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Covalent Bonding

Covalent Bonding. F [He]     F 2 molecule F [He]     2s 2p O [He]     O 2 molecule O [He]       2s 2p N [He]     N 2 molecule N [He]     2s 2p.

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Covalent Bonding

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  1. Covalent Bonding F [He]  F2 molecule F [He]  2s 2p O [He]  O2 molecule O [He]    2s 2p N [He]  N2 molecule N [He]  2s 2p

  2. Covalent Bonding: Various Representations F [He]  F2 molecule F [He]  F – F 2s 2p F : F O [He]  O2 molecule O [He]  O = O   2s 2p O :: O N [He]  N2 molecule N [He]  N  N 2s 2p N ::: N

  3. Covalent Bonding: Octets Ne [He]  Ne 2s 2p complete “octet” of electrons in valence shell F [He] F F [He] F complete “octet” of electrons in valence shell

  4. Covalent Bonding: Octets F atoms in F2 also have complete octet through sharing F [He]  F [He]  “lone pairs” “bonding pair” F F

  5. Covalent Bonding: Using Lewis Dot Approach • Layout positions of atoms. • Usually, least EN atom in center, most EN atom outside. Some exceptionsapply. • Sum total # valence e- from all atoms. • If anion, add e-; if cation, subtract e- • Put pair of e- (or dash) to connect central atom with other atoms. • Distribute e- on outside atoms to give each an octet first. Put remaining e-on central atom. • Can’t make octets? Move a lone pair to become a bonded pair.

  6. Covalent Bonding: Using Lewis Dot Approach In most compounds, • H atoms form 1 bond • C atoms form 4 bonds • N atoms form 3 bonds • O atoms form 2 bonds • Halogens (on the outside) form 1bond Copy this down for the next activity!

  7. Covalent Bonding: Lewis Dot Practice CH2Cl2 January O2 H2O2 N2 CO2 NO2 * N2O SO2* HCN O3 CO NH3 December Work with a neighbor Draw Lewis structure for substance according to your birth month. When you have an answer, come down and write it on the board. We need answers from two groups for each substance for confirmation. If answers don’t agree, add another answer up on the board. Waiting? Try other ones. Debrief in 10 mins.

  8. More Covalent Bonding: Lewis Dot Practice PCl3January PCl5 NO2- NO3- XeF4 SiO2 N3- SO3 SO42- C6H6 PO43-December Same Routine

  9. Exceptions to Octet Rule 1) Incomplete Octets (Less than 8 valence e- ) • Found in groups II and III • i.e.) BF3, BeF2 2) Expanded valence shells (Greater than 8 valence e- ) • Found in nonmetals third period and beyond • i.e.) PCl5, SO2, SF6, XeF4 3) Odd number of e- • NO, NO2, ClO2     3s 3p 3d

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