1 / 67

1. What are the structural differences between ionic and molecular compounds?

1. What are the structural differences between ionic and molecular compounds?. 2. How do those differences affect their chemical formulas?. The chemical formula for a covalent compound is called a molecular formula ;. The chemical formula for an ionic compound is called a formula unit.

ifama
Download Presentation

1. What are the structural differences between ionic and molecular compounds?

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. 1. What are the structural differences between ionic and molecular compounds? 2. How do those differences affect their chemical formulas?

  2. The chemical formula for a covalent compound is called a molecular formula; The chemical formula for an ionic compound is called a formula unit.

  3. The chemical formula for a covalent compound is called a molecular formula; Example: H2O is the molecular formula of water The chemical formula for an ionic compound is called a formula unit. Example: NaCl is the formula unit of common table salt

  4. What’s the dif?

  5. A nice VISUAL look at the difference will help out:

  6. We’ll look at sodium chloride, NaCl, as an example ionic compound.

  7. NaCl does not exist as a single unit like a molecule.

  8. Like any ionic compound, sodium chloride exists as a crystal:

  9. The formula unit for sodium chloride is NaCl. However, if we look inside the crystal, the Na+ and Cl- ions are each bonded to six oppositely charged neighbors:

  10. Let’s shrink the ions so we can take a peek inside

  11. Let’s shrink the ions so we can take a peek inside

  12. We’ll take a look at this Cl- ion.

  13. How many Na+ ions is the Cl- close enough to bond with?

  14. We’ll start again from the head-on view

  15. We’ll start again from the head-on view

  16. And, how many Cl- ions is each Na+ ion bonded to?

More Related