Lewis structures of some molecules with multiple bonds Multiple bonds are repres

Question

Lewis structures of some molecules with multiple bonds Multiple bonds are represented with more than one straight line between atoms. A double bond is formed when two atoms share two pairs of electrons and is stronger than a single bond. A triple bond s formed when two atoms share three pairs of electrons and is stronger than a double bond. What is the total number of electrons shown in the Lewis structure in Model 5 for each molecule? Compare your answers to CTQs 19 and 21. How does one determine the total number of electrons that should be used to generate a Lewis structure? For N_2, is the sum of the bonding electrons and the lone pair electrons around each N atom consistent with the Lewis model? In other words, does each N have an octet? Write a sentence to explain. For H_2CO: a. Is the sum of the bonding electrons and the lone pair electrons around each C atom consistent with a complete octet? b. Is the sum of the bonding electrons and the lone pair electrons around each 0 atom consistent with a complete octet? Using the information from above, construct a checklist that can be used to determine if a Lewis structure for a molecule is correct. Try to think of at least three criteria. Compare your criteria with your team and try to come to agreement. List any questions that remain with your team about Lewis dot structures.

Explanation / Answer

Q21

b) Cl2 --> 6 lones pairs + 1 bond = 6*2 + 1*2 = 14 electrons

b) N2 --> 2 lone pairs, 1 triple bond = 2*2 + 1*6 = 10 electrons

c) H2CO --> 2 lonepairs + 4 bonds= 2*2 + 4*2 = 12 electrons

Q22

can't compare with Q19

Q23

For N2 ... yes, it is consistent, since it has its octect complete (3 triple bonds = 6 electrons + lone pair = 6+2 = 8 electrons in total)

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