List all the known chemical elements that have six valence...

List all the known chemical elements that have six valence electrons (and no more). Then, without referring to Tables B or $\mathrm{C}$, circle those elements that commonly give up or share all six of those valence electrons with more electronegative elements to achieve an oxidation number of six. Give the atomic numbers of the next five elements that can be expected to have six valence electrons.

Key Concepts

Periodic Group Trends

Elements in the periodic table are organized into groups based on similar valence electron configurations and chemical properties. Grouping elements by the number of valence electrons, for instance, those with six valence electrons, helps predict trends such as oxidation states, reactivity, and bonding patterns. These trends also serve as a guide for anticipating the properties of heavier elements with similar configurations.

Electronegativity

Electronegativity is a measure of an atom’s ability to attract electrons in a chemical bond. It plays a key role in determining whether an atom will tend to lose, gain, or share electrons when it reacts with other elements. In the context of achieving high oxidation numbers, elements with six valence electrons may interact with more electronegative atoms to fully share or transfer those electrons, allowing the formation of bonds where the central element reaches a high oxidation state.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that participate in chemical bonding. Their number determines the chemical reactivity and bonding behavior of an element. In many cases, having a certain number of valence electrons leads to specific group properties in the periodic table, such as the tendency to lose, gain, or share electrons during interactions with other atoms.

Oxidation Number

The oxidation number (or oxidation state) is a number assigned to an element in a chemical compound that represents the number of electrons lost, gained, or shared in bonding. It is a useful formalism for keeping track of electron transfer in redox reactions and helps in predicting the types of bonds an element might form, particularly how an element reaches a stable electron configuration by giving up or sharing its valence electrons.

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