<p>016c201c96e1b861ad37a08ee9f66961.doc SNC2D – Chemistry – Chemical Reactions</p><p>Date: ______Ionic Compounds</p><p>Most elements are ______They achieve stability by ______Bonds are electron ______that fill or complete the outer (______) shell to maximum for each element involved In some of these bonds, changes will occur in order to achieve stability What are the elements in an ionic bond? ______</p><p>How are electrons involved? Electrons (e-) are ______from the ______to the ______Metals become ______Non-metals become ______Ions are held together by the ______attraction (remember grade 9) Example: Sodium (metal) and Chlorine (non-metal) Both are ______elements if consumed Sodium ______Chlorine ______</p><p>Page 1 of 6 016c201c96e1b861ad37a08ee9f66961.doc SNC2D – Chemistry – Chemical Reactions</p><p>Let’s look at the Bohr Rutherford Diagrams</p><p>Lewis Dot Structures The kernel consists of the ______and the ______A kernel is denoted by using the ______for the element The valence electrons are shown as ______</p><p>Square _____ brackets are used to separate ions and the ______on the ion is shown on the outside of the brackets Recall that atoms are most stable when they have a ______(______) shell How can the requirements of Na solve the requirements of Cl in stability achievement? They form an ionic compound called sodium chloride (table salt) It would appear that bond formation changes ______of elements</p><p>Draw Lewis Dot Diagrams for the following compound: Ca and O Mg and Cl Li and S</p><p>Crystal Lattice Ionic compounds do not exist as ______, but rather in large complexes called crystal lattices</p><p>Page 2 of 6 016c201c96e1b861ad37a08ee9f66961.doc SNC2D – Chemistry – Chemical Reactions</p><p>Formulae for Ionic Compounds In ionic bonds we looked at the ______of the atoms involved in the compound To create a compound, we take the charge of the ions involved and use the ______rule Since compounds need to be neutral, we can determine the proper ______of the cations and anions to create a neutral compound Subscripts are used to denote the ratio in ______</p><p>Ionic Bonds Since you know the charge on each ion, you can “______” the charges to write the chemical formula Use the criss-cross rule: Ca and F Li and I Mg and O Na and S</p><p>Page 3 of 6 016c201c96e1b861ad37a08ee9f66961.doc SNC2D – Chemistry – Chemical Reactions</p><p>Polyatomic Ions Some ions are made up of ______atoms The entire unit carries a ______Examples</p><p>1- 1- 1- OH NO3 CH3COO</p><p>When working with polyatomic ions, you can follow the criss-cross rule to write the chemical formula</p><p>Use the criss-cross rule:</p><p>2- 2- - - Ca and SO4 Li and CO3 Mg and NO3 Na and ClO3</p><p>Multivalent Metals Some metal atoms can have more than ______These metal cations are listed with ______to indicate what the charge on the ion is Examples: ______</p><p>Use the criss-cross rule:</p><p>1+ 2- 2+ 2- 2+ - 4+ - Cu and SO4 Cu and SO4 Sn and NO3 Sn and NO3</p><p>Page 4 of 6 016c201c96e1b861ad37a08ee9f66961.doc SNC2D – Chemistry – Chemical Reactions</p><p>Naming Ionic Compounds Binary Compounds Binary means _____ The general rule is that the metal gets named first Non-metal has an “______” ending Examples: NaCl is ______</p><p>MgCl2 Na2O Ca3P2 Al2S3</p><p>Polyatomic Ions List of common polyatomic ions</p><p>+ - NH4 Ammonium CH3COO Acetate</p><p>- 2- OH Hydroxide SO4 Sulfate</p><p>- 2- ClO3 Chlorate CO3 Carbonate</p><p>- 2- NO3 Nitrate CrO4 Chromate</p><p>- 3- CN Cyanide PO4 Phosphate</p><p>To name a compound with a polyatomic ion, name the metal first, followed by the polyatomic ion</p><p>Example: NaNO3</p><p>KNO3 NH4Cl Ca3(PO4)2 Al2(SO4)3</p><p>There is a pattern to the naming of polyatomic ions In all the following changes, the charge of the polyatomic ion ______The base name for a polyatomic ion ends with “-ate” If we add a single oxygen, we add “______” to the front of the name of the polyatomic ion Removing an oxygen changes the “-ate” to “_____” Removing 2 oxygen atoms adds a “______” to the front of the name, while the ending is “______”</p><p>- - - - ClO ClO2 ClO3 ClO4</p><p>Page 5 of 6 016c201c96e1b861ad37a08ee9f66961.doc SNC2D – Chemistry – Chemical Reactions</p><p>More Examples:</p><p>MgClO NaNO2 CuSO3 (Ba)3(PO3)2</p><p>Sometimes polyatomic ions with a valence (charge) of two or greater can have one or more hydrogen atoms When naming these polyatomic ions, “______” is added in front of the polyatomic ion name The overall charge is changed on the root polyatomic ion by ___ for every hydrogen that is added</p><p>- 2- HCO3 H2PO4 hydrogen sulfite</p><p>Multivalent Metals When naming ionic compounds containing multivalent metals, we add in ______to tell us the charge on the metal</p><p>Example: PbCl2 ______</p><p>FeO Fe2O3 Cu3PO4 Cu3(PO4)2</p><p>Page 6 of 6</p>