1 / 32

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.

abla
Download Presentation

Naming Chemical Compounds

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  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

More Related