11a+Net+Ionic+Equations

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Notes:
If a chemical is soluble or in a solution, write the ions apart. IONS MUST HAVE A CHARGE written by them. When you balance the equation, The number of atoms of each element must balance and the total charges on each side of the --> have to be equal.
 * Note: PPT means precipitate. Precipitates are insoluble products in a reaction.**

Ionic Solubility Rules:
Solubility Rules 1. All common salts (any we may use) of Group 1 and ammonium are soluble. 2. All common acetates and nitrates are soluble. 3. All binary compounds of Group 17 elements (other than F) with metals are soluble except those of silver, mercury (I), and lead. 4. All sulfates are soluble except: barium, strontium, lead, calcium, silver, and mercury (I). 5. Except for those in Rule 1, carbonates, silicates, and phosphates are insoluble. 6. All salts of sulfides are insoluble except for those of Group I and II elements and of ammonium. 7. Gases: Are always written in molecular form (not soluble). 8. Oxides: Are always written in molecular form.

9. All group 1 and 2 all make strong bases with hydroxide except beryllium otherwise they are weak. 10.Binary acids: HCl, HBr, & HI are strong acids and written as ions (HCl is written as H+ and Cl- in a net ionic equation.), all other acids are written in molecular form. 11.Ternary acids: If the number of oxygen atoms is TWO more than the number of hydrogen atoms it is strong. (H2SO4, HNO3, HClO3 are examples of strong acids. HP3O4, H2SO3 are examples of weak acids.)
 * Strong Acids and Bases are soluble (Strong written apart/Weak written together) **

Lecture 1 Ions and Ionic Equations
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Solubility rules:
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