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Ionic Compounds

Learn about ions, cations, and anions in Ionic compounds. Discover how ions are formed and the physical properties of ionic compounds.

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Ionic Compounds

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  1. Ionic Compounds November 2014

  2. What do you call iron blowing in the wind? • FeBreeze

  3. What is an ion? Cation? Anion? • An ion is an atom or group of atoms with a positive or negative charge. • A cation is a positively charged ion. • An anion is a negatively charged ion.

  4. Ionic Compounds • Chemical Bond – the force that holds two atoms together • Ionic Bond – electrostatic force that holds oppositely charged particles together in an ionic compound • Ionic Compound – compounds that contain ionic bonds • Between a metal and a nonmetal • Metals and Oxygen are called oxides • Metals and any other nonmetal is called a salt

  5. Forming Ions • Metals form cations • Transition metals can have multiple charges. • Also metals under the stair step line can have multiple charges • Al3+, Zn2+, Ag1+ • Nonmetals form anions

  6. Forming Cations • Look at the orbital diagrams and your electron dot structures to determine how many electrons are being lost to get to 8 valence electrons.

  7. What charge would the following cations have? • Beryllium • Rubidium • Aluminum • Strontium • Be2+ • Rb1+ • Al3+ • Sr2+

  8. Forming Anions • Look at the orbital diagrams and your electron dot structures to determine how many electrons are needed to get to 8 valence electrons.

  9. What charges would the following anions have? • Oxygen • Chlorine • Sulfur • Phosphorus • O2- • Cl1- • S2- • P3-

  10. Forming Ions with equations • Use orbital diagrams of the atoms • Determine if the atom will gain or lose electrons • Determine where the energy goes

  11. Electron – dot structures to form compounds • Write the electron dot structure for both atoms • Determine where the electrons will move • Always releases energy

  12. Physical Structure of Ions • Ions have a crystal lattice structure • 3D geometric arrangement of particles • Positive ions surrounded by negative ions

  13. Physical Properties • Usually high melting point and boiling point • NaCl: melt: 801°C boil:1413°C • Hard, rigid, and brittle solids • Melting point, boiling point, and hardness depend on how strongly the particles are attracted to one another • Ionic Crystals require a large amount of energy to be broken apart

  14. Conducting Electricity • Ionic solids do not conduct electricity • Dissolved in water the ions are free to move around • Ionic compound whose aqueous solution conducts electricity • Electrolyte

  15. What happened to the man who was stopped for having sodium chloride and a nine-volt in his car? • He was booked for a salt and battery.

  16. Did you hear the joke about cobalt, radon, and yttrium. • Yes but it’s kind of CoRnY

  17. Energy • Energy is either absorbed or released during a chemical reaction • Absorbed is endothermic • Released is exothermic • Formation of ionic solids is always exothermic • If the amount of energy released during formation is reabsorbed, the bonds holding the positive and negative ions together will break apart

  18. Lattice Energy • The energy required to separate 1 mole of the ions from an ionic compound • Greater the lattice energy the stronger the force of attraction • Smaller ions have stronger bonds • Less distance

  19. Ionic compounds • Formula Unit – represents the simplest ratio of the ions involved • MgCl2 • Monoatomic Ion - a one atom ion • Mg2+ or Cl- • Oxidation numbers or oxidation state • The charge of a monoatomic ion

  20. Determining the Formula Unit of an Ionic Compound

  21. Practice • Potassium and iodide • Magnesium and chloride • Aluminum and bromide • Cesium and nitride • KI • MgCl2 • AlBr3 • Cs3N

  22. Naming Binary Ionic Compounds • Name the cation followed by the anion. Remember that the cation is always written first in the formula. • For monoatomic cations, use the element name. • For monoatomic anions, use the root of the element name plus the suffix –ide. • Example: CsBr  cesium bromide

  23. Practice • NaBr • CaCl2 • SrO • AlF3 • Sodium bromide • Calcium chloride • Strontium oxide • Aluminum fluoride

  24. Naming Involving a Transition Metal • To distinguish between multiple oxidation numbers of the same element, the name of the chemical formula must indicate the oxidation number of the cation. The oxidation number is written as a Roman numeral in parentheses after the name of the cation. • Example: • Fe2+ and O2- FeO  iron (II) oxide • Fe3+ and O2- Fe2O3  iron (III) oxide

  25. Practice • CuCl2 • Fe3P2 • PbO2 • In3N • Copper (II) chloride • Iron (II) phosphide • Lead (IV) oxide • Indium (I) nitride

  26. Naming involving a Polyatomic Ion • When the compound contains a polyatomic ion, simply name the cation followed by the name of the polyatomic ion. • Example: • NaOH  sodium hydroxide • (NH4)2S  ammonium sulfide

  27. Polyatomic Ions • Ions made up of more than one atom • Ones to memorize from list: • Ammonium, hydroxide, nitrite, nitrate, phosphate, acetate, perchlorate, chlorate, chlorite, hypochlorite, sulfate, sulfite, carbonate, hydrogen carbonate

  28. Practice – write formulas • Sodium and nitrate • Calcium and chlorate • Aluminum and carbonate • Potassium and phosphate • NaNO3 • Ca(ClO3)2 • Al2(CO3)3 • K3PO4

  29. Do on your own Write the formula Write the name Cu(NO2)2 Al2O3 Zn(OH)2 KCl NaOH (NH4)3PO4 CrF2 Mn(OH)3 • Titanium (II) acetate • Lithium iodide • Silver bromide • Copper (I) carbonate • Calcium oxide • Aluminum sulfate • Lead (IV) nitride • Beryllium chloride

  30. Answers Write the formula Write the name Cu(NO2)2 : copper (II) nitrite Al2O3 : aluminum oxide Zn(OH)2 : zinc hydroxide KCl : potassium chloride NaOH: sodium hydroxide (NH4)3PO4: ammonium phosphate CrF2 : chromium (II) fluoride Mn(OH)3 : Manganese (III) hydroxide • Titanium (II) acetate: Ti(C2H3O2)2 • Lithium iodide: LiI • Silver Bromide: AgBr • Copper (I) carbonate: Cu2CO3 • Calcium Oxide: CaO • Aluminum sulfate: Al2(SO4)3 • Lead (IV) nitride: Pb3N4 • Beryllium chloride: BeCl2

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