review1 - 2 and sp hybridized atomic orbitals of carbon....

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Discussion 1 January 23, 24 1 . The following table contains the elements most commonly encountered in Chem 343. Fill in the blanks, using the row for hydrogen as an example. Name/Symbol Atomic No. No. of electrons Electronic configuration Lewis structure (outer electrons) Hydrogen / H 1 1 1s 1 H A Carbon Nitrogen Oxygen Fluorine Chlorine Bromine Iodine 2 . Place the electrons in the appropriate energy levels (1s, 2s, 2p. ....) for the elements carbon, nitrogen and oxygen. Use Figure 1.6 in the textbook as an example. Energy 8 Carbon Nitrogen Oxygen 3 . Indicate the correct geometry of the sp 3 , sp
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Unformatted text preview: 2 and sp hybridized atomic orbitals of carbon. Draw in any p orbitals that are present. sp 3 sp 2 sp 4 . Draw structures for the following molecules showing all bonds, and non-bonding electron pairs. ( a ) ethane, ethylene, acetylene ( b ) CH 4 , NH 3 , H 2 O, Br 2 5 . ( a ) Draw structures for the following acids showing all bonds and non-bonding electron pairs. Acid Conjugate base HBr H 2 SO 4 HNO 3 H 3 PO 4 H 2 CO 3 ( b ) In the second column, draw the structure of the conjugate base of each acid in part ( a ). Be sure to place the formal charge on the correct atom....
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This note was uploaded on 03/27/2008 for the course CHEM 343 taught by Professor Whitlock during the Fall '07 term at Wisconsin.

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review1 - 2 and sp hybridized atomic orbitals of carbon....

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