Interpretation: It should be determined for the S atom which exceeds the Octet configuration in the following molecule.
Concept Introduction:
Octet Rule:
Thus is a chemical rule of thumb that reflects observation that atoms of main – group elements tend to combine in such a way that each atom has eight electrons in its valence shell.
Resonance structures:
A molecule or ion which show more than structure but none of them are accurately correct show the known property of that molecule, and can lie between the canonical structure is known as resonance or canonical or contributing structure.
Polarity is the separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multiple moments.
Polar molecule must contain polar bond due to presence of electronegativity dereference between the bonded atoms.
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
Chemistry & Chemical Reactivity
- Use condensed electron configurations and Lewis electron-dot symbols to depict the ions formed from each of the follow-ing atoms, and predict the formula of their compound:(a) Ba and Cl (b) Sr and O (c) Al and F (d) Rb and Oarrow_forwardPart A) Out of the following, the species with a single covalent bond is: (a) CO (b) CN- (c) Cl2 (d) N2 Part B) Which of the following compounds has ionic bonds only? (a) NH4ClO4 (b) Mg3N2 (c) Mg3(PO4)2 (c) CHCl3 Part C) The molecular shape and polarity of xenon tetrafluoride are: (a) Tetrahedral & non-polar (b) square planar & non-polar (c) Square pyramidal & polar (d) square planar & polararrow_forwardIn developing the concept of electronegativity, Pauling used the term excess bond energy for the difference between the actual bond energy of X¬Y and the average bond energies of X¬X and Y¬Y (see text discussion for the case of HF). Based on the values as shown, which of the following substances contains bonds with no excess bond energy?(a) PH3 (b) CS2 (c) BrCl (d) BH3 (e) Se8arrow_forward
- In developing the concept of electronegativity, Pauling usedthe term excess bond energy for the difference between the ac-tual bond energy of X−Y and the average bond energies of X−X and Y−Y (see text discussion for the case of HF). Based on the values in Figure , which of the following sub-stances contains bonds with noexcess bond energy?(a) PH₃ (b) CS₂(c) BrCl(d) BH₃ (e) Se₈arrow_forwardWhich compound in each of the following pairs has the larger lattice energy? Note: Mg2+ and Li+ have similar radii; O2– and F– have similar radii. Explain your choices.(a) MgO or MgSe(b) LiF or MgO(c) Li2O or LiCl(d) Li2Se or MgOarrow_forward(c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F. 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smalleor going down the halogen group from HF to HI Describe these observationsarrow_forward
- Which of the following elements does not follow the octet rule? (a) sodium (b) helium (c) krypton (d) carbon (e) sulfurarrow_forwardChemistry 7. An ionic bond is formed between a cation A+ and anion B. How would the energy of the ionic bond be affected (smaller/higher/double etc) by the following changes? (a) Doubling the radius of A+ (b) Tripling the charge on A+ (c) Doubling the charges on A (d) Decreasing the radii of A and B to half their original values. and Barrow_forwardPredict which one of thefollowing orderings of lattice energy is correct for theseionic compounds.(a) NaCl > MgO > CsI > ScN (b) ScN > MgO > NaCl > CsI(c) NaCl > CsI > ScN > CaO a(d) MgO > NaCl > ScN > CsI(e) ScN > CsI > NaCl > MgOarrow_forward
- Use condensed electron configurations and Lewis electron-dot symbols to depict the ions formed from each of the follow-ing atoms, and predict the formula of their compound:(a) Cs and S (b) O and Ga (c) N and Mg (d) Br and Liarrow_forwardWhich compound in each of the following pairs has the larger lattice energy? Note: Ba2+ and K+ have similar radii; S2– and Cl– have similar radii. Explain your choices.(a) K2O or Na2O(b) K2S or BaS(c) KCl or BaS(d) BaS or BaCl2arrow_forward(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe—O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in (a) yields the most favorable formal charges for the molecule?arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning