1 / 15

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.

gur
Télécharger la présentation

Ionic Compounds

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 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

More Related