Chap5LecPartAx

Chap5LecPartAx - DRAFT (Chap 5, Part A) Page 3 Draw Lewis...

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DRAFT (Chap 5, Part A) Page 1 Another type of bond … Covalent Bond (molecules) Electrons play different roles in molecules (we will ignore “core” electrons when discussing bonding and concentrate only on valence electrons) More on Lewis Structures Bonding electrons (glue that holds the atoms together). The electrons in a covalent bond are attracted to both + nuclei and, therefore, they keep the atoms together. Non-bonding electrons (lone-pair electrons or unshared electron pairs)
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DRAFT (Chap 5, Part A) Page 2 Bond length (more glue results in pulling the atoms closer together) Single bond C 2 H 6 Ethane Double bond C 2 H 4 Ethene Triple bond C 2 H 2 Acetylene (organic molecules … mostly C and H, covalent bonds) Bond energy (which do you think is the strongest … requires the most energy to break and/or releases the most energy when formed?) Triple > Double > Single
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Unformatted text preview: DRAFT (Chap 5, Part A) Page 3 Draw Lewis Dot formula to determine the valence of an atom (number of covalent bonds an atom can form). C N O S Cl H DRAFT (Chap 5, Part A) Page 4 Drawing Lewis Structures (can be challenging) First some examples, then some rules PCl 3 C 2 H 6 DRAFT (Chap 5, Part A) Page 5 Rules: 1. Determine the total number of valence electrons. (If you are drawing a structure for an ion, you must add electrons for negative charge and subtract electrons for positive charge). 2. Draw a skeleton molecule using single bonds for all bonds. 3. Put an octet around all the atoms surrounding the central atom. (Except hydrogen atoms) 4. Put any left over electrons on the central atom. 5. If you dont have enough electrons to give all atoms an octet, try making multiple bonds. H 2 O CCl 4 DRAFT (Chap 5, Part A) Page 6 CO 2 HCN IO 3-...
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Chap5LecPartAx - DRAFT (Chap 5, Part A) Page 3 Draw Lewis...

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