1 / 31

Ionic Bonding in Review

Ionic Bonding in Review. Ionic Bonds. B etween metals & nonmetals Electrons form a give take relationship metals give e- ( cation ) nonmetal take e- (anion) Held together by attraction of opposite charges. Names to Formulas. You have to be able to determine the charges of ions ….

viho
Download Presentation

Ionic Bonding in Review

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Ionic Bonding in Review

  2. Ionic Bonds • Between metals & nonmetals • Electrons form a give take relationship • metals give e- (cation) • nonmetal take e- (anion) • Held together by attraction of opposite charges

  3. Names to Formulas You have to be able to determine the charges of ions …

  4. Predicting Ionic Charges from periodic table Group 1: Lose 1 electron to form 1+ ions H+ Li+ Na+ K+

  5. Predicting Ionic Charges from periodic table Group 2: Loses 2 electrons to form 2+ ions Be2+ Mg2+ Ca2+ Ba2+ Sr2+

  6. Predicting Ionic Charges from periodic table Group 13: Loses 3 electrons to form 3+ ions B3+ Al3+ Ga3+

  7. Predicting Ionic Charges from periodic table Lose 4 electrons or gain 4 electrons? 4+ or 4- ion Group 14:

  8. Predicting Ionic Charges from periodic table Nitride N3- Group 15: Gains 3 electrons to form 3- ions P3- Phosphide As3- Arsenide

  9. Predicting Ionic Charges from periodic table Oxide O2- Gains 2 electrons to form 2- ions Group 16: S2- Sulfide Se2- Selenide

  10. Predicting Ionic Charges from periodic table F1- Fluoride Br1- Bromide Group 17: Gains 1 electron to form 1- ions Cl1- Chloride I1- Iodide

  11. Predicting Ionic Charges from periodic table Group 18: Stable Noble gases do not form ions!

  12. Predicting Ionic Charges from periodic table Many transition elements have more than one possible oxidation state. The only way to know their charge is by looking at the roman numeral in the name !!! Groups 3 - 12: Iron(III) = Fe3+ Iron(II) = Fe2+

  13. Predicting Ionic Charges from periodic table Groups 3 - 12: Some transition elements have only one possible oxidation state. Write these on your Periodic Table Silver = Ag+ Zinc = Zn2+ 2+ 1+

  14. Predicting Ionic Charges of Polyatomic Ions PolyatomicIons • The prefix poly- means many in Greek. • ion consisting of a molecule with manycovalently bonded atoms • act as a single unit • Usually end in –ate & –ite • To know their charge memorize the list or look it up • -ide usually indicates binary compounds except hydroxide

  15. Rules for Formulas • Write the cation (metal) first. Write the anion (nonmetal) second. • The net ionic charge is zero. • Use subscripts to indicate multiple ions. • Write the formula unit in the lowest whole number ratio. • Use parenthesis to indicate multiple polyatomic ions.

  16. Class Practice Names to Formulas

  17. Silver Chloride Ag+1 Cl-1 AgCl

  18. Lead (IV) Sulfide (Galena) Lead (IV) Pb+4 S-2 PbS2

  19. Zinc Phosphide Zn+2 P-3 Zn3P2

  20. Aluminum Oxide Al+3 O-2 Al2O3

  21. Magnesium Sulfate Mg+2 SO4-2 MgSO4

  22. Iron (II) oxide Iron (II) Fe+2 O-2 FeO

  23. Iron (III) oxide (Hematite) Iron (III) Fe+3 O-2 Fe2O3

  24. Copper (II) Nitrate Copper (II) Cu+2 NO3-1 Cu(NO3)2

  25. Mistakes to Avoid • Roman numerals are not written in the formula • Charges are not written in the formula • Don’t drop polyatomic subscripts • Hydroxide, OH, needs parentheses to indicate multiples. • Cu(II)O CuO • K+1Br-1KBr • CaNO2 Ca(NO3)2 • CaOH2 Ca(OH)2

  26. Examples #1- Formulas to Names 1. Write the names of the ions = 0 -2 2. Determine the charge of the positive ion CuSO3 2. Does the cation form more than one oxidation charge? Cu +2 SO3 x X + (- 2) = 0 I’m a polyatomic ion You must know the charge on the sulfite ion is -2 The sum of the positive and negative charges must equal zero +2 +2 X = +2 copper sulfite (II) Final Name Next

  27. Examples #2- Formulas to Names 1. Write the names of the ions KMnO4 2. Does the cation form more than one oxidation charge? I’m a polyatomic ion potassium permanganate Final Name

  28. Examples #3- Formulas to Names 1. Write the names of the ions 2. Does the cation form more than one oxidation charge? NH4NO3 I’m a polyatomic ion ammonium nitrate Final Name

  29. Examples #4- Formulas to Names 1. Write the names of the ions SnF2 2. Does the cation form more than one oxidation charge? X = +2 X + 2(-1) = 0 Snx (F-1)2= 0 tin fluoride (II) Final Name

  30. Examples #5- Formulas to Names 1. Write the names of the ions Ba(ClO4)2 2. Does the cation form more than one oxidation charge? I’m a polyatomic ion barium perchlorate Final Name

  31. Examples #6- Formulas to Names 1. Write the names of the ions Cu2S 2. Does the cation form more than one oxidation charge? X = +1 2X + (-2) = 0 2Cux(S)-2= 0 I’m not a polyatomic ion copper sulfide (I) Final Name

More Related