\mathrm{Pb},$ Sb. (In each case use electron configuration and effective nuclear charge to explain your answer.)

For each of the following pairs, indicate which element has the smaller first ionization energy: (a) $\mathrm{Ti}, \mathrm{Ba} ;(\mathrm{b}) \mathrm{Ag}, \mathrm{Cu} ;(\mathrm{c}) \mathrm{Ge}$
$\mathrm{Cl} ;$ (d) $\mathrm{Pb},$ Sb. (In each case use electron configuration and effective nuclear charge to explain your answer.)

Key Concepts

First Ionization Energy

This is the energy required to remove the most loosely held electron from a neutral gaseous atom. It serves as an indicator of how strongly an electron is attracted to the nucleus and is influenced by factors such as atomic size, the effective nuclear charge acting on the electron, and the electron’s position in the atom’s electron configuration.

Electron Configuration

Electron configuration describes the arrangement of electrons in an atom’s orbitals. Understanding an atom’s electron configuration enables one to predict its chemical properties, including its ionization energy, as electrons in different orbitals experience varying levels of shielding and effective nuclear charge.

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom, after accounting for the shielding effect of inner electrons. It is a critical concept for explaining trends in ionization energy because a higher effective nuclear charge generally results in a stronger attraction between the nucleus and the electrons, thereby increasing the ionization energy.

Periodic Trends

Periodic trends refer to predictable patterns in element properties, such as ionization energy, across the periodic table. These trends arise from changes in effective nuclear charge, atomic size, and electron shielding as one moves across periods and down groups, and are crucial for comparing the relative ease of electron removal among different elements.

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