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Naming & Writing Formulas

Naming & Writing Formulas. For Molecular & Ionic Compounds. Naming Molecular Compounds. Non-metal + Non-metal Step 1: write the element name for the first non-metal add a prefix ….(if there is more than one atom) Step 2: Write the second element name and add an ide ending

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Naming & Writing Formulas

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  1. Naming &Writing Formulas For Molecular & Ionic Compounds

  2. Naming Molecular Compounds Non-metal + Non-metal • Step 1: • write the element name for the first non-metal • add a prefix ….(if there is more than one atom) • Step 2: • Write the second element name and add an ide ending • Add a prefix

  3. Exceptions hexa mono 1 = 6 = 2 = 7 = 3 = 8 = 4 = 9 = 5 = 10 = hepta di tri octa tetra nona penta deca • DO NOT use any prefixes at all if the first element is hydrogen ……these are acids Prefixes

  4. Examples BrH7 P4O10tetraphosphorus decaoxide bromine heptahydride H2S hydrogen sulfide

  5. Try the Following CO(g) CO2(g) N3F8 carbon monoxide carbon dioxide Trinitrogen octafluoride

  6. Writing Formulas for Molecular Compounds Steps: Write each elements symbol Write the subscript number (the prefix) E.g. dinitrogen oxide N2O Sulfur dioxide S20

  7. Try the Following oxygen dibromide diphosphorus pentasulphide carbon tetraiodide phosphorus pentachloride OBr2 P2S5 CI4 PCl5

  8. Molecular Compounds that Must be memorized !!! NH3( g) = ammonia H2O ( l) = water H2S ( g) = hydrogen sulphide CH4 ( g) = methane CH3OH ( l) = methanol C2H6 ( g) = ethane C2H5OH ( l) = ethanol C6H12O6 ( s) = glucose C12H22O11 ( s) = sucrose O3 ( g) = ozone hydrogen peroxide H2O2 ( l) =

  9. Naming Binary Ionic Compounds Metal + non-metal • DO NOT USE PREFIXES • Steps 1.Write the metal 1st 2. Write the non-metal 2nd with an ide ending

  10. E.g. NaF Na2S sodium fluoride sodium sulphide two sodium ions are bonded with one sulphide ion… this doesn’t matter for naming ionic compound

  11. Try the Following LiF KCl BeS Rb3P MgF2 Na2O CsBr lithium fluoride potassium chloride beryllium sulphide rubidium phosphide magnesium fluoride sodium oxide cesium bromide

  12. Try the Following potassium chloride magnesium bromide barium nitride scandium phosphide KCl MgBr2 Ba3N2 ScP

  13. Writing Formulas for Binary Ionic Compounds • Steps 1.Look up the symbol for each…& write the metal first 2.Balance the charges (total + charges = total – charges) 3.Use subscripts to show the # of each element

  14. sodium oxide 2  Charge 1+ Charge 1+2= 2+ 21 = 2 Na2O

  15. calcium phosphide 3  Charge 2+ Charge 3 2 = 6  2+3= 6+ Ca3P2

  16. Try the Following MgCl2 CaCl2 ZnS Ag2S GeO2 Ca3As2 Mg3N2 magnesium chloride calcium chloride zinc sulphide silver sulphide germanium oxide calcium arsenide magnesium nitride

  17. Try the Following LiI ZnF2 Sr3P2 Ag2O Ge3As4 lithium iodide zinc fluoride strontium phosphide silver oxide germanium arsenide

  18. Naming Multivalent Ionic Compounds transition metal + non-metal Cu2+, Cu+, Fe3+, Fe2+ Transition metal ions have more than one possible charge

  19. Roman Numerals (I,II,III,IV,V,VI,VII) • Steps 1. Write metal 1st with the charge in roman numerals 2.Write non-metal second remember the charges have to balance

  20. Examples UF6 • uranium (VI) fluoride • chromium (III) nitride • cobalt (II) chloride • U6+ F– • Cr3+ N3- • Co2+ Cl- CrN CoCl2

  21. Try the Following gold (I) bromide chromium (II) chloride cobalt (III) oxide vanadium (IV) sulphide plutonium (VI) nitride AuBr CrCl2 Co2O3 VS2 PuN2

  22. Naming Complex Ions E.g.) PO43 Note: NH4+ (ammonium ion) is the only positive complex ion…it will take the place of a metal Metal + complex ion • Steps: 1. Name the metal ion 2. Name the complex ion

  23. Examples CaCO3 Ba(OH)2 (NH4)3N

  24. Solutions • CaCO3 • Ba(OH)2 • (NH4)3N Calcium carbonate Barium hydroxide Ammonium nitride

  25. Try the Following potassium iodate sodium acetate magnesium sulphite ammonium nitrate calcium phosphate KIO3 NaCH3COO MgSO3 NH4NO3 Ca3(PO4)2

  26. Writing Formulas For Complex Ions 2+ 1 - • Steps: 1. Look up the symbol for each ion 2. Balance the charges • Note: if you need more than 1 complex ion to balance the charges use brackets • E.g. Ca(CH3COO)2

  27. Try the Following AlPO4 CaSO3 Sc(CH3COO)3 (NH4)2SO4 Ni3(PO4) 2 Al(ClO3)3 aluminum phosphate calcium sulphite scandium acetate ammonium sulphate nickel (II) phosphate aluminum chlorate

  28. Solubility Will the compound dissolve in water?

  29. Soluble Refers to whether or not the compound dissolves in water If it is…. the compound is aqueous (aq) All acids are soluble Some ionic compounds are soluble… the rest are solids

  30. Is It soluble? • This will apply to ionic compounds (only) • Steps 1. Find each ion in the boxes across the top 2. if it is soluble it will have (aq) aqueous 3. If it does not dissolve it will have (s) solid.

  31. Determine if the following compounds are soluble in water. Use the proper subscript to indicate the state. • AgCl • BaCO3 • LiOH • Ca2(PO4)3 • NaCl • CaI2 • Pb(NO3)2 • HMnO4

  32. AgCl • BaCO3 • LiOH • Ca2(PO4)3 • NaCl • CaI2 • Pb(NO3)2 • HMnO4 (s) (s) (aq) (s) (aq) (aq) (aq) (aq)

  33. Acids & Bases

  34. Acids They are always soluble in water Conduct electricity Taste sour React with metals to produce hydrogen gas (H2(g)) Neutralize a base

  35. they ALWAYS have hydrogen ….usually as the first element • E.g. HCl(aq) , H3PO4(aq) • There are three types: • Binary • Oxo • Organic

  36. Binary Acids contain only H and one other element (Cl, Br, etc.) E.g. HCl (aq)

  37. Oxo Acids Contain H and Oxygen E.g. H3PO4(aq)

  38. Organic Acids Contain C, H, & O The H is written at the end All have COO- E.g. CH3COOH(aq) – acetic acid

  39. C6H5COOH(aq) - benzoic acid HOOCCOOH(aq) – oxalic acid

  40. Acid Indicators Turns blue litmus paper red Able to turn bromothymol blue to yellow Phenolphthalein remains colorless E.g. lemon juice

  41. Bases Are usually soluble in water Conduct electricity (not weak ones) Neutralize acids Taste bitter Usually solids Feel slippery

  42. Base Indicators Turns red litmus paper blue Bromothymol blue remains blue Turns phenolphthalein pink E.g. baking soda, Rolaids, soap, Draino crystals

  43. Naming Acids • Steps: • Hydrogen ____ide becomes hydro____ic acid • Hydrogen ____ate becomes _______ic acid • Hydrogen ____ ite becomes _______ ous acid

  44. Examples hydrogen fluoride = hydrofluoric acid hydrogen sulphite = sulphurous acid hydrogen borate = boric acid Hydrogen chloride (not an acid) • HF (aq) • H2SO3 (aq) • H3BO3 (aq) • HCl (g)

  45. Try the Following hydrosulphuric acid phosphorus acid       carbonic acid hydrogen sulphide H2S (aq) 1+ 2- hydrogen phosphite H3PO3 (aq) 1+ 3- hydrogen carbonate H2CO3(aq) 1+ 2-

  46. Writing Acid Formulas H2S(aq) hydrogen sulphide • Steps: 1. Use the naming rules in the opposite direction • Example: hydrosulphuric acid

  47. Try the Following hydrogen carbonate H2CO3(aq) hydrogen chlorite HClO2(aq) carbonic acid chlorous acid

  48. Naming Bases • Steps: 1. Write the metal name 1st 2. Write hydroxide or bicarbonate E. g. NaOH sodium hydroxide

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