Use covalent Lewis structures to explain why each element or family of elements occurs as diatomic molecules: a. hydrogen b. the halogens c. oxygen d. nitrogen.

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1. <Hydrogen (H) atoms each have one electron and need one more to achieve a stable electron configuration like helium. By sharing their electrons, two hydrogen atoms form a single covalent bond, resulting in the diatomic molecule H₂.>
2. <Halogens (e.g., F, Cl, Br, I) have seven valence electrons and need one more to complete their octet. By sharing one electron with another halogen atom, they form a single covalent bond, resulting in diatomic molecules like F₂, Cl₂, etc.>
3. <Oxygen (O) atoms have six valence electrons and need two more to complete their octet. By sharing two pairs of electrons, two oxygen atoms form a double covalent bond, resulting in the diatomic molecule O₂.>
4. <Nitrogen (N) atoms have five valence electrons and need three more to complete their octet. By sharing three pairs of electrons, two nitrogen atoms form a triple covalent bond, resulting in the diatomic molecule N₂.>
5. <In each case, the formation of diatomic molecules allows the atoms to achieve a more stable electron configuration, similar to that of the nearest noble gas.>