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How To Name Chemical Formulas

How To Name Chemical Formulas. Supplemental to Chapter 20. Rules for Naming Binary Compounds. Binary Compounds are ionic bonds between one metal (+) and one nonmetal (-). When you name binary ionic compounds, you always mention the cation ( + ion) first (usually the metal).

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How To Name Chemical Formulas

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  1. How To Name Chemical Formulas Supplemental to Chapter 20

  2. Rules for Naming Binary Compounds Binary Compounds are ionic bonds between one metal (+) and one nonmetal (-). When you name binary ionic compounds, you always mention the cation (+ ion) first (usually the metal). When you name the second ion (the – anion), you will change the ending to “ide”

  3. Common Binary Anions Oxygen oxide Phosphorus phosphide Nitrogen nitride Sulfur sulfide Chlorine chloride

  4. Name These Binary Compounds RbCl = NaF = CuO = AlN= K2S = NaCl =

  5. Name These Binary Compounds RbCl = Rubidium Chloride NaF = Sodium Fluoride CuO = Copper Oxide AlN= Aluminum Nitride K2S = Potassium Sulfide NaCl = Sodium Chloride

  6. Polyatomic Ions Polyatomic ions are a group of ions (2+ elements) that are covalently bonded together. • You would say the first element as is. • You would then say the rest of the bonded polyatomic ions after the first element, using their specific endings.

  7. Polyatomic Ion Endings Ammonium NH4 Acetate C2H3O2 Chlorate ClO3 Hydroxide OH Nitrate NO3 Carbonate CO3 Sulfite SO3 Sulfate SO4 Phosphate PO4 Peroxide O2

  8. Oxygen vs Peroxide Normally an Oxygen molecule by itself is O2. However, if it is in a polyatomic bond, the O2 becomes peroxide. O2 = oxygen, Na2O2 = sodium peroxide Remember the difference between the chemical formulas for water and hydrogen peroxide: water = H2O; hydrogen peroxide = H2O2

  9. Rules for Polyatomic Ions • You have to memorize the chart, including SO3(Sulfite) and O2 (Peroxide). Remember, O2 is peroxide only when used as a polyatomic ion. Otherwise it is oxygen (oxide.)

  10. Naming Polyatomic Ions HSO4 - NaNO3 - Ba(OH)2 - KNO3 - CaCO3 - CuSO3 – CaSO4 – (notice the different endings of the last two polyatomic ions.)

  11. Naming Polyatomic Ions HSO4 - Hydrogen Sulfate NaNO3 - Sodium Nitrate Ba(OH)2 - Barium hydroxide KNO3 - potassium nitrate CaCO3 - calcium carbonate CuSO3 – copper sulfite CaSO4 – calcium sulfate H2O2 – hydrogen peroxide

  12. Prefixes for Covalent Compounds The prefixes indicate how many atoms of each element are in a binary covalent compound. These occur when 2 nonmetals covalently bond.

  13. Prefixes for Covalent Compounds Mono = 1 Di = 2 Tri = 3 Tetra = 4 Penta = 5 Hexa = 6 Hepta = 7 Octa = 8

  14. How to Say Covalent Compounds P2O5 - this is named diphosphorus pentoxide, because there are two phosphorus atoms and five oxygen atoms.  CO - this is carbon monoxide (you need the "mono-" because there's only one oxygen atom).CF4 - this is carbon tetrafluoride

  15. The Covalent Bond of Water • Water is a covalent bond (2 Hydrogen atoms share the 6 Oxygen valence electrons of one atom) H2O Dihydrogen monoxide This is a chemical formula you should know.

  16. Naming Covalent Bonds Rules • Use specific prefixes to indicate the total number of atoms involved. • Don’t write 2 vowels together unless it is dioxide. (CO2 = carbon dioxide) • If there is only one atom for both elements, you don’t write the “mono” for the first element, but you do for the 2nd element. Examples: CO = carbon monoxide

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