1 / 28

Ionic Bonding and Nomenclature

Ionic Bonding and Nomenclature. Naming and Writing Formulas for Ionic Compounds. Naming and Writing Formulas for Ionic Compounds. Objectives 1. Name and write the symbols for common anions, cations, and polyatomic ions. 2. Determine the formula of an ionic compound between any two given ions.

keita
Download Presentation

Ionic Bonding and Nomenclature

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Ionic Bonding and Nomenclature Naming and Writing Formulas for Ionic Compounds

  2. Naming and Writing Formulas for Ionic Compounds Objectives 1. Name and write the symbols for common anions, cations, and polyatomic ions. 2. Determine the formula of an ionic compound between any two given ions. 3. Name ionic compounds, given their formulas. 4. Correctly use Roman numerals when naming compounds containing transition metals with more than one oxidation number. 5. Write formulas for ionic compounds, given their names. Back to main menu

  3. Naming and Writing Formulas for Ionic Compounds In forming a chemical compound, an atom can gain, lose or share one or more valence electrons. Back to main menu

  4. Positive Ions A cation is an atom or group of atoms with a positive charge. A cation has fewer electrons than a neutral atom of the element. Back to main menu

  5. Symbols of Ions for Cations The metals in groups 1, 2 and 13 lose electrons when they form ions. Group 1 forms +1 ions. Group 2 forms +2 ions Group 13 forms +3 ions. Back to main menu

  6. Naming and Writing Symbols for Cations Ca2+ Calcium ion Na+ Sodium ion Al3+ Aluminum ion Back to main menu

  7. Metals with More than One Common Oxidation Number The metals in groups 3-12 are called transition metals. They often have more than one common oxidation number (ionic charge). Back to main menu

  8. Metals with More than One Common Oxidation Number Here are some of the more commonly used transition metals and their oxidation numbers. Notice that a Roman numeral is used to indicate the charge on the ion when naming the ions formed. Fe2+ Iron(II) ion Fe3+ Iron(III) ion Cu+ Copper(I) ion Cu2+ Copper(II) ion Hg22+ Mercury(I) ion Hg2+ Mercury(II) ion Pb2+ Lead(II) ion Pb4+ Lead(IV) ion Sn2+ Tin(II) ion Sn4+ Tin(IV) ion Cr2+ Chromium(II) ion Cr3+ Chromium(III) ion Cr6+ Chromium(VI) ion Mn2+ Manganese(II) ion Mn3+ Manganese(III) ion Co2+ Cobalt(II) ion Co3+ Cobalt(III) ion Ni2+ Nickel(II) ion Ni3+ Nickel(III) ion Ag+ Silver ion Zn2+ Zinc ion Cd2+ Cadmium ion Back to main menu

  9. Negative Ions An anion is an atom or group of atoms with a negative charge. An anion has more electrons than a neutral atom of the element. Group 17 forms -1 ions. Group 16 forms -2 ions. Group 15 forms -3 ions. The names of monatomic anions end in ide. Back to main menu

  10. Naming and Writing Formulas for Anions Cl- Chloride ion N3- Nitride ion O2- Oxide ion Back to main menu

  11. You Try It Complete the following table. S2- 2 e- gained 1 e- lost Copper(I) ion Ba2+ 2 e- lost Aluminum ion 3 e- lost Fe3+ 3 e- lost Lithium ion 1 e- lost 3 e- gained P3- Back to main menu

  12. Predicting Formulas of Ionic Compounds Ionic compounds are composed of charged particles called ions. They are electrically neutral. This means that the total positive charge is equal to the total negative charge. Binary ionic compounds usually consist of a metal, such as an alkali metal, bonded to a nonmetal, such as a halogen. Empirical formulas are used to represent ionic compounds. An empirical formula is the simplest ratio in which the atoms combine to form a compound. Back to main menu

  13. Predicting Formulas of Ionic Compounds Examples: Write the formulas for the compounds formed between the following pairs of ions. KCl MgS Na2S Al2S3 SnO2 • a. K+,Cl- • Mg2+, S2- • Na+, S2- • Al3+, S2- • Sn4+, O2- Back to main menu

  14. You Try It Write the formulas for the following binary ionic compounds. Hint: First determine the symbols for the ions involved. Always write the cation first. The first one has been done for you as an example. Na+, Br- Mg2+, S2- Cu+, Cl- Ca2+, Br- Sr2+, F- NaBr MgS CuCl CaBr2 SrF2 • Sodium bromide • Magnesium sulfide • c. Copper(I) chloride • d. Calcium bromide • e. Strontium fluoride Back to main menu

  15. You Try It Write the formulas for the following binary ionic compounds. Hint: First determine the symbols for the ions involved. Always write the cation first. The first one has been done for you as an example. f. Sodium oxide g. Lead(II) bromide h. Zinc sulfide i. Aluminum oxide j. Chromium(VI) nitride Na+, O2- Pb2+, Br- Zn2+, S2- Al3+, O2- Cr6+, N3- Na2O PbBr2 ZnS Al2O3 CrN2 Back to main menu

  16. Naming Binary Ionic Compounds Binary ionic compounds are named by writing the name of the cation followed by the name of the anion (-ide ending). a. Na2S b. LiF c. BaCl2 Sodium sulfide Lithium fluoride Barium chloride Back to main menu

  17. Roman Numerals Sometimes it is necessary to use a Roman numeral when naming an ionic compound. When do you use a Roman numeral when naming an ionic compound? You use a Roman numeral when the metallic element forms more than one common ion. This is common of the transition metals. CuCl is CuCl2 is Copper(I) Chloride Copper(II) Chloride Back to main menu

  18. Roman Numerals Never use a Roman numeral when the metallic element is from Group 1, Group 2, or for aluminum, cadmium, zinc or silver. Circle the compounds below that would need a Roman numeral when naming them. SnCl2 Fe2O3 BaCl2 LiF MgS CaO SrF2 CoI3 Back to main menu

  19. Roman Numerals How do I determine the charge of the Roman numeral? To determine the charge of the Roman numeral you have to first identify the ions making up the compound. Back to main menu

  20. Roman Numerals Examples. Fe2O3 Iron(III) oxide Cu2S Copper(I) sulfide Cobalt(II) iodide Co2+, I- SnO2 Sn4+, O2- Fe2+, S2- Iron(II) sulfide Cu+, N3- Copper(I) nitride Back to main menu

  21. You Try It Write formulas for the following compounds. Remember to determine the ions involved first. Li+, O2- Li2O SnS2 Sn4+, S2- Ba3N2 Ba2+, N3- Na+, F- NaF Back to main menu

  22. You Try It Name the following compounds. a. CaS b. FeN c. K2O d. PbO Calcium sulfide Iron(III) nitride Potassium oxide Lead(II) oxide Back to main menu

  23. Naming and Writing Formulas for Ternary Ionic Compounds Ternary ionic compounds contain more than two elements. They usually contain one or more polyatomic ions. Back to main menu

  24. Writing Formulas for Ternary Ionic Compounds Writing the formulas for ternary ionic compounds is just like writing the formula for binary ionic compounds. You write the symbol and charge of the ions involved and then balance the charges. Back to main menu

  25. Writing Formulas for Ternary Ionic Compounds Examples: a. K+, NO3- b. Ba2+, PO43- KNO3 Ba3(PO4)2 Back to main menu

  26. You Try It 1. Write the formulas for the following ternary ionic compounds, given the ions involved. a. Ca2+, SO42- b. K+, PO43- c. NH4+, N3- d. Al3+, SO42- CaSO4 K3PO4 (NH4)3N Al2(SO4)3 Back to main menu

  27. You Try It 2. Write the formulas for the following ternary ionic compounds given their names. Lithium hypochlorite Sodium sulfite Calcium acetate Barium phosphate Copper(II) nitrite Li+, ClO- Na+, SO32- Ca2+, C2H3O2- Ba2+, PO43- Cu2+, NO2- LiClO Na2SO3 Ca(C2H3O2)2 Ba3(PO4)2 Cu(NO2)2 Back to main menu

  28. You Try It 3. To name a compound, write the name of the cation followed by the name of the anion. Calcium nitrate Potassium sulfate Lead(II) sulfite Sodium Acetate Ammonium sulfide a. Ca(NO3)2 b. K2SO4 c. PbSO3 d. NaC2H3O2 e. (NH4)2S Back to main menu

More Related