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Unit 2 Chemistry

This lesson explains the concept of ionic bonds, which occur between metals and non-metals. It covers the rules for naming ionic compounds, emphasizing that the cation (metal) name remains unchanged, while anions (non-metals) take on the suffix "-ide." Examples include sodium chloride (NaCl) and potassium oxide (K2O). The lesson also discusses the complexity of naming compounds with polyatomic ions, such as sodium hydroxide (NaOH) and calcium carbonate (CaCO3), and addresses the need for identifying metal charges with Roman numerals in cases like iron (III) oxide (Fe2O3).

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Unit 2 Chemistry

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  1. Unit 2 Chemistry Naming Compounds

  2. Ionic bonds • What is an ionic bond? • Quick rule: never use capital letters when writing names

  3. Why name compounds? • So we know what is in products and what could be dangerous • Compounds found at home = chemical names • Bleach = sodium hypochlorite • Baking soda = sodium bicarbonate • Antifreeze = ethylene glycol • Table salt = sodium chloride • Vinegar = acetic acid • Nail polish remover = acetone Glass cleaner = ammonia Toothpaste = sodium fluoride

  4. Ionic Bond naming • An ionic bond is between a metal and non-metal • First write the cation (metal) first and do not change the name at all • Then write the anion (non-metal) second but add the suffix –ide to the name • Ex oxide, carbide, hydride, sulfide, chloride

  5. Examples • NaCl- • sodium chloride • LiBr- • lithium bromide • K2O- • potassium oxide • BeF2- • beryilliumflouride

  6. Ionic bonds with polynomials • If there are more than two elements in the bond then one is a polynomial • The polynomial is almost always the anion except for NH4- ammonia • First write the metal name unchanged • Next write the polynomial name unchanged • You find the names of polynomials from the back of the table

  7. Examples • NaOH- • sodium hydroxide • CaCO3- • calcium carbonate • MgNO3- • magnesium nitrate

  8. Easy right? • some metals have more than one charge making it more complicated • Ex: Fe can have +3 or +2 Mn can have +2 or +4 V can have +5 or +4

  9. When a metal has more than one charge you need to determine what the charge is: • Ex iron and oxygen can be FeO or Fe2O3

  10. Finding charges • Find what the negative charge is and then the positive charge has to be equal to that • FeO- O is -2 so Fe has to be +2 • Put the charge of the metal in roman numerals right after the metal • iron (II) oxide

  11. Fe2O3- oxygen is -2*3= -6 so the cations add up to +6 • Since there are 2 Fe, each one would be +3 (+6/2) • iron (III) oxide • CuCl- Cl=-1 so Cu must be +1 • copper (I) chloride

  12. Examples • V2O5- O=-2*5=-10 • V= +10/2= +5 • vandium (V) oxide

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