1 / 39

Chapter 6 Chemical Nomenclature

Chapter 6 Chemical Nomenclature. Metals, Nonmetals and Metalloids. The stair-step line in the periodic table separates metals from nonmetals. Elements bordering this line are metalloids. Formulas of Elements. For most elements, the smallest independent particle is an atom.

jules
Download Presentation

Chapter 6 Chemical Nomenclature

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. Chapter 6Chemical Nomenclature

  2. Metals, Nonmetals and Metalloids The stair-step line in the periodic table separates metals from nonmetals. Elements bordering this line are metalloids

  3. Formulas of Elements For most elements, the smallest independent particle is an atom. The formula of the element is the elemental symbol. ElementFormula Helium He Lithium Li

  4. Seven elements form stable diatomic molecules Formulas of Elements

  5. Compounds of Two Nonmetals Binary Molecular Compound A compound formed by two nonmetals or a metalloid and a nonmetal.

  6. Compounds of Two Nonmetals Naming Binary Molecular Compounds The first word is the name of the first element. A prefix is used to indicate the number of atoms. The second word is the name of the second element, changed to end in –ide. A prefix is used to indicate the number of atoms.

  7. Compounds of Two Nonmetals Number prefixes used in chemical names NumberPrefixNumberPrefix 1 mono- 6 hexa- 2 di- 7 hepta- 3 tri- 8 octa- 4 tetra- 9 nona- 5 penta- 10 deca-

  8. Compounds of Two Nonmetals Write the name of N2O5. N = nitrogen; 2 = di The first word is dinitrogen O = oxygen, Change oxygen to end in -ide: oxide; 5 = penta The second word is pentoxide (the letter a in prefixes is omitted if the resulting word sounds better) dinitrogenpentoxide

  9. Compounds of Two Nonmetals Write the formula of nitrogen trifluoride. No prefix on the first word, so mono- is implied = 1 atom. The symbol of nitrogen is N. Tri- prefix on the second word = 3 atoms. -fluoride is an “-ide modified” fluorine = F. NF3

  10. Compounds of Two Nonmetals Two compounds are so common they are always called by their traditional names: H2O is water NH3 is ammonia

  11. Ions, Cations, Anions Ion Charged particle formed when a neutral atom or molecule loses or gains electrons. Cation Positively charged ion. Anion Negatively charged ion.

  12. Ions formed by One Element The charge on a main-group (U.S. A group) ion corresponds to its group number: Group 1A 2A 3A 5A 6A 7A Charge 1+ 2+ 3+ 3– 2– 1–

  13. Ions Formed by One Element

  14. Ions Formed by One Element Name of a monatomic cation Name of element, followed by the word ion. Name of a monatomic anion Name of element changed to end in -ide, followed by the word ion.

  15. Ions Formed by One Element What is the formula of a sodium ion? Na+

  16. Ions Formed by One Element What are the name and formula of the ion formed from a chlorine atom? Cl– Change the name chlorine to end in –ide. Chloride ion

  17. Ions Formed by One Element Many transition elements (U.S. B groups) form multiple ions. The charge is shown by a Roman numeral enclosed in parentheses. Cr2+ is the chromium(II) ion Cr3+ is the chromium(III) ion

  18. Ions Formed by One Element Some transition element ions always occur with only one charge Zn2+ is zinc ion Ag+ is silver ion Ni2+ nickel ion Special Case Hg22+ is called mercury(I) ion.

  19. Cations

  20. Anions

  21. Acids and Their Anions Acid Molecular compound that reacts with water to produce a hydrated hydrogen ion and an anion. Ionization of hydrochloric acid HCl H2O + HCl→ H3O+ + Cl– H3O+ is called hydronium ion.

  22. Acids and Their Anions The Acids of Chlorine and Their Anions # of O atoms Acid prefix Anion prefix Compared with and/or suffix and/or suffix -ic acid and -ate anion(Example)(Example) One more per- -ic per- -ate HClO4 (perchloric) (perchlorate) Same -ic -ate HClO3 (chloric) (chlorate) One fewer -ous -ite HClO2 (chlorous) (chlorite) Two fewer hypo- -ous hypo- -ite HClO (hypochlorous) (hypochlorite) No oxygen hydro- -ic -ide HCl (hydrochloric) (chloride)

  23. Acids and Their Anions The names and formulas of following acids should be memorized AcidIonization Equation Ion Name Chloric acid HClO3 H+ + ClO3– Chlorate ion Nitric acid HNO3 H+ + NO3– Nitrate ion Sulfuric acid H2SO4 2 H+ + SO42– Sulfate ion Carbonic acid H2CO3 2 H+ + CO32– Carbonate ion Phosphoric acid H3PO4 3 H+ + PO43– Phosphate ion

  24. Acid Anions Step-by-Step Acid Anion Nomenclature H3PO4 phosphoric acid H2PO4– dihydrogen phosphate ion HPO42– hydrogen phosphate ion PO43– phosphate ion

  25. Acids and Their Anions

  26. Formulas of Ionic Compounds Ionic Compound A compound made up of ions. The formula unit must have an equal number of positive and negative charges.

  27. Formulas of Ionic Compounds Formula of the cation, followed by the formula of the anion. (omit the charges). Subscripts are used to show the number of each ion in the formula unit. (sum of charges must equal to zero) Omit the subscript if only one ion is needed. Enclose formula of the polyatomic ion in parentheses and place the subscript after the closing parentheses.

  28. Formulas of Ionic Compounds What is the formula of magnesium chloride? Magnesium is in Group 2A, so its ion is Mg2+. Chlorine is in Group 7A, so its ion is Cl–. Two 1– ions are needed to balance the 2+ ion. MgCl2.

  29. Formulas of Ionic Compounds What is the formula of barium nitrate? Barium cation is Ba2+ Nitrate anion is NO3– Nitrate ion must be enclosed in parentheses Ba(NO3)2

  30. Other Acids and Ions Memorize the following common and important ions: Hydroxide ion OH– Ammonium ion NH4+

  31. Names of Ionic Compounds Example: Write the name of Zn(NO3)2. Solution: Zinc ion has only one common charge, 2+, so the magnitude of the charge is not included in its name: zinc ion. NO3– comes from the memorized acid HNO3, nitric acid. To name the ion, the -ic ending changes to -ate: nitrate ion. Zinc nitrate

  32. Names of Ionic Compounds How to Write the Name of an Ionic Compound • Write the name of the cation. • Write the name of the anion.

  33. Names of Ionic Compounds Write the name of CoCl2. There is more than one common charge for cobalt ions. We will have to use the anion to determine this charge. Chlorine is in Group 7A, so the charge on the ion is 1–: Cl–. The name of the anion is changed to end in -ide: chloride ion. Two 1– ions require a 2+ ion to balance the charge: cobalt(II) ion. Cobalt(II) chloride

  34. Hydrate A solid compound that includes water molecules as part of its crystal structure. Hydrates

  35. Hydrates Water of crystallization Water molecules that are part of the crystal structure in a hydrate. Anhydrous compound An ionic compound without water.

  36. Hydrates Formulas of Hydrated Compounds Formula of ionic compound, followed by the number of water molecules, separated by a dot. Example: Copper (II) sulfate pentahydrate CuSO4 • 5 H2O There are five water molecules for every formula unit of copper (II) sulfate.

  37. Hydrates Names of Hydrated Compounds Use the prefixes for naming binary molecular compounds to indicate the number of water molecules associated with each formula unit of the anhydrous compound. Example: MgSO4 • 7 H2O Magnesium sulfate heptahydrate

  38. Hydrates Example: What is the formula of iron(III) sulfate nonahydrate? Solution: Iron(III) ion is Fe3+. Sulfuric acid is H2SO4, so sulfate ion is SO42–. Nona- is the prefix for 9. -hydrate refers to water of hydration, H2O. 2 × 3+ balances 3 × 2–. Fe2(SO4)3 • 9 H2O

  39. Homework Homework for chapter 6: 3, 5, 9, 13,15, 19, 21, 23, 25, 33, 35, 39, 41,43, 45, 47, 49 Fill the tables 6-13, 6-14, 6-15 and 6-16

More Related