Concept explainers
Interpretation : Whether each molecule or ion in figures 2.2 and 2.3 are legitimate Lewis structures or not should be confirmed.
Concept Introduction : A legitimate Lewis structure is an electron dot and line bond representation in which the total number of valence electrons is indicated. Number of valence electrons around hydrogen is two. Number of valence electrons around carbon, nitrogen, oxygen, fluorine atom is eight. This is called the octet rule.
Answer to Problem 1CTQ
All the given Lewis structures are legitimate.
Explanation of Solution
In
Total number of valence electrons =
Number of electrons consumed for bonds =
Number of remaining electrons =
The remaining four electrons are added to oxygen atom. Then it completes its octet. Therefore, given Lewis structure for water molecule is a legitimate structure.
In
Total number of valence electrons =
Number of electrons consumed for bonds =
Number of remaining electrons =
The remaining twelve electrons are added to two fluorine atom six for each. Then those complete their octet. Therefore, given Lewis structure for
In
Total number of valence electrons =
Number of electrons gained from negative charges =
Total Number of electrons =
Therefore, given Lewis structure for
In
Total number of valence electrons =
Number of electrons consumed for bonds =
Number of remaining electrons =
The remaining two electrons are added to nitrogen atom. Then it completed its octet. Therefore, given Lewis structure for
In
Total number of valence electrons =
Number of electrons consumed for bonds =
Number of remaining electrons =
The remaining six electrons are added to fluorine atom. Then it completed its octet. Therefore, given Lewis structure for
Thus, all the given Lewis structures are legitimate.
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Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
- Give typed full explanation Look at figure 3-22 that shows the electron density that occurs abound the Si-O bond. This electron density map gives the "shape" of the O and Si atoms when they are bonded together. Think about the answer in Q9 and choose the best response below: (Select answer choice) a. This figure shows that the Si and O atoms, when they bond together, do not form spheres, which is due to the fact that the Si-O bond is strongly covalent and these shared electrons affect atomic shape. This change in shape limits the applicability of Pauling's Coordination principle since that principle is based on the geometry of perfect spheres. b. This figure shows that the Si and O atoms, when they bond together are close to perfect spheres, which is due to the fact that the Si-O bond is strongly covalent. This figure shows that Pauling's Coordination principle should apply very precisely to any substance that contains Si-O bonds c. This figure shows that the Si and O atoms, form in a…arrow_forward1. Molecule: CF4 indicate the number of available electrons that electrons ae = are in the molecule. in the space to the right connect all of the atoms to the central atom and then make each atom follow the octet rule Trial Structure: (duet rule for hydrogen). How many electrons are necessary in the trial ne = structure? Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geOm Hybridization:arrow_forwarda.)Draw a Lewis diagram for IO4- in which the central I atom has a formal charge of zero and show all NONZERO formal charges on all atoms. note overall charge of ion is -1 b.)Draw a Lewis structure for IO4- in which the octet rule is satisfied on all atoms and show all NONZERO formal charges on all atoms. C.Based on formal charge, what is the best Lewis structure for the ion? smallest formal charge or octet rule satisfied for all atomsarrow_forward
- Shown below is the major resonance structure for a molecule. Draw the second best resonance structure of the molecule. Include all non- zero formal charges. c* :0: н н || .C. Click and drag to start drawing a H H structure.arrow_forwardHow do you know when to draw a solid wedge vs a dashed wedge when drawing 3D bond-line structures? I know that solid-wedge means the atom is pointing towards you and dashed wedge means it's in the back, but how do you know which atoms are in the front as opposed to the back? How can you tell what the configuration will look like in space just by looking at the lewis structure or name?arrow_forwardIn the following Lewis structure of [SiF6]²;, every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). :F: :F: 2+ 2- :L: :L:arrow_forward
- In the following Lewis structure of [SiF6]², every atom, bond and lone pair is positioned. To complete the structure, drag the formal charge tags to the appropriate atom(s). Each marker may be used more than once, or not at all. If an atom has a formal charge of zero, do not drag a tag to it. When you drag the marker in, place the little crosshairs in the upper left corner of the marker directly over the atom(s) in question (not above them). :F: :F : :ד: Si 1 :F: 0 0 0 2+ :H: Ë: 0 2-arrow_forwardThe Lewis structure for the chlorate ion is Calculate the formal charge on the chlorine (C1) atom. Express your answer as an integer. ► View Available Hint(s) formal charge on Cl = Submit Previous Answers Incorrect; Try Again; 3 attempts remaining Part B Calculate the formal charge on each of the oxygen (O) atoms labeled a, b, and c in the following Lewis structure. b :O: Express your answers as integers separated by commas. ► View Available Hint(s) b :0: formal charge on Oa, Ob, Oc c =arrow_forwardDraw three resonance structures for CS,. This species has its three atoms bonded sequentially in the following fashion: S-C-S. Draw your resonance structures so that the atoms in them are bonded together in this order. Select the most important resonance structure for this species based on the formal charges on the atoms of the three resonance structures you have drawn. Select the choices from below which make the statements true about this (most important) resonance structure. (a) The leftmost bond (between S and C) is a single v bond. (b) The rightmost bond (between C and S) is a single v bond. (c) The formal charge on the leftmost (S) atom is -Select-v (d) The formal charge on the central (C) atom is -Select---v (e) The formal charge on the rightmost (S) atom is Select-v (f) The number of nonbonding pairs (lone pairs) of electrons in the leftmost (S) atom is Select-v pairs. (g) The number of nonbonding (lone) pairs of electrons in the rightmost (S) atom is -Select-- v pairs.arrow_forward
- a) Draw the Lewis structure for the molecule on the left (labeled as Molecule A above). Draw the Lewis structure which has minimum formal charges. b) Draw the correct Lewis structure for the molecule on the right (labeled as Molecule B above). Draw the Lewis structure which has minimum formal charges. c) Select the three TRUE statements from those provided below. The molecule on the right (Molecule B) is planar (all atoms lie within the same plane). The molecule on the left (Molecule A) is planar (all atoms lie within the same plane). The molecule on the right (Molecule B) has polar bonds. The molecule on the left (Molecule A) has polar bonds. We can distinguish between the two molecules (Molecule A and Molecule B) based upon their dipole moment.arrow_forwardDraw the Lewis structures for the following four molecules, being sure to SHOW ALL STEPS. Structures without work shown will be marked incorrect. Also, one of these molecules has resonance structures – for this compound, make sure to include all resonance structures, indicate formal charges for each atom. SO2 OF2 IF3 NH4+arrow_forwardSome of the figures below represent invalid sets of resonance structures for this molecule.arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning