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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Ch.8 - Basic Concepts of Chemical Bonding
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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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lewis Structure
A Lewis structure is a diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons that may exist. It uses dots to represent valence electrons and lines to represent covalent bonds. For BeCl2, the Lewis structure will show beryllium bonded to two chlorine atoms, illustrating how electrons are shared to form bonds.
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04:28
Lewis Dot Structures: Ions
Octet Rule
The octet rule is a chemical guideline stating that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. In the case of BeCl2, it is important to analyze whether beryllium and chlorine achieve this stable configuration through the Lewis structure drawn.
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01:27Octet Rule
Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom. Understanding the geometry of BeCl2, which is linear due to its two bonding pairs and no lone pairs on beryllium, helps in visualizing the molecular structure and its implications for reactivity and properties.
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01:33Molecular Geometry with Two Electron Groups
Related Practice
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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