2Objective/Warm-up SWBAT name ionic compounds. Criss-Cross the following:Ca+2 and SO4-2Na+1 and PO4-3Al+3 and O-2Mg+2 and N-3
3DefinitionsAn IONIC COMPOUND consists of a metal cation bonded to a nonmetal anion. Electrostatic attraction holds them together.Metal Cation Nonmetal anionNa+ Cl-
4A quick reviewDo you remember how to find the charges on different elements from the periodic table?
5Type I Binary Ionic Compounds The metal cations in these compounds have only ONE possible charge.Na+ Zn2+ Al3+ Ca2+sodium zinc aluminum calciumThe charges are memorized or predicted using a periodic table!The cations are bonded to nonmetal anions:O2- N3- F- Br -oxide nitride fluoride bromideNotice that simple anions are always named with the suffix “ide”
6In an ionic compound, the charges of the cations and anions must always cancel out. Subscripts are used if more than one atom is needed to cancel the charges:sodium chloride: Na+ and Cl- ® NaCllithium oxide: Li+ and O2- ® Li2Oaluminum bromide: Al3+ and Br - ® AlBr3zinc nitride: Zn2+ and N3- ® Zn3N2potassium iodide: K+ and I- ® KIsilver phosphide: Ag+ and P3- ® Ag3P
10Type II Binary Ionic Compounds These are ionic compounds where the metal cation can form TWO different charges.Fe2+ iron (II) Fe3+ iron (III)Ni nickel (II) Ni nickel (III)Co2+ cobalt (II) Co3+ cobalt (III)Cu copper (I) Cu2+ copper (II)Au gold (I) Au3+ gold (III)Sn tin (II) Sn4+ tin (IV)An older system uses suffixes and Latin names, -ous for the lower charge, -ic for the higher charge:Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic
11Why do transition metals have different charges? Why do you think so?Write the shorthand electron configuration for Iron and draw orbital diagrams for iron to see if you can figure it out.
12Answer The shorthand electron configuration for Iron is This shows that it has 2 valence electrons that it would like to lose so it explains why it can exist with a +2 charge.If Iron loses 2 electrons its electron configuration will be This will make it easy for another electron to be lost because all electrons like to be alone rather than paired. See below.
13Examples: Type II Binary Ionic Compounds Write the formulas:iron (II) oxidecopper (II) chloridetin (IV) sulfidecupric nitridenickel (III) oxide
14Examples: Type II Binary Ionic Compounds Write the names:Fe2O3SnSNiBr2CuSPb3P2CuBrFeCl3iron (III) oxideTin (II) SulfideNickel (II) BromideCopper (II) SulfideLead (II) PhosphideCopper(I) Bromideiron (III) Chloride
15Polyatomic (Complex) Ions All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons.A complex ion is a charged molecule. Complex ions may be cations or anions.examples:nitrate: NO3- sulfate: SO42- hydroxide: OH-
16Things to NoticeMost complex ions are anions. Ammonium, NH4+, is the most common complex cation.Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms:perchlorate ClO4- sulfate SO42-chlorate ClO3- sulfite SO32-chlorite ClO2-hypochlorite ClO- nitrate NO3-nitrite NO2-
17Lets do some practiceUse the handout to write the names for the following.
19Objective/ Warm-up SWBAT write formulas and name ionic compounds. Please give the name for the following formulas:(a) Ag3P (b) Fe2O3 (c) Ag2SO4Please give formulas for the following names:(a) Tin (II) Sulfide (b) Iron (III) nitrite
20ClosureWhen do we need to use roman numerals in a name?