Warm-Up What is an ion? How is it formed?

NOMENCLATURE Naming and Writing Compounds

Three categories of compounds Acids – begin with a hydrogen (HCl) Ionic – metal bonded with a non-metal or polyatomic ion Covalent – non-metal bonded with non-metal FIRST DETERMINE WHAT TYPE OF COMPOUND YOU ARE DEALING WITH

Identify the compounds below as ionic compounds, covalent compounds, or as acids NaBr SO2 HF P3O8 HC2H3O2 REMINDER Acids – begin with a hydrogen (HCl) Covalent – non-metal bonded with non-metal Ionic – metal bonded with a non-metal or polyatomic ion

Identify the compounds below as ionic compounds, covalent compounds, or as acids NaBr SO2 HF P3O8 HC2H3O2 REMINDER Acids – begin with a hydrogen (HCl) Covalent – non-metal bonded with non-metal Ionic – metal bonded with a non-metal or polyatomic ion

Identify the compounds below as ionic compounds, covalent compounds, or as acids WP2 NaCN HNO3 BeF2 CO2 REMINDER Acids – begin with a hydrogen (HCl) Covalent – non-metal bonded with non-metal Ionic – metal bonded with a non-metal or polyatomic ion

Identify the compounds below as ionic compounds, covalent compounds, or as acids WP2 NaCN HNO3 BeF2 CO2 REMINDER Acids – begin with a hydrogen (HCl) Covalent – non-metal bonded with non-metal Ionic – metal bonded with a non-metal or polyatomic ion

Identify the compounds below as ionic compounds, covalent compounds, or as acids HClO4 Cu2O ZnCl2 Ca(IO3)2 H2O REMINDER Acids – begin with a hydrogen (HCl) Covalent – non-metal bonded with non-metal Ionic – metal bonded with a non-metal or polyatomic ion

Identify the compounds below as ionic compounds, covalent compounds, or as acids HClO4 Cu2O ZnCl2 Ca(IO3)2 H2O REMINDER Acids – begin with a hydrogen (HCl) Covalent – non-metal bonded with non-metal Ionic – metal bonded with a non-metal or polyatomic ion

Naming Acids Chemical formula starts with HYDROGEN (H) Water (H2O) is NOT AN ACID Examples: HCl HF H2CO3 HClO

Naming Acids Look at the negative (anion) part of the acid to determine if it is: An element A polyatomic ion ending in –ate (from page 7 of your chemistry reference table) A polyatomic ion ending in –ite (from page 7 of your chemistry reference table)

Naming Acids If is is an element: Hydro (element) ic acid HCl  Hydro ic acid 2) HF  Hydro ic acid

Naming Acids If is is an element: Hydro (element) ic acid HCl  Hydrochloric acid 2) HF  Hydrofluoric acid

Naming Acids A polyatomic ion ending in –ate (name of polyatomic ion, minus –ate)ic acid H2CO3  (name of CO32-) ic acid

Naming Acids A polyatomic ion ending in –ate (name of polyatomic ion, minus –ate)ic acid H2CO3  Carbonic acid

Naming Acids A polyatomic ion ending in –ite (name of polyatomic ion, minus –ite)ous acid HClO  (name of ClO-) ous acid

Naming Acids A polyatomic ion ending in –ite (name of polyatomic ion, minus –ite)ous acid HClO  Hypochlorous acid

Naming Acids Try a few on your own! HClO4 HClO3 H2S HNO2 HCN HI H2SO4

Naming Acids Try a few on your own! HClO4  perchloric acid HClO3  chloric acid H2S  hydrosulfuric acid HNO2  nitrous acid HCN  hydrocyanic acid HI  hydroiodic acid H2SO4  sulfuric acid

Writing ACID formulas Write the symbol(s) for the negative part. Find the charge for the negative part (anion). After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript) to make the compound neutral.

Writing ACID formulas Practice! Hydrochloric acid Nitrous acid Write the symbol(s) for the negative part. Find the charge for the negative part (anion). After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript) Practice! Hydrochloric acid Nitrous acid Acetic acid Hydroselenic acid Permanganic acid

Writing ACID formulas Practice! Hydrochloric acid  HCl Write the symbol(s) for the negative part. Find the charge for the negative part (anion). After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript) Practice! Hydrochloric acid  HCl Nitrous acid  HNO2 Acetic acid  HC2H3O2 Hydroselenic acid  H2Se Permanganic acid  HMnO4

Writing ACID formulas Practice! 6. Hypochlorous acid Write the symbol(s) for the negative part. Find the charge for the negative part (anion). After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript) Practice! 6. Hypochlorous acid 7. Hydrocyanic acid 8. Chromic acid 9. Phosphoric acid 10. Hydrosulfuric acid

Writing ACID formulas Practice! 6. Hypochlorous acid  HClO Write the symbol(s) for the negative part. Find the charge for the negative part (anion). After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript) Practice! 6. Hypochlorous acid  HClO 7. Hydrocyanic acid  HCN 8. Chromic acid  H2CrO4 9. Phosphoric acid  H3PO4 10. Hydrosulfuric acid  H2S

Ionic Compounds This is a bond between a metal and non-metal OR involving a polyatomic ion (ex.  NH4+)

Ionic Compounds This is a bond between a metal and non-metal OR involving a polyatomic ion (ex.  NH4+) Write the name of the first element or polyatomic ion Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide Add a roman numeral if the metal is a transition or inner transition metal (in the middle block) to identify the metals charge! Exceptions: Ag1+, Zn2+, Cd2+, Al3+

Ionic Compounds NaCl K2S MgSO4 Mn(OH)2 Li2S Write the name of the first element or polyatomic ion Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A) Exceptions: Ag1+, Zn2+, Cd2+, Al3+

Ionic Compounds NaCl  sodium chloride K2S  potassium sulfide MgSO4  magnesium sulfate Mn(OH)2  manganese (II) hydroxide Li2S  lithium sulfide Write the name of the first element or polyatomic ion Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A) Exceptions: Ag1+, Zn2+, Cd2+, Al3+

Ionic Compounds CaBr2 Ni(CN)2 HgI2 Fe2(SO4)3 TiCl3 Write the name of the first element or polyatomic ion Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A) Exceptions: Ag1+, Zn2+, Cd2+, Al3+

Ionic Compounds CaBr2  calcium bromide Ni(CN)2  nickel (II) cyanide HgI2  mercury (II) iodide Fe2(SO4)3  iron (III) sulfate TiCl3  titanium (III) chloride Write the name of the first element or polyatomic ion Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A) Exceptions: Ag1+, Zn2+, Cd2+, Al3+

Writing IONIC formulas Write the symbol and find the charge of the positive side (cation) Write the symbol and write the charge of the negative side (anion) Determine how many of each ion are needed to make a neutral compound. Erase the charges of each ion and add subscripts to show the number of each ion needed. Write the cation first! If a polyatomic ion needs a subscript, put parentheses around the ion formula!

Writing IONIC formulas Write the symbol and find the charge of the positive side (cation) Write the symbol and write the charge of the negative side (anion) Determine how many of each ion are needed to make a neutral compound. Erase the charges of each ion and add subscripts to show the number of each ion needed. Write the cation first! If a polyatomic ion needs a subscript, put parentheses around the ion formula! Practice! Sodium bromide Lithium sulfide Potassium iodide Copper (II) chloride Beryllium phosphide

Writing IONIC formulas Write the symbol and find the charge of the positive side (cation) Write the symbol and write the charge of the negative side (anion) Determine how many of each ion are needed to make a neutral compound. Erase the charges of each ion and add subscripts to show the number of each ion needed. Write the cation first! If a polyatomic ion needs a subscript, put parentheses around the ion formula! Practice! Sodium bromide = NaBr Lithium sulfide = Li2S Potassium iodide = KI Copper (II) chloride = CuCl2 Beryllium phosphide = Be3P2

Writing IONIC formulas Write the symbol and find the charge of the positive side (cation) Write the symbol and write the charge of the negative side (anion) Determine how many of each ion are needed to make a neutral compound. Erase the charges of each ion and add subscripts to show the number of each ion needed. Write the cation first! If a polyatomic ion needs a subscript, put parentheses around the ion formula! Practice! Lead (II) nitrate Calcium carbonate Magnesium hydroxide Sodium phosphate Magnesium acetate

Writing IONIC formulas Practice! Lead (II) nitrate = Pb(NO3)2 Calcium carbonate = CaCO3 Magnesium hydroxide = Mg(OH)2 Sodium phosphate = Na3PO4 Magnesium acetate = Mg(C2H3O2)2 Write the symbol and find the charge of the positive side (cation) Write the symbol and write the charge of the negative side (anion) Determine how many of each ion are needed to make a neutral compound. Erase the charges of each ion and add subscripts to show the number of each ion needed. Write the cation first! If a polyatomic ion needs a subscript, put parentheses around the ion formula!

Covalent Compounds A non-metal bonded to another non-metal

Covalent Compounds A non-metal bonded to another non-metal Name first element (add a prefix if there is more than one of that element) Add a prefix and write the name of the second element. Change the suffix to -ide

Covalent Compounds Name first element (add a prefix if there is more than one of that element) Add a prefix and write the name of the second element. Change the suffix to –ide Practice! SO2 N2O4 P4O10 NO2 N2Cl4

Covalent Compounds 1. Name first element (add a prefix if there is more than one of that element) 2. Add a prefix and write the name of the second element. Change the suffix to -ide SO2  sulfur dioxide N2O4  dinitrogen tetroxide P4O10  tetraphosphorous decoxide NO2  nitrogen dioxide N2Cl4  dinitrogen tetrachloride

Covalent Compounds Name the first element (add a prefix if there is more than one of that element) Add a prefix and write the name of the second element. Change the suffix to -ide Practice! SO3 ClO2 CS2 XeF2 S2Cl2

Covalent Compounds Name first element (add a prefix if there is more than one of that element) Add a prefix and write the name of the second element. Change the suffix to -ide Practice! SO3  sulfur trioxide ClO2  chlorine dioxide CS2  carbon disulfide XeF2  xenon difluoride S2Cl2  disulfur dichloride

Writing COVALENT formulas Write the symbol for the first element. If there is a prefix add that number as the subscript. Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono).

Writing COVALENT formulas Write the symbol for the first element. If there is a prefix add that number as the subscript. Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono) Practice! Boron trichloride Dinitrogen monoxide Dihydrogen monoxide Carbon monoxide Carbon dioxide

Writing COVALENT formulas Write the symbol for the first element. If there is a prefix add that number as the subscript. Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono) Practice! Boron trichloride  BCl3 Dinitrogen monoxide  N2O Dihydrogen monoxide  H2O Carbon monoxide  CO Carbon dioxide  CO2

Writing COVALENT formulas Write the symbol for the first element. If there is a prefix add that number as the subscript. Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono) Practice! Sulfur trioxide Phosphorus trihydride Diphosphorus tetrabromide Silicon dioxide Sulfur hexafluoride

Writing COVALENT formulas Write the symbol for the first element. If there is a prefix add that number as the subscript. Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono) Practice! Sulfur trioxide  SO3 Phosphorus trihydride  PH3 Diphosphorus tetrabromide  P2Br4 Silicon dioxide  SiO2 Sulfur hexafluoride  SF6