1 / 26

Bonding and Nomenclature

Bonding and Nomenclature. Ionic. Valence Electrons. Electrons in the highest occupied energy levels of an atom Number of valence electrons largely determines the chemical properties of an element. Octet Rule. A stable atom contains 8 valence electrons

vilmos
Download Presentation

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. Bonding and Nomenclature Ionic

  2. Valence Electrons • Electrons in the highest occupied energy levels of an atom • Number of valence electrons largely determines the chemical properties of an element

  3. Octet Rule • A stable atom contains 8 valence electrons • Atoms will try to achieve this stable configuration

  4. Cations • Any atom or group of atoms with a positive charge • Neutral atoms loses electrons • Group I and group II metals, other metals, transition and inner transition metals and Al Group 1 form +1 ion Group 2 form +2 ions Al forms +3 ion Ag forms +1 ion Cd forms + 2 ion Zn forms +2 ion

  5. Anions • Atoms or group of atoms with a negative charge • Neutral atom gains electrons • Group VII, VI, V • Non-metals

  6. Lewis Electron Dot Diagrams • Show only the valence electrons • Valence electrons are represented as dots • Which group of the periodic table does Li belong to? • Write the electron configuration for Li • 1s22s1

  7. Draw Electron Dot Diagrams • Na K Be Mg • Ca Cl F Br • O S Se

  8. Determine Valence Electrons • ELEMENT#valence electonsgroup # • Rb • Calcium • Al • Iodine • Bromine • O • F • Sodium

  9. Determine Valence Electrons • ELEMENT#valence electonsgroup # • Rb 1 1 • Calcium 2 2 • Al 3 3 • Iodine 7 7 • Bromine 7 7 • O 6 6 • F 7 7 • Sodium 1 1

  10. Existence Of Ions • Predict whether the following ions are likely to exist. • H- H+ Sr2+ Al3+ • Xe- Zn6- Zn2+

  11. Ionic Compounds • Composed of a cation and an anion • Cation is always written first • Cation donates electrons and the anion takes electrons so that all atoms have 8 electrons in their valence shell

  12. http://www.dnatube.com/view_video2.php?viewkey=650923ea331c15af3b16http://www.dnatube.com/view_video2.php?viewkey=650923ea331c15af3b16

  13. Formula Unit • ·Is a chemical formula that shows the kinds and numbers of atoms in an ionic substance • ·The lowest whole number ration of ions in a compound • ·The compound has a neutral charge

  14. Crystal Lattice Structure

  15. Writing Formula Units • Cation(+) first • Anion(-) last • Subscripts after anion and/or cation to indicate how many are necessary to create a neutral compound

  16. Naming Ionic Compounds Binary ionic compound: cation name remains the same, anion ending changes to “ide” NaCl MgCl2 AlF3

  17. Write The Formulas • Rubidium chloride • Barium nitride • Aluminum sulfide • Sodium fluoride • Magnesium oxide

  18. Naming Ionic Compounds • Ternary ionic compound: cation name remains the same, anion is the same as the polyatomic ion • Na2CO3 • Al2(SO4)3

  19. Naming Ionic Compounds • Transition and other metals: use a roman numeral after the cation to specify the ionic charge of the cation • CuSO4 • Cr2O3 • Fe(CN)2

  20. Classical Name • Formula Stock Name Classical Name • Cu+ copper(I) ion Cuprous ion • Cu2+ copper(II) ion Cupric ion • Fe2+ iron(II) ion Ferrous ion • Fe3+ iron(III) ion Ferric ion • Exceptions: Ag+, Cd2+, Zn2+

  21. Naming Acids • Anion • EndingAcid NameExample 1. -ide begins with hydro, HCl ends with -ic and acid 2. –ite ends with –ous and acid H2SO3 3. –ate ends with –ic and acid H2SO4

  22. Common Acids • HCl Hydrochloric Acid • H2SO4 Sulfuric Acid • HNO3 Nitric Acid • HC2H3O2 Acetic Acid • H3PO4 Phosphoric Acid • H2CO3 Carbonic Acid

  23. Properties of Ionic Compounds Hard crystalline solids High melting points Conduct electricity in solution or molten

  24. Naming Ionic Compounds • Silver nitrate 12. Copper(II) sulfate • Iron(II) phosphate 13. Cobalt(II) iodide • Chromium(III) oxide 14. Cesium phosphate • Nickel(II) fluoride 15. Magnesium acetate • Copper(I) nitrate 16. Potassium oxide • Lead(II) carbonate 17. Strontium nitrate • Iron(II) fluoride 18. Aluminum sulfate • Iron(III) hydroxide 19. Calcium chlorate • Zinc phosphate 20. Rubidium cyanide • Potassium chlorate 21. Tin(IV) oxide • Ammonium chromate 22. Titanium(II) iodide

  25. Ionic Formulas • BaCl2 10. FeCl3 • Pb(NO3)2 11. Ca(CN)2 • TiI3 12. Cu2S • NH4OH 13. Ag2CO3 • K2CrO4 14. Cd(ClO)2 • CoO 15. SnO2 • Mg(ClO4)2 16. NaHCO3 • CuSO4 17. Al(C2H3O2)3 • Na2SO3 18. Ni3(PO4)2

  26. Quest: Ionic Compounds • If anion is a non-metal, then change ending to –ide. • If anion is a polyatomic ion, then simply use name of polyatomic ion. • If cation is a transition metal or other metal, then need roman numeral to clarify the charge of the cation. Exceptions: Ag, Zn, Cd, Al. • Acid formulas always have H+ as the cation. Know the six acids in your notes.

More Related