Answer the following questions about the Lewis structure for the organic molecule CH3CH2CH2CN (see examples in Chapter 10) There are valence electrons. The molecule has single bonds, double bonds, and triple bonds. The three central C atoms on the left have REDS and the shape at each of these is The central C on the right has REDS and the shape is The AENC-N = 0.49 which is only slightly polar and we will consider it to be nonpolar. %3D Since there is only slightly polar covalent bond, the molecule is mostly а. О b. 1 С. 2 d. 3 е. 4 f. 5 g. 8 h. 10 i. 12 j. 14 k. 16 I. 18 m. 20 n. 24 О. 28 р. 30 q. 32 r. 34 S. 36 t. diatomic u. pyramidal v. linear w. monoatomic ions x. tetrahedral y. trigonal planar z. bent aa. 120° bb. 180° dd. 109.5° cc. no bond angles, no central atom nonpolar ее. polar ff. gg. ionic hh. C and C

Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure :Z: I :Z: c=0 0 0 0 Is the proposed Lewis structure reasonable? O Yes. O No, it has the wrong number of valence electrons. The correct number is: O O No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* ■ Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* O Yes. O No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* * If two or more atoms of the same element don't satisfy the octet rule, just enter the chemical symbol as many times as necessary. For example, if two oxygen atoms don't satisfy the octet rule, enter "0,0". X 3

Choose the best Lewis structure from those presented below. (It will help to work out the missing formal charges for the atoms in these different structures) [Image description: Lewis structure A has a N atom singly bound to two O atoms. There is one electron pair on N. One O atom has three electron pairs and the other O atom has two electron pairs and another single bond to a H atom. Lewis structure B has a O atom, 01, singly bound to a N atom and doubly bound to another O atom, O2. There is one electron pair on O1 and two electron pairs on O2. On the N atom there are two electron pairs and another single bond to a H atom. Lewis structure C has a O atom, 01, singly bound to another O atom, O2, and doubly bound to a N atom. There are is one electron pair on 01 and two electron pairs plus another singly bond to a H atom on 02. There are two electron pair on N. Lewis structure D has a N atom singly bound to a O atom, O1, and doubly bound to another O atom, O2. There are two electron…

Two possible Lewis structures for the cyanate ion are shown below, with formal charges (FC) calculated for each atom. One structure has carbon as the central atom and the other has a nitrogen as a central atom. By considering formal charges, which arrangement of atoms is the best, and therefore most likely structure for cyanate? FC: -1 0 0 FC: -1 +1 -1 |:0—C=N:1 STRUCTURE A STRUCTURE B Structure A Structure B Both are equally likely QUESTION 19 Two possible Lewis structures for the thiocyanate ion are shown below, with formal charges (FC) calculated for each atom. One structure has carbon as the central atom and the other has a nitrogen as a central atom. By considering formal charges, which arrangement of atoms is the best, and therefore most likely structure for thiocyanate? FC: 00-1 FC: -1 +1 -1 Ec: STRUCTURE A STRUCTURE B O Structure A Structure B

= O ELECTRONIC STRUCTURE AND CHEMICAL BONDING Counting bonding and nonbonding electron pairs in a Lewis... Below is the Lewis structure of the methoxide H H:C:O: H e (CH₂O) ion. Count the number of bonding pairs and the number of lone pairs around the carbon atom. bonding pairs: lone pairs: X Ś 1/5

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An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of +1. Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just draw one Lewis structure. Be sure to write in any non-zero formal charges.

Draw a Lewis structure for the molecular formula: SnI3– This molecule only contains tin and iodine atoms.  Only one atom in this molecule should have a nonzero formal charge.  Has to show this nonzero formal charge in your Lewis structure. What is the geometry of the electron groups around iodine?