L. C. Allen has suggested that a more meaningful formal charge can be obtained by taking into account theelectronegativities of the atoms involved Men’s formula for this type of charge—referred to as the Lewis—Langmuir ( L — L ) charge —of an atom, A, bonded to another atom, B, is L − Lcharge = ( US ) group number of A — number of unshared electrons on A − 2 ∑ B x A x A + X B ( number of bonds between A and B ) where X A and X B designate the electronegativities. Using this equation, calculate the L − L charges for CO, NO − , and HF, andcompare the results with the corresponding formal charges Do you think the L − L charges are a better representation ofelectron distribution? (See L C Alien, J. Am Chem Soc., 1989 111, 9115; L. D. Garner, T.L Meek, B. G. Patrick,THEOCHEM, 2003, 620, 43.)
L. C. Allen has suggested that a more meaningful formal charge can be obtained by taking into account theelectronegativities of the atoms involved Men’s formula for this type of charge—referred to as the Lewis—Langmuir ( L — L ) charge —of an atom, A, bonded to another atom, B, is L − Lcharge = ( US ) group number of A — number of unshared electrons on A − 2 ∑ B x A x A + X B ( number of bonds between A and B ) where X A and X B designate the electronegativities. Using this equation, calculate the L − L charges for CO, NO − , and HF, andcompare the results with the corresponding formal charges Do you think the L − L charges are a better representation ofelectron distribution? (See L C Alien, J. Am Chem Soc., 1989 111, 9115; L. D. Garner, T.L Meek, B. G. Patrick,THEOCHEM, 2003, 620, 43.)
Solution Summary: The author explains the Lewis-Langmuir charge formula for CO, NO, and HF, comparing the results with corresponding formal charges.
L. C. Allen has suggested that a more meaningful formal charge can be obtained by taking into account theelectronegativities of the atoms involved Men’s formula for this type of charge—referred to as the Lewis—Langmuir
(
L
—
L
)
charge —of an atom, A, bonded to another atom, B, is
L
−
Lcharge
=
(
US
)
group number of A
—
number of unshared electrons on A
−
2
∑
B
x
A
x
A
+
X
B
(
number of bonds
between A and B
)
where
X
A
and
X
B
designate the electronegativities. Using this equation, calculate the
L
−
L
charges for CO,
NO
−
, and HF, andcompare the results with the corresponding formal charges Do you think the
L
−
L
charges are a better representation ofelectron distribution? (See L C Alien, J. Am Chem Soc., 1989 111, 9115; L. D. Garner, T.L Meek, B. G. Patrick,THEOCHEM, 2003, 620, 43.)
How many resonance structures can be drawn for the hydrogen tellurate ion (HTeO4–) in which the central tellurium atom bears a –1 formal charge and the oxygens bear formal charges of either zero or –1? Enter your answer as a whole number.
Write down the Lewis dot structures of each of the following molecules. Check the formal charge in each case and make use of it to decide on the correct structure where necessary. In cases where delocalised bonding occurs show all the resonance forms. In each case show all steps in arriving at the structure.a) CH2Cl2b) CH3CH2NH3+(here the 3 H atoms are attached to one C atom, and 2 H atoms and a Natom to the other C atom)c) CH3NNN (here 3 H atoms and 1 N are attached to the C atom and the N atoms form a 3atom chain). [Challenging: hint, share leftover electron pairs equally between the two Natoms in the middle after you have completed the octet on the end N]d) NCl3e) ClO3−(chlorate anion = chlorine bonded to 3 oxygen atoms, Hint: Cl does not obey theoctet configuration)
What is the formal charge on the chlorine (Cl) atom in PCl₆⁻?
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