The more polar bond has to be indicated using partial charge of δ + o r δ − . C − O a n d C − N Concept Introduction: The partial negative ( δ – ) end of a bond is the atom with the larger electronegativity. The partial positive ( δ + ) end of a bond is the atom with the smaller electronegativity.
The more polar bond has to be indicated using partial charge of δ + o r δ − . C − O a n d C − N Concept Introduction: The partial negative ( δ – ) end of a bond is the atom with the larger electronegativity. The partial positive ( δ + ) end of a bond is the atom with the smaller electronegativity.
Solution Summary: The author explains that the more polar bond can be indicated using partial charge of delta –) and the positive end of a bond is the smaller electronegativity.
The more polar bond has to be indicated using partial charge of δ+orδ−.
C−OandC−N
Concept Introduction:
The partial negative (δ–) end of a bond is the atom with the larger electronegativity. The partial positive (δ+) end of a bond is the atom with the smaller electronegativity.
(b)
Interpretation Introduction
Interpretation:
The more polar bond has to be indicated using partial charge of δ+orδ−.
B−OandP−S
Concept Introduction:
Refer part (a).
(c)
Interpretation Introduction
Interpretation:
The more polar bond has to be indicated using partial charge of δ+orδ−.
P−HandP−N
Concept Introduction:
Refer part (a).
(d)
Interpretation Introduction
Interpretation:
The more polar bond has to be indicated using partial charge of δ+orδ−.
Consider a solution of 0.00304 moles of 4-nitrobenzoic acid (pKa = 3.442) dissolved in 25 mL water and titrated with 0.0991 M NaOH. Calculate the pH at the equivalence point
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