Combining Capacity or Electron Charge

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1 CHEMISTRY UNIT LESSON FIVE Formulas and Names Ionic Compounds Combining Capacity or Electron Charge The periodic table can be used to predict how elements combine to form. compounds (+) You know that an element with a ion combines with an element having a (-) ion. The positive and negative values of the ions are called valence numbers. These valence numbers can be used to write the formula of an ionic. compound 1

2 Combining Capacity or Electron Charge The alkali metals have a combining capacity of +1 and the halogens have a combining capacity of -1. easily These two families form compounds. You can tell from their valence numbers that one ion of lithium should combine with one ion of chlorine to form one formula unit of lithium chloride -. LiCl Combining Capacity or Electron Charge The alkali earth metals have a valence number of +2. Beryllium (Be +2 ) and chlorine (Cl -1 ) combine to form beryllium chloride -. BeCl 2 Here we see that one ion of beryllium combines with two ions of chlorine. 2

3 When writing correct formulas for these ionic compounds, there are several rules to follow. Beryllium and chlorine will be used as examples. Rule 1: Write the symbol of the metallic element. In the example, Be is written first. The non-metal, chlorine, is written. second first Be 2+ Cl 1- Rule 2: Place the ionic charge number (valence number) of one element at the base (as a subscript) of the other element as shown below. Use only the valence number, not the charge (+ or -). This is where the name crisscross comes from. 1 2 BeCl 2 The formula becomes. Note that the valence number of beryllium is placed as a subscript to Cl and the valence number of chlorine has been placed as a subscript to beryllium. Notice also that the beryllium subscript of 1 has been left out. Which brings us to rule

4 Rule 3: If a subscript has a value of one, leave it out. Notice that Be has no subscript in the example. Rule 4: Reduce the subscripts when necessary by the greatest common factor. For example, when magnesium combines with sulfur, the formula might appear as Mg 2 S 2, but it should be reduced to MgS by dividing both subscripts by two. Mg 2+ S The formation of an ionic bond is illustrated using Bohr models. The following example shows the formation of calcium fluoride. 4

5 1 This example shows that Ca 2+ ion is needed along with F 2 1- ions to produce a formula unit of calcium fluoride that is neutral. These are the numbers of ions in lowest numbers required to make a formula unit. CaF 2 Therefore the formula for calcium fluoride is. Practice writing formulas for ionic compounds Write chemical formulas for the following binary ionic compounds using the rules described on previous pages (don t forget the criss-cross method!). KCl Potassium combines with chlorine Magnesium combines with bromine Calcium combines with oxygen MgBr 2 CaO 5

6 Naming Ionic Compounds when given the Formula As a general rule, the following two rules apply to naming ionic compounds: metal Name the or ion first by writing the full name of the metallic element. non-metal Name the or ion next by dropping the last syllable(s) of the name of the element and adding the suffix. ide (+) (-) Naming Ionic Compounds when given the Formula Fill in the table below which gives the names of the most commonly used ions of non-metallic elements. Element Ion Ion Name Nitrogen N 3- Oxygen O 2- Fluorine Phosphorus F 1- Sulfur S 2- Chlorine P 3- Cl 1- Bromine Br 1- Nitride Oxide Fluoride Phosphide Sulfide Chloride Bromide 6

7 Lesson Five Work/Homework Exercise #5 Handout 7

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