### Formal Charges Exercise#### Objective:Specify the formal charges (both sign and magnitude) on the atoms labeled **a**, **b**, and **c**.---#### Problem 1![Molecule 1 Diagram]The first molecule is a compound with the structure H₃C─P─CH₃ and an oxygen atom double-bonded to the phosphorus (P) atom. The atoms are labeled as follows:- Atom **a**: Oxygen (O) atom with lone pairs- Atom **b**: Phosphorus (P) atom- Atom **c**: Carbon (C) atom`Learners' Task: Choose the correct formal charges for atoms a, b, and c from the dropdown menus.`**Annotated Solution:**- a: -1- b: +1- c: 0This annotated solution indicates that atoms should have the following formal charges:- Oxygen (O): -1- Phosphorus (P): +1- Carbon (C): 0---#### Problem 2![Molecule 2 Diagram]The second molecule is a compound with the structure (C₆H₅)₃P─C(CH₃)─H and with a lone pair on the phosphorus atom. The atoms are labeled as follows:- Atom **a**: Phosphorus (P) atom- Atom **b**: Carbon (C) atom- Atom **c**: Hydrogen (H) atom`Learners’ Task: Choose the correct formal charges for atoms a, b, and c from the dropdown menus.`**Dropdown Options for Problem 2:**- a: -1, 0, +1- b: -1, 0, +1- c: -1, 0, +1---This exercise helps students understand and calculate the formal charges of atoms in a molecule, aiding in the study of molecular structure and chemical bonding.

The answer of the above question is given following steps

Answered: Specify the formal charges (both sign…

Specify the formal charges (both sign and magnitude) on the atoms labeled a-c. H3CP-CH3 CH3 1) а -1 b +1 b a (C3H5)3P CH3 2) b >>> >>>

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

+ || A Lewis structure with placeholder elements is shown below. If the formal charge of the central atom is +1, choose the possible identity or identities of the central atom. A) Cl, Br, or I B) Xe C) S or Se D) N, P, or As E) O, S, or Se
What are the formal charges of each atom.
A student proposes the following Lewis structure for the nitrite Z: N (NO2) ion. Assign a formal charge to each atom in the student's Lewis structure. atom formal charge ✗ N ☐ central O ☐ right O ☐
4. Assign any formal charges to atoms that need them (show the details) I I Н I н н Н Н н н 0: Н
Draw the Lewis structure for thiosulfate (S,0,2) with minimized formal changes. How many TOTAL equivalent likely resonance structures exist for S,0,2? Hint: In this case, it is more stable (preferred) to place a negative charge on the larger atom. A) 1 B) 2 C) 3 D) 4 E) 5
A bonded atom is considered to "own" all its nonbonding electrons but only half of the bonding electrons because these are shared with another atom. Therefore, the formal charge formula can be rewritten as follows: TC ▼ Part A FC= valence e in free atom nonbonding e shown Formal Charge for H, O, F, O = + 1 2 bonding e shown [)] Due to the small and highly electronegative nature of fluorine, the oxyacids of the this element are much less common and less stable than those of the other halogens. Bonding theory, however, does allow one to propose structures for these acids and use formal charges for the evaluation of these structures. For al molecule of fluorous acid, the atoms are arranged as HOFO. (Note: In this oxyacid, the placement of fluorine is an exception to the rule of putting the more electronegative atom in a terminal position.) What is the formal charge on each of the atoms? Enter the formal charges in the same order as the atoms are listed. Express your answers as charges…
3. Lewis structures of two chemical species are shown below. For each, give (i) the formal charge on each atom and (ii) the overall charge on each species. Structure a Structure b :F :O-CFo H- Atom 1 Atom 2 Atom 3 Atom 4 Atom 5 Хе Oa Ob Fa Fb H Cl Oa Ob Ос రీరేజిి
Consider the structures below. Calculate the formal charge of each atom in each structure, then indicate which structure is the most accurate. Explain your choice and do NOT base it on the choice of central atom.
Which one is the best Lewis structure? Why? E%3D the first one since the formal charge on the N is -1 O the second one since the formal charge of -1 is on the O :0: : Z
Consider the incomplete structure. Add formal charges as necessary to the structure. What is the net charge on the species? a) +1 b) 0 c) +2 d) −1 e) −2