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Bonds

  • Ionic bonds

    • Metal + Nonmetal

    • If the difference between 2 atoms electronegativity is >2.0 , higher electronegativity atom steals electron from lower electronegativity atom

    • Particles of opposite charge (+ and -) have electrostatic attraction and forms ionic bond

  • Covalent bonds

    • Nonmetal + Nonmetal

    • Difference in electronegativity <1.7, share electrons

    • Polar vs. Nonpolar

      • Polar covalent bond - difference in electronegativity > 0.5 - electrons skew towards one atom

      • Nonpolar covalent bond - difference in electronegativity <0.5

  • <0.5 - Nonpolar Covalent

  • 0.5 to 1.7 - Polar Covalent Bond

  • >2.0 - Ionic Bond

Valence Electrons and Lewis Structures

  • Valence electrons count valence electrons by each dot

  • Fill each side of letter up before pairing

  • Covalent bonds represented by a line

  • Formal Charge

    • Occurs if the # of electrons an atom contributes to the structure is different from typical valence (ion)

Octet Rule and Exceptions

  • Allows us to predict how atoms will form chemical bonds

  • 8 valence electrons = octet

  • Many exceptions

Molecular & Electron Geometries and Bond Angles

  • VSEPR - Valence Shell Electron Pair Repulsion

  • Electron clouds repel eachother, therefore molecules automatically adopt a geometry so atoms can be as far away as possible

  • Hybridized orbitals

  • number of electron domains → hybridization of central atom → electron domain geometry

  • Lone pairs connected to central atom count as electron domains but don’t take up much space - Angles represent a higher amount of atoms but there are less (H2O)

Acids

  • All acids start with H

  • Binary acids: HYDROGEN + NONMETAL ELEMENT

  • Oxyacids: HYDROGEN + OXYGEN + ONE OTHER ELEMENT

    • Hydrogen bonded to oxygen

  • Naming: Hydro + Stem + -ic acid

  • Ionic compounds with oxygen added

    • ate ending - ic acid

    • ite ending - ous acid

    • hypo - ite ending becomes hypo - ous acid

    • per - ate ending becomes per - ic acid

Ionic Compounds

  • H+ PO 3- 4 → H3 PO4

  • H+, H+