Polyatomic Ions Transition Metals Polyatomic Ions are atoms

Polyatomic Ions & Transition Metals

Polyatomic Ions are atoms that combine and react as a group. The Charge applies to the ENTIRE GROUP. MEMORIZE THESE!!! 1. Ammonium: NH 4+ 2. Hydroxide: OH 3. Nitrate: NO 3 - 4. Sulfate: SO 425. Carbonate: CO 326. Phosphate: PO 43 - DON’T EVER CHANGE THE SUBSCRIPT!!!

Ohana means family. Family means no one gets left behind - Stitch ( ) Sulfate: 2 (SO 4)

Bonding Rules for Polyatomics 1. Balance the charges between ions (like before) 2. The entire group acts like one ion -Use parentheses if you need more than 1 polyatomic ion (Don’t Change Subscript!): Ex: 2 NO 3 = (NO 3)2 Try: 3 CO 3 = _____ 2 PO 4 = _____

1+ Na with CO 3 2 - Na 2 CO 3

3+ Al with SO 4 2 - Al 2(SO 4)3

NH 4 with CO 3 + 2 - (NH 4)2 CO 3

Polyatomic Ions Practice (Remember: The entire group acts like one ion) n Practice: u. K+ + OH- KOH u. Na+ + SO 4 -2 Na 2 SO 4 u. Ca+2 + OH- Ca(OH)2 potassium hydroxide sodium sulfate calcium hydroxide

Summary: �How do you bond a polyatomic ion? Why are parentheses important?

1. Transition Metals n Transition (are weird!) metals can take on different charges n Roman numerals represent the charge: Fe+2 Fe+3 Iron(II) Iron(III)

Naming Transition Metals Naming Rules for Transition Metals: 1. Separate the ions 2. Figure out the anion 3. Figure out the charge of the cation n Example: u. Fe. Cl 2 Fe 2 Cl. Name: iron (II) chloride Roman Numerals: I, III, IV, V, VII

Practice! n Cu. Cl 2

Practice! n Cu. Cl 2 n Fe. Cl 3 n Pb. O

Writing Formulas from Names n Example: Copper (II) oxide Practice: u. Iron (II) bromide u. Mercury (I) chloride