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Understanding Polyatomic Ions and Their Compounds: Classification and Formulas

This comprehensive guide explores polyatomic ions, including chlorate, carbonate, phosphate, ammonium, and more. It details how to identify and describe compounds composed of multiple elements, providing insight into atomic structures and the role of chemical formulas. Readers will learn to distinguish between atomic elements, molecular elements, and ionic compounds. Additionally, practical exercises demonstrate calculating the total number of atoms in compound formulas. Perfect for chemistry students seeking to enhance their understanding of ionic and covalent bonding.

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Understanding Polyatomic Ions and Their Compounds: Classification and Formulas

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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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