Explain the relationship between a main-group element’s lettered group number (the number of the element’s column) and its valence electrons. The lettered group number of a main-group element is equal to the number of valence electrons for that element.

Group 0 contains non-metal elements placed in the vertical column on the far right of the periodic table . The elements in group 0 are called the noble gases . They exist as single atoms .

The number of valance electrons is equal to the group number of the representative elements. The relation between the group number and valance electrons is that “group number is equal to the number of valance electrons”.

For representative elements the number of valence electrons is the same as the periodic group number, and the number needed to match the next noble-gas configuration is 8 minus the group number.

Group 8 elements do not react and so have a valency of 0 .

Group number and valency has no relation in group 0 (or Group 18) since the elements in group 0 are noble gases. They are inert and thus do not form compounds easily.

The s-block elements share electron configurations. s-block elements are the elements found in Group 1 and Group 2 on the periodic table. Because they have 2 valence electrons they are less reactive than group 1. Hydrogen is a nonmetal grouped with the alkali metals because it has one electron in its valence shell.

element scandium

Groups 3–12 contain transition metals. They are less reactive than metals in groups 1 and 2. Groups 13–16 each contain at least one metalloid.

Group 18 of the periodic table contains the noble gases. These are the elements in the 18th column of the periodic table, at the far right. They are all nonmetals, and are found in their standard state as monatomic gases. Noble gases are relatively inert and nonreactive due to their full outer shell of electrons.

Noble gas, any of the seven chemical elements that make up Group 18 (VIIIa) of the periodic table. The elements are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), radon (Rn), and oganesson (Og).

The noble gases (Group 18) are located in the far right of the periodic table and were previously referred to as the “inert gases” due to the fact that their filled valence shells (octets) make them extremely nonreactive. The noble gases were characterized relatively late compared to other element groups.