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Ionic Naming. Objective/Warm-up n SWBAT name ionic compounds. n Criss-Cross the following: 1) Ca +2 and SO 4 -2 2) Na +1 and PO 4 -3 3) Al +3 and O -2.

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Presentation on theme: "Ionic Naming. Objective/Warm-up n SWBAT name ionic compounds. n Criss-Cross the following: 1) Ca +2 and SO 4 -2 2) Na +1 and PO 4 -3 3) Al +3 and O -2."— Presentation transcript:

1 Ionic Naming

2 Objective/Warm-up n SWBAT name ionic compounds. n Criss-Cross the following: 1) Ca +2 and SO ) Na +1 and PO ) Al +3 and O -2 4) Mg +2 and N -3

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

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

5 Type I Binary Ionic Compounds n The metal cations in these compounds have only ONE possible charge. Na + Zn 2+ Al 3+ Ca 2+ sodiumzinc aluminumcalcium The charges are memorized or predicted using a periodic table! n The cations are bonded to nonmetal anions: O 2 - N 3 - F - Br - oxide nitride fluoride bromide Notice that simple anions are always named with the suffix “ide”

6 n In an ionic compound, the charges of the cations and anions must always cancel out. n Subscripts are used if more than one atom is needed to cancel the charges: sodium chloride: Na + and Cl -  NaCl lithium oxide: Li + and O 2-  Li 2 O aluminum bromide: Al 3+ and Br -  AlBr 3 zinc nitride: Zn 2+ and N 3-  Zn 3 N 2 potassium iodide: K + and I -  KI silver phosphide: Ag + and P 3-  Ag 3 P

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 Write the names: K 3 N AgI ZnBr 2 Al 2 O 3 Ba 3 P 2 LiH Potassium Nitride Silver Iodide Zinc Bromide Aluminum Oxide Barium Phosphide Lithium Hydride

10 Type II Binary Ionic Compounds n These are ionic compounds where the metal cation can form TWO different charges. Fe 2 + iron (II) Fe 3 + iron (III) Ni 2 + nickel (II) Ni 3 + nickel (III) Co 2 + cobalt (II) Co 3 + cobalt (III) Cu + copper (I) Cu 2 + copper (II) Au + gold (I) Au 3 + gold (III) Sn 2 + tin (II) Sn 4 + 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? n Why do you think so? n Write the shorthand electron configuration for Iron and draw orbital diagrams for iron to see if you can figure it out.

12 Answer n The shorthand electron configuration for Iron is n 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. n 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: Fe 2 O 3 SnS NiBr 2 CuS Pb 3 P 2 CuBr FeCl 3 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 n All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons. n A complex ion is a charged molecule. Complex ions may be cations or anions. examples: nitrate: NO 3 - sulfate: SO hydroxide: OH -

16 Things to Notice n Most complex ions are anions. Ammonium, NH 4 +, is the most common complex cation. n Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms: perchlorateClO 4 - sulfateSO 4 2- chlorateClO 3 - sulfiteSO 3 2- chloriteClO 2 - hypochloriteClO - nitrateNO 3 - nitriteNO 2 -

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

18 Writing formulas with Complex Ions A.NH 4 Cl B.Ag 2 SO 4 C.Al(OH) 3 D.Ca 3 (PO 4 ) 2 E.Fe(NO 2 ) 3 F. Cu(MnO 4 ) 2 G.(NH 4 ) 2 Cr 2 O 7 H.Zn(CH 3 COO) 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 n SWBAT write formulas and name ionic compounds. n Please give the name for the following formulas: (a) Ag 3 P (b) Fe 2 O 3 (c) Ag 2 SO 4 n Please give formulas for the following names: n (a) Tin (II) Sulfide (b) Iron (III) nitrite

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


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