Two possible Lewis diagrams for sulfine (H2CSO) are H H. c=s-ö: C-s=0 H H (a) Compute the formal charges on all atoms. (b) Draw a Lewis diagram for which all the atoms in sulfine have formal charges of zero.
Q: In the molecule below, the formal charge on the left O is v, on the N is v, and on the right O is
A: Formal charge on atom in a molecule = ( total no. of valence e-) - ( total no. of non-bonding e-) -…
Q: Acetyl chloride, CH:C(O)CI, is used as a reagent for the acylation of salicylic acid in the…
A: Answer: The molecule which has a net dipolemoment would be the polar in nature. The acetyl chloride…
Q: Cyanic acid, HOCN, and isocyanic acid, HNCO, dissolve in water to yield the same anion on loss of…
A: The structure which represents the valence shell electrons in a molecule, is called the Lewis…
Q: Specify the formal charges (both sign and magnitude) on the atoms labeled a-c.
A:
Q: 1.38, Assuming the following species consist of ions, write the tions and (if appropriate) the Lewis…
A: Here, we have to write the electronic configurations and draw the Lewis symbol for the cations that…
Q: Write the Lewis structures for the following molecules, including all resonance forms, and show…
A:
Q: Which of the followings shows the correct formal charges on the atoms of SCN-1 ion?
A: To calculate formal charge of an atom in a molecule. Formal charge=Valence electrons - Non bonding…
Q: What is the formal charge of nitrogen in nitrate ion, NO3-? A. 0 B +1 C. -1 D. +2
A: Formal charge: The formal charge (FC) is the charge assigned to an atom in a molecule, assuming that…
Q: Write the Lewis structure for each ion. Include resonance structures if necessary and assign formal…
A: The molecule considered is SO42-, the sulfate ion.
Q: Calculate the formal charge of carbon and oxygen in the 2 compounds and compare the polarity of each…
A: Formal charge is the charge acquired over an element in compound after bond formation and is given…
Q: H3C-Se-CH,
A: Specify the formal charges (both sign and magnitude) on the atoms labeled a-c in the given…
Q: Calculate the formal charge of oxygen in the compound H. H.
A: In this question we have to calculate formal charge on oxygen atom . First we have to know valence…
Q: Draw a Lewis dot structure for the fictitious molecular ion [ZO6]-4. Assume that the central Z atom…
A: The molecular geometry of molecule is octahedral when central atom is bonded to six atoms. The given…
Q: Specify the formal charges (both sign and magnitude) on the atoms labeled a-c
A: Calculate the formal charge on a,b,c in the given structure?
Q: Determine the formal charge on each atom in the ion H3O+ ?
A: The given molecule is H3O+.
Q: In the cyanate ion, OCN-, carbon is the central atom. (a) Draw as many resonance structures as you…
A:
Q: In the structure below, identify the atom that carries a non-zero formal charge. :i: -NH 0: Give…
A:
Q: O.
A:
Q: Draw a Lewis diagram for BrO4- in which the central Br atom has a formal charge of zero and show all…
A: Steps involved to write Lewis structures 1. Determine total number of valence electrons 2. Least…
Q: chloric acid (HCIO3) Calculate the formal charge of each atom by drawing the possible Lewis…
A:
Q: Write the Lewis structures for the following molecules, including all resonance forms, and show…
A: Lewis structure is shows bonding electron between atoms and lone pair on elements. Resonance…
Q: d) For the structure below, calculate the formal charge of each atom. 2- :0: Lö: e) Does this…
A: Introduction : Formal Charge : The formal charge of an atom in a polyatomic ion or molecule may be…
Q: The hypochlorite ion, ClO-, is the active ingredient inbleach. The perchlorate ion, ClO4-, is a main…
A: Hey, since there are multiple sub-parts posted, we will answer first three sub-parts. If you want…
Q: Part A The Lewis structure for the chlorate ion is b :0: Calculate the formal charge on the chlorine…
A:
Q: What are the formal charges on the sulfur (S), carbon (C), and nitrogen (N) atoms, respectively, in…
A: Solution: Formal charge = valance electrons - (no of bonded electrons / 2) - non bonded electrons.
Q: A student generates three possible resonance structures for the compound NCCI, which are provided in…
A: Since you have asked a question with multiple sub-parts, we will solve first three sub-parts for…
Q: Specify the formal charges (both sign and magnitude) on HC=CH 1) > > >
A: The charge present on an atom in a polyatomic molecule or a polyatomic ion is knowns as the formal…
Q: Draw the Lewis structure of ClO3-. Include formal charges.
A: In ClO3- ion the central atom is chlorine and the number of valence electrons present is seven.…
Q: (a) Draw Lewis structure of the following: (i) H3PO4 (ii) N3 - (b) How…
A: a) i) ii)
Q: Lewis structures showing all valence electrons. Assign formal charges in structure as appropriate
A: Formal charge is calaculated by the given formula, Formal charge(FC)=V-N-B2.......1V=Valance…
Q: Calculate the formal charge of oxygen in the compound * H -1
A:
Q: Write a Lewis electron dot diagram for phosphoryl chloride,POCl3 (Fig. 3.29). Assign formal charges…
A: Lewis dot structures are proposed by the scientist named Lewis to show the valence electrons around…
Q: Draw the Lewis structure with lowest formal charges, anddetermine the charge of each atom in (a)…
A: (a) The total number of valence electrons present in BF4- is calculated as, The total number of…
Q: s the Lewis structure of formaldehyde, also known as "formalin", a fixative for biological…
A: We can use the concept of dipole moment to find the partial positive and negative charge.
Q: What are the formal charges present in in the ion CH3NH3*? Assume all atoms other an hydrogen hau an…
A: Given molecule is , CH3NH3+
Q: In the Lewis structure shown here, A, D, E, Q, X, and Z representelements in the first two rows of…
A: In the Lewis structure, a solid line indicates a bond formed by sharing of two electrons between the…
Q: e formal charge on the Nitrogen atom in NO3-
A: Formal charge = Group No. - ( bonds + bonding electrons) Or Formal charge = Valence electrons -…
Q: Determine the formal charges on all the atoms in the following Lewis diagrams. A в :C=S- 0: s=c=ö…
A:
Q: Specify the formal charges(both sign and magnitude) on the atoms labeled a-c.
A:
Q: Write the Lewis structure for each ion. Include resonance structures if necessary and assign formal…
A: Lewis structure of SO32-
Q: What is the formal charge on each atom in HNO3 and the Lewis structure for it?
A: The Lewis structure for HNO3 is shown below,
Q: What is the formal charge on each atom in CH3Cl and the Lewis structure for it?
A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…
Q: COO + 1 H₂N-C-H ساد O گیا۔ ی =0
A: formal charge is charge on the atom in an ion as it has more or less electrons than it normally…
Q: Draw a Lewis dot structure for the fictitious molecular ion [ZO4]-3. Assume that the central Z atom…
A: formal charge is the charge assigned to an atom in a molecule as you mean that electrons in all…
Q: Draw Lewis structures for these ions and show which atom (or atoms) in each bears the formal charge.…
A:
Q: How many resonance structures can be drawn for the hydrogen tellurate ion (HTeO4–) in which the…
A: The formal charge (FC) of an atom in a molecule can be determined by relating the valence electrons…
Q: 3. Lewis structures of two chemical species are shown below. For each, give (i) the formal charge on…
A:
Q: Which of the following structures would we expect for nitrous acid? Determine the formal charges:…
A:
Q: Which atom would you expect to be in the center of the Lewis Structure of HCN and what is the formal…
A: Answer: HCN is called as hydrogen cyanide, in which four valencies of carbon are being completed by…
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 9 images
- Compare the electron dot structures of the carbonate</o:p> (CO32- ) and borate (BO33- ) ions.</o:p> (a) Are these ions isoelectronic?</o:p> (b) How many resonance structures does each ion have?</o:p> (c) What are the formal charges of each atom in these ions?</o:p> (d) If an H+ ion attaches to CO32- to form the bicarbonate ion, HCO3- , does it attach to an O atom or to the C atom?</o:p> </o:p>The hypochlorite ion, ClO-, is the active ingredient inbleach. The perchlorate ion, ClO4-, is a main componentof rocket propellants. Draw Lewis structures for both ions. (a) What is the formal charge of Cl in the hypochlorite ion?(b) What is the formal charge of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (c) What is theoxidation number of Cl in the hypochlorite ion? (d) Whatis the oxidation number of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (e) In a redox reaction,which ion would you expect to be more easily reduced?Assign formal charges to all atoms in the following Lewis diagrams. (a) ClO, :ö: (b) SO2 ö-s=0 :ö-Cl-ö: :0: (e) BrO5 :0-Br-ö: (d) NOŽ ö=N-ö: :0:
- Consider the formate ion, HCO2", which is the anion formed when formic acid loses an H* ion. The H and the two O atoms are bonded to the central C atom. (a) Draw the best Lewis structure(s) for this ion. (b) Are resonance structures needed to describe the structure? Explain briefly (c) Would you predict that the C-O bond lengths in the formate ion would be longer or shorter relative to those in CO2? Explain brieflyCyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.#6. Consider the Lewis structure below where X is an element from the third period (Na-Ar). (a) Identify the central atom, X, when n = - -1. (b) Determine the formal charge on X. (c) Draw a Lewis structure so that the formal charge on X is equal to +1. :Ö: [+] n-
- A stable triatomic molecule can be formed that contains one atom each of nitrogen, sulfur, and fluorine. Three bonding structures are possible, depending on which is the central atom: NSF, SNF, and SFN. (a) Write a Lewis diagram for each of these molecules, indicating the formal charge on each atom. (b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule— namely, NSF, which has a central sulfur atom? (c) Does consideration of the electronegativities of N, S, and F from Figure 3.18 help rationalize this observed structure? Explain. 100. The gasWrite Lewis dot symbols for the following atoms and ions: (a) I (b) I-(c) S(d) S2-(e) P (f) P3-(g) Na (h) Na+(i) Mg (j) Mg2+Draw Lewis structures for HFO4, HFO3, HC0O4, HC0O3, HCO2. (These molecules have the halogen atom as the central atom. All O atoms are attached to the halogen. The hydrogen atom is bonded to one of the O atoms.) Use formal charges to determine which molecule is least likely to occur in nature. (A) HFO4 (B) HC(O2 (C) HC!O3 (D) HFO3 (E) HC\O4 DO000
- Draw resonance structures for the bicarbonate ion, HCO3-. (a) Does HCO3- have the same number of resonance structures as the CO32- ion? Are any less likely than others? (b) What are the formal charges on the O and C atoms in HCO3- ? What is the average formal charge on the O atoms? Compare this with the O atoms in CO32- . (c) Protonation of HCO3- gives H2CO3. How do formal charges predict where the H+ ion will be attached?Help meA stable triatomic molecule can be formed that containsone atom each of nitrogen, sulfur, and fluorine. Threebonding structures are possible, depending on which is thecentral atom: NSF, SNF, and SFN.(a) Write a Lewis diagram for each of these molecules,indicating the formal charge on each atom.(b) Often, the structure with the least separation of formal charge is the most stable. Is this statement consistent with the observed structure for this molecule—namely, NSF, which has a central sulfur atom?(c) Does consideration of the electronegativities of N, S,and F from Figure 3.18 help rationalize this observedstructure? Explain.