Some notes in case you didn't get them down at the VC; - valence electrons=the outershell electrons
- isoelectronic=species with the same electron configuration. e.g F-, Ne, Na+ all have 10 electrons
- octet rule-atoms endeavor to get 8 outershell electrons to enable them to be stable
- ionic bonding =transfer of electrons from one atom to another atom (metals lose electrons, non-metals gain electrons). The bond is the electrostatic attraction between the positive and negative ion.
- covalent bonding=atoms share electrons to try to obey the octet rule
- Note: boron may not obey the octet rule and may only have 6 electrons in the outer shell.
- I will email you the answers to page 44/45 mid week after you have had time to try them.
Note: if you scroll down the left hand side of the page and click on 2.4, there is a video clip there explaining polar bonds. It is called "15 ionic, covalent and polar covalent bonds". Work for this week: - complete p44/45 of the lab book on Lewis structures.
- read p83-86 in Study Guide.
- complete Act 11A
- read Study Guide p87-89
- Write notes on : polar bonds, non polar bonds, definition for electronegativity.(There are notes in the attachments).
- Complete Act 11B
- complete p46/47 in lab book.
- complete worksheet in the attachments below.
At Friday's VC we will be doing shapes of molecules. |
 Updating... Ċ Maree Pullar, 23 Jul 2012, 14:52 Ċ Maree Pullar, 19 Jul 2012, 19:32
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