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Chemical Nomenclature

Chemical Nomenclature. Chapter 7. Molecular Compounds. Consists of nonmetals covalently bonded to: Nonmetals Metalloids. TOXIC !. Laughing Gas. Molecular Compounds. First Element: Only use a prefix if there is more than one Simply state the element name Second Element :

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Chemical Nomenclature

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  1. Chemical Nomenclature Chapter 7

  2. Molecular Compounds • Consists of nonmetals covalently bonded to: • Nonmetals • Metalloids

  3. TOXIC! Laughing Gas Molecular Compounds First Element: • Only use a prefix if there is more than one • Simply state the element name Second Element: • Always use a prefix • Change the ending of the second word to –ide • Drop any double vowels (except for i) NO2 nitrogen dioxide dinitrogenmonoxide N2O

  4. Prefixes for naming covalent compounds Number of atoms/example Number of atoms/example Hexa 6 SCl6 Hepta 7 IF7 Octa 8 Np3O8 Nona 9 I4O9 Deca 10 S2F10 • Mono 1 CO • Di 2 SO2 • Tri 3 SO3 • Tetra 4 CCl4 • Penta 5PCl5

  5. Molecular Compound Examples Carbon Dioxide Sulfur Dioxide Dinitrogen monoxide Dinitrogen Trioxide DinitrogenTetroxide Phosphorus Trichloride Ammonia (an exception) DiphosphorusPentoxide Silicon Dioxide Oxygen Difluoride • CO2 • SO2 • N2O • N2O3 • N2O4 • PCl3 • NH3 • P2O5 • SiO2 • OF2

  6. DIATOMIC ELEMENTS Some elements do not like to be alone… so they bond to themselves! DO NOT USE PREFIXES – just name the element. 7 HOFBrINCl

  7. Acids • acid: is a type of molecular compound • Binary acids are acids that consist of two elements, hydrogen and usually a halogen. • Use “hydro” to represent the hydrogen • For the 2nd element, write the root word and add “ic acid” • example:HCl = hydrochloric acid

  8. Acids, continued • Oxyacids are acids that contain hydrogen, oxygen, and a third element (usually a nonmetal). • Naming is based on polyatomic ion: • First, name the polyatomic ion root name • Second, add the suffix as follow: • ates = ic acids • ites = ous acids • sulfuric acid H2SO4 sulfate • nitric acid HNO3nitrate • phosphoric acid H3PO4phosphate

  9. Acid nomenclature Nitric acid Hydrochloric acid Sulfuric acid Sulfurous acid Acetic acid Hydrobromic acid Nitrous acid Phosphoric acid Hydrosulfuric acid Carbonic acid • HNO3 • HCl • H2SO4 • H2SO3 • HC2H3O2 • HBr • HNO2 • H3PO4 • H2S • H2CO3

  10. 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

  11. 2 x +3 = +6 1 x +2 = +2 1 x +2 = +2 3 x -2 = -6 1 x -2 = -2 2 x -1 = -2 Formula of Ionic Compounds Al2O3 Aluminum oxide Write ions Find LCM Make equal (these #’s become subscript) Calcium bromide Write ions Find LCM Make equal (these #’s become subscript) Sodium carbonate Write ions Find LCM Make equal (these #’s become subscript) Al3+ O2- CaBr2 Ca2+ Br- Na2CO3 Na+ CO32-

  12. NAMING ionic COMPOUNDS RULE 1 Metal – Nonmetal • Write the metal (positive ion) first by just saying the metal name or ammonium • Change the ending of the second word to -ide

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

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

  15. Rule 2 Examples • BaSO4 • BaSO3 • Na2CO3 • NaHCO3 • (NH4)3PO4 • NH4OH Barium Sulfate Barium Sulfite Sodium Carbonate Sodium Bicarbonate Ammonium Phosphate Ammonium Hydroxide

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

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

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

  19. Name to Formula – Least Common Multiple • Lithium fluoride • Sodium sulfide • Aluminum bromide • Iron (III) oxide • Sulfuric acid • Calcium carbonate • Magnesium acetate • Lead (IV) oxide • Ammonium sulfite • Barium hypochlorite

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