Chemical Names and Formulas

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Presentation transcript:

Chemical Names and Formulas

Review What are ionic compounds? What are covalent compounds?

Relate the forming of compounds to orbital diagrams Good Examples to use: NaCl CaCl2 H2O

Always ask this question Is it ionic or covalent? Two nonmetals= covalent Metal and a nonmetal = ionic Look at the periodic table

Naming Molecules What are molecules?

Molecular Nomenclature CO2 Carbon dioxide Carbon monoxide CO What about water? H2O Dihydrogen monoxide

Molecular Nomenclature Prefix System (binary compounds) 1. Less e-neg atom comes first. 2. Add prefixes to indicate # of atoms. Omit mono- prefix on first element. 3. Change the ending of the second element to -ide.

Molecular Nomenclature PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10

Molecular Nomenclature CCl4 N2O SF6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride

Molecular Nomenclature arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl3 N2O5 P4O10

Molecular Nomenclature The Seven Diatomic Elements Br2 I2 N2 Cl2 H2 O2 F2 H N O F Cl Br I

Naming Ionic compounds What are ionic compounds?

Ionic Nomenclature sodium chloride magnesium nitrate Charges are called oxidation number magnesium nitrate copper(II) chloride Na+ Cl-  NaCl Mg2+ NO3-  Mg(NO3)2 Cu2+ Cl-  CuCl2

Ionic Nomenclature NO PREFIXES Depends on charges Charges are called oxidation numbers

Ionic Nomenclature – Binary Compounds potassium chloride calcium chloride K+ Cl-  KCl Ca2+ Cl-  CaCl2

Ionic Nomenclature – Binary Compounds NaBr sodium bromide

Ionic Nomenclature Ionic Names Write the names of both ions, cation first. Overall charge must equal zero. Change ending of monatomic ions to -ide. Polyatomic ions have special names. Stock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

Ionic Nomenclature Common Ion Charges 1+ 2+ 3+ NA 3- 2- 1-

Polyatomic Ions A polyatomic ion is a covalent molecule that has an ionic charge. Poly = many Atomic = atoms Ion = charged particle

Polyatomic Ions Examples: Sulfate = SO4-2 Nitrate = NO3-1 Phosphate = PO4-3 Chlorate = ClO3-1 Carbonate = CO3-2 Notice the ending has changed to –ate.

Ionic Nomenclature Consider the following: Does it contain a polyatomic ion? -ide  no -ate, -ite,  yes Does it contain a Roman numeral? Check the table for metals not in Groups 1 or 2.

Ionic Nomenclature – Polyatomic compounds magnesium nitrate Mg2+ NO3-  Mg(NO3)2

Ionic Nomenclature – Polyatomic compounds Na2CO3 sodium carbonate

Transition Metals May have more than one charge For element with more than one charge write the charge using Roman numerals and put it in parenthesis after the elements name Example: FeSO4  Iron (II) Sulfate

Ionic Nomenclature – Transition Metals copper(II) chloride Cu2+ Cl-  CuCl2

Ionic Nomenclature – Transition Metals SnCO3 tin(II) carbonate

Practice Practice ions and molecules before adding acids

Naming Acids

Definition Acid Compound that forms H+ in water. Formula usually begins with ‘H’. All of ours will start with ‘H’. Examples: HCl, HNO3, H2SO4

Acid Names 4.) If the root has a prefix, keep it.

Acid names HBr H2CO3 H2SO3 Other Hydrogen Bromide hydrobromic acid Hydrogen Carbonate carbonic acid H2SO3 Hydrogen Sulfite sulfurous acid Other HClO Hydrogen Hypochlorite hypochlorous acid HClO4 Hydrogen Perchlorate perchloric acid

Acid Formulas hydrofluoric acid sulfuric acid nitrous acid -ide  HF -ate  H2SO4 -ite  HNO2