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Ionic Reminder

Ionic Reminder. Cation : A positive ion Mg 2+ NH 4 + Anion: A negative ion Cl - SO 4 2 -. Define : Polyatomic Ion - a n ion made up of two or more elements covalently bonded. Polyatomic Ions . Naming Ionic Compounds. cation = name of the element Ca 2+ = calcium ion

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Ionic Reminder

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  1. Ionic Reminder • Cation: A positive ion • Mg2+ NH4+ • Anion: A negative ion • Cl- SO42- Define: Polyatomic Ion- an ion made up of two or more elements covalently bonded.

  2. Polyatomic Ions

  3. Naming Ionic Compounds • cation= name of the element • Ca2+ = calcium ion • anion=root + -ide • Cl-=chloride ion • CaCl2 = calcium chloride

  4. Naming Ionic Compounds(continued) • Many transition metals can form more than one cation • Use a Roman numeral to show the charge • I= 1 • II = 2 • III = 3 • IV = 4 • V= 5

  5. Metals with Varying charges

  6. Example: CuCl2 (Cu = Copper… can be eitherCu+1orCu+2) Cu 2+ + 2 Cl1- = CuCl2 = Copper(II) chloride Cu 1+ + Cl1- = CuCl = Copper(I) chloride

  7. Writing Ionic Compound Formulas Example: Aluminum sulfide 1. Find the charges for the cation & anion 2. Check to see if charges are balanced. 3. Balance charges Al3+ S2- Al2S3 2 3 Not balanced!

  8. Writing Ionic Compound Formulas Example: Iron(III) Chloride 1. Find the charges for the cation & anion 2. Check to see if charges are balanced. 3. Balance charges Fe3+ Cl- 3 FeCl3 Not balanced!

  9. Writing Ionic Compound Formulas Example: Magnesium carbonate 1. Find the charges for the cation & anion 2. Check to see if charges are balanced. Mg2+ CO32- MgCO3 They are balanced!

  10. Writing Ionic Compound Formulas Example: Barium Nitrate 1. Find the charges for the cation & anion 2. Check to see if charges are balanced. 3. Balance charges Ba2+ ( ) NO3- 2 Ba(NO3)2 Not balanced!

  11. Writing Ionic Compound Formulas Example: Zinc Hydroxide 1. Find the charges for the cation & anion 2. Check to see if charges are balanced. 3. Balance charges ( ) Zn2+ OH- Zn(OH)2 2 Not balanced!

  12. Naming Covalent Compounds • Name the least electronegative element first • If there is only one atom, DO NOT use the prefix “mono”. • If there is more than one, DO use a prefix. • Name the more electronegative element next. • Use a prefix EVERYTIME on the second element!

  13. List of Prefixes(For Covalent Compounds only!) • 1 = mono • 2 = di • 3 = tri • 4 = tetra • 5 = penta • 6 = hexa • 7 = hepta • 8 = octa • 9 = nona • 10 = deka

  14. Naming Covalent Compounds P2O5= diphosphoruspentoxide CO2 = carbon dioxide CO = carbon monoxide N2O = dinitrogenmonoxide

  15. Quick Check- • What is the name for each of these compounds? • Fe2O3 PO2

  16. Quick Check- • What is the formula for each of these compounds? • Barium Oxide Dinitrogen tetrachloride

  17. Acid Nomenclature • Acids • Compounds give off H+ in water. • Formulas usually begin with ‘H’. • In order to be an acid instead of a gas, binaryacids(which means 2 things)must be aqueous (dissolved in water) • Ternaryacids (which means 3 things)are ALL aqueous • Examples: • HCl(aq) – hydrochloric acid • HNO3 – nitric acid • H2SO4 – sulfuric acid

  18. Acid Nomenclature Flowchart Memory hint: I ate something icky

  19. Name These Acids • HI (aq) • HCl(aq) • H2SO3 • H2S (aq) • HNO3 • HClO4 • H2CO3

  20. Write the Formula! • Remember, these are acids because they have a H+ ions… so you’ll have to balance charges to determine how many cations & anions there are! • Hydrobromicacid • Nitrous acid • Carbonic acid • Phosphoric acid • Hydrotelluric acid

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