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Ionic Compounds

Ionic Compounds. Review. What is an ion? An Ion is a charged atom or a particle . What is a cation ? A Cation is a + charged ion . What is an anion? An Anion is a – charged ion. Finding the Charge of an Ion.

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Ionic Compounds

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  1. Ionic Compounds

  2. Review • What is an ion? • An Ion is a charged atom or a particle. • What is a cation? • A Cation is a + charged ion. • What is an anion? • An Anion is a – charged ion.

  3. Finding the Charge of an Ion • Group 1 metal make a +1 ion because it has 1 e- in its valence shell and will lose it • Group 2 metal make +2 ion because it has 2 e- in its valence shell and will lose them • Group 13 METALS make +3 ions because it has 3 e- in its valence shell • Group 17 are nonmetals and make a -1 charge because it will accepts an e- to complete the valence shell • Group 16 are nonmetals and make a -2 charge accept two e- to complete the valence shell

  4. Other Ion Charges • Transitional metals typically make various positive charges • ie. Pb2+ and Pb4+ , Fe2+ and Fe4+ • Metals always form positively charge ions, nonmetals always form negatively charged ions

  5. How does the size of an ion relate to the size of the parent atom? • Table of the size of an ion compared to its parent element on p411 • Positive ions (Cations) are smaller than parent atom • Negative ions (anions) are larger than parent atom

  6. Writing Formula for Ionic Compounds • An ionic Compound is a compound between a metal and a nonmetal • Rules to follows for Writing ionic Compounds 1. Chemical compounds must have a net charge of zero 2. Both + ions and – ions must be present 3. The # charge of cations = the # charge of anions

  7. Examples For Writing Ionic Compounds • Na+ + Cl-NaCl • Charge +1 -1 0 • *Atoms don’t spontaneously lose e-. The gain or loss is always paired. One atom loses the e- while another atom simultaneously gain the e-. • Mg2+ + Cl- MgCl2 • Charge 2+ -1 0 • Li+ + N3- Li3N • Charge +1 3- 0

  8. Practice • Write the ionic Compound for the following element combinations. • Calcium and Chloride • Sodium and Sulfur • Calcium and Phosphorous • Potassium and Iodine • Magnesium and Nitrogen • Aluminum and Oxygen

  9. Naming CompoundsBinary Ionic Compounds are formed when a metal (cation) and a nonmetal (anion) form a compound.Two types of cations • Type I (simple) • Always contain the same charge • Group 1, Group 2, Group 13, and silver • Type II • Metals can form two or more different charges • Most Transitional Metals

  10. Rules for Naming Type I Ionic Compounds • The cationis named first and the anion is named second • The simple cation takes its name from the element. • The simple anion takes the first part of its name from the element and adds the root –ide to the end.

  11. Practice Naming • Name each of these compounds. What is the charge on each ion? How many cations are in the compound? How many anions are in each compound? • KCl4. Al2S3 • BaH2 5. MgI2 • AlCl3 6. CaBr2

  12. Rules for Naming Type II Ionic Compounds • Some Cations can form multiple charges. • ie. Pb2+ and Pb4+, Cr2+ and Cr2+ and Cr3+, Fe2+ and Fe3+, Au+ and Au3+ • Chemist decided to use roman numerals to specify charge. • Ie. FeCl2 = Iron (II) Chloride • FeCl3 = Iron (III) Chloride • The old way of naming these compounds was to use the ending –ous for the lower charger and –ic for the higher charge. • Ie. FeCl2 = Ferrous Chloride • FeCl3 = Ferric Chloride

  13. Distinguish Type I and Type II Cations • Group I and Group 2 metals are always Type I cations. • Transitional Metals almost always are Type II cations. • Metals that form only one cation do not need to be identified with a Roman Numeral.

  14. Practice naming Type II Cations • Write the name of each compound, the charge of each element, the number of cations, and the number of anions, and the molecular mass. • CoCl3 MnO2 • SnBr4 HgO • CuClPbS

  15. Finding the Molecular Weight • Also known as Molar mass or Formula Weight • For Na+ + Cl-NaCl • 1 mol Na+ = 22.99g Na+ • 1 molCl- = 35.45g Cl- • 1 mol of NaCl = 58.44g NaCl • For Iron (II) Oxide = Fe2O3 • 1 mol of Fe = 55.85g Fe • 1mol of O = 16.00g O • 1 mol of Fe2O3 = 159.70g of Fe2O3

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