Ionic Bonding Review Replacement

Valence Electrons In the periodic table, elements are arranged in order of atomic number (the number of protons), and the columns or groups show elements with the same number of valence electrons. (The total number of elements in a row or period gives the total electrons to fill that electron shell.) On the left side of the periodic table, group 1 elements have a single electron in their valence shell, and group 2 elements have two electrons. On the far right, group 8 elements have a full outer shell, and group 7 are missing one electron to fill their valence shell. Valence Electrons How many electrons are in the valence shell for these elements? carbon 4 selenium 6 barium 2 xenon 8 Ions Sort the ions into correctly represented ions or incorrectly represented ions. based on what charge they would have if they gained or lost electrons to have a full valence shell. Correct IONS F-1 P-3 Mg+2 Incorrect IONS He+ Al+2 Li-1 Ionic Bonds Ionic Bondsform between metals and nonmetals. In an ionic bond, the metal transfers its valence or outermost shell electron(s) to the nonmetal, so that both become ions with full valence shells. The metal becomes positively charged (a cation) when it donates its electron(s); the nonmetal becomes negatively charged (an anion) when it accepts the electron(s). The positively charged metal and negatively charged nonmetal are then attracted to each other and form an ionic compound.Ionic Bonding Simulation - Explore Learning Ionic compounds Write the chemical formula for the binary compound that forms from each of the ion pairs. Recall that the compound must be neutral (i.e. zero charge). Also give the name of the compound (Hint: the name will be of the form "cation anion", with an "-ide" ending to the anion. See the example in the table. Use no spaces or subscripts when writing the chemical formulas. Example: Na2O Use only lower case letters when writing the formula names (sodium oxide rather than Sodium oxide). Ions Compound formula Compound name Li+1 and O-2 Li2O (or you can write this as Li2O) lithium oxide Ca+2 and Cl-1 CaCl2 calcium chloride Al+3 and S-2 Al2S3 aluminum sulfide K+1 and Br-1 KBr potassium bromide Fe+2 and S-2 FeS iron sulfide Na+1 and I-1 NaI sodium iodide H+1 and O-2 H2O water Mg+2 and F-1 MgF2 magnesium fluoride Be+2 and N-3 Be3N2 beryllium nitride Cations and Anions Determine the formulas and charges of the cations and anions in the following ionic compounds. (Hint: some transition metals can have more than one charge.) Use no spaces or superscripts Make sure polyatomic ions have their parenthesis in place. Example: (PO4)-3 Be sure to place the - or + before the number with no spacing. Ionic Compound Cation Anion CsCl Cs+1 (or you can write this as Cs+1) Cl-1 (or you can write this as Cl-1) CaF2 Ca+2 F-1 NaOH Na+1 (OH)-1 Ca(OH)2 Ca+2 (OH)-1 KNO3 K+1 (NO3)-1 Fe(NO3)2 Fe+2 (NO3)-1 Fe2O3 Fe+3 O-2 Al2(SO4)3 Al+3 (SO4)-2 FeO Fe+2 O-2