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Names & Formulas of Ionic Compounds

Names & Formulas of Ionic Compounds. Ionic compounds are named using the names of the ions that compose them. To name an ionic compound: Cation name followed by anion name Learn the names and formulas of the ions in your syllabus.

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Names & Formulas of Ionic Compounds

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  1. Names & Formulas of Ionic Compounds • Ionic compounds are named using the names of the ions that compose them. • To name an ionic compound: Cation name followed by anion name • Learn the names and formulas of the ions in your syllabus. • The following slides explain the systematic way that ions are named.

  2. Naming Cations • Cations formed from metal ions have the same name as the metal. K+ potassium ion Ca2+ calcium ion Al3+ aluminum ion

  3. Naming Cations • Cations with varying charges • the charge of the specific cation is given by Roman numeral in parentheses after the name of the metal Fe2+ iron (II) ion Fe3+ iron (III) ion Cu+ copper (I) ion Cu2+ copper (II) ion

  4. Naming Cations • One common polyatomic cation found in ionic compounds NH4+ ammonium ion • Note:Compounds whose formulas start with NH4 are ionic even though they are composed only of non-metals.

  5. Naming Anions • Monoatomic anions • drop the ending of the element’s name • add “ide” N nitrogen O oxygen N3- O2- nitride oxide

  6. Naming Anions • Some simple polyatomic anions use the “ide” ending as well OH- hydroxide CN- cyanide O22- peroxide

  7. Naming Oxyanions • Oxyanions (polyatomic anions containing oxygen) have names ending in: • “ate” most common oxyanion of the element • “ite” same charge, 1 less oxygen NO3- nitrate SO42- sulfate NO2- nitrite SO32- sulfite CO32- carbonate PO43- phosphate PO33- phosphite

  8. Oxyanions (cont.) • Some elements like the halogens can form more than two oxyanions: • “per” 1 more O than the “ate” oxyanion • “hypo” 1 less O than the “ite” oxyanion ClO4- perchlorate ClO3- chlorate ClO2- chlorite ClO- hypochlorite

  9. Oxyanions • Anions derived by adding H+ to an oxyanion: • add “hydrogen” or “dihydrogen” as prefix to oxyanion name CO32- carbonate HCO3- hydrogen carbonate (usually called bicarbonate) PO43- phosphate H2 PO4- dihydrogen phosphate

  10. Naming Ionic Compounds • Name ionic compounds using cation name followed by anion name NaCl sodium chloride CaBr2 calcium bromide NaClO sodium hypochlorite Cu(NO3)2 copper (II) nitrate

  11. Naming Ionic Compounds Example: Write the names of these ionic compounds. • Na2O • FeCl3 • (NH4)3PO4 • KClO4 • SnO2 • Cu(NO3)2

  12. Writing Formulas from Names • Given the name of a compound, you must be able to write its formula. • Identify the symbol and charge for each ion. • Determine the correct number of each ion needed to balance the charges (write an electrically neutral formula).

  13. SO42- NH4+ NH4+ Writing Formulas from Names Example: Write the empirical formula for ammonium sulfate ammonium sulfate NH4+ (NH4)2SO4 SO42-

  14. Writing Formulas from Names Example: Write the formulas for these ionic compounds • lithium chloride • barium nitrate • sodium perchlorate • iron(III) oxide • sodium hydrogen phosphate • Lead (IV) sulfate

  15. Names & Formulas of Acids • Acid: a substance whose molecules form H+ ions when dissolved in water • HCl (aq) • HCN (g) • HClO3 (aq) • Name of acid depends on: • Type of acid • Oxygen present or not • Pure or aqueous • Name of anion

  16. Names & Formulas of Acids • Three naming systems for acids: • Oxyanion-based acids (with oxygen) • Acids with “ide” anions (no oxygen) • aqueous solutions • gases

  17. Oxyanion Based Acids • If the acid contains oxygen, identify the anion and write its name • Change the ending of the anion name: • “ite”  “ous acid” • “ate”  “ic acid” HClO4 perchlorateperchloricacid HClO2 chloritechlorousacid

  18. Oxyanion Based Acids • Naming acids derived from oxyanions of S and P: • H2SO4 : • oxyanion = sulfate • Sulfic acid Sulfuric acid • H3PO4 : • oxyanion = phosphate • Phosphic acid Phosphoricacid

  19. Acids Without Oxyanions • If the acid does not contain oxygen and is dissolved in water (aq): hydro + (anion name minus “ide”) + “ic acid” HCl (aq) hydro + chloride + ic acid hydrochloric acid “Hydro”= no oxygen and (aq)

  20. Acids Without Oxyanions • If the acid does not contain oxygen and is a gas (g): • name the acid as an ionic compound: • hydrogen followed by anion name HCl (g)hydrogen chloride “Hydrogen”= no oxygen and (g)

  21. Naming Acids • To name an acid: • Does it have oxygen? • Yes • Write name of anion • Change “ate” to “ic acid” • Change “ite” to “ous acid” • If no oxygen, is it (aq)? • Yes • Start with hydro • Add the name of anion • Change “ide” to “ic acid”

  22. Naming Acids • If no oxygen, is it (g)? • Yes • Start with hydrogen • Add the name of the anion

  23. Naming Acids Example: Name the following acids. • HNO3 • HBr (aq) • H2S (g)

  24. Writing Formulas from Acid Names • To write the formula of an acid starting with the name of the acid, first decide which category of acid it is: • Oxyanion based • No oxygen, (aq) (begins with “hydro”) • No oxygen, (g) (begins with “hydrogen”) • Write the formula for the anion (including charge). • Add enough H+ ions to make a neutral compound.

  25. ClO4- H+ Writing Formulas from Acid Names Example: Write the formula for perchloric acid. Category: oxyanion containing acid Anion: perchloric acid  perchlorate (ClO4-) Formula: HClO4

  26. Writing Formulas from Acid Names Example: Write the formula for each of the following acids. • Phosphoric acid: • Hydrobromic acid: • Hydrogen cyanide:

  27. Naming Acids • You must know the names and formulas for the following acids: HF (aq)hydrofluoricacid HCl (aq)hydrochloricacid HBr (aq)hydrobromicacid HI (aq)hydroiodicacid HClO4perchloricacid HClO3chloricacid H2SO4sulfuricacid HNO3nitricacid

  28. Naming Acids • You must know the names and formulas for the following acids: H3PO4phosphoric acid HC2H3O2acetic acid H2CO3carbonic acid H2S (g)hydrogen sulfide HCN (g)hydrogen cyanide

  29. Binary Molecular Compounds • Binary molecular compound: compound composed of molecules with two different types of atoms • Remember: Many molecular compounds are composed strictly of non-metals. SO2 N2O4 H2O PCl5 P4O10 CO

  30. Binary Molecular Compounds • The names of binary molecular compounds give both the type and number of each type of atom present. • The general pattern for naming binary molecular compounds is: prefix element name prefix element name with ide ending

  31. Binary Molecular Compounds • The first element is named using the name of the element. • The second element is named using the “ide” ending. • Greek prefixes are used to indicate the number of each type of element present. prefix element name prefix element name with ide ending

  32. Greek Prefixes Prefix Meaning mono 1 di 2 tri 3 tetra 4 penta 5 hexa 6 hepta 7 octa 8 nona 9 deca 10 You must know these!! P4S10 = tetraphosphorus decasulfide

  33. Binary Molecular Compounds • Special conventions for using Greek prefixes: • Mono is never used with the first element • The “a” or “o” in the prefix is dropped if the name of the element begins with a vowel. • CO: • carbon monooxide • carbon monoxide

  34. Binary Molecular Compounds Example: Name the following compounds. • N2O4 • PCl5 • Cl2O7

  35. Binary Molecular Compounds Example: Write the formulas for the following compounds. • tetraphosphorus decoxide • sulfur trioxide • disulfur dichloride

  36. Naming — Revisited • Before you can correctly name a compound or write its formula, YOU MUSTdetermine which type of compound it is: • Ionicstarts with a metal orNH4 • Acidstarts with H or Hn • Binary Moleculartwo non-metals • THEN use the appropriate naming system or method to write the formula.

  37. Simple Organic Compounds • Organic compounds: • compounds that contain carbon and hydrogen, often in combination with oxygen or nitrogen.

  38. Simple Organic Compounds • You must know the names and structural formulas of the following simple organic compounds: • Methane • Propane • Methanol • Ethanol • Acetic acid • Acetone

  39. Simple Organic Compounds • Methane: • Ethane: • Methanol: • Ethanol:

  40. Simple Organic Compounds • Propane: • Acetic Acid: • Acetone:

  41. Common “Household” Chemicals • You are responsible for knowing the names and formulas for the chemical present in: • Water (H2O) • Ammonia (NH3) • Baking soda • sodium bicarbonate • NaHCO3 • Natural gas • Methane • CH4 • Vinegar • Acetic acid • HC2H3O2 (structure on previous slide)

  42. Common “Household” Chemicals • You are responsible for knowing the names and formulas for the chemical present in: • Table salt • Sodium chloride • NaCl • Bleach • Sodium hypochlorite • NaClO • Hydrogen peroxide • H2O2

  43. Common “Household” Chemicals • You are responsible for knowing the names and formulas for the chemical present in: • Drinking alcohol • Ethanol • C2H5OH • Rubbing alcohol • Isopropyl alcohol • Nail polish remover • Acetone

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