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Ch.8 - Basic Concepts of Chemical Bonding
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All textbooksBrown 14th EditionCh.8 - Basic Concepts of Chemical BondingProblem 65a

Chapter 8, Problem 65a

In the vapor phase, BeCl2 exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule?

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Hi everyone here. We have a question asking us to provide the lewis structure for boron. Track chloride using only single bonds. And it's asking is the real satisfied for the structure? So we have boron With three valence electrons. We have three corinne So three times 7 valence electrons. So that gives us a total of 24 valence electrons And 12 electron pairs. So boron is going to be our central atom and it's going to be paired to our three corinne And we have 12 electron pairs to work with. So we're going to put We already have three. So we're going to put four 567, eight nine, 10, 11, 12. So this is a LewiS structure for boron tri chloride using only single bonds. And now is the octet rule satisfied. So boron Only has three bonds Which is only six electrons. So the octet rule is not satisfied. And that is our final answer. Thank you for watching. Bye.
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Related Practice
Textbook Question

(b) Which of these compounds or ions is an exception to the octet rule: borohydride (BH4-), borazine (B3N3H6, which is analogous to benzene with alternating B and N in the ring), or boron trichloride?

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Textbook Question
For Group 13–17 elements in the third row of the periodic table and beyond, the octet rule is often not obeyed. A friend of yours says this is because these heavier elements are more likely to make double or triple bonds. Another friend of yours says that this is because the heavier elements are larger and can make bonds to more than four atoms at a time. Which friend is more correct?
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Textbook Question

Draw the Lewis structures for each of the following molecules or ions. Identify instances where the octet rule is not obeyed; state which atom in each compound does not follow the octet rule; and state how many electrons surround these atoms: (a) PF6-, (b) BeCl2, (c) NH3, (d) XeF2O (the Xe is the central atom), (e) SO42- .

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Textbook Question

In the vapor phase, BeCl2 exists as a discrete molecule. (c) On the basis of the formal charges, which Lewis structure is expected to be dominant for BeCl2?

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Textbook Question

(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe¬O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in part (a) yields the most favorable formal charges for the molecule?

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Textbook Question

There are many Lewis structures you could draw for sulfuric acid, H2SO4 (each H is bonded to an O). (a) What Lewis structure(s) would you draw to satisfy the octet rule?

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