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Naming Ionic Compounds

Learn how to name ionic compounds by understanding the charges of metal and nonmetal ions, as well as the rules for naming polyatomic ions. Also, discover the process for determining the formula of an ionic compound from its name.

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Naming Ionic Compounds

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  1. Naming Ionic Compounds

  2. Chemical reactions occur when atoms gain, lose, or share electrons. Metals Nonmetals gain / accept Nonmetals _____________ electrons. This gives them a ____ charge. Negative ions are called ___________. _ anions Metals ________________ electrons. This gives them a ____ charge. Positive ions are called ___________. lose / donate + cations

  3. Remember that the charge of an ion can be determined by its place on the Periodic Table. +1 0 +4 or -4 +2 -2 -1 +3 -3 Look for the Roman Numeral!

  4. For each elements on your notes, predict the charge of its most common ion using the periodic table. -3 0 +2 +2 -1 0 +1 +2 -1 -2 +1 -1 -2 +1 -3 +1 -1 0

  5. Rules for Naming Ions When metals lose electrons they become ions, but their name does not change. Na Na+ + e- electron sodium sodium Mg Mg+2 + 2e- 2 electrons magnesium magnesium

  6. Rules for Naming Ions When nonmetals gain electrons they become ions, and their name does change. F + e- F- fluoride fluorine electron S + 2e- S-2 sulfur 2 electrons sulfide

  7. Rules for Naming Ions 1. The names of metals do not change. 2. Changing the name of nonmetals: root of element name + -ide = name of ion Examples: The name of chlorine’s ion: chlor- + -ide = chloride The name of nitrogen’s ion: nitr- + -ide = nitride

  8. Examples of naming ions: The name of calcium’s ion: calcium (The names of metals don’t change!) The name of oxygen’s ion: ox- + -ide = oxide The name of aluminum’s ion: aluminum (The names of metals don’t change!)

  9. Write the name of each of the ions on your notes. sulfide lithium nitride bromide potassium chloride oxide hydrogen (+), hydride (-)

  10. There are also ions that form after elements have shared electrons. These ions are known as polyatomic ions, and each polyatomic ion already has a name.

  11. Write the name of each of the polyatomic ions on your notes using your reference sheet as a guide. sulfate carbonate permanganate sulfite hydroxide nitrate

  12. Steps for Naming Ionic Compounds CaBr2 calcium bromide Step 1: Write the name of the metal ion. Step 2: Write the name of the nonmetal ion. Step 3: YOU ARE DONE! It is that easy.

  13. 1. NaF 2. MgO sodium fluoride magnesium oxide 3. SrCl2 4. Li2S strontium chloride lithium sulfide 5. CaO 6. KI calcium oxide potassium iodide

  14. When polyatomic ions are used, simply use the name of the polyatomic ion in the compound. 1. NH4F 2. CaSO4 ammonium fluoride calcium sulfate 3. Mg(NO3)2 4. NaOH magnesium nitrate sodium hydroxide

  15. Name the ionic compounds that are found on your notes. calcium chloride potassium sulfide potassium permanganate barium oxide ammonium chloride cesium chloride magnesium sulfate sodium bromide aluminum phosphide

  16. You can also determine the formula of an ionic compound from its name. To do this, you will need to use what you already know about the Periodic Table. magnesium iodide Mg I +2 - MgI2 Step 1: Write the symbol of the metal ion. Step 2: Write the symbol of the nonmetal ion. Step 3: Determine the charges using the periodic table. Step 4: Determine the formula from the ions.

  17. This is just as easy to do with polyatomic ions. You just need to use the name of the polyatomic ion. strontium nitrate Sr NO3 +2 - Sr(NO3)2 Step 1: Write the symbol of the metal ion. Step 2: Write the formula of the polyatomic ion. Step 3: Determine the charges using the periodic table and the table of polyatomic ions. Step 4: Determine the formula from the ions.

  18. Be very careful that you do not mix up the names of ions. This is very common for beginners to naming. Decide which name goes with each ion. nitrate N-3 NO3- nitride sulfide S-2 SO3-2 sulfite phosphate P-3 PO4-3 phosphide

  19. Remember that the names of transition metals include their charge because their charges are less predictable. What are the charges of the transition metals below: +2 +3 Iron (II) _______ Iron (III) _______ Copper (II) _______ Copper (I) _______ Tin (IV) _______ Tin (II) _______ Lead (II) _______ Lead (IV) _______ +2 +1 +4 +2 +2 +4 We know they are positive because metals are always positive.

  20. The charges of the transition metals are important when you are determining the formula of an ionic compound. iron (III) oxide Fe O +3 -2 Fe2O3 Step 1: Write the symbol of the cation. Step 2: Write the symbol of the anion. Step 3: Determine the charges using the periodic table and the roman numerals. Step 4: Determine the formula from the ions.

  21. Helpful Hint: If the ion ends in –ide, it is probably from the periodic table. If the ion ends in –ate or –ite, it is a polyatomic ion. Examples: sulfate sulfide sulfite SO4-2 S-2 SO3-2 nitride nitrite nitrate N-3 NO2- NO3-

  22. Write the formula of each of the ionic compounds named on your notes. KI SnCl4 BaSO4 NaCl SrS CuCO3 AlBr3 Li3N

  23. Naming Binary Covalent Compounds

  24. shared electrons Nonmetals Chemical reactions occur when atoms gain, lose, or share electrons. Sharing electrons creates a covalent bond Nonmetals can _______ electrons to form a covalent bond. This creates a ___________. share molecule

  25. Determining if a compound is ionic or covalent is easy. What elements do covalent compounds contain? Covalent compounds contain only nonmetals. What elements do ionic compounds contain? Ionic compounds contain a metal and a nonmetal.

  26. Decide whether the compounds on your notes are ionic or covalent. C C I I C I

  27. Important Facts: Because hydrogen only has 1 proton and 1 electron, it behaves differently than any other element on the periodic table of elements. Hydrogen can donate its 1 electron. H+ H2 Hydrogen can share electrons. Hydrogen can gain 1 electron. H- This means that hydrogen can act as either a metal or a nonmetal!

  28. There are 7 elements that exist in nature as diatomic molecules. What elements exist as diatomic molecules? H2, N2, O2, F2, Cl2, Br2, I2

  29. There are millions of covalent compounds. These can be classified into many different types of compounds. Each type of compound has a different set of rules for naming. You will be learning about the easiest type of covalent compound to name: Binary Covalent Compounds • Binary means 2. What does binary mean? Binary covalent compounds are between 2 different nonmetals.

  30. Nonmetals can share electrons in many different ways. This means that two nonmetals can create multiple compounds together. carbon and oxygen phosphorous and chlorine CO CO2 PCl3 PCl5 nitrogen and oxygen N2O4 N2O3 Each of these contains a different ratio of elements. Because of this, we have to make sure that the name of the compound explains the correct ratio.

  31. To show the correct ratio of elements, we use prefixes.

  32. Steps for Naming Binary Covalent Compounds N2O4 dinitrogen tetroxide nitrogen oxide Step 1: Write the name of the first nonmetal. Step 2: Write the name of the second nonmetal changing its ending to -ide. Step 3: Add prefixes to specify how many of each element are present.

  33. Rules for Using Prefixes Rule 1: Prefixes are only for BINARY COVALENT compounds. Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1. Example:CO2 is carbon dioxide, and not monocarbon dioxide. Rule 3: Remove the -o or -a from a prefix before adding it to oxide. Example:CO is carbon monoxide, and not carbon monooxide.

  34. How would you write each of the prefixes in front of oxide? Remember: Remove the -o or -a from a prefix before adding it to oxide. Leave -i alone. mono- ____________ di- ____________ tri- ____________ tetra- ____________ penta- ____________ hexa- ____________ hepta- ____________ octa- ____________ nona- ____________ deca- ____________ monoxide dioxide tetroxide trioxide pentoxide hexoxide octoxide heptoxide decoxide nonoxide

  35. Name the binary covalent compounds that are found on your notes. carbon dioxide carbon disulfide phosphorous tribromide phosphorous pentabromide diphosphorouspentasulfide dinitrogenmonosulfide silicon disulfide nitrogen tribromide dinitrogen tetrachloride

  36. Because of the prefixes, it is very easy to go from the name of a binary covalent compound to its formula. dinitrogen tetrafluoride N2 F4 Step 1: Write the symbol of the first nonmetal and the subscript that matches the prefix. Step 2: Write the symbol of the second nonmetal and the subscript that matches the prefix.

  37. Write the formulas of the binary covalent compounds in your notes. CCl4 IF7 PCl5 N2O4 N2O PCl3 CS CO BH3 ICl S2Br6 S4N4 H2O SiS2 PI3 ClF5 NO2 NCl3

  38. Naming Ionic and Covalent Compounds Review

  39. Chemical reactions occur when atoms gain, lose, or share electrons. This is what creates compounds! gain / accept Nonmetals _____________ electrons. This gives them a ____ charge. Negative ions are called ___________. _ anions Metals ________________ electrons. This gives them a ____ charge. Positive ions are called ___________. lose / donate + cations

  40. What elements do ionic compounds contain? Ionic compounds contain a metal and a nonmetal. Nonmetals Metals

  41. Steps for Naming Ionic Compounds MgCl2 magnesium chloride Step 1: Write the name of the metal ion. Step 2: Write the name of the nonmetal ion. Remember that we change the name of nonmetal ions to –ide. YOU ARE DONE! It is that easy.

  42. shared electrons Nonmetals Chemical reactions occur when atoms gain, lose, or share electrons. Sharing electrons creates a covalent bond Nonmetals can _______ electrons to form a covalent bond. This creates a ___________. share molecule

  43. What elements do covalent compounds contain? Covalent compounds contain only nonmetals. Nonmetals

  44. Steps for Naming Covalent Compounds P2S4 phosphorous tetrasulfide sulfide diphosphorous Step 1: Write the name of the first nonmetal. Step 2: Write the name of the second nonmetal changing its ending to -ide. Step 3: Add prefixes to specify how many of each element are present.

  45. Rules for Using Prefixes with Covalent Compounds Rule 1: Prefixes are only for COVALENT compounds. Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1. Example:PCl3 is phosphorous trichloride, and not monophosphorous trichloride. Rule 3: Remove the -o or -a from a prefix before adding it to oxide. Example:N2O4 is nitrogen tetroxide, and not nitrogen tetraoxide.

  46. Determining if a compound is ionic or covalent is easy. What elements do ionic compounds contain? Ionic compounds contain a metal and a nonmetal. What elements do covalent compounds contain? Covalent compounds contain only nonmetals.

  47. Decide whether the compounds on your notes are ionic or covalent. C I I I C I I C I C C I

  48. Once you decide if a compound is ionic or covalent you know whether or not to use prefixes. Only COVALENT COMPOUNDS use PREFIXES! Do NOT make the mistake of using prefixes with ionic compounds. You will be forced to decide between answer choices with and without prefixes on your exam. Know the difference!

  49. Steps for Naming a Compound Step 1: Decide if the compound is ionic or covalent. Step 2: Write the name of the first element as it appears on the periodic table, change the name of the second element to end with -ide. Ioniccompounds are finished at this point. Step 3: If, and only if, the compound is covalent, add prefixes.

  50. Remember, if polyatomic ions appear in an ionic compound, simply use the name of the ion as it appears in the table of polyatomic ions. 1. NH4Cl 2. MgSO3 ammonium chloride magnesium sulfite 3. Ca(NO2)2 4. KOH calcium nitrite potassium hydroxide

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