Listed below are two atomic properties of the element...

Listed below are two atomic properties of the element germanium. Refer only to the periodic table on the inside front cover and indicate probable values for each of the following elements, expressed as greater than, about equal to, or less than the value for Ge. $$\begin{array}{lcc} \hline \text { Element } & \text { Atomic Radius } & \begin{array}{c} \text { First lonization } \\ \text { Energy } \end{array} \\ \hline \mathrm{Ge} & 122 \mathrm{pm} & 762 \mathrm{kJ} / \mathrm{mol} \\ \mathrm{Al} & ? & ? \\ \mathrm{In} & ? & ? \\ \mathrm{Se} & ? & ? \\ \hline \end{array}$$

Listed below are two atomic properties of the element germanium. Refer only to the periodic table on the inside front cover and indicate probable values for each of the following elements, expressed as greater than, about equal to, or less than the value for Ge.
$$\begin{array}{lcc}
\hline \text { Element } & \text { Atomic Radius } & \begin{array}{c}
\text { First lonization } \\
\text { Energy }
\end{array} \\
\hline \mathrm{Ge} & 122 \mathrm{pm} & 762 \mathrm{kJ} / \mathrm{mol} \\
\mathrm{Al} & ? & ? \\
\mathrm{In} & ? & ? \\
\mathrm{Se} & ? & ? \\
\hline
\end{array}$$

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Key Concepts

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom, after accounting for electron shielding. It plays a crucial role in periodic trends, influencing both the atomic radius and ionization energy as its increase leads to a stronger pull on electrons, resulting in a smaller radius and higher ionization energy.

First Ionization Energy

First ionization energy is the energy required to remove the outermost electron from a neutral atom. This property generally increases across a period because of a higher effective nuclear charge and decreases down a group as the electron being removed is farther from the nucleus and more shielded by inner electrons.

Atomic Radius

Atomic radius is defined as the distance from the nucleus to the boundary of the surrounding cloud of electrons. The trend typically shows a decrease in atomic radius across a period as effective nuclear charge increases and an increase down a group due to the addition of electron shells.

Periodic Trends

Periodic trends describe how certain properties such as atomic radius and ionization energy change predictably across periods and down groups on the periodic table. These trends are driven by variations in parameters like nuclear charge, electron shielding, and electron configuration.

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