Writing Formulas and Naming Compounds

Writing Formulas and Naming Compounds

Writing Formulas and Naming Compounds Binary Compounds Compounds that are made up of only 2 elements Two types of binary compounds: 1. Ionic Compounds metals and nonmetals (Ex: NaCl, MgBr2, K2O) 2. Covalent Compounds 2 nonmetals (Ex: CO2, H2O, SO3) Practice Ionic or Covalent? 1.

2. 3. 4. NO2 P2O4 Fe2O3 CaF2 covalent covalent ionic

ionic Naming Covalent Compounds 1. Use prefixes to indicate the number of each element hexa 6 mono 1 hepta 7 di 2 octa 8 tri 3 nona 9 tetra 4

deca 10 penta 5 Naming Covalent Compounds 2. Name the first element. If you have only one atom of the first element, do NOT use the prefix mono-. 3. Name the second element with prefixes. Change the ending to -ide. Naming Covalent Compounds Practice 1. CO2

carbon dioxide 2. SO3 sulfur trioxide 3. N2O4 dinitrogen tetroxide 4. CCl4

carbon tetrachloride 5. H2O dihydrogen monoxide Writing Covalent Compounds 1. phosphorus trichloride PCl3 2. nitrogen dioxide

NO2 3. sulfur hexabromide SBr6 4. diphosphorus pentoxide P2O5 Naming Ionic Compounds 1. Name the first element (metal) 2. Name the second element (nonmetal) and change the

ending to -ide 3. NO PREFIXES!!! Naming Ionic Compounds - Practice 1. NaCl sodium chloride 2. CaF2 calcium fluoride

3. Ag2O silver oxide 4. AlBr3 aluminum bromide 5. ZnS zinc sulfide

Writing Ionic Formulas Ionic compounds are composed of a positive ion called a cation and a negative ion called an anion. 1. Write the metal ion first ( + ion: cation) 2. Write the nonmetal last ( - ion: anion) 3. Balance the charges! Charges must add up to zero to form a neutral compound. Writing Ionic Formulas To determine the charge: You can look at the position of the element on the periodic table to determine the charge of the element when it forms

an ion There is a difference between a neutral element (K) and an ion (K+) Periodic Table Charges Writing Ionic Compound Formulas 1. sodium chloride Na+ Cl-

NaCl 2. calcium chloride Ca+2 ClCl- CaCl2 Writing Ionic Compound Formulas 3. aluminum chloride Al+3 ClClClAlCl3

Writing Ionic Compound Formulas 4. potassium bromide K+ BrKBr 5. potassium oxide K+ O-2 K+ K2O Writing Ionic Compound Formulas 6. aluminum oxide O-2 Al+3

-2 +3 O Al O-2 Al2O3 Ionic Compounds with Roman Numerals The roman numeral gives the charge of the metal ion. Ex: Fe(II) Fe+2

Fe(III) Fe+3 Transition metals need roman numerals in the name. Pb and Sn need roman numerals because they have charges of +2 and +4. Ag and Zn do NOT need roman numerals because Ag is always +1 and Zn is always +2. Ionic Compounds with Roman Numerals Write the Formula 1. nickel (II) bromide NiBr2

2. lead (IV) oxide PbO2 3. iron (III) sulfide Fe2S3 Ionic Compounds with Roman Numerals Name the Following 1. CrCl3

2. FeO 3. SnCl4 chromium (III) chloride iron (II) oxide tin (IV) chloride copper (I) oxide 4. Cu2O Review: Write the Formula 1. strontium fluoride

SrF2 2. chromium (III) oxide Cr2O3 3. sulfur hexabromide SBr6 4. iron (III) sulfide

Fe2S3 5. carbon disulfide CS2 Review: Name the Following. 1. K2Se potassium selenide

2. CaI2 calcium iodide 3. NiCl2 nickel (II) chloride 4. PCl3 phosphorus trichloride

5. BaNa2 banana Naming Compounds with Polyatomic Ions 1. Name the metal 2. Name the polyatomic ion 3. Use roman numeral if needed Naming Polyatomic Ions Practice: Name the Compound

1. MgCO3 magnesium carbonate 2. Na2SO4 sodium sulfate 3. Cu(OH)2 copper (II) hydroxide

4. Zn(C2H3O2)2 zinc acetate Naming Polyatomic Ions Practice: Write the Formula 1. aluminum nitrate Al(NO3)3 2. ammonium sulfite (NH4)2SO3

3. iron (III) chlorate Fe(ClO3)3 4. calcium phosphate Ca3(PO4)2 Review: Covalent compounds are made up of nonmetals only. Use prefixes in the names of covalent compounds. Covalent compounds do not have charges!

Ionic compounds are made up of a metal and a nonmetal. Balance the charges when you write a formula for ionic compounds. Never use prefixes in the names of ionic compounds!

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