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Chapter 4.3

Chapter 4.3. Compound names and formulas. I. Naming Ionic Compounds. A. Ionic compounds are formed by the strong attractions between cations and anions. 1. Since both ions are important to the compounds structure, both are included in the name.

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Chapter 4.3

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  1. Chapter 4.3 Compound names and formulas

  2. I. Naming IonicCompounds A. Ionic compounds are formed by the strong attractions between cations and anions. 1. Since both ions are important to the compounds structure, both are included in the name. B. Names of ionic compounds include the ions of which they are composed. 1. The name of the cation is the same as the names of the element a. A cation is a positive ion. b. Cations are ions that have lost electrons

  3. 2. An anion that is made of one element has a name similar to the element. a. The last letters of the name of an anion are changed to –ide.

  4. C. Some cation names show their charge 1. Transition metals may form several cations-each with a different charge a. A cation is a positive ion. b. Cations are ions that have lost electrons

  5. D. Determining the charge of a transition metal cation. 1. Ionic compounds have a total charge of zero, so the total positive charges equals the negative charge. 2. Negative charges are constant so by using the constant negative charges you can find the positive charge. II. Writing formulas for ionic compounds A. You can determine the chemical formula for a compound if you are given its name. 1. List the symbols for each ion. Aluminum= Al+3 Flouride= F-1 2. Write the symbols for the ions with the cation first. Al+3F-1 3. Criss-cross the ions charges, but drop the signs Al1F3 4. Write the chemical formula, indicating with subscripts how many of each ion are needed to make a neutral compound. (you do not have to write 1’s) AlF3

  6. III. Naming covalent compounds A. You have different rules for naming covalent compounds than you do ionic compounds B. Numerical prefixes are used to name covalent compounds of two elements. 1. These prefixes tell how many atoms of each element are in a molecule. a. If there is only one atom in the first element it does not get a prefix. b. The element that is farther to the right on the periodic table is named second and ends in –ide.

  7. Lithium Oxide Beryllium chloride Titanium (III) nitride Magnesium bromide Rubidium oxide Sodium chloride Lithium nitride Potassium sulfide Sodium oxide Tin (II) flouride Practice: Writing Ionic Formulas

  8. Diarsenic pentoxide Silicon tetraiodide Tetraphosphorus trisulfide Tetraphosphorus decaoxide Selenium dioxide Phosphorus tricloride Sulfur tetraflouride Dinitrogen monoxide Phosporus tribromide Diphosphorus pentoxide Practice: writing covalent formulas

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