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IONIC COMPOUNDS

IONIC COMPOUNDS. Naming and Formula Writing. Predicting Charges on Monatomic Ions KNOW THESE !!!!. +1 +2 -3 -2 -1 0. Cd +2. Naming Positive Ions. Before you name an Ion you have to know the charge.

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IONIC COMPOUNDS

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  1. IONIC COMPOUNDS Naming and Formula Writing

  2. Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Cd+2

  3. Naming Positive Ions • Before you name an Ion you have to know the charge. • Group 1 = always +1 • Group 2 = always +2 • Aluminum = always +3 • Zinc and Cadmium = always +2 • Silver = always +1

  4. The Other Metals • All other metals can have various positive charges from +1 to +7 • Roman Numerals are used to tell the charge

  5. Monatomic Ions

  6. Naming Postive Ions • With group 1, 2, Al, Zn, Cd, and Ag you just give the name of the atom • Na+ is Sodium • Mg+2 is Magnesium • Ag+ is Silver • Al+3 is Aluminum

  7. All the other metals • With all other metals you give the name Metal followed by a roman numerial • Cu+ - Copper (I) • Cu+2 – Copper (II) • Fe+2 – Iron (II) • Fe+3 – Iron (III) • U+6 – Uranium (VI)

  8. Naming negative ions • All negative ions have their endings changed to –ide • Oxygen becomes oxide • Fluorine becomes Fluoride • Nitrogen becomes Nitride • Chlorine becomes Chloride

  9. Names of other Negative Ions • Carbide = what you want your parents to do for you • Boride = what happened at the rodeo • Silicide = what you are seeing right now • Fluoride = a state in the union • Iodide = Very sad, I guess we will have to Barium.

  10. Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions  – Na  +  F :  Na+ : F :  NaF  sodium + fluorine sodium fluoride formula Charge balance: 1+1- = 0

  11. Writing a Formula Write the formula for the ionic compound that will form between Ba2+ and Cl. To cancel out Ba’s +2, then two -1 Cl’s are needed. Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba2+ ClCl 3. Write the number of ions needed as subscriptsBaCl2

  12. Balancing a formula by math • Every ionic compound should have a formula that has a charge that equals zero. • Barium Fluoride • Ba+2 F- • How many F’s are needed to balance Ba+2 ? • Two • Formula is BaF2

  13. Another way – Drop, Swap, Reduce • Aluminum Oxide • Al is always +3 • Oxide is always -2 • Al+3, O-2 • DROP: Al3O2 • SWAP: Al2O3 • REDUCE: 2 and 3 are lowest integers, so leave alone

  14. Another example • Magnesium Oxide • Mg is +2 • Oxide is -2 • Mg+2, O-2 • DROP: Mg2O2 • SWAP: Mg2O2 • REDUCE: MgO, 2 and 2 divide each other out.

  15. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na+, S2- a) NaS b) Na2S c) NaS2 2. Al3+, Cl- a) AlCl3 b) AlCl c) Al3Cl 3. Mg2+, N3- a) MgN b) Mg2N3 c) Mg3N2

  16. Solution 1. Na+, S2- b) Na2S 2. Al3+, Cl- a) AlCl3 3. Mg2+, N3- c) Mg3N2

  17. Naming Compounds Binary Ionic Compounds: • 1. Cation first, then anion • 2. Monatomic cation = name of the element • Ca2+ = calciumion • 3. Monatomic anion = root + -ide • Cl- = chloride • CaCl2 = calcium chloride

  18. Examples: NaCl ZnI2 Al2O3 sodium chloride zinc iodide aluminum oxide Naming Binary Ionic Compounds

  19. Learning Check Complete the names of the following binary compounds: Na3N sodium ________________ KBr potassium ________________ Al2O3 aluminum ________________ MgS _________________________

  20. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu+,Cu2+ Fe2+, Fe3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

  21. Names of Variable Ions These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and themetalsin groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl3(Fe3+) iron (III) chloride CuCl (Cu+ ) copper (I) chloride SnF4 (Sn4+) tin (IV) fluoride PbCl2 (Pb2+) lead (II) chloride Fe2S3 (Fe3+) iron (III) sulfide

  22. Examples of Older Names of Cations formed from Transition Metals(you do not have to memorize these)

  23. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 iron (_____) bromide CuCl copper (_____) chloride SnO2 ___(_____ ) ______________ Fe2O3 ________________________ Hg2S ________________________

  24. Polyatomic Ions • Some ions are composed of more then one atom. • These are called polyatomic ions • Poly = more

  25. Formulas and names • Nitrate = NO3- • Sulfate = SO4-2 • Silver nitrate • Ag+ NO3- • DSR = AgNO3 • Copper (I) Sulfate • Cu+ SO4-2 • Cu2SO4

  26. More Polyatomics • Lead (IV) Phosphate • Pb+4 PO4-3 • Pb3(PO4)4 • Notice: When more then one Polyatomic is present you surround it with () • Big: The subscripts on Polyatomic ions are NEVER changed.

  27. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na+, PO4-3 a) NaPO4 b) Na2PO4 c) Na3PO4 2. Al3+, NO3- a) Al(NO3)3 b) AlNO3 c) Al3NO3 3. NH4+, N3- a) NH4N b) NH4N c) (NH4)3N

  28. Answers • 1. Na+, PO4-3 c) Na3PO4 • 2. Al3+, NO3- • a) Al(NO3)3 • 3. NH4+, N3- • c) (NH4)3N

  29. Polyatomic Ions you have to know

  30. More on Polyatomics • Most polyatomic ions end in –ate. • The ending –ite means one less oxygen is present then in the ending –ate. • Example: Nitrate versus Nitrite: • NO3- NO2- • NOTICE: Only the number of O’s changed, not the charge.

  31. Even More • The Prefix Hypo means two less oxygen’s are present then in –ate. • Example: Hyposulfite: SO2-2 • The Prefix Per- means one extra oxygen is present then in –ate. • Examples: • Perchlorate ClO4- • Chlorate ClO3- • Chlorite ClO2- • HypoChlorite ClO-

  32. What if Hydrogen is in it? • The Prefix Bi means that a Hydrogen is added, and the charge is reduced by one. • Example: • BiCarbonate HCO3-

  33. Properties of Ionic Compounds • Ionic compounds are: • also known as salts • They are usually hard and brittle • Conduct electricity when molten or dissolved • Have very high melting and boiling points • Most are soluble in water • Normally composed of at least one metal and one nonmetal

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