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Ionic Naming.

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Presentation on theme: "Ionic Naming."— Presentation transcript:

1 Ionic Naming

2 Objective/Warm-up SWBAT name ionic compounds.
Criss-Cross the following: Ca+2 and SO4-2 Na+1 and PO4-3 Al+3 and O-2 Mg+2 and N-3

3 Definitions An IONIC COMPOUND consists of a metal cation bonded to a nonmetal anion. Electrostatic attraction holds them together. Metal Cation Nonmetal anion Na+ Cl-

4 A quick review Do you remember how to find the charges on different elements from the periodic table?

5 Type I Binary Ionic Compounds
The metal cations in these compounds have only ONE possible charge. Na+ Zn2+ Al3+ Ca2+ sodium zinc aluminum calcium The charges are memorized or predicted using a periodic table! The cations are bonded to nonmetal anions: O2- N3- F- Br - oxide nitride fluoride bromide Notice that simple anions are always named with the suffix “ide”

6 In 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- ® NaCl lithium oxide: Li+ and O2- ® Li2O aluminum bromide: Al3+ and Br - ® AlBr3 zinc nitride: Zn2+ and N3- ® Zn3N2 potassium iodide: K+ and I- ® KI silver phosphide: Ag+ and P3- ® Ag3P

7 Lets do some practice

8 Examples: Type I Binary Ionic Compounds
Write the formulas: potassium oxide zinc chloride silver sulfide aluminum nitride gallium oxide calcium iodide

9 Potassium Nitride Silver Iodide Zinc Bromide Aluminum Oxide
Write the names: K3N AgI ZnBr2 Al2O3 Ba3P2 LiH Potassium Nitride Silver Iodide Zinc Bromide Aluminum Oxide Barium Phosphide Lithium Hydride

10 Type 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

11 Why 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.

12 Answer 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. 

13 Examples: Type II Binary Ionic Compounds
Write the formulas: iron (II) oxide copper (II) chloride tin (IV) sulfide cupric nitride nickel (III) oxide

14 Examples: Type II Binary Ionic Compounds
Write the names: Fe2O3 SnS NiBr2 CuS Pb3P2 CuBr FeCl3 iron (III) oxide Tin (II) Sulfide Nickel (II) Bromide Copper (II) Sulfide Lead (II) Phosphide Copper(I) Bromide iron (III) Chloride

15 Polyatomic (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-

16 Things to Notice Most 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-

17 Lets do some practice Use the handout to write the names for the following.

18 Writing formulas with Complex Ions
A. NH4Cl B. Ag2SO4 C. Al(OH)3 D. Ca3(PO4)2 E. Fe(NO2)3 F. Cu(MnO4)2 G. (NH4)2Cr2O7 H. Zn(CH3COO)2 a) Ammonium chloride b) Silver sulfate c) Aluminum hydroxide d) Calcium phosphate e) Iron (III) nitrite f) Copper(II) permanganate g) Ammonium dichromate h) Zinc acetate

19 Objective/ Warm-up SWBAT write formulas and name ionic compounds.
Please give the name for the following formulas: (a) Ag3P (b) Fe2O3 (c) Ag2SO4 Please give formulas for the following names: (a) Tin (II) Sulfide (b) Iron (III) nitrite

20 Closure When do we need to use roman numerals in a name?

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