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Understanding Covalent and Ionic Bonding in Molecular Compounds

This chapter explores the fundamentals of covalent and ionic bonding, explaining how atoms lose or gain electrons to become ions, leading to the formation of cations and anions. It highlights the attractive forces between these ions and how they create crystalline structures in solids. Additionally, it discusses metallic bonds and the "sea of electrons" model, emphasizing characteristics of metals. The chapter also covers the octet rule, molecular formation, and various types of bonds, including single, double, and coordinate bonds.

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Understanding Covalent and Ionic Bonding in Molecular Compounds

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  1. Chapter 8Covalent Bonding Molecular Compounds

  2. Ionic Compounds-Review • atoms that lose or gain electrons become ions • cations have + charge • anions have – charge • cations and anions are attracted to each other by elecrostatic force.

  3. bonds between ions form repeating patterns • can take the form of crystals when solid • usually a metal with a nonmetal • formula units, NOT molecules

  4. Metallic Bonds Review • “sea of electrons” • sharing of electrons between atoms of the same metal (different metals would be alloys) • characteristics of metals are a result of this sharing of electrons • most common in the transition metals (d-block)

  5. Reviewing the Octet Rule • outer electrons (the highest energy level electrons) are called valence electrons. • the most stable valence electron configuration is that of noble gases (8). • every atom will attempt to have its valence electrons conform to noble gas nearest it. • for most elements, this means the atom will have s2 and p6 filled when stable

  6. Molecules

  7. formed by two or more nonmetals • molecules are a neutral group of atoms joined by covalent bonds in order to satisfy the octet rule (there are exceptions to this) • atoms are held together by sharing electrons • diatomic molecules are two of the same atoms covalently bonded

  8. O2

  9. N2

  10. atoms of different elements can covalently bond to form molecular compounds • tend to have lower melting and boiling points than ionic compounds

  11. Water

  12. single covalent bond- share a pair of electrons

  13. often there is a pair of valence electrons that are not shared (unshared pair)

  14. double or triple bonds share two or three pairs of electrons

  15. Coordinate covalent bonds • instead of each atom contributing one electron to be shared, one atom contributes both bonding electrons

  16. Molecular Formulas • shows how many atoms of each element • methane is one carbon and four hydrogen • CH4 • does not tell you about the molecule’s structure (structural formula)

  17. Resonance • refers to the idea that there are two or more valid electron dot formulas for a molecule or ion

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