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BELLWORK 11/29/16

Learn how to write formulas for binary and ternary ionic compounds using metals, non-metals, and polyatomic ions.

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BELLWORK 11/29/16

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  1. BELLWORK 11/29/16 • All metals _______ electrons, and have a ________ charge. • All non-metals ________ electrons, and have a ________ charge.

  2. WRITING IONIC FORMULAS

  3. Cations and Anions Label these charges on your Periodic Table +1 +2 -3 -2 -1 +3 Skip transition Metals Skip

  4. Writing Binary Ionic Compound Formulas • A Binary Ionic Compounds is composed of two elements. • Ionic Compounds have to have an overall neutral (zero) charge. • In order to achieve this, we must balance the charges on the cation and the anion to make sure the resulting compound formed has a neutral charge.

  5. Example #1 • What is the overall charge on the Ionic Compound formed between these two atoms? Na+1 and Cl-1

  6. Example #2 • What is the overall charge on the Ionic Compound formed between these two atoms? Mg+2 and O-2

  7. Example #3 • What is the overall charge on the Ionic Compound formed between Mg+2 and Cl-1 Since this compound has an overall positive charge, we need to balance the positive and negative charges. We use subscripts and multiply them by the charge to achieve an overall charge of of zero.

  8. Example #4 • What is the overall charge on the Ionic Compound formed between Ca+2 and P-3 Since this compound has an overall negative charge, we need to balance the charges

  9. Writing Neutral Ionic Formulas Sodium chloride Metal Non-metal Na Cl • Identify the chemicals as either a metal, transitional metal or non-metal • Write out the chemical symbols of each

  10. sodium chloride metal non-metal + 1 - 1 Na Cl + 1 - 1 • 1. Identify the metal and non-metal • 2. Write the symbols • Write the charges • Swap-n-drop the charges and write them as subscripts. • A subscript of 1 is understood, and not written. NaCl

  11. Calcium oxide metal non-metal + 2 - 2 Ca O + 2 1 - 2 1 CaO

  12. magnesium chloride metal non-metal + 2 - 1 Mg Cl - 1 + 2 MgCl2

  13. calcium phosphide metal non-metal + 2 - 3 Ca P - 3 + 2 Ca3P2

  14. PRACTICE QUESTIONS BeF2 BaBr2 Na3N Ga2S3 CaS ZnBr2 AlCl3 Cs3P Li3P GeO2

  15. Writing Ionic Formulas Using Transitional Metals

  16. Sometimes, the metal in your Ionic Compound is a Transitional Metal ( A metal found in group 3-12 on the periodic table). • When your metal is a transitional metal, it will be listed in the Left Column under Common Ions on your Chemistry Reference Page

  17. How is A Transitional Metal Different from a Main group Metal? • A transitional metal can have more than one charge. • If we have a transition metal the charge will be shown in parentheses after the element name.

  18. Examples: • 1. Copper (II) and Bromine • 2. Iron (II) and Oxygen • 3. Lead (II) and chlorine • 4. Mercury (II) and sulfur • 5. Tin (II) and Fluorine • 6. Iron (III) and Oxygen

  19. BELLWORK 11/28/16 • WHAT CHARGE DOES HYDROGEN HAVE? • Ex: HBr - cation NaH - anion

  20. Writing Ternary Ionic Formulas using Polyatomic Ions

  21. Polyatomic Ions – Acts as the non-metal in an Ionic Compound • Sometimes a group of atoms are chemically bonded, and act as one anion with a negative charge. • A list of Polyatomic ions is listed in the two right-hand columns on your Chemistry Reference Page under Common Ions. • Exceptions: There are 2 polyatomic ions that have a positive charge. (NH4+(ammonium and Hg22+ (dimercury)

  22. Examples: • Potassium sulfate- • Lithium Nitrate – • Copper (I) sulfate –

  23. ANSWERS • K+SO42- K2SO4 • Li+NO3-LiNO3 • Cu+SO42-  Cu2SO4

  24. Homework • Ch. 6 Worksheet #2

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