Module Figures: Periodic Table IV • Visionlearning

Figure 1: Metals (blue), metalloids (green), and nonmetals (red) are shown grouped on the periodic table.

Figure 3: The alkali metals occupy the first column on the left. The one exception is hydrogen, which is not an alkali metal and is the only element located outside its chemical family on the periodic table.

While the alkali metals differ from one another in their overall electron configuration, they have a similar valence electron configuration, which means they have similar reactivity. Consider lithium, sodium, and cesium as examples:

Li = {1s}^{2} {2s}^{1}

Na = {1s}^{2} {2s}^{2} {2p}^{6} {3s}^{1}

Cs = {1s}^{2} {2s}^{2} {2p}^{6} {3s}^{2} {3p}^{6} {3d}^{10} {4s}^{2} {4p}^{6} {4d}^{10} {5s}^{2} {5p}^{6} {6s}^{1}

The configurations shown above tell us that even though they have different numbers of electrons, all three have one valence electron (indicated in red). And for each, that valence electron occupies an s-type subshell. Refer to our Periodic Table III module for details regarding subshells. But in summary, subshells help describe an atom’s electron configuration. Subshells consist of electron orbitals – regions around a nucleus where you’re most likely to find electrons. Besides s-orbitals, there’s also p, d, and more.

Figure 4: The halogens occupy column 17, the second-from-right column of the periodic table.

Figure 5: The alkaline earth metals occupy column 2 on the periodic table.

Figure 7: The transition metals occupy the center of a periodic table and are the biggest chemical family.

Figure 9: Post-transition metals lie to the left of the metalloids.

Figure 12: Reactive nonmetals cluster in the upper-right of the periodic table, with one exception, hydrogen, which resides on the upper-left.

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Figure 12: Reactive nonmetals cluster in the upper-right of the periodic table, with one exception, hydrogen, which resides on the upper-left.

Figure 14: The noble gases occupy the right-hand column of the periodic table.

Figure 15: The lanthanides and actinides usually lie in the space below the rest of the periodic table.

Figure 16: Though the extended periodic table presentation is rarely shown, it accurately displays the placement of the actinides and lanthanides with the rest of the periodic table.