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Nomenclature

This chapter explores the key concepts in chemical nomenclature, focusing on molecular and ionic compounds. It differentiates between molecular formulas, which specify the exact number of atoms, and empirical formulas that show the simplest ratio of elements. Learn the rules for naming compounds, including the use of prefixes for nonmetals and the significance of polyatomic ions. The section also covers diatomic elements, acids, bases, and hydrates, providing a comprehensive overview of how to write and interpret chemical formulas in modern chemistry.

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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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