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Hydrogen Bonds –

Hydrogen Bonds – attraction between MOLECULES (NOT ATOMS!) that are both polar covalently bonded. weakest of all chemical bonds Very important for LIFE. Responsible for unique properties of: Water Structure of proteins Shape of DNA. * Refer to Hydrogen handout*. -. +.

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Hydrogen Bonds –

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  1. Hydrogen Bonds – • attraction between MOLECULES (NOT ATOMS!) that are both polar covalently bonded. • weakest of all chemical bonds • Very important for LIFE. • Responsible for unique properties of: • Water • Structure of proteins • Shape of DNA

  2. * Refer to Hydrogen handout* - +

  3. 4. Polyatomic ions – • Covalently bonded atoms that have either lost or gained electrons • generally contain one or more elements combined with oxygen • most end in suffix -ate or –ite • most compound we use such as baking soda, soaps, cleaners • in formulas they are often shown in parenthesis to remind that they act as single ion • Ex: Ammonium sulfate (NH4)2SO4

  4. D. Chemical Reactions – process by which chemical changes occur 1. Parts: “yields” Reactants Products

  5. 2. Balancing Equations Account for the Conservation of Mass! atoms on each side of equation must match in number Cannot change the formulas – must leave the subscripts alone! Only can place numbers (coefficients) in front of the formulas Coefficients of 1 are assumed and do not appear in balanced equation. when done, CHECK each element to verify

  6. Ex: ____ P4 + ____ Br2 ____ PBr3 _1__ P4 + _6__ Br2_4__ PBr3

  7. Ex: ____ Mn + ____ HI  ____ H2 + ____ MnI3 2 Mn + 6 HI 3 H2 + 2 MnI3

  8. Ex: ____ HBr + ____ Mg(OH)2 ____ MgBr2 + ____ H2O 2 HBr + 1 Mg(OH)21 MgBr2 + 2 H2O

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