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Ionic Compounds

Ionic Compounds. Nomenclature. Introduction. We use the periodic table to tell us the most commonly expected charges for the ions of elements. For example: Group 1 (1A) elements have a 1+ charge. Na becomes Na + Group 2 (2A) elements have a 2+ charge. Mg becomes Mg 2+

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Ionic Compounds

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  1. Ionic Compounds • Nomenclature

  2. Introduction • We use the periodic table to tell us the most commonly expected charges for the ions of elements. • For example: • Group 1 (1A) elements have a 1+ charge. • Na becomes Na+ • Group 2 (2A) elements have a 2+ charge. • Mg becomes Mg2+ • Group 13 (3A) elements have a 3+ charge. • Al becomes Al3+

  3. Introduction • We use the periodic table to tell us the most commonly expected charges for the ions of elements. • For example: • Group 15 (5A) elements have a 3- charge. • N becomes N3- • Group 16 (6A) elements have a 2- charge. • O becomes O2- • Group 17 (7A) elements have a 1- charge. • Cl becomes Cl-

  4. Forming Ionic Compounds • We form ionic compounds by matching the charges of the ions to form a neutral compound. • For example: • Combining Na+ with Cl- gives NaCl. • Combining Ca2+ with S2- gives CaS. • Combining Ga3+ with N3- gives GaN. • Each of these combinations gives a neutral compound.

  5. Forming Ionic Compounds • More complex combinations of ions also need to be balanced to produce neutral compounds. • For example: • Combining Na+ with O2- gives Na2O. • Combining Ca2+ with Br- gives CaBr2. • Combining Al3+ with F- gives AlF3. • Each of these combinations gives a neutral compound.

  6. Forming Ionic Compounds • For even more complex combinations of ions we use a trick to produce neutral compounds. • For example: • Combining Ca2+ with N3-: Ca2+ Ca 2 N N3- 3 • To find the proper number of Ca2+, we use the 3 of the N3-. • To find the proper number of N3-, we use the 2 of the Ca2+. • We can use this “criss-cross” when ever we have a complex combination of ions.

  7. Binary Ion Nomenclature • When we name binary ionic compounds (ionic compounds made from the ions of two elements), we name the cation first followed by the anion. • In general, cations that are metals are given the name of the elemental metal. • NaCl is named sodium chloride. • BaF2 is named barium fluoride. • Ca3P2 is named calcium phosphide.

  8. Binary Ion Nomenclature • When we name binary ionic compounds (ionic compounds made from the ions of two elements), we name the cation first followed by the anion. • In general, anions are given the name of the element followed by the suffix “-ide.” • NaCl is named sodium chloride. • BaF2 is named barium fluoride. • Ca3P2 is named calcium phosphide.

  9. nitride phosphide oxide fluoride chloride bromide iodide sulfide C N O F arsenide selenide P S Cl As Se Br I Binary Ion Nomenclature • The single element anions are: 3- 2- 1-

  10. Cu+, Cu2+ Sn2+, Sn4+ Sc2+ V2+, V3+, V4+ Cr2+, Cr3+ Mn2+, Mn3+ Fe2+, Fe3+ Co2+, Co3+ Mo2+ Zn2+ Ti2+ Ag+ Au+, Au3+ Zn Cu Ni Sc Ti V Cr Mn Fe Co Ga Cd Ag Pd Pb2+, Pb4+ Y Zr Nb Mo Tc Ru Rh In Sn Hg Au Pt Lu Hf Ta W Re Os Ir Tl Pb Bi Po Uub Rg Ds Lr Rf Db Sg Bh Hs Mt Binary Ion Nomenclature • Transition (d-block) metals most commonly have a 2+ charge. • There are exceptions to this rule. • Some transition and main group metals have two or • more common charges.

  11. Binary Ion Nomenclature • Since these cations can have different charges, we need a nomenclature that will distinguish between the different cations. • The Stock system is used to identify different ions. • We use the element name followed by the charge of the ion in parenthesis. • For example: • Cu+ is written as copper(I) • Cu2+ is written as copper(II) • Pb2+ is written as lead(II) • Pb4+ is written as lead(IV)

  12. Binary Ion Nomenclature • Examples of Stock nomenclature: • CuCl = copper(I) chloride • CuCl2 = copper(II) chloride • FeO = iron(II) oxide • Fe2O3 = iron(III) oxide • PbS = lead(II) sulfide • PbS2 = lead(IV) sulfide • VO = vanadium(II) oxide • V2O3 = vanadium(III) oxide • VO2 = vanadium(IV) oxide

  13. Polyatomic Ion Nomenclature • Polyatomic ions are single ions that are made up of several atoms. • Examples of polyatomic ions include: • nitrate: NO3- • sulfate: SO42- • phosphate: PO43- • ammonium: NH4+ • nitrite: NO2- • hydroxide: OH- • dimercury: Hg22+ • acetate: CH3COO-

  14. Polyatomic Ion Nomenclature • Each of these units acts as a single ion. • Nitrate (1-)acts in the same manner as chloride. • Sodium nitrate is NaNO3. • Calcium nitrate is Ca(NO3)2. • Aluminum nitrate is Al(NO3)3. • Sulfate (2-) acts in the same manner as oxide. • Sodium sulfate is Na2SO4. • Calcium sulfate is CaSO4. • Aluminum sulfate is Al2(SO4)3. • Phosphate (3-) acts in the same manner as nitride. • Sodium phosphate is Na3PO4. • Calcium phosphate is Ca3(PO4)2 • Aluminum phosphate is AlPO4.

  15. ammonium: NH4+ nitrate: NO3- sulfate: SO42- dimercury: Hg22+ sulfite: SO32- nitrite: NO2- cyanide: CN- carbonate: CO32- silicate: SiO32- hydroxide: OH- chromate: CrO42- perchlorate: ClO4- dichromate: Cr2O72- chlorate: ClO3- oxalate: C2O42- chlorite: ClO2- hypochlorite: ClO- phosphate: PO43- acetate: CH3COO- phosphite: PO33- hydrogen carbonate: HCO3- Polyatomic Ion Nomenclature • Cations: • Anions:

  16. Ba2+ (NO3)- Polyatomic Ion Nomenclature • When we form ionic compounds from polyatomic ions, we treat the polyatomic ions as individual units of charge. • For example: • barium 2+ and nitrate 1- Ba(NO3)2 barium nitrate We use the criss-cross trick to find the formula of the compound.

  17. (NH4)+ (SO4)2- Polyatomic Ion Nomenclature • When we form ionic compounds from polyatomic ions, we treat the polyatomic ions as individual units of charge. • For example: • ammonium 1+ and sulfate 2- (NH4)2SO4 ammonium sulfate We use the criss-cross trick to find the formula of the compound.

  18. Knowledge Check • Determine the formulas of the following compounds: • sodium carbonate • copper(II) sulfate • lead(IV) phosphate • aluminum nitrite • ammonium sulfide Na+ Na2CO3 (CO3)2- CuSO4 Cu2+ (SO4)2- Pb4+ (PO4)3- Pb3(PO4)4 Al(NO2)3 Al3+ (NO2)- (NH4)2S (NH4)+ S2-

  19. Knowledge Check • Determine the names of the following compounds: • Fe2(CrO4)3 • VO2 • Cr(CH3COO)2 • AuPO4 • NaClO iron(III) chromate vanadium(IV) oxide chromium(II) acetate gold(III) phosphate sodium hypochlorite

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