Recitation Packet 1 (F2021)

3. Do the following compounds have dipole moments? If so, use the crossed arrow to indicate the net molecular dipole on top of those structures. H a. b. H C. CI CI a CI 4. Calculate the formal charge for each of the indicated atoms in the compounds below. с H H CI CI H CI H F H₂C H₂C-O-B-F d. e.

Which of the following Lewis structures represents a better resonance form of [CH3CO]+ than the Lewis structure below? + H3C-C-0 a. O b. О с. O d. H H3C-C H3C -C-00 ✪ H₂C-Co .. H3C-C 00

26. 0-S-S-0 has three resonance Lewis structures that complete the octet for all the atoms. Which statements about these structures are correct? I. All are equivalent. II. All are nonequivalent. III. Two are equivalent, and one is nonequivalent. The formal charges on all the atoms are zero in at least one structure. V. All the bonds have double-bond character. IV. а. III and V d. I and V b. I and IV II and IV e. III, IV, and V с.

References] Consider the following reaction: H. H. CI CI CC (9) + CLg) H-C-C-H( AH-172 kJ H. H H Estimate the carbon-chlorine bond energy given that the C-0 bond energy is 347 /mol, the 0-C bond energy is 614 kJmol, and the Cl-O1 bond energy is 239 KJmol. Doa Umol

Pls help ASAP

What is the formal charge of O in the molecule below? a. 0 O b.-2 O C. -1 O d. +2 :0:- :C1:

What are the formal charges on the starred atoms from left to right? All lone pairs present in the molecules are shown in the structures below. A.+1,+1 B.-1,0 C.+1,-1 D.-1.-1 E.0,0

7. Write the correct Lewis structures for the following compounds (relative positions of atoms are shown correctly).  a.     F         F           B            F   b.     F         F            N            F     c.   H             C    F     O   d.  H C C H    e.  O Sn O   f.  H O F g.  H C N

Draw a Lewis structure for each of the following species. Again, assign charges where appropriate. a. H-H¯ b. CH3-CH3 c. CH3+CH3 d. CH3 CH3 e. CH3NH3+CH3NH3 f. CH30-CH3O¯ g. CH2CH2 - h. HC2-(HCC) HC2 (HCC) i. H202×(HOOH) H₂O₂ (HOOH) Norton

Lone Pai. ahedral 2. Consider the following Lewis symbols for elements X and Y. a. What are the Group numbers of X and Y? b. Will a compound of X and Y be ionic or molecular? Page 1 of 9 3. For each of the following bonds, indicate the positive end with a and the negative end with a. Draw an arrow to show the dipole for each. а. N—F b. Si-Br с. c. N-P 4. Which of the following bonds are polar? Circle the more electronegative atom in the pairs that are polar. C-O a. b. H Cl (gas) с. 0-O Page 3 of 9

BENZENE RESONANCE Which of the following structures do all atoms have full octets A. C. CH3 o Br B. NO ₂ OH of an OCH3 D. E. O NO₂ NO₂

17. Name the following molecular covalent compounds. a. PBrs b. NgP3 C. Si,Os d. C,F8 T e. N,S4 Learning Target: use electron dot formulas and structural formulas to d U 18. The following compounds have covalent bonds. Complete valence electrons, drawing a Lewis dot diagram, and identifyin Lewis Do Compound Valence Electrons

63. Write a Lewis structure that obeys the octet rule for each mole- cule or ion. Include resonance structures if necessary and assign formal charges to each atom. MISSED THIS? Read Section 10.8; Watch KCV 10.8, IWE 10.7 b. CO3²- d. NO₂ a. SeO2 c. CIO Write a Louis structure that obos the octet rule for each ion.

D).  Difference between sigma n pi

Lewis structure #4

1. Excluding hydrogen, what are the formal charges on each of the following atoms? a. b. C. d. CH3 H3C_1 H3C-C: H. HT -NECH 4-X-N=C² H H3C CH3

How many lone pairs of electrons need to be added to the Lewis structure of carbonic adid shown below? H-0-C -0-H O A. 3 О в. 6 O C. 0 D. 4

Decide whether the proposed Lewis structure below is reasonable. proposed Lewis structure Is this a rcasonable structure? res O No H. H. C-H O Yes O No O Yes O No H. H. O Yes H. O No H H H 日、

Decide whether the proposed Lewis structure below is reasonable. proposed Lewis structure Is this a reasonable structure? ?. ih Yes H. O No H H. H. OYes O No :0: H. O Yes O No H. H. O Yes H. O No