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Ch. 4 Notes---Nomenclature: Chemical Names & Formulas

Ch. 4 Notes---Nomenclature: Chemical Names & Formulas. salts. metal. Ionic Compounds ( “ ________ ” ): Name or formula starts with a _________ (or NH 4 + , ammonium). Other quick ways to tell if the compound is ionic: formula uses parentheses Example: ________________

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Ch. 4 Notes---Nomenclature: Chemical Names & Formulas

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  1. Ch. 4 Notes---Nomenclature: Chemical Names & Formulas salts metal • Ionic Compounds (“________”): • Name or formula starts with a _________ (or NH4 +, ammonium). • Other quick ways to tell if the compound is ionic: • formula uses parentheses Example: ________________ • formula contains more than 2 elements (capital letters) Example: ________________ • name uses Roman numerals Example: ________________ • name ends in “-ate” or “ite”. Example: _________________ Ca(OH)2 FeCrO4 lead(II) chloride barium sulfate

  2. Click for Lecture • http://danreid.wikispaces.com/file/view/Ch.%206%20Names%20and%20Formulas%20Lecture.swf

  3. molecules nonmetal • Molecular Compounds (“____________”): • Name or formula starts with a ____________ (exception: NH4 +) • Other quick ways to tell if the compound is molecular: • Name has prefixes and also ends in “-ide”. (It must have both!) Examples: _________________,_______________________ Naming Ionic Compounds • Just use your ion sheet and find the names of the ions. cation name anion name Practice Problems: Name the following ionic compounds. a) NaC2H3O2 b) (NH4)2CO3 c) Fe(OH)3 d) PbSO4 carbon dioxide dinitrogen pentoxide (III) lead (II) iron sodium acetate ammonium carbonate sulfate hydroxide

  4. Writing Formulas for Ionic Compounds • Step 1-- Use your ion sheet and find the ions and their charges. • Step 2-- “Cross the charges” if they don’t balance out. • Step 3-- Use parentheses around polyatomic ion “chunks”. Practice Problems: Write the formula for each ionic compound. copper(II) bromide ____________________ aluminum nitrite _________________________ barium hydrogen carbonate ___________________________ Cu+2 Br -1 CuBr2 …(don’t show 1’s) = Al+3 NO2-1 Al(NO2)3 = Ba+2 HCO3-1 Ba(HCO3)2 =

  5. charges share Naming Molecular Compounds • You do not use the ion sheet for molecules because no __________ are needed. They ______________ electrons instead of transferring them. • Use ________________ to indicate the # and kind of atom in the compound. mono=1 di=2 tri=3 tetra=4 penta=5 hexa=6 hepta=7 octa=8 non=9 deca=10 • Use the general format shown below… prefix-(except mono)-name the 1st elementprefix-name the 2nd element ending with -ide Practice Problems: Name the following molecules. N2O5 CO Cl4F7 SO3 prefixes carbon monoxide tetrachlorine heptafluoride sulfur trioxide dinitrogen pentoxide

  6. subscripts Writing Molecular Formulas • The prefixes in the name tell you the # of atoms of each element there are. (Those become the _________________ in the formula!) Practice Problems: Write the formula for each molecule. nitrogen monoxide carbon tetrachloride diphosphorous pentoxide Acids • All acids begin with the element ________________. • General format: H(X), where “(X)” represents the ______________. • There are 2 general types of acids: • If the name of “(X)” ends in –ite or –ate, then it is an _________ acid. • If the name of “(X)” ends in –ide, then it is a ____________ acid. The acids just contains ____ elements, hydrogen and a nonmetal. (There’s NO oxygen!) CCl4 P2O5 NO hydrogen anion oxy- binary 2

  7. Naming Oxy-Acids • If the name of “(X)” ends in –ate… (anion root)-ic acid • If the name of “(X) ends in –ite… (anion root)-ous acid Practice Problems: Name these acids. H2SO4 H3PO3 HNO3 H2CO3 HC2H3O2 HClO2 Naming Binary Acids If the name of “(X)” ends in –ide… hydro- (anion root)-ic acid Practice Problems: Name these acids. H2S HCl HF sulfuric acid phosphorous acid nitric acid carbonic acid acetic acid chlorous acid hydrosulfuric acid hydrochloric acid hydrofluoric acid

  8. hydro Writing the Formulas for Acids FIRST You must determine the formula for the anion, “(X)”. • If the acid’s name starts with “________” (and ends in “–ic”), the name of the anion used ends in “_______”. Therefore, it is a _________ acid. (There’s only hydrogen and one other nonmetal in the formula!) • The subscript on the hydrogen equals the anion’s charge! Examples: hydrobromic acid = ________ hydroiodic acid = _______ hydrosulfuric acid = ________ -ide binary HBr HI H2S

  9. -ic -ate oxy- • If the acid’s name ends with “______” without the “hydro-” prefix, the name of the anion used ends in “_______”. Therefore, it is an ____ acid. • The subscript on the hydrogen equals the anion’s charge! Examples: perchloric acid = __________ oxalic acid = ___________ • If the acid’s name ends with “______”, the name of the anion used ends in “_______”. (It’s is also an oxy-acid.) • The subscript on the hydrogen equals the anion’s charge! Examples: hypochlorous acid = __________ nitrous acid = ____________ sulfurous acid = ____________ HClO4 H2C2O4 -ous -ite HClO HNO2 H2SO3

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