Concept explainers
(a)
Interpretation: The formal charge on the
Concept Introduction: Formal charge is the electrostatic charge an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms. The formal charge for an atom in a molecule or ion is calculated on the basis of the Lewis structure of the molecule or ion.
(b)
Interpretation: The formal charge on the
Concept Introduction: Formal charge is the electrostatic charge an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms. The formal charge for an atom in a molecule or ion is calculated on the basis of the Lewis structure of the molecule or ion.
(c)
Interpretation: The formal charge on the
Concept Introduction: Formal charge is the electrostatic charge an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms. The formal charge for an atom in a molecule or ion is calculated on the basis of the Lewis structure of the molecule or ion.
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ORGANIC CHEMISTRY-ACCESS
- In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.arrow_forwardWrite Lewis structures for the following: (a) SeF6 (b) XeF4 (c) SeCl3+arrow_forwardWhat is the most polar bond in the molecule?arrow_forward
- If a molecule requires two or more resonance structures to draw it, which of the following statements is true? Select one: A. The molecule does not have a single structure but dynamically oscillates between the resonance structures drawn for it. B. The molecule has lower energy than the computed energy of any of the resonance structures that are drawn for it. O C. The molecule is less stable than any of the resonance structures drawn for it. D. The molecule's resonance structures coexist in an equilibrium with the lower energy form predominating.arrow_forward1. Draw all resonance structures for each of the following molecules or ions. Be sure to include curved arrows that indicate which pair of electrons are shifted in going (flowing) from one resonance structure to the next. a. b. C. 0-2,000arrow_forwardA. Find the moleular formula of diazomethane. b. Draw iits lewis structure and resonance forms as neccessary c. Explain why diazomethane is not very stablearrow_forward
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