1 / 16

Compound Names and Formulas

Compound Names and Formulas. Section 4.3. Naming Compounds. Each compound has a unique name Relatively easy rules for naming ionic and covalent compounds. Naming Ionic Compounds. Name of cation stays the same Lithium atom  lithium (ion) Magnesium atom  magnesium (ion)

olga-watkins
Download Presentation

Compound Names and Formulas

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Compound Names and Formulas Section 4.3

  2. Naming Compounds • Each compound has a unique name • Relatively easy rules for naming ionic and covalent compounds

  3. Naming Ionic Compounds • Name of cation stays the same • Lithium atom  lithium (ion) • Magnesium atom  magnesium (ion) • Name of anion turns into an “ide” • Chlorine atom  chloride (ion) • Iodine atom  iodide (ion) • Name = cation + anion • Lithium + Chlorine  Lithium Chloride

  4. More examples of ionic compounds • Barium Chloride • Magnesium Bromide • Sodium Sulfide • Cesium Nitride • Rubidium Oxide • Lithium Fluoride • Potassium Chloride

  5. Predicting the number of cations & anions in an ionic compound • Example: Magnesium Fluoride • Magnesium cation has a +2 charge • Fluoride has a -1 charge • Mg2+F-1 • Rule: Erase charges, replace superscripts with subscripts and switch the numbers between the ions

  6. Example: 2+ 2 1- 1 Mg F

  7. Why? • Magnesium cation: +2 charge • Fluoride anion: -1 charge • It takes TWO fluoride ions to cancel out the charge of the magnesium cation. -1 -1 2+

  8. Example #2: -2 -2 -2 3+ 3+ 3 2- 2 Al O 3+ It takes 2 aluminum ions and 3 oxide ions to cancel out the charges!

  9. Example #3: -2 2+ 2+ 2 2- 2 Ca S Since the charges are equal, it only takes one of each to make the compound neutral!

  10. Ionic bonds with transition metals • Many transition metals can take on more than one charge as an ion: • Cu+, Cu2+ • Fe2+, Fe3+ • If Cu+ bonds to F-, you get CuF • If Cu2+ bonds to F-, you get CuF2 • Both cannot be called “Copper Fluoride” • What can we do?

  11. The answer! • Designate the charge of the cation in the name by using Roman numerals! • CuF contains a copper cation of charge +1 • We call this Copper (I) Fluoride • CuF2 contains a copper cation of charge +2 • We call this Copper (II) Fluoride • Rule: When working with transition metals, put the charge of the cation in parentheses using Roman numerals!

  12. Naming Covalent Compounds • Let’s look at one we already know: • Carbon Dioxide (CO2) • The first element is named regularly (carbon) • The second element gets an “-ide” • The number of each element is represented by a prefix. • Rule: If there is only one atom of the first element, it does not get a prefix. • Otherwise, the first and second elements get prefixes according to the following table:

  13. Table of prefixes

  14. Examples • H2O • N2O4 • P4S3 • SiI4 • PCl3 • P4O10

  15. Remember the Name • Chemistry Remix • Follow along with the lyrics on the back of your HRL

More Related