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Understanding Binary Molecular Compounds and Covalent Bonding

Binary molecular compounds consist of two nonmetal elements bonded by covalent bonds, where electrons are shared to achieve stable octets. Diatomic molecules, such as N2 and O2, play a vital role in this category. Unlike ionic compounds, molecular compounds have no charge. Drawing Lewis structures helps visualize electron sharing, showing single, double, and triple bonds through lines and dots. Structures can also represent resonance and, in some cases, expanded octets. Common examples include H2, H2O, NH3, CO2, and SF6.

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Understanding Binary Molecular Compounds and Covalent Bonding

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  1. Binary Molecular (Covalent) Compounds

  2. Molecule: a neutral group of elements joined by a covalent compound • Diatomic Molecule: A molecule consisting of two atoms • Diatomic Elements: (7 of them, form a 7 on the PT) and they end in –ine or gen (N, O, F, Cl, Br, I, H)

  3. Molecular compound: Compound composed of molecules 1. Binary molecular compounds are made up of 2 elements • Typically these elements are nonmetals • There are no charges in a molecular compound • Molecular compounds are held together by covalent bonds

  4. A covalent bond is a sharing of electrons so that each element forms an octet • We can show the sharing of e- by drawing Lewis structures (dot diagrams) • The first rule for drawing a molecular Lewis structure is to get the formula

  5. Next, count the number of electrons • Each bond that is formed requires 2 electrons • We can show a single bond with 2 electrons or with 1 line • We can show a double bond with 4 e- or with 2 lines • We can show a triple bond with 6 e- or with three lines

  6. Valence electrons that are shared b/w 2 elements are called bonding electrons • Valence e- that are not shared b/w 2 elements are called lone pair electrons • In the end, each element should always have/share 8 e-, except for H b/c this element can only have 2 e-

  7. H2 • H2O • NH3

  8. CO2 • N2 • HCN • SO3

  9. 16. A resonance structure is a structure that occurs when two or more valid electron dot structures are able to be drawn. • An arrow indicates multiple resonance structures. See page 224 in book

  10. Examples: • SO3 • O3

  11. Some elements form “expanded octets: in which more than 8 electrons can be had. Phosphorus and sulfur do this a lot! ex: SF6 and PCl5

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