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Naming Chemical Compounds

Naming Chemical Compounds. Naming Ions. What are ions? Atom that has gained or lost electrons Cations? Atom that has lost electrons. (+ charge) Anions? Atom that has gained electrons. (- charge) Cations and Anions are named differently. Naming Cations.

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Naming Chemical Compounds

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  1. Naming Chemical Compounds

  2. Naming Ions • What are ions? • Atom that has gained or lost electrons • Cations? • Atom that has lost electrons. (+ charge) • Anions? • Atom that has gained electrons. (- charge) • Cations and Anions are named differently.

  3. Naming Cations • Which elements on the periodic table are cations? (have a positive charge?) • Elements on the left side • Which Groups? • 1A, 2A, 3A • For all Cations (Elements in groups 1A, 2A, 3A) you add the work ion after the elemental name.

  4. Naming Cation examples • Na1+ • Sodium ion • Al3+ • Aluminum ion • Ca2+ • Calcium ion

  5. Naming Anions • Which elements on the periodic table are anions? (have a negative charge?) • Elements on the right side • Which Groups? • 5A, 6A, 7A • For all anions you add the suffix (ide) at the end of the root of each elemental name. • Flourine (F-1) is called • Flouride

  6. Naming Anions Example • Chlorine (Cl1-) • Chloride • Sulfur (S2-) • Sulfide • Nitrogen (N3-) • Nitride

  7. Naming Transition Metals • Where are the Transition metals located? • Many Transition metals for more than one ion • Fe2+, Fe3+, Cu+, Cu2+ • Thus, when naming transition metals signify the number of electrons gained or lost after the elements name. • Example: Fe2+ and Fe3+ becomes… • Iron (II) ion and Iron (III) ion

  8. Naming Transition Metals Examples • Tin (Sn2+) • Tin (II) ion • Tin (Sn4+) • Tin (IIII) ion • Manganese (Mn2+) • Manganese (II) ion • Manganese (Mn3+) • Manganese (III) ion

  9. Monatomic Ions • Monatomic Ions consist of a single atom with a positive or negative charge. • All ions we have studied up to this point have been Monatomic Ions • Now we will begin looking at Polyatomic ions.

  10. Polyatomic Ions • If monatomic ions are single atoms. Polyatomic ions are….? • Polyatomic ions are composed of more than one atom.

  11. Examples of Polyatomic Ions • Examples: Sulfur and Oxygen combine to form… SO42- • Carbon, Hydrogen, and Oxygen form… C2H3O21- • These polyatomic ions are tightly connected and behave like 1 element. Tough to separate them.

  12. Naming Polyatomic Ions • Most polyatomic ions end in ite or ate. • Luckily we do not need to memorize rules for these. • You will be given a list of popular polyatomic and monatomic ions that will guide you for the rest of the year.

  13. Practice Problems • Answer the questions in your lab notebook • Monatomic Ion Naming practice: • For each question indicate the name of the ion and whether each is a cation or anion. • 1.Sodium 7.Chlorine • 2.Calcium 8.Sulfur • 3.Bromine 9.Oxygen • 4.Potassium 10.Lithium • 5.Iodine 11.Beryllium

  14. Binary Ionic Compounds • Compounds? • Compounds are substances made up of 2 or more elements • A Binary Ionic Compound is a substance made up of 2 ionic elements. • Examples: • NaCl • Li2O • BaS

  15. Naming Binary Ionic Compounds • To name any Binary Ionic Compound you place the name of the cation first, followed by the anion. • NaCl • Sodium Chloride • Li2O • Lithium Oxide • BaS • Barium Sulfide • CuO • Coppper (II) Oxide • Fe2O3 • Iron (III) Oxide • CaS • Calcium Sulfide

  16. Writing Binary Ionic Compound Formulas • Copper (I) Sulfide, What is its chemical formula? • Use The Criss Cross Method • Copper (I) = Cu1+ Sulfide = • Cation Written first: Anion Second • Cu1+ S2- • Criss Cross the charges to the other element • Cu1+ S2- Becomes • Cu2S • Examples on Board…

  17. Naming Binary Compounds With Polyatomic Ions • The same as before… • State the name of the cation first and then the name of the anion. • LiCN • Lithium Cyanide • NaClO • Sodium Hypochlorite • AgNO3 • Silver Nitrate

  18. Writing Formulas for Polyatomic Ions • It is the exact same as before! Criss Cross Method! • Cation is written first and Anion second • Calcium = Ca2+ Acetate = C2H3O21- • Ca2+ C2H3O21- • Then criss cross the charges • Ca1C2H3O22 • Add parentheses. 2 acetate ions not 22 Oxygens • Ca(C2H3O2)2 Examples on the Board

  19. Practice!!!! • Either name the compound or write the chemical formula for the compound. • CaCl2 • Sodium Hydroxide • MgSO4 • Magnesium Sulfate • Cr(NO3)3 • Cesium Sulfide • NaCl • Sodium Iodide • NaClO4 • Magnesium Hydroxide

  20. Quiz Write the name or formula for the following compounds. • Cesium Sulfide • NaCl • Sodium Iodide • NaClO4 • Magnesium Hydroxide • Magnesium Sulfate Write the name for the following ions. • Sodium • Chlorine • Calcium • Sulfur

  21. Binary Molecular Compounds • Binary Molecular Compounds are compounds made up of 2 or more nonmetals. • What type of bond is typically bonded between 2 nonmetals? • Covalent bond.

  22. Naming Binary Molecular Compounds • Use the prefixes stated below. • 1 atom = mono- • 2 atom = Di- • 3 atom = Tri- • 4 atom = Tetra- • 5 atom = Penta- • 6 atom = Hexa- • 7 atom = Hepta- • 8 atom = Octa- • 9 atom = Nona- • 10 atom = Deca-

  23. Naming Binary Molecular Compounds • N2O • 2 Nitrogens 1 Oxygen • Prefix for 2 and 1? • Di and Mono • Put the di in front of Nitrogen • Dinitrogen • Put the mono in front of oxygen and add ide • Monoxide • Put the 2 together. • Dinitrogen Monoxide

  24. Naming Binary Molecular Compounds • P2O3 • 2 Phosphorous 3 Oxygen • Prefix for 2 and ? • Di and Tri • Put the di in front of Phosphorous • Diphosphorous • Put the tri in front of oxygen and add ide • Trioxide • Put the 2 together. • Diphosphorous Trioxide

  25. Naming Binary Molecular Compounds • CO • Monocarbon Monoxide? NOPE!!! • When there is one atom of the first element you drop the mono • Carbon Monoxide • CO2 • Carbon Dioxide

  26. Writing formulas for Binary Molecular Compounds • To write formulas for these compounds you use the prefix in the name to tell you the element’s subscript. • Carbon Tetrabromide • 1 carbon • 4 bromines. Use them as subscripts. • CBr4 • Chlorine Triflouride • 1 Chlorine and 3 Flourides • ClF3

  27. Practice • NI3 • BCl3 • N2O3 • Cl2O7 • Silicon Tetraflouride • Carbon Tetrachloride • Iodine Dioxide

  28. Naming Acids • Name of the anion ends in ide the acid names begins with hydro and then ends in ic. Followed by the work acid. • HCl – Hydrogen Chloride • Hydrochloric acid • Name of the anion ends in ite, change the ite to ous followed by the word acid. • H2SO4 - Hydrogen Sulfite • Sulfurous acid • Name of the anion ends in ate, change the ate to a ic followed by the word acid. • HNO3 – Hydrogen Nitrate • Nitric acid

  29. Naming Acids

  30. Writing Formulas for Acids • Use the reverse rules for writing formulas • Hydrobromic Acid • Hydro in front and ic at end. = anion ends in ide • Must be Hydrogen and Bromide ions • HBr • Phosphourus Acid • ous ending means = anions ends in ite • Must be Hydrogen and Phosphite ions • H3PO4 • Formic Acid • Ic ending means = anion ends in ate • Must be Hydrogen and Formate ions • HCOOH

  31. Names and Formulas for Bases • Same as other ionic compounds • Name of cation followed by name of anion • NaOH • Sodium Hydroxide • Formulas use the Criss Cross Method • Aluminum Hydroxide • Al 3+ OH1- • Al(OH)3

  32. Practice • In your lab notebook write the name of the acid or base. Or write the formula of the acid or Base. • HNO2 • HCN • HMnO4 • H2S • Carbonic Acid • Sulfurous Acid • Iron (III) Hydroxide • Strontium Hydroxide • LiOH • Mg(OH)2 • Pb(OH)2

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