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5.5/5.6 Ions and Ionic Compounds Learning Goals (5.5) Define an ion and compare an anion to a cation (5.6) Draw a Bohr-Rutherford diagram for the following elements: sodium, lithium, fluorine, oxygen, sulfur, nitrogen, phosphorus, neon, helium (5.6) State the rules for designing a chemical formula and a chemical name for an ionic compound. Write names and formulae for ionic compounds An ion is a charged particle that results when an atom gains or loses electrons. If the atom LOSES electrons, the ion becomes POSITIVE and is called a CATION. If the atom GAINS electrons, the ion becomes NEGATIVE and is called an ANION. A Bohr-Rutherford diagram demonstrates how ions form. Example: A lithium atom (Li: atomic # of 3) has 3 protons therefore 3 electrons in the orbits around the nucleus. A Fluorine atom (F: atomic # of 9) has 9 protons therefore 9 electrons in the orbits around the nucleus. A Lithium ION, however, results when the atom loses the single electron in the outer most level during a chemical reaction with the fluorine. The fluorine ION forms when it gains the electron lost by the lithium. The lithium is now equivalent to Helium and the Fluorine to Neon in terms of the number of electrons. The result is an ionic compound (metal + non-metal) being held by an ionic bond (cation + anion). The chemical FORMULA is LiF because 1 atom of each element could be combined to create a particle with FILLED ORBITALS. The chemical NAME is Lithium fluoride because the cation always goes first and the anion always ends in “-ide”. Copy and try these. 1. State the chemical formula for the following combinations of elements. Lithium and Chlorine Sodium and Fluorine LiCl NaF Lithium and Oxygen Sodium and Sulfur Li2O Na2S Sodium and Nitrogen Lithium and Phosphorus Na3N Li3P 2. State the chemical NAME for the following combinations of elements. Lithium and Chlorine Sodium and Fluorine Lithium chloride Sodium fluoride Lithium and Oxygen Sodium and Sulfur Lithium oxide Sodium sulfide Sodium and Nitrogen Lithium and Phosphorus Sodium nitride Lithium phosphide Read section 5.7 and answer the following into your notes. Don’t forget to include the questions with the answers. CYL # 2,3,6 & 7 on page 200