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Bonding

Bonding. Basics. Ionic. Need to know Valence electrons Octet rule Cations Anions Ionic compounds Obviously, you need both a cation and an anion to create one of these…remember, net charge = 0. Ionic compounds.

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Bonding

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  1. Bonding Basics

  2. Ionic • Need to know • Valence electrons • Octet rule • Cations • Anions • Ionic compounds • Obviously, you need both a cation and an anion to create one of these…remember, net charge = 0.

  3. Ionic compounds • Chemical formula: the kinds and #s of atoms that make up the smallest unit of a substance/cpd. • Formula unit: lowest whole number ratio of the atoms making up a cpd. • Properties: brittle, crystalline solids, generally high melting pts., • Coordination number: # of atoms of opposite charge that surround an ion in the crystal structure • Ionic cpds. will conduct a current

  4. Metallic bonds • Free sea of electrons…this is what allows the ductile and malleable nature to occur. • 202: body-centered, face-centered, hexagonal close packed xl structures. • Alloys: solutions

  5. Molecules and cpds. • Covalent bonds: sharing electrons to satisfy the octet rule. Again, remember, net charge =0. • Diatomic molecule: molecule with 2 atoms. • Diatomic elements: H, N, O, F, Cl, Br, I. • Molecular cpds: lower MP & BP.

  6. Molecular Formulas • How many atoms of each element in a molecule of a given compound

  7. Bonds • Single bond: the sharing of 2 (aka 1 pair) of electrons between 2 atoms. • Double bond: the sharing of 4 (aka 2 pairs) of electrons between 2 atoms. • Triple bond: the sharing of 6 (aka 3 pairs) of electrons between 2 atoms. • No, no quadruple bonds…sorry. 

  8. More on bonds • Sigma and pi bond discussion: 230-231 • VSEPR: valence shell electron pair repulsion theory: orbitals hybridize as needed for capacity for electrons. 232-236

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