1 / 11

Unit 9: Covalent Bonding

Unit 9: Covalent Bonding. Chapters 8 & 9 Chemistry 1K Cypress Creek High School. Lewis Structures. Count up total number of valence electrons Connect all atoms with single bonds “multiple” atoms usually on outside “single” atoms usually in center; C always in center,

saxton
Download Presentation

Unit 9: Covalent Bonding

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. Unit 9:Covalent Bonding Chapters 8 & 9 Chemistry 1K Cypress Creek High School

  2. Lewis Structures • Count up total number of valence electrons • Connect all atomswith single bonds • “multiple” atoms usually on outside • “single” atoms usually in center; • C always in center, • H always on outside. • Complete octets on exterior atoms (not H, though) • no unpaired electrons 4) Check • valence electrons match with Step 1 • all atoms (except H) have an octet; if not, try multiple bonds • any extra electrons? • Put on central atom

  3. Cl Cl C Cl Cl Lewis Structure Practice • Carbon tetrachloride • Total valence electrons • 32 • Central atom • carbon • Bond to each of the chlorines • Fill up the octet of each of the chlorines • Check number of valence electrons • Check octet of each atom

  4. H C O H H H H H H C C H Lewis Structure Practice • Methane (CH4) • Ethyne (C2H2) • Water (H2O)

  5. Diatomic Elements • Some nonmetal elements on the periodic table exist in nature only as pairs called diatomic molecules; bonded covalently • H, O, F, Br, I, N, Cl Hydrogen Molecule (H2) http://web.jjay.cuny.edu/~acarpi/NSC/5-bonds.htm

  6. Molecular Shapes • Applies to covalent compounds only. • Use VSEPR steps (valence shell electron pair repulsion): • 1) Identify the central atom as the element that can form the most bonds • 2) Draw the Lewis dot structure for the molecule • 3) Count total # of electron pairs around the central atom • 4) Count # of bonding pairs of electrons around the central atom • 5) Count # of lone pairs of electrons around the central atom • 6) Look at summary chart, identify shape

  7. Molecular Shapes

  8. Exceptions to Octet Rule • Beryllium • Has 2 valence electrons • Full with 4 valence electrons • Ex: BeI2 • Aluminum • 3 valence electrons • Full with 6 valence electrons • Ex: AlCl3 • Boron • 3 valence electrons • Full with 6 valence electrons • Ex: BH3

  9. Expanded Octets • Some atoms bond so they have more than 8e- in the outer level • Occur only around a central nonmetallic atom from period 3 or higher PCl5 SF6

  10. Molecular Shape Example • What is the shape of water (H2O)? • 1) Central atom? oxygen • 2) Draw Lewis Dot… • 3) # of total electron pairs around central atom? 4 • 4) # of bonding pairs around central atom? 2 • 5) # of lone pairs around central atom? 2 • 6) Refer to chart to identify shape…angular (bent)

  11. Molecular Shape Prediction • Try to predict the shape using VSEPR and your shape chart: 1) BCl3 2) CH4 3) NH3 Lewis Dot Central Atom # e- pairs # bonded pairs # lone pairs Shape

More Related