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Ionic Nomenclature

Ionic Nomenclature. GPS Standards: SC1. Students will analyze the nature of matter and its classifications. c. Predict formulas for stable ionic compounds (binary and tertiary) based on balance of charges.

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Ionic Nomenclature

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  1. Ionic Nomenclature GPS Standards: SC1. Students will analyze the nature of matter and its classifications. c. Predict formulas for stable ionic compounds (binary and tertiary) based on balance of charges. d. Use IUPAC nomenclature for both chemical names and formulas: Ionic compounds, Covalent compounds, Acidic compounds (all Binary and tertiary) 10/18/11

  2. all ionic compounds consist of two parts: a cation (a positive ion) and an anion (a negative ion). ions are combined in simple, whole-number ratios to balance their charges. This results in a net charge of zero, which all ionic compounds MUST have. the “cross technique” is used to create the correct ratio of ions needed. Example: aluminum (Al+3) and oxygen (O-2). +3-2 +3-2 AlO AlO AlO 2 3 23 1. Write the symbols, then write the charges on each symbol (from PT of ions) 3. Clean up the formula (completely erase all charges) and reduce if necessary. 2. Cross the charges, dropping the + and – symbols (don’t write 1s) Let’s try a few simple examples before we discuss reducing.

  3. Ex1: magnesium + iodide = _____ _____  ________ Ex2: sodium + sulfide = _____ _____  ________ Ex3: beryllium + chloride = _____ _____  ________ Ex4: aluminum + bromide = _____ _____  ________ Mg+2 MgI2 I- Na+ Na2S S-2 Be+2 BeCl2 Cl- Al+3 AlBr3 Br- +3-2 +3-2 AlO AlO AlO 2 3 23 1. Write the symbols, then write the charges on each symbol (from PT of ions) 3. Clean up the formula (completely erase all charges) and reduce if necessary. 2. Cross the charges, dropping the + and – symbols (don’t write 1s) So when do you need to reduce?

  4. here’s two examples of when the ratio needs to be reduced: Ex5: rhodium + nitride = _____ _____ ______________ Ex6: zirconium + oxide = _____ _____ ______________ Reducible ratios MUST be reduced. It is not optional!!! +2-2 CaO CaO CaO 2 2 +4-2 SnS2 SnS SnS 2 4 2 Rh+3 Rh3N3 N-3 RhN Zr+4 O-2 Zr2O4 ZrO2

  5. some ionic compounds contain polyatomic ions. These ions must be placed in parenthesis first before more than one can be shown in a compound. Examples: Ex7: magnesium + iodite = _____ ______  ___________ Ex8: zinc + phosphate = _____ ______  ____________ Ex9: osmium + sulfate = _____ ______  ____________ Ex10: aluminum + bromate = _____ ______  ___________ +3-2 Al(SO4) Al SO4 23 +-3 NH4 P (NH4) P 3 IO2- Mg+2 Mg(IO2)2 PO4-3 Zn+2 Zn3(PO4)2 SO4-2 Os+4 Os2(SO3)4 Os(SO3)2 reduce! BrO3- Al+3 Al(BrO3)3

  6. Two very important things to remember: 1. Never, ever, EVER add, delete, change, or move a subscript on a polyatomic ion! The only number that “moves” in the cross technique is the charge (which is a superscript). 2. You must use parenthesis on ANY polyatomic ion when you are indicating two or more, even if there is no little subscript on it to remind you to do so! +-3 NH4 P This 4 NEVER moves or changes because it is a subscript. This 1 and 3 can move (be crossed) because they are superscripts. +3- +2- Al OH Fe ClO Al(OH) Fe(ClO) 3 2

  7. 2. You must use parenthesis on ANY polyatomic ion when you are indicating two or more, even if there is no little subscript on it to remind you to do so! Ex11: zinc + hypoiodite = _____ ______  __________ Ex12: tantalum + cyanide = _____ ______  __________ Now, on to naming ionic compounds... +3- +2- Al OH Fe ClO Al(OH) Fe(ClO) 3 2 IO- Zn+2 Zn(IO)2 CN- Ta+5 Ta(CN)5

  8. ionic compounds are named with the following rules: the cation name goes first, the anion name goes second. cations are usually metals. The name of the cation does not change from the name of the element. note: If the element is polyionic (meaning it can have more than one type of charge), this must be indicated by placing a roman numeral after the name to indicate the size of the charge. anions are either: (1) a single negatively charged element (monatomic)—name of the element with the ending taken off and “-ide” added. or Zn+2 = zinc Sc+3 = scandium Fe+2 = iron (II) Fe+3 = iron (III)

  9. anions are either: (1) a single negatively charged element (monatomic)—name of the element with the ending taken off and “-ide” added. or (2) a group of elements that carry a negative charge (polyatomic ions = PAIs)—PAIs have their own special names (on PT of ions). Naming Examples: Ex13: NaCl = ______________________________ Ex14: Al2(SO4)3 = ___________________________ Ex15: KCN = ______________________________ Ex16: Ag2S2O3 = ____________________________ Ex17: Mn3(PO4)2 = __________________________ Ex18: CuNO3 = ____________________________ Ex19: FeO = _______________________________ Ex20: Sn(SO3)2 = ____________________________

  10. Naming Examples: Ex13: NaCl = ________________________________ Ex14: Al2(SO4)3 = _____________________________ Ex15: KCN = ________________________________ Ex16: Ag2S2O3 = ______________________________ Ex17: Mn3(PO4)2 = ____________________________ Ex18: CuNO3 = ______________________________ Ex19: FeO = _________________________________ Ex20: Sn(SO3)2 = ______________________________ sodium chloride aluminum sulfate potassium cyanide silver thiosulfate manganese ( ) phosphate II copper ( ) nitrate I iron ( ) oxide II tin ( ) sulfite IV

  11. Practice: these are set up as you’ll see them on your funsheet! Provide the requested name or formula. Remember, chemistry is cumulative!!! A comprehensive, completeunderstanding of nomenclature procedures is vital for many of the topics we will cover in later parts of this course. MgF2 Pb(C4H4O6)2 scandium dichromate titanium (III) phosphate PtCO3 Li2C2O4 iron (III) oxide manganese (II) nitrite Y(OH)3 Rb2WO4 neodymium selenate chromium (III) periodate Co(CrO2)3 NiS2O3 sodium citrate rhenium chloride

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