Three elements have the electron configurations 1 s^2 2 s^2...

Three elements have the electron configurations $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$ $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4},$ and $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} .$ The first ionization energies of these elements (not in the same order) are 0.590 $0.999,$ and 0.738 MJ/mol. The atomic radii are $104,160,$ and $197 \mathrm{pm} .$ Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration. Complete the following table with the correct information.

Three elements have the electron configurations $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$ $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4},$ and $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} .$ The first ionization
energies of these elements (not in the same order) are 0.590 $0.999,$ and 0.738 MJ/mol. The atomic radii are $104,160,$ and $197 \mathrm{pm} .$ Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration. Complete the following table with the correct information.

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Key Concepts

Electron Configuration

Electron configuration is the notation that shows the distribution of electrons among the orbitals of an atom. It is fundamental in identifying elements, understanding their position in the periodic table, and predicting their chemical reactivity and properties.

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. This concept is important in understanding how tightly electrons are held by the nucleus, and it exhibits predictable trends across periods and down groups in the periodic table.

Atomic Radius

Atomic radius is a measure of the size of an atom, typically defined as the average distance from the nucleus to the boundary of the surrounding electron cloud. It is influenced by the effective nuclear charge and electron shielding, showing a decrease across a period and an increase down a group.

Periodic Trends

Periodic trends describe the systematic variations in properties such as ionization energy and atomic radius across different elements in the periodic table. These trends arise from the periodic nature of the electron configurations, effective nuclear charge, and electron shielding, and they allow us to make predictions about the behavior of elements.

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