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Nomenclature

Nomenclature. Chapter 2. molecular. empirical. H 2 O. Chemical Formula. Molecular formula: Shows the exact number of atoms of each element in the smallest unit of a substance Empirical formula: Shows the simplest whole number ratio of the atoms in a substance. H 2 O. CH 2 O.

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Nomenclature

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  1. Nomenclature Chapter 2

  2. molecular empirical H2O Chemical Formula • Molecular formula: • Shows the exact number of atoms of each element in the smallest unit of a substance • Empirical formula: • Shows the simplest whole number ratio of the atoms in a substance H2O CH2O C6H12O6 O3 O N2H4 NH2

  3. DIATOMIC ELEMENTS Some elements do not like to be alone… so they bond to themselves! 7 HOFBrINCl

  4. Ionic Compounds • consist of a combination of cationsand anions formed from a transfer of electrons • the formula is always the same as the empirical formula • the sum of the charges on the cation(s) and anion(s) in each formula unit must equal zero The ionic compound NaCl

  5. 2 x +3 = +6 1 x +2 = +2 1 x +2 = +2 3 x -2 = -6 2 x -1 = -2 1 x -2 = -2 Formula of Ionic Compounds Al2O3 Al3+ O2- CaBr2 Ca2+ Br- Na2CO3 Na+ CO32-

  6. NAMING COMPOUNDS RULE 1 Metal – Nonmetal • Write the metal (positive ion) first • Change the ending of the second word to -ide

  7. Rule 1 Examples Potassium Bromide Calcium Bromide Lithium Fluoride Lithium Oxide Magnesium Oxide Barium Sulfide Potassium Phosphide Sodium Nitride • KBr • CaBr2 • LiF • Li2O • MgO • BaS • K3P • Na3N

  8. NAMING COMPOUNDS RULE 2 Polyatomic Ions • DO NOT CHANGE ANYTHING! • When you have NH4, change the second word to -ide

  9. Rule 2 Examples Barium Sulfate Barium Sulfite Sodium Carbonate Sodium Bicarbonate Ammonium Phosphate Ammonium Hydroxide • Ba(SO4) • Ba(SO3) • Na2(CO3) • Na(HCO3) • (NH4)3(PO4) • (NH4)(OH)

  10. NAMING COMPOUNDS RULE 3 Transition Metals • Can have more than one type of charge • Write the charge number in roman numerals

  11. Rule 3 Examples Copper (I) Oxide Copper (II) Oxide Iron (II) Chloride Iron (III) Chloride Tin (IV) Chloride Manganese (III) Oxide Lead (II) Sulfide • Cu2O • CuO • FeCl2 • FeCl3 • SnCl4 • Mn2O3 • PbS

  12. Molecular Compounds • Consists of nonmetals covalently bonded • nonmetals or nonmetals + metalloids • element further left in periodic table is 1st • element closest to bottom of group is 1st

  13. TOXIC! Laughing Gas NAMING COMPOUNDS RULE 4 Nonmetal – Nonmetal USE PREFIXES! • Change the ending of the second word to -ide • No mono on the first word • Drop any double vowels NO2 nitrogen dioxide N2O dinitrogen monoxide

  14. Rule 4 Examples Carbon Monoxide Carbon Dioxide Sulfur Dioxide Sulfur Trioxide DinitrogenTetrahydride Dinitrogen Trioxide Phosphorus Trichloride Silicon Dioxide DiphosphorusPentoxide Carbon Disulfide Aluminum Oxide • CO • CO2 • SO2 • SO3 • N2H4 • N2O3 • PCl3 • SiO2 • P2O5 • CS2 • Al2O3

  15. Acids • acid: is a type of molecular compound • Binary acids are acids that consist of two elements, usually hydrogen and a halogen. • Oxyacids are acids that contain hydrogen, oxygen, and a third element (usually a nonmetal).

  16. Acids, continued • a substance that yields hydrogen ions (H+) when dissolved in water. • example:hydrochloric acid refers to a water solution of the molecular compound hydrogen chloride, HCl • Many polyatomic ions are produced by the loss of hydrogen ions from oxyacids. • examples: • sulfuric acid H2SO4 sulfate • nitric acid HNO3nitrate • phosphoric acid H3PO4phosphate

  17. sodium hydroxide NaOH potassium hydroxide KOH Ba(OH)2 barium hydroxide Bases • Base: a substance that yields hydroxide ions (OH-) when dissolved in water.

  18. Hydrates • What is a hydrate? • Hydrates are named: Compound • Prefix-Hydrate FeCl3 • 6H2O = Iron (III) Chloride Hexahydrate

  19. Name to Formula – Criss Cross Rule • Lithium Fluoride • Sodium Sulfide • Aluminum Bromide • Iron (III) Oxide • Carbonic Acid • Calcium Carbonate • Magnesium Acetate • Copper Sulfate Pentahydrate • Ammonium Sulfite • Barium Hypochlorite

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