1 / 14

Lesson 3.2 – Naming Compounds

Lesson 3.2 – Naming Compounds. J. Venables Northwestern High School Chemistry 1 Honors. Naming of compounds, nomenclature, is divided into organic compounds (those containing C) and inorganic compounds (the rest of the periodic table).

tiara
Download Presentation

Lesson 3.2 – Naming 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. Lesson 3.2 – Naming Compounds J. Venables Northwestern High School Chemistry 1 Honors

  2. Naming of compounds, nomenclature, is divided into organic compounds (those containing C) and inorganic compounds (the rest of the periodic table). • Cations formed from a metal have the same name as the metal. • Example: Na+ = sodium ion. • If the metal can form more than one cation, then the charge is indicated in parentheses in the name. • Examples: Cu+ = copper(I); Cu2+ = copper(II). • Cations formed from non-metals end in -ium. • Example: NH4+ = ammonium ion.

  3. Negative Ions • Monatomic anions (with only one atom) are called -ide. • Example: Cl- is ____________. • Exceptions: hydroxide (OH-), cyanide (CN-), peroxide (O22-). • Polyatomic anions (with many atoms) containing oxygen end in -ate or -ite. (The one with more oxygen is called -ate.) – see sheet. • Examples: NO3- is nitrate, NO2- is _______.

  4. Chemical nomenclature is a systematic way of naming compounds. • Name the cation followed by the anion. • For monatomic cations use the element name. • For monatomic anions, use the root element name and the suffix –ide. • To distinguish between different oxidation states of the same element, the oxidation state is written in parentheses after the name of the cation. (no roman numerals for group 1, group 2, Al, Zn, Cd, Ag) • When the compound contains a polyatomic ion, name the cation followed by the name of the polyatomic ion.

  5. Naming Ionic Compounds • Name the cation then anion for the ionic compound. • Example: BaBr2 = barium bromide. • Examples – Name each: • Ca(HSO3)2 • Ba(ClO3)2 • Na3N • Al(CN)3 • (NH4)3PO4 • LiNO3 • Cu(NO2)2

  6. Naming Ionic Compounds • Name the cation then anion for the ionic compound. • Example: BaBr2 = barium bromide. • Examples – Name each: • Ca(HSO3)2 calcium hydrogen sulfite • Ba(ClO3)2 barium chlorate • Na3N sodium nitride • Al(CN)3 aluminum cyanide • (NH4)3PO4 ammonium phosphate • LiNO3 lithium nitrate • Cu(NO2)2copper (II) nitrite

  7. Examples of Writing Formulas • Example: barium chlorate = Ba(ClO3)2. • Examples – Write the formula for each: • Ammonium chloride • Potassium carbonate • Aluminum sulfate • Magnesium acetate • Cobalt (III) nitrate • Lead (IV) bromide • Mercury (II) chlorite

  8. Examples of Writing Formulas • Example: barium chlorate = Ba(ClO3)2. • Examples – Write the formula for each: • Ammonium chloride NH4Cl • Potassium carbonate K2CO3 • Aluminum sulfate Al2(SO4)3 • Magnesium acetate Mg(C2H3O2)2 • Cobalt (III) nitrate Co(NO3)3 • Lead (IV) bromide PbBr4 • Mercury (II) chlorite Hg(ClO2)2

  9. Naming Binary Molecular (Covalent) Compounds • The first element is always named first using the entire element name. • The second element is named using its root and adding the suffix –ide. • Prefixes are used to indicate the number of atoms of each element in a compound.

  10. Examples • Dinitrogen tetroxide • Sulfur hexafluoride • Dihydrogen monoxide • P2O5 • XeF4 • PF3

  11. Examples • Dinitrogen tetroxide N2O4 • Sulfur hexafluoride SF6 • Dihydrogen monoxide H2O • P2O5diphosphorus pentoxide • XeF4xenon tetrafluoride • PI3phosphorus triiodide

  12. Names and Formulas for Acids • Acids are compounds that start with hydrogen (H). H is bonded to a negative ion • The names of acids are related to the names of anions: • -ide becomes hydro-….-ic acid; • -ate becomes -ic acid; • -ite becomes -ous acid.

  13. Examples • HCl • HNO3 • H2SO3 • Chlorous acid • Perbromic acid • Hydrosulfuric acid

  14. Examples • HCl Hydrochloric acid • HNO3Nitric acid • H2SO3 Sulfurous acid • Chlorous acid HClO2 • Perbromic acid HBrO4 • Hydrosulfuric acid H2S

More Related