1 / 15

Compound Names and Formulas

Compound Names and Formulas. Overview. Naming Ionic Compounds Writing Formulas for Ionic Compounds Naming Covalent Compounds Chemical Formulas for Covalent Compounds. Naming Ionic Compounds. To do this you need some terminology. Cation - Positive Ions Anions- Negative Ions

judith
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

  2. Overview • Naming Ionic Compounds • Writing Formulas for Ionic Compounds • Naming Covalent Compounds • Chemical Formulas for Covalent Compounds

  3. Naming Ionic Compounds • To do this you need some terminology. • Cation- Positive Ions • Anions- Negative Ions • These form when ionic bonds form. Ones that lose electrons are Cations and ones that gain electrons are anions.

  4. Which is which? • NaCl • MgO • CaS • KBr • NaF

  5. Naming Ionic Compounds • Names of cations stay the same- Sodium, Potassium…etc • Name of anions change-you must cut off the end and add ide for the majority- examples include. • Oxygen to oxide • Fluorine to Fluride • Bromine to Bromide. • Once you get the anion and the cation names you just put them together. Ex. Sodium Chloride. NaCl

  6. Name That Ionic Compound • KCl • MgO • LiF • MgS • CaO • CaS • NaF

  7. Some Cations must indicate their Charge • Transition Metals act differently so they have special names. They are named for their positive charge. • Example if it is an iron atom that is +2 than it is Iron II. • If it is an iron atom that is +3 than it is Iron III • If it is an iron atom that is +1 that it is Iron I. • Then just add the anion- Iron(II)Oxide

  8. Special Cations • Copper that is +1 • Copper that is +2 • Nickel that is +2 • Nickel that is +3 • They have these in table 6 on page 160 of the book.

  9. Writing Ionic Formulas • Must do the math to figure out the ratio. Then once you figure out the right number of each then you write out the formula with the cation first. • Magnesium Fluoride- Magnesium has 2 valence electrons so it must give away two. Fluorine needs 1 valence electron so there must be two Fluorine atoms to accommodate Magnesium.

  10. Examples • CaO • LiO • CaN • NaO • Page 161 practice at the bottom of the page do numbers 1-4 and turn it in.

  11. Covalent Compounds • Numerical Prefixes are used to name covalent compounds of two elements. • Examples-Table 7 Page 162 • These denote the number of atoms present of that given element • Only denote the number of the first elements atoms if there are more than one.

  12. Examples • CO • CO2 • CO3 • NF2 • N2F2 • N3F

  13. Covalent Compounds • The element that is furthest to the left on the periodic table goes first. • The element that is furthest to the right on the periodic table goes last and ends in ide. • NO-Nitrogen monoxide • NO2-Nitrogen Dioxide

  14. Examples • BF4 • CF3 • NO2 • PBr2

  15. Going Backwards • We can also work backwards to get the formula. • Take into account how many of each atom and write it out using the simple. • Carbon Dioxide • Carbon Monoxide • Dinitrogentetraoxide.

More Related