Concept explainers
(a)
Interpretation:
The assigned formal charge in
Concept Introduction :
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure
(b)
Interpretation:
The assigned formal charge in
Concept Introduction :
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure
(c)
Interpretation:
The assigned formal charge in
Concept Introduction :
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure
(d)
Interpretation:
The assigned formal charge in
Concept Introduction :
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure
(e)
Interpretation:
The assigned formal charge in
Concept Introduction :
Formal Charge = Group Number − Number of lines − Number of dots
Group Number refers to the column number on the periodic table.
Number of lines indicates the number of line bonds to the atom in the Lewis structure or it shows the number of bonded pair of electrons.
Number of dots represent the number of non-bonded electrons on an atom in the Lewis structure
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Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
- Based on the following Lewis structure { 3 } { 1} {2} N= A EN: B :N EN -N Match each of the following with its correct answer The formal charge on the nitrogen (1) in structure (B) is Choose... Choose... -2 -1 The formal charge on the nitrogen (1) in structure (A) is zero +1 The formal charge on the nitrogen (1) in structure (C) is Choose... The formal charge on the nitrogen (2) in structure (C) is Choose... The formal charge on the nitrogen (2) in structure (A) is :0:arrow_forwardPROVISIONAL LEWIS STRUCTURES T01/S02 For each provisional structure, enter the central atom formal charge (if not zero, enter the sign before the value) and, separating by comma without any space, indicate (Y or N) if it is the correct Lewis structure. For example, your answer could be "-2,Y". :ä: - P | :a: PCI4+ PCI3 NO NH2" :ö:arrow_forwardPlease select ALL plausible Lewis Dot structures which are theoretically possible. Note: This question has multiple correct answers. An extra H atom can be a part of the correct answer. Hint: Calculate the Formal Charge and check if any of the structures contradict it. H3C H A H3C-º-H (cation-radical) G DA ОВ Ос Н HAC-H OD D OE OF OG OH H3C² Н H3C в E с-н Н Н Ө, H3CH H₂C с F H3C- Н I H CHarrow_forward
- Calculate the formal charges of all of the atoms in each of the following molecules. Part A CO Enter the charge in the order in which the atoms are numbered. Seperate each charge with a comma. Make sure to include the appropriate "+" or "-" if the charge is not "O. :C=0: Πν ΑΣφarrow_forwardWhich of the following resonance structures is the most stable? || I ||| ON II III ∞-∞ IV N Varrow_forwardWhat is the dipole moment of a molecule with a bond length of 154.6 pm and a charge of 0.167 e on the ends of the bond? (enter the number only!). You may submit work for partial credit. remember: 1D=3.34 x 10-30 C m le = 1.602 x 10-19 C 1m= 1012 pmarrow_forward
- Specify the formal charge at each of the labeled atoms, a - c, in each of the following structures. (a) H (b) a Н а. Н н а. C Н b с C=C: Ь. b :0: a b. ОН нн нн с. н Harrow_forward2. For the following ion, (1) draw important resonant forms to show delocalization of charge. Indicate the major resonance form(s), and justify your answerfs); (2) use a formal charge calculation to show why the ion shown below has a negative charge. NHarrow_forwardIn this problem I’m supposed to add the Hydrogens (originally not shown), valence electrons, and pi bonds to create C7H6NO- with a -1 formal charge on oxygen. This is what I got for this question and it keeps telling me it’s wrong. On the next part of the question it’s the same problem except the -1 formal charge is on the Nitrogen and I’m not sure how to draw that one either. Thank you!arrow_forward
- Calculate the formal charge on oxygen in NO+. Group of answer choices 0 -1 + 1 +5arrow_forwardWhat is the formal charge of "E"? A N: H O 0 -1 +1 ;Br C U:O: B Harrow_forwardIII. Using curved arrows, to show the movement of electrons that coverts a Lewis form to a more stable resonance form, for each of following Lewis structures. Be DH sure to specify nonzero formal charges, lone pairs, if any. (8 pts) ОН (a). OH (b). 0:0 HOarrow_forward
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