1) Classify each bond below as ionic, non-polar covalent, or polar covalent. For the polar covalent compounds, indicate the direction of the dipole. H-CI H3C-CH,CH3 H,CO-H Na-Br H-OH H,C-CF, H-CH, Br-Br F-CI H,C-OH Br-Mg -Br Li-CH,CH3 2) Determine the formal charge on each of the bold atoms below. Lone pairs have been drawn in for you. H2 H,C-cEc: H,C CH, H,C OH2 H. 3) Determine the formal charge on each of the bold atoms below. You must draw in lone pairs as appropriate. H. HC CH H-O HC. CH N. HC P_H H,C H H,C CH CH

For C ~ F, you need draw the proper Lewis structure first, then draw the resonances

Xenon can be the central atom of a molecule by expanding beyond an octet of electrons. Draw Lewis structures for the given xenon compounds. Show all lone pairs. XeF2XeF2           SelectDrawRingsMoreEraseSelectDrawRingsMoreEraseSelectDrawRingsMoreEraseSelectDrawRingsMoreEraseSelectDrawRingsMoreErase XeF XeF2OXeF2O           SelectDrawRingsMoreEraseSelectDrawRingsMoreEraseSelectDrawRingsMoreEraseSelectDrawRingsMoreEraseSelectDrawRingsMoreErase XeOF

Draw the Lewis structures (with formal charges) of each of the species in the indicated pair and use the lewis stucture to answer which has the longer bond? and which has the stronger bond? 1.) O2 or O2^2+  2.) NO- or NO^3-  3.) F2 or F2^2+  4. NO2+ or NO2^3-  5.) OF2 or FO+

draw the lewis structure of ClO-3 following the octet rule. How many double bonds are present? How many lone pairs? What is the formal charge of Cl? What is the formal charge of O?

10. Molecule: CzHj0 Indicate the number of available electrons that are in the molecule. ae = Trial Structure: in the space to the right connect all of the atoms to the central atoms (all Cs in a chain) and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? ne = Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom: Hybridization:

Draw the bonding pattern for the third resonance structure of the azide ion, N3. Two of the resonance structures are shown below. (Include double/triple bonds and any formal charges.) Edit Drawing eTextbook and Media NEN-N: A How many lone pair electrons are on the central nitrogen atom? # of lone pair electrons on the central nitrogen atom: 0 2-:N-N=N: B How many lone pair electrons are on the each of the other two nitrogen atoms? # of lone pair electrons on each of the other nitrogen atoms: 4 Why do both bonds of the azide ion have the same length? O The bond lengths are the same because the resonance structure you drew was tetrahedral. O The bond lengths are the same because single, double, and triple bonds are always the same length. The bond lengths are the same because structures A and B are equivalent and therefore make equal contributions to the hybrid.

Draw the lewis structure with formal charges. If the lewis structure has resonance please show all possible resonance structures. 1. SeO2 2. HC2O4^-

Calculate the formal charge for the (fictional) elements below using the information given below, for the polyatomic ion shown below the table. Complete the sentence with your answers. Element Symbol Number of Valence Electrons Electronegativity Value A 1 0.53 X 1 0.62 E 2 0.91 R 3 1.32 M 4 1.62 T 5 2.70 D 6 3.05 L 7 3.21

Decide whether these proposed Lewis structures are reasonable. proposed Lewis structure |N—N=N] : 0: :0-C H .. I :Ö: H 1 O-H + Is the proposed Lewis structure reasonable? 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: 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: * 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: * * 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".