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Ionic/Covalent Compound Names and Formulas

Ionic/Covalent Compound Names and Formulas. +1. +2. +3 -5. + 4. -3 +5. -2. -1. 0. We want to bond Magnesium and Oxygen. +1. +2. +3 -5. + 4. -3 +5. -2. -1. 0. Step 1: What are the oxidation states?. Use the periodic table trick:. Mg +2. O -2. Step 2: Are charges balanced?.

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Ionic/Covalent Compound Names and Formulas

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  1. Ionic/Covalent Compound Names and Formulas

  2. +1 +2 +3 -5 +4 -3 +5 -2 -1 0 We want to bond Magnesium and Oxygen

  3. +1 +2 +3 -5 +4 -3 +5 -2 -1 0 Step 1: What are the oxidation states? • Use the periodic table trick:

  4. Mg+2 O-2 Step 2: Are charges balanced? • To be balanced, the net (overall) charge MUST be ZERO. How many positive charges are there? How many negative charges are there?

  5. Mg+2 O-2 Step 3: Figure out your formula What is +2 + -2? Is the overall charge zero? So what is your formula? MgO

  6. Mg+2 O-2 Step 4: What is your compound called? • The cation ALWAYS comes first and keeps its name the way it is written. • Magnesium • The anion ALWAYS comes second and the end comes off and is replaced with -ide • Oxygen gets changed to oxide Magnesium Oxide

  7. +1 +2 +3 -5 +4 -3 +5 -2 -1 0 Let’s Practice • Let’s combine Magnesium and Chlorine. • Step 1: What are the ox. states?

  8. Cl-1 Mg+2 • Step 2: Are the charges balanced? • Is the overall charge ZERO? • NO! We have too many positive charges. How many positive charges are there? How many negative charges are there?

  9. Cl-1 Cl-1 Mg+2 What do we do now? • How can we make the charges balance? -2 -1 +2

  10. Cl-1 Cl-1 Mg+2 What’s the formula? • What would the formula for this ionic compound be? MgCl2 What would we call it? Magnesium chloride

  11. Try the following: • With your neighbor, make a balanced formula and the correct names for these ionic compounds: Na + Cl Al + Cl Mg + S K + O Na + O Ca + F Al + O (This one’s hard!)

  12. Covalent Compound Names/Formulas

  13. Remember this…. • A covalent compound forms between two or more nonmetals so we don’t have to worry about ion formation or oxidation states.

  14. A simple set of rules can be used to name them: • Step 1: Name the elements in the order they appear in the formula. For example, CO2 would be named carbon oxygen. Or is it?

  15. What about the subscripts? • Step 2: Use prefixes to indicate how many elements there are of each type. This rule may be modified to improve how the name sounds.

  16. For example, CO2 would be monocarbon dioxygen. Or is it?

  17. What type of ending do I use? • Step 3: Use the ending –ide for the second element listed in the formula.

  18. So this means that ……… • CO2 would be named carbon dioxide.

  19. Practice Naming Covalent Compounds

  20. How would I write the formula if given the name? • Use the symbols of the elements with their corresponding prefix numbers. • Dinitrogen Trioxide would be __________.

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