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5.2-5.5

5.2-5.5. Polyatomic Ions . Chlorate Carbonate Phosphate Ammonium Acetate Iodate. Nitrate Cyanide Bicarbonate Sulfate Hydroxide . Formulas Describe Compounds. A compound is a distinct substance that is composed of atoms of two or more elements

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5.2-5.5

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  1. 5.2-5.5

  2. Polyatomic Ions • Chlorate • Carbonate • Phosphate • Ammonium • Acetate • Iodate • Nitrate • Cyanide • Bicarbonate • Sulfate • Hydroxide

  3. Formulas Describe Compounds • A compound is a distinct substance that is composed of atoms of two or more elements • Describe the compound by describing the number and type of each atom in the simplest unit of the compound • Molecules or ions • Each element is represented by its letter symbol • The number of atoms of each element is written as a subscript • If there is only one atom, the 1 subscript is not written • Polyatomic groups are placed in parentheses • Polyatomic ions come as packages!!! • If more than one

  4. Practice—Determine the Total Number of Atoms or Ions in One Formula Unit of Each of the Following. • Mg(C2H3O2)2 • (Hg2)3(PO4)2 1 Mg + 4 C + 6 H + 4 O = 15 6 Hg + 2 P + 8 O = 16

  5. Classifying Materials • Atomic elements = Elements whose particles are single atoms • Molecular elements(diatomic)= Elements whose particles are multi-atom molecules • Molecular compounds = Compounds whose particles are molecules made of only nonmetals. • Ionic compounds = Compounds whose particles are cations and anions.

  6. Molecular Elements • Certain elements occur as diatomic molecules. • 7 diatomic elements—The Rule of 7s • The seventh element is H2. • H O N F Cl Br I 7 N2 O2 F2 H2 Cl2 Br2 I2

  7. Molecular Compounds • Two or more nonmetals • Smallest unit is a molecule

  8. Ionic Compounds • Metals + nonmetals • No individual molecule units, instead have a 3-dimensional array of cations and anions made of formula units.

  9. Classify Each of the Following as Either an Atomic Element, Molecular Element, Molecular Compound, or Ionic Compound. • Aluminum, Al • Aluminum chloride, AlCl3 • Chlorine, Cl2 • Acetone, C3H6O • Carbon monoxide, CO • Cobalt, Co

  10. Ionic vs. Covalent Compounds IONIC • Formed from two ions • Consists of a METAL and a nonmetal or polyatomic ion • Formed from two NONMETALS COVALENT

  11. Ionic Compounds • Ionic compounds are made of ions. • Ionic compounds always contain cations and anions • Cations = + charged ions; anions = − charged ions. • The sum of the + charges of the cations must equal the sum of the − charges of the anions • The overall charge of a compound is ZERO!!

  12. Writing Formulas for IONIC Compounds • Write the elemental symbol for each element • Write the charges for each element (How do I figure this out?) • The total charge of all compounds equal ZERO!!!

  13. Example • Magnesium Fluoride • Ammonium Sulfide

  14. Practice—What Are the Formulas for Compounds Made from the Following Ions? • Potassium ion with a nitride ion. • Calcium ion with a bromide ion. • Aluminum ion with a sulfide ion.

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