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Chemical Naming & Formulas

Chemical Naming & Formulas. Categories of Naming. Covalent Ionic Organic Entire unit in Chem 30S. Covalent Naming. Generally a bond between 2 non-metal elements General Rules First element is named as listed on periodic table Second element has the suffix – ide

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Chemical Naming & Formulas

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  1. Chemical Naming & Formulas

  2. Categories of Naming • Covalent • Ionic • Organic • Entire unit in Chem 30S

  3. Covalent Naming • Generally a bond between 2 non-metal elements • General Rules • First element is named as listed on periodic table • Second element has the suffix –ide • Prefix used for each element to indicate the # of atoms • If only one atom of first element → No prefix used

  4. Covalent Naming - Prefixes Number Prefix 1 mono 2 di 3 tri 4 tetra 5 penta 6 hexa 7 hepta 8 octa 9 nona 10 deca

  5. Covalent - Examples • Name the following • CO2 • CO • CCl4 • N2O4 • SF6 • P2Cl5 • PI3 • P5Cl8 Carbon dioxide Carbon oxide Carbon tetrachloride Dinitrogen tetraoxide Sulfur hexafluoride Diphosphorus pentachloride Phosphorus triodide Pentaphosphorus octachloride

  6. Covalent - Examples • Write the formulas for the following • Tetranitrogen decaoxide • Disulfur pentafluoride • Hexaselenium tribromide • Nitrogen monoxide • Aluminum Chloride N4O10 S2F5 Se6Br3 NO IONIC

  7. Ionic • 3 subcategories • Monatomic Ions • Polyatomic Ions • Transitional Metals • Can use both monatomic and polyatomic • Rules • Formula must be neutral • No # prefixes used as only one possible combination with ions involved • Cation (+ve) listed first, Anion (-ve) listed second

  8. Ionic – Monatomic Ions (Naming) • Monatomic ions are ions that contain only 1 atom • Anion has suffix –ide • Examples • NaCl • AlCl3 • MgO • Ga2P3 • HF • NaH Sodium Chloride Aluminum Chloride Magnesium Oxide Gallium Phosphide Hydrogen Fluoride Sodium Hydride

  9. Ionic – Monatomic Ions (Formulas) • Entire unit MUST be neutral • Add appropriate # of each ion to balance charges • Example • Aluminum Fluoride Al3+ F- +3 -1 = +2 Al3+ 3F- +3 -3 = 0 AlF3

  10. Ionic – Monatomic Ions (Formulas) • Example • Gallium Oxide Ga3+ O2- +3 -2 = +1 Ga3+ 2O2- +3 -4 = -1 2Ga3+ 2O2- +6 -4 = +2 2Ga3+ 3O2- +6 -6 = 0 Ga2O3

  11. Ionic – Monatomic Ions (Formulas) • Examples • Write the formulas for the following • Lithium Sulfide • Magnesium Bromide • Hydrogen Nitride • Aluminum Phosphide • Boron Sulfide Li2S MgBr2 H3N AlP B2S3

  12. Ionic – Polyatomic Ions (Names) • Ions with more than one atom • Eg) • NO3- (Nitrate) • PO43- (Phosphate) • NH4+ (Ammonium) • The entire item has a charge, not each element in the polyatomic ion • Look at page. 257 • The exact ion name is used

  13. Ionic – Polyatomic Ions (Names) • Examples • NaBrO3 • Na2C2O4 • Ca(NO3)2 • NH4Cl • Al2(SO3)3 Sodium Bromate Sodium Oxalate Calcium Nitrate Ammonium Chloride Aluminum Sulfite

  14. Ionic – Polyatomic Ions (Formulas) • Entire unit MUST be neutral • Add appropriate # of each ion to balance charges • Example • Potassium Permanganate K+ MnO4- +1 -1 = 0 KMnO4

  15. Ionic – Polyatomic Ions (Formulas) • Example • Magnesium Nitrite Mg2+ NO2- +2 -1 = +1 Mg2+ 2NO2- +2 -2 = 0 Mg(NO2)2

  16. Ionic – Transitional Metals • Transitional Metals can have different charges • Depends on the situation • Example • Fe2+ • Fe3+ • Ti2+ • Ti4+ • When naming, must determine what the charge is • Indicated by using Roman numerals • Must know Roman numerals 1-10

  17. Ionic – Transitional Metals (Naming) • Example • FeO Fe2+ O2- -2 = 0 +2 Iron (II) Oxide

  18. Ionic – Transitional Metals (Naming) • Example • Fe2(CO3)3 2Fe 3CO32- 3+ -6 = 0 +6 Iron (III) Carbonate

  19. Ionic – Transitional Metals (Naming) • Write the names for the following • TiS2 • CuCl • AgNO3 • CuSO4 • V(ClO4)5 Titanium (IV) Sulfide Copper (I) Chloride Silver (I) Nitrate Copper (II) Sulfate Vanadium (V) Perchlorate

  20. Ionic – Transitional Metals (Formulas) • The name indicates the charge • Balance as normal • Example • Zinc (II) Chloride Zn2+ Cl- +2 -1 = +1 Zn2+ 2Cl- +2 -2 = 0 ZnCl2

  21. Ionic – Transitional Metals (Formulas) • Examples • Nickel (II) Nitride • Chromium (IV) Oxalate • Iron (III) Cyanide • Mercury (I) Acetate (careful) Ni3N2 Cr(C2O4)2 Fe(CN)3 Hg2(CH3COO)2

  22. Tricky Items • Peroxide • A polyatomic ion with 2 oxygen atoms with a 2- charge • Very reactive ion • Explosive in some cases • H20 Dihydrogen Monoxide (Covalent) • H2O2 Hydrogen peroxide (Ionic)

  23. Tricky Items • Example • MgO2 • If the oxygen is an oxide ion, then we would have -4 • The Mg is +2 • This is not balanced • Therefore the O2 item must have a -2 charge • Peroxide (O22-)

  24. Textbook Assignment • P.282 #’s 65-70 • Omit #67 d) & #69 i) & #66 h)

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