1Types of Chemical Compounds Classify the following compounds as ionic or molecular (covalent). 1. CaCl2 _______ionic________ 11. MgO ____________________ 2. CO2 ____________________ 12. NH4Cl ____________________ 3. H2O ____________________ 13. Sr(NO3)2 ____________________ 4. Na2SO4 ____________________ 14. KI ____________________ 5. K2O ____________________ 15. Ba(OH)2 ____________________ 6. NaF ____________________ 16. NO2 ____________________ 7. Na2CO3 ____________________ 17. Ca3(PO4)2 ____________________ 8. CH4 ____________________ 18. FeCl3 ____________________ 9. Mg(NO3)2 ____________________ 19. P2O5 ____________________ 10. LiBr ____________________ 20. N2O3 ____________________ Binary Ionic Compounds – Compounds with monatomic ions in it, a metallic ion and a nonmetallic ion. This allows only two types of atoms in the formula. Ex: Rb2O Ternary Ionic Compounds – Compounds with at least one polyatomic ion in it. This allows three or more types of atoms in the formula. Ex: RbNO3 Classify the following compounds as binary ionic or ternary ionic. 21. KOH ____ternary ionic___________ 26. Na2Cr2O7 _______________________ 22. CoO _________________________ 27. MgSO4 _________________________ 23. Fe(NO3)2 _______________________ 28. Cu2S _________________________ 24. MgH2 _________________________ 29. SnO2 _________________________ 25. Cs2S _________________________ 30. NH4NO3 ________________________ Naming Ions Polyatomic Ions Rule: Look up the name or symbol from your polyatomic ion sheet. Example 1: ammonium ion ____________________ Example 2: NO3- ____________________ Example 3: NO2 ____________________ Monatomic Ions • CATIONS Rule A: If the atom always forms the same charge when forming an ion, (all group 1, group 2, and Zn2+, Ag+, Cd2+, & Al3+), take the name of the atom that the ion is formed from, and add “ion”. Example 4: Na+ ____________________ Example 5: Mg2+ ____________________ Example 6: aluminum ion ____________________ Rule B: If the atom can form more than one charge when forming an ion, (any of the transition metals and any metals underneath the staircase), take the name of the atom that the ion is formed from, place the charge as a Roman numeral in parentheses, and then add “ion”. Example 7: Pb2+ _________________ Example 9: copper(I) ion __________ Example 8: Fe2+ _________________ Example 10: copper(II) ion _________ 15. Fe3+ ____________________ Try These: 11. Rb+ ____________________ 16. cobalt(II) ion _________________ 12. Ca ____________________ 13. Ni+ ____________________ 14. Ag+ ____________________ 2+ 17. lithium ion ________________ 18. zinc ion _________________ • ANIONS Rule: Take the nonmetal atom name, remove the ending and add “-ide ion” to it. Example 21: S2- ____________________ Example 22: N3- ____________________ Example 23: bromide ion ____________________ Example 24: telluride ion ____________________ Example 25: iodide ion ____________________ Example 26:selenide ion ____________________ Example 27:F- ____________________ Example 28:O2- ____________________ Let’s Compare some ions: N3- ____________________ sulfide ion ____________________ sulfite ion ____________________ sulfate ion ____________________ NO2- ____________________ NO3- ____________________ Understanding Ion Nomenclature IONS CATIONS MONATOMIC *one possible charge *Groups 1 & 2 and others POLYATOMIC *more than one possible charge Na+ sodium ion Fe2+ Ca2+ calcium ion Fe3+ + Ag silver ion Cu+ 2+ Zn zinc ion Cu2+ Cd2+ cadmium ion Al3+ aluminum ion ANIONS iron(II) ion iron(III) ion copper(I) ion copper(II) ion *few NH4+ ammonium ion MONATOMIC *ends in –IDE Cl- chloride ion O2- oxide ion N3- nitride ion POLYATOMIC *ends in –ITE -ATE or –IDE (a few) SO32- sulfite ion SO42- sulfate ion CN- cyanide ion Monatomic cation with one possible charge – Name of atom and add “ion” Monatomic cation with more than one possible charge – Name of atom, with charge as Roman numeral in parentheses, and add “ion” Monatomic anion – Name of atom, remove ending, and add “-ide ion” Polyatomic ions – no naming rules…just know them Ions ‐ Worksheet Name the following ions. 1. Ca2+ ______________________________ 2. O2- ______________________________ 3. H+ ______________________________ 4. H- ______________________________ 5. Cu+ ______________________________ 6. Fe3+ ______________________________ 7. CO32- ______________________________ 8. NH4+ ______________________________ 9. Zn2+ ______________________________ 10. N3- ______________________________ Write the formulas for the following ions. 11. acetate ion ______________________________ 12. phosphide ion ______________________________ 13. phosphate ion ______________________________ 14. iron(II) ion ______________________________ 15. strontium ion ______________________________ 16. nickel(II) ion ______________________________ 17. tin(II) ion ______________________________ 18. sulfate ion ______________________________ 19. sulfite ion ______________________________ 20. sulfide ion ______________________________ Microsoft Word - Chemical Formulas All Worksheets 2011.docx | [Document subtitle] Ionic Compound Nomenclature ALL COMPOUNDS ARE NEUTRAL! When ions combine, they will form neutral compounds. These formulas are written in the lowest, wholenumber ratio. These lowest, whole-number ratios are called “formula units”. An ionic compound is often referred to as a “salt”. One of the most common ionic compounds is NaCl. This is why we usually refer to it as salt or table salt. When determining the formula for an ionic compound, determine the charges of each ion and be sure to combine them so that the number of positive charges is equal in magnitude to the number of negative charges. Example: Al2O3 - aluminum oxide It is made of two Al3+ ions (aluminum ions) and three O2- ions (oxide ions). 2 Al3+ ions would make a total positive charge of +6. 3 O2- ions would make a total negative charge of -6. This makes a neutral compound. Ionic Compounds are named after the ions they contain. Example: CaI2 This contains 1 Ca2+ ion and 2 I- ions. They are written in a 1:2 ratio in the compound so it is neutral. However, when naming the compound, just write the names of the two types of ions. So the name is calcium iodide. Example: MnO2 This contains 1 Mn+4 ion and 2 O2- ions. I had to determine the charge on the Mn. It is a transition metal and needs a roman numeral in its name. I first looked at the O and knew it was a 2-. I then thought that if there were two 2- ions, then that would be a total negative charge of 4-. In order to make a neutral compound, the positives would have to add up to 4+. If there is only one Mn in the compound, then its entire charge would be 4+. So, the compound is made of manganese(IV) ions and oxide ions. The name is manganese (IV) oxide. Example: copper (I) sulfide This contains Cu+ ions and S2- ions. Two Cu+ ions are needed for each S2- ion, making Cu2S. Microsoft Word - Chemical Formulas All Worksheets 2011.docx | [Document subtitle] Binary Ionic Compounds – Worksheet #1 A. Write the formulas for the compounds formed from these elements. Remember, the cation is always written first. 1. rubidium and iodine ___________ 5. sulfur and sodium ___________ 2. barium and chlorine ___________ 6. aluminum and oxygen ___________ 3. lithium and selenium ___________ 7. silver and phosphorus ___________ 4. nitrogen and magnesium ____________ 8. fluorine and zinc ___________ B. Write the names for these binary ionic compounds. 9. Cs2S ____________________________ 16. FeF3 ___________________________ 10. BaO ___________________________ 17. Mg3N2 _________________________ 11. AlI3 ____________________________ 18. Ni3P2 ___________________________ 12. MnO2 __________________________ 19. UO2 ___________________________ 13. Tc3P4 __________________________ 20. HF ____________________________ 14. CdBr2 __________________________ 21. CoN ___________________________ 15. NaCl ___________________________ 22. K2S ____________________________ C. Write the formulas for these binary ionic compounds. 23. rubidium sulfide _______________ 30. europium(II) nitride ______________ 24. mercury(II) oxide _______________ 31. cesium phosphide _______________ 25. calcium nitride _______________ 32. lead(II) chloride _______________ 26. zinc bromide _______________ 33. cadmium oxide _______________ 27. uranium(VI) fluoride _____________ 34. tin(IV) fluoride _______________ 28. silver phosphide _______________ 35. iron(II) oxide _______________ 29. platinum(II) selenide ______________ 36. iron(III) oxide _______________ Microsoft Word - Chemical Formulas All Worksheets 2011.docx | [Document subtitle] Binary Ionic Compounds – Worksheet #2 If the name of the compound is given, write the formula. If the formula of the compound is given, write the name. 1. KBr ________________________________________ 2. V2O5 ________________________________________ 3. cobalt(III) oxide ________________________________________ 4. barium phosphide ________________________________________ 5. cadmium nitride ________________________________________ 6. Cu3P ________________________________________ 7. Ag2S ________________________________________ 8. Sn3N4 ________________________________________ 9. radium iodide ________________________________________ 10. beryllium selenide ________________________________________ 11. Fe2S3 ________________________________________ 12. SrO ________________________________________ 13. CrCl2 ________________________________________ 14. mercury(II) fluoride ________________________________________ 15. lead(IV) bromide ________________________________________ 16. CuSe ________________________________________ 17. FeP ________________________________________ 18. lithium oxide ________________________________________ 19. cobalt(III) fluoride ________________________________________ 20. CdI2 ________________________________________ Ternary Ionic Compounds ‐ Worksheet If the name of the compound is given, write the formula. If the formula of the compound is given, write the name. 1. calcium nitrite ________________________________________ 2. BaSO4 ________________________________________ 3. silver acetate ________________________________________ 4. SrSO3 ________________________________________ 5. nickel(II) phosphate ________________________________________ 6. Na2CO3 ________________________________________ 7. LiHCO3 ________________________________________ 8. ammonium phosphate ________________________________________ 9. Be(ClO)2 ________________________________________ 10. aluminum oxalate ________________________________________ 11. rubidium dichromate ________________________________________ 12. KHSO3 ________________________________________ 13. calcium hydroxide ________________________________________ 14. manganese(II) silicate ________________________________________ 15. HCN ________________________________________ 16. cesium hydrogen sulfate ________________________________________ 17. Ti(OH)4 ________________________________________ 18. ammonium chloride ________________________________________ 19. Ca(ClO3)2 ________________________________________ 20. rubidium cyanate ________________________________________ 21. copper(II) sulfate ________________________________________ 22. CuCl ________________________________________ 23. iron(II) arsenate ________________________________________ 24. NH4OH ________________________________________ Latin Nomenclature Some ions have Latin names for them that are commonly used. When there are two possible charges for similar ions, the lower of the two is the “-ous” ion and the higher of the two is the “-ic” ion. For your information, the Latin roots for the name of the metals are: Cu “cupr”, Fe “ferr”, Cr “chrom”, Sn “stann”, Co “cobalt”, and Pb “plumb”. Cu+ - copper(I) ion – cuprous ion Cu2+ - copper(II) ion – cupric ion 2+ Fe - iron(II) ion – ferrous ion Fe3+ - iron(III) ion - ferric ion Cr2+ - chromium(II) ion – chromous ion Cr3+ - chromium(III) ion – chromic ion 2+ Sn - tin(II) ion – stannous ion Sn4+ - tin(IV) ion – stannic ion Pb2+ - lead(II) ion – plumbous ion Pb4+ - lead(IV) ion – plumbic ion You must learn all of these Latin names. Remember the lower of the two is “ous” and the higher of the two is “ic”. Name the following compounds with both methods: 1. Fe2O3 iron(III) oxide ferric oxide 3.SnO2 ______________________________ 2. Cu2O ____________________ _ 4.PbO ___________________________ Hydrate Nomenclature hydrate – a compound that releases water when heated Example: CuSO4▪5H2O Cu SO4 ▪ 5 copper(II) sulfate part of the compound penta hydrate H2 O __magnesium sulfate heptahydrate_______ Example: MgSO4▪7H2O Example: aluminum chloride hexahydrate _____AlCl3▪6H2O________________ Name the following hydrates: 1. MgCl2▪6H2O = 2.Cd(NO3)2▪4H2O = 3.ZnCl2▪6H2O = 4.Na2S2O3▪5H2O = 5.CaCl2▪2H2O = Write the formulas for the following hydrates: 1.barium hydroxide octahydrate ______________________________ 2. sodium sulfate decahydrate ______________________________ 3. lithium chloride tetrahydrate ______________________________ 4. cobalt(II) chloride hexahydrate ______________________________ 5. sodium carbonate decahydrate ______________________________ All Ionic Compounds ‐ Worksheet If the name of the compound is given, write the formula. If the formula of the compound is given, write the name. 1. lead(II) nitrate ________________________________________ 2. sodium carbonate ________________________________________ 3. potassium iodide ________________________________________ 4. AgNO3 ________________________________________ 5. barium nitrate ________________________________________ 6. Na2SO3 ________________________________________ 7. potassium carbonate ________________________________________ 8. sodium nitrate ________________________________________ 9. barium acetate ________________________________________ 10. hydrogen peroxide ________________________________________ 11. potassium biphosphate ________________________________________ 12. Ba(OH)2 ________________________________________ 13. FeCl3 (use the Latin nomenclature)___________________________________ 14. Fe3(PO4)2 ________________________________________ 15. aluminum sulfate ________________________________________ 16. calcium hydroxide ________________________________________ 17. tin(II) oxide ________________________________________ 18. aluminum hydrogen carbonate ________________________________________ 19. sodium perchlorate ________________________________________ 20. copper(I) dichromate ________________________________________ 21. potassium selenide ________________________________________ 22. 22. ZnS ________________________________________ 23. stannic dichromate ________________________________________ 24. sodium hydrogen phosphate ________________________________________ 25. Fe(ClO)2 ________________________________________ 26. NH4CH3COO ________________________________________ 27. copper(II) nitrate ________________________________________ 28. potassium hypochlorite ________________________________________ 29. iron(III) chromate ________________________________________ 30. Ag2SO4 ________________________________________ Molecular Compound Nomenclature Molecular compounds are composed of individually covalently bonded atoms. The simplest unit of a molecular compound is called a “molecule”. These compounds are composed of all nonmetals. They are sometimes called covalent compounds. One system for naming these compounds is based on the use of prefixes. monodi- one two tritetrapentahexaheptaoctanonadeca- three four five six seven eight nine ten When naming the molecular compound, the prefix that indicates the number of each atom is placed before the atom in the name. All molecular compounds end in “-ide”. Example: N2O IS dinitrogen monoxide NOT dinitride monoxide (the first element does not end in “-ide”) NOT dinitrogen monoxygen (the second element should end in “-ide”) NOT dinitrogen monooxide (often the “o” is dropped before a vowel) Also, mono is not used to indicate one atom if it applies to the first atom. Example: CO IS carbon monoxide NOT monocarbon monoxide (no mono necessary to indicate the first) NOT carbon oxide (the mono is necessary to indicate the number of O) NOT carbon monooxide (often the “o” is dropped before a vowel) Molecular Compounds ‐ Worksheet If the name of the compound is given, write the formula. If the formula is given, write the name. 1. CF4 ________________________________________ 2. N2O5 ________________________________________ 3. CS2 ________________________________________ 4. SO3 ________________________________________ 5. P4O8 ________________________________________ 6. iodine tribromide ________________________________________ 7. chlorine dioxide ________________________________________ 8. sulfur hexafluoride ________________________________________ 9. difluorine octachloride ________________________________________ 10. tribromine nonatelluride ________________________________________ 11. H2O ________________________________________ 12. P2S4 ________________________________________ 13. N2O4 ________________________________________ 14. XeF4 ________________________________________ 15. SI4 ________________________________________ 16. carbon dioxide ________________________________________ 17. trinitrogen hexabromide ________________________________________ 18. diiodine heptaselenide ________________________________________ 19. CO ________________________________________ 20. dicarbon octafluoride ________________________________________ 21. P4O10 ________________________________________ 22. Si3N4 ________________________________________ 23. Cl2S7 ________________________________________ 24. NBr5 ________________________________________ 25. phosphorus trichloride ________________________________________ 26. PI3 ________________________________________ 27. disulfur trioxide ________________________________________ 28. PCl5 ________________________________________ 29. diiodine dichloride ________________________________________ 30. dinitrogen monoxide ________________________________________ 31. I4O9 ________________________________________ 32. dihydrogen monoxide ________________________________________ Acid Nomenclature If a hydrogen atom, H, (1p+, 1e-, 0no) loses an electron to become a hydrogen ion, H+, what is left? Only a proton is left. So, sometimes, a proton is written as H+. Often, an acid is referred to as a “proton donor”. If something is a proton donor, it has an H+ in the formula to donate to another substance during a chemical reaction. There are many definitions of acids. For naming purposes, we will only be naming acids that begin with “H” in the formula. Acids are said to be “aqueous”. Aqueous means something is dissolved in water. It is written as (aq), although acids are not always written with the (aq). binary acid – an acid that contains only two different elements: hydrogen and one of the more electronegative elements Example: HCl(aq) – hydrochloric acid oxyacid – an acid that contains hydrogen, oxygen and a third element, usually a nonmetal. Example: HNO3(aq) – nitric acid NAMING RULES: Since all the acids we are naming begin with a hydrogen ion, they are differentiated by the anion in the formula. If the anion is identified, then the acid can be named. -ide ions hydro__stem___ic acid Ex: HCl(aq) Cl- chloride ion hydrochloric acid -ite ions _____ stem _____ous acid Ex: HClO2(aq) ClO2- chlorite ion -ate ions _____ stem _____ic acid chlorous acid Ex: HClO3(aq) ClO3- chlorate ion chloric acid Sulfur and phosphorus are exceptions. For sulfur you place sulfur in the blank. For phosphorus, you place phosphor in the blank. When taking the name and writing the formula, be sure to combine the appropriate amount of H+ with the anion to make a neutral compound. Example: phosphoric acid phosphor-ic acid is from the phosph–ate ion, PO43Therefore the formula is H3PO4(aq). So, if the citrate ion is C6H5O73-, what is the formula for citric acid? More Acids… monoprotic acid diprotic acid triprotic acid polyprotic acid - ______________________________________________________________________________ Acids ‐ Worksheet If the name of the acid is given, write the formula. If the formula of the acid is given, write the name. 1. hydrocyanic acid ________________________________________ 2. dichromic acid ________________________________________ 3. hydrobromic acid ________________________________________ 4. nitrous acid ________________________________________ 5. sulfuric acid ________________________________________ 6. H2SiO3(aq)________________________________________ 7. HF(aq) ________________________________________ 8. H3PO3(aq) ________________________________________ 9. H2CO3(aq) ________________________________________ 10. H2S(aq) ________________________________________ 11. acetic acid ________________________________________ 12. sulfurous acid ________________________________________ 13. perchloric acid ________________________________________ 14. hydroselenic acid ________________________________________ 15. carbonic acid ________________________________________ 16. HClO(aq) ________________________________________ 17. HClO2(aq) ________________________________________ 18. H2C2O4(aq) ________________________________________ 19. H3P(aq) ________________________________________ 20. HMnO4(aq) ________________________________________ 21. hydrochloric acid ________________________________________ 22. chromic acid ________________________________________ 23. phosphoric acid ________________________________________ 24. HCl(g) ________________________________________ Chapter Review of All Naming If the name of the substance is given, write the formula. If the formula is given, write the name. 1. cadmium nitrate ______________________________ 2. chromate ion ______________________________ 3. dinitrogen monoxide ______________________________ 4. potassium bromide ______________________________ 5. nitrous acid ______________________________ 6. HPO42- ______________________________ 7. PCl3 ______________________________ 8. V2O5 ______________________________ 9. HClO4 ______________________________ 10. BaSO4 ______________________________ 11. sulfur hexafluoride ______________________________ 12. cuprous oxide ______________________________ 13. sulfuric acid ______________________________ 14. hydrogen peroxide ______________________________ 15. carbonate ion ______________________________ 16. BaO ______________________________ 17. HClO2 ______________________________ 18. SrSO3 ______________________________ 19. Fe ______________________________ 20. acetic acid ______________________________ 21. CBr4 ______________________________ 22. hypochlorite ion ______________________________ 23. (NH4)2SO4▪6H2O ______________________________ 24. calcium hydroxide ______________________________ 25. Na2CO3 ______________________________ 26. Cu3P ______________________________ 27. HI ______________________________ 28. lead(II) acetate ______________________________ Polyatomic Ion Practice (Some of these, you did not have to memorize.) NO2- __________________________________ hydroxide ion _______________ CO32- SCN- __________________________________ hydrogen sulfate ion ___________ __________________________________ hydrogen phosphate ion ________ __________________________________ hydrogen carbonate ion ________ __________________________________ chlorate ion _______________ H2PO4- __________________________________ B4O72HSO3- ammonium ion _______________ C2O42- H3O+ __________________________________ perchlorate ion _______________ __________________________________ hypochlorite ion ______________ __________________________________ nitrate ion _______________ AsO43- __________________________________ cyanide ion _______________ NH4+ __________________________________ sulfate ion _______________ MnO4- __________________________________ sulfite ion _______________ BO33- __________________________________ PO43- __________________________________ chlorite ion _______________ Cr2 O72 O22- __________________________________ _______________ I3- __________________________________ cyanate ion PO33- chromate ion _____________ acetate ion __________________________________ thiosulfate ion _______________ _______________